GIFT OF
MICHAEL REESE
ALUMINIUM:
ITS HISTORY, OCCURRENCE, PROPERTIES,
METALLURGY AND APPLICATIONS,
INCLUDING ITS ALLOYS.
BY
JOSEPH W. RICHARDS, A.C.,
CHEMIST AND PRACTICAL METALLURGIST ; MEMBER OF THE DEUTSCHE
CHEMISCHE GESELLSCHAFT.
ILLUSTRATED BY SIXTEEN ENGRAVINGS.
PHILADELPHIA :
HENRY CAREY BAIRD & CO.,
INDUSTRIAL PUBLISHERS, BOOKSELLERS AND IMPORTERS,
810 WALNUT STREET.
LONDON:
SAMPSON LOW, MARSTON, SEARLE & RIVINGTON,
CROWN BUILDINGS, 188 FLEET STREET.
1887,
COPYRIGHT BT
JOSEPH W. RICHARDS,
COLLINS PRINTING HOUSE,
705 Jayne Street.
PREFACE.
Xo apology is necessary in presenting a work on
aluminium in English. In 1858 Tissier Bros, pub-
lished in France a small book on the subject. H.
St. Claire Deville, the originator of the aluminium
industry, published a treatise, also in French, in
1859. Deville's book is still the standard on the
subject. Until December, 1885, we have an inter-
mission, and then a work by Dr. Mierzinski,
forming one of Hartleben's Chemisch-Techuische
o
Bibliothek, which is a fair presentation of the
industry up to about 1883, this being a German
contribution. Probably because the English-
speaking people have taken comparatively little
hand in this subject we find no systematic trea-
tise on aluminium in our language. The present
work aims to present the subject in its entirety to
the English reader.
Tissier, Deville, Mierzinski, and the German,
French, and English scientific periodicals have
IV PREFACE.
been freely consulted and extracted from, full
credit being given in each case to the author or
journal. As this art has of late advanced so
rapidly it has been a special aim to give every-
thing that has been printed up to the time of pub-
lication.
The different parts of the work are arranged in
what seemed their logical order, corresponding
closely to that followed by Deville. The Appendix
contains an account of laboratory experiments, etc.,
several of which, it is trusted, may be of value.
In conclusion, the author wishes to thank the
faculty of his "Alma Mater," Lehigh University,
for their permission to use his Thesis on Alumin-
ium as the basis of this treatise ; also, to acknowl-
edge his indebtedness to Dr. Wm. H. Greene, of
Philadelphia, for assistance rendered in the prep-
aration of the work for the press.
J. W. R.
PHILADELPHIA, November 25, 1886.
LIST OF REFERENCES.
Tissier Recherche de 1' Aluminium. C. & H.
Tissier. Paris, 1858.
Deville De 1' Aluminium. H. St. Claire De-
ville. Paris, 1859.
Watts Watts' s Dictionary of Chemistry,
vol. i.
Mierzinski .... Die Fabrikation des Aluminiums.
Dr. Mierzinski. Vienna, 1885.
Compt. Rend. . . . Comptes Rendus de les Sciences de
1'Academie. Paris.
Wagner's Jahresb. . Wagner's Jahresbericht der Chem
ische Technologic.
Phil. Mag The London and Edinburgh Philo-
sophical Magazine.
Mon. Scientif. . . . Le Moniteur Scientifique. Dr.
Quesnesville.
Fremy Encyclopedic Chemique. Fremy.
Paris, 1883.
Dingl. Joul Dingler's Polytechnisches Journal.
Pogg. Ann Poggendorff''s Annalen.
Jrnl. der Pharm. . . Journal der Pharmacie.
Bull, de la Soc. Chem. Bulletin de la Soci6t6 Chemique de
Paris.
Sci. Am. (Suppl.) . . Scientific American (Supplement).
Eng. and Mng. Jrnl. . The Engineering and Mining Journal.
Chem. News . . . The Chemical News.
Jahresb. der Chem. . Jahresbericht ueber die Fortschritte
der Chemie.
FO RMU L JE.
Al . . . . Aluminium.
A12O3 . . . Alumina.
A12C16 . . . Aluminium chloride.
K . . . . Potassium.
KOH . . . Caustic Potash.
KC1 . . . Potassium chloride.
Na. . . . Sodium.
Al2Cl6.2NaCl. Aluminium-sodium double chloride.
Si ... . Silicon.
Fe . . . . Iron.
Cu . . . . Copper.
TEMPERATURES.
Unless stated otherwise, all temperatures given are in Centi-
grade degrees.
CONTENTS.
PART I.
HISTORY OF ALUMINIUM.
PAGE
Lavoisier's suggestion of the existence of metallic bases
of the earths and alkalies ; Researches in preparation
of aluminium, by Davy, Oerstedt, and Wohler . . 25
Isolation of aluminium, by H. St. Claire Deville, in 1854 26
Patronage of Emperor Napoleon III. ; Aluminium at the
Paris Exhibition, 1855; Its manufacture on a large
scale at Glaciere, Nanterre, and Salindres ; Tissier
Bros.' book on aluminium in 1858 .... 28
Deville' s book, 1859 ; History of the works near Rouen 29
Deville's explanation of the uses of the new metal . 30
Alfred Monnier's production of aluminium at Camden,
N. J., 1856 31 '
W. J. Taylor claiming the possible cost of aluminium at
§1 per pound; Kerl and Stohman's r£sum£ of the
manufacture of aluminium up to 1874 ... 32
Dr. Clemens Winckler's retrospect of the development of
aluminium, 1879 33
Manufacture of aluminium in England, France, and Ger-
many ; Aluminium beams for balances, made by Sar-
torius of Gottingen; Difficulties in using aluminium for
mathematical instruments ; Action of molten aluminium
upon earthen crucibles ...... 35
Vlll CONTENTS.
PAGE
Prices of aluminium and of aluminium bronze in France ;
Webster's aluminium works in England . . .36
Col. William Frishmuth's invention for producing alu-
minium at reduced cost; Opinion of his invention by
Major Ricarde-Seaver, F.R.S.E 37
Col. Frishmuth's works in Philadelphia ; Aluminium cast-
ing for the Washington Monument, made by Col. Frish-
muth ; Census report of his annual production ; His
price in bars ........ 39
Imports and consumption of aluminium in the United
States from 1870 to 1884 ; Its production in Philadel-
phia by Col. Frishmuth in 1883, 1884 ... 40
Cowle's process for making aluminium bronze at Cleve-
land, Ohio ; Present state of aluminium industry as
described by Prof. Charles F. Mabery, of Cleveland,
Ohio, and Dr. T. Sterry Hunt, of Montreal . .41
PART II.
OCCURRENCE OF ALUMINIUM IN NATURE.
Combinations of aluminium with oxygen, alkalies, and
acids, etc. ; Formulae of aluminium silicates . . 43
Appearance of most of the aluminium compounds ; For-
mulae of some of the precious stones .... 44
Minerals most used for producing aluminium; Beauxite . 45
Analyses of beauxite 46
Cryolite ; Where found, description, and general uses ;
Its importation by the Pennsylvania Salt Co., of Phila-
delphia ; Native cryolite in the United States . . 48
Imports of cryolite into the United States ; Corundum ;
Its great source of supply 49
Probable sources of supplies of materials for production
of aluminium in the United States and Great Britain . 50
CONTENTS. IX
PART III.
PHYSICAL PROPERTIES OF ALUMINIUM.
PAGE
Table of analyses of commercial aluminium ... 51
Free and combined silicon in aluminium ; Gases in alu-
minium ......... 52
Composition of the aluminium apex of the Washington
Monument at Washington, D. C., cast by Col. Frish-
muth ; Color of aluminium ; As described by Deville,
Fremy, Mallet, and Mierzinski ..... 53
Mat ; As described by Deville, Mierzinski, and Bell Bros. 54
Polish and lustre ; Processes for producing as given by
Deville, Bell Bros, and Kerl and Stohman . . 55
Odor ; As given by Deville and Watts .... 56
Taste — Deville; Malleability — Deville and Mallet on this
subject ......... 57
M. Degousse's success in beating aluminium into leaves;
Substitution of aluminium for silver leaf; Kerl &
Stohman on rolling and annealing aluminium . . 58
Bell Bros, on beating aluminium ; Mierzinski on extensi-
bility of aluminium ....... 59
Aluminium leaf first made by C. Falk & Co., Vienna;
Ductility ; Drawing aluminium wire ; Results obtained
by Deville, Vangeois, and Bell Bros. ... 60
Elasticity, Tenacity, Hardness — Deville, Wertheim, Mul-
let, Fremy; Kerl & Stohman on engraving aluminium 61
Mierzinski and W. H. Barlow on tensile strength;
Tables ; Comparative mechanical value of aluminium,
steel, etc 62
Table of strength of aluminium wire; Sonorousness; Re-
sults obtained by Deville and M. Lissajous in making
bells and tuning-forks ...... 63
Results obtained by Faraday and Watts ; Density ; De-
ville's table of comparison with other metals . . 64
X CONTENTS.
PAGE
Comparative value of equal volumes of aluminium and
silver ; Specific gravity of absolutely pure aluminium,
Mallet ; Fusibility ; As given by Deville, Mallet, and
Mierzinski ...... 65
Fixity ; As given by Deville, Watts, and Fremy ; Elec-
tric conductivity ; Results obtained by Deville and M.
Buff , ... .66
Comparison with copper and magnesium, Fremy ; Ther-
mal conductivity; Deville, Faraday, and Watts, etc.,
on this subject . . . . • . . . .67
Mierzinski, Calvert, and Johnson on this subject ; Spe-
cific heat ; Deville, Regnault, Paul Morin, Mallet, and
Fremy on this subject 68
Magnetism; Deville, MM. Poggendorff and Reiss ; Crys-
talline Form ; Deville on this subject ... 69
PART IV.
CHEMICAL PROPERTIES OF ALUMINIUM.
Remark; Action of air; Deville' s observations . . 70
Cupellation of aluminium ; Observations of Wohler, Peli-
got, Watts, etc. 71
Action of water ; Deville on this subject . . .72
Mierzinski and the Chemical News ; Action of hydro-
gen sulphide and sulphur ; Deville and Fremy . . 73
Sulphuric acid ; Deville, M. de la Rive, and Fremy . 74
Nitric acid ; Deville and M. Hulot ; Hydrochloric acid ;
Deville, M. Favre, and others ..... 75
Potash, soda, and lime ; Deville, Mallet, Mierzinski . 77
Aqua ammonia ; Deville and Wohler ; Organic acids,
vinegar, etc. ; Deville, M. Paul Morin ; Use of Alu-
minium for culinary articles ..... 78
Solutions of metallic salts ; Precipitation of other metals
by aluminium ; Deville, Tissier, Paul Morin, Mourey,
Christofle, Hulot .79
CONTENTS. XI
PAGE
Mierzinski. Fremy and Watts 81
Nitre ; Purification by nitre ; Deville, Fremy, and Mier-
zinski on this subject 83
Silicates and borates ; Action on glass and crucible clay ;
Deville and Tissier ; Fluorspar ; Tissier on its use as
a flux 84
Phosphate of lime, Tissier on this subject ; Sodium chlo-
ride and chlorides, Deville; Tissier on their use as
fluxes 85
Metallic oxides ; Tissier' s experiments .... 86
Mierzinski ; Beketoff 's experiments ; Animal matters ;
Deville and M. Charriere on the use of aluminium in
surgery . . . . . . . . .87
Miscellaneous agents; Tissier and Mierzinski on this
subject .88
General observations on the properties of aluminium,
Deville 88
PART V.
METALLURGY OF ALUMINIUM.
.Oerstedt's original paper on isolation of aluminium, 1824 90
AYohler, the true discoverer of the metal ; Wohler's first
paper . .91
Wohler's second paper ....... 93
Deville' s remarks on the metal obtained by Wohler . 95
Deville' s improvement, 1854-55 ..... 96
Deville' s apparatus at Javel and Glaciere described and
illustrated ......... 98
Deville's experiments with sodium vapor . . . 100
Reduction from cryolite ; H. Rose's entire paper . . 103
Dr. Percy's investigations as laid before the Royal Insti-
tution 115
Allan Dick's paper, November, 1855 . . . .116
Xll CONTENTS.
PAGE
Deville's account of his researches . . . .118
Wohler's improvement on Deville's process; Watts on
the reduction of cryolite ; Gerhard's furnace . .126
Watts's summary of the use of cryolite . . .127
General remarks . . . . . . .128
PART VI.
THE MANUFACTURE or SODIUM.
Preliminary observations . . . . . .130
Summary, taken principally from Mierzinski ; Efforts of
Davy, Gay Lussac, Thenard, Curaudau, Brunner,
Donny, and Mareska . . . . . .131
Donny and Mareska's condenser, illustrated; Deville's
account of its operation . . . . • . . 132
Object of and disadvantage in use of chalk ; Preliminary
calcination of the mixture ; Illustration of the furnace. 133
Decomposition retorts, illustrated 134
Operation in the retorts . . . . . .135
Deville, Rivot, and Tissier on the temperature . . 137
Wagner's improvement; Attempts to reduce potassium
and sodium together . . 138
Weldon's calculation of the cost of sodium ; Making of
sodium in New York City, N. Y. ; Castner's Ameri-
can patent process . . . . • • .139
Claims made in Castner's patent ... . 141
Reduction of sodium by electricity, Mierzinski, Davy;
Jablochoff's apparatus described and illustrated . . 142
PART VII.
MANUFACTURE OF ALUMINA.
Present state of the industry ; Tilghman's process . . 144
Manufacture from cryolite ; Dry way . . . . 146
CONTENTS. Xlll
PAGB
Thomson's furnace described and illustrated . . .147
Preference for mechanical furnaces as used in manufac-
ture of soda, potash, etc 148
Precipitation of solution of sodium aluminate, according
to Lowig 151
Wet way 152
Manufacture from alum-stone or shales . . . .153
PART VIII.
MANUFACTURE OF THE DOUBLE CHLORIDE OF ALUMINIUM
AND SODIUM.
Preliminary remarks 154
Mierzinski, Deville, and M. Dullo on this subject . . 155
Manufacture by using hydrochloric acid and carbon di-
sulphide 157
PART IX.
MANUFACTURE OF ALUMINIUM AT SALINDRES (GARD).
Aluminium as made by A. R. Pechiney & Co., successors
to Henry Merle & Co 158
Reactions involved in and outline of the process . .158
Preparation of the aluminate of soda ; Material used ;
Composition of mixture ; Calcination, washing, filter-
ing, with illustration of filtering apparatus . . . 159
Preparation of the alumina ; Description of precipitating
tank and method of precipitation, washing, and dry-
ing, illustrated 163
Preparation of aluminium — sodium double chloride . 166
Illustration of furnace ; Mixing and shaping the charge ;
Condenser . . . . . . . .167
2
XIV CONTENTS.
PAGE
Reduction of the double chloride by sodium ; Illustration
of furnace ; Difficulties met ; Method of charging, re-
ducing, and running out 168
Average cost of manufacture at Salindres in 1872. . 172
Later improvements in Deville's process ; Webster's pro-
cess; History and description of the plant ; Where its
advantages lie ; Utilization of bye products . .173
Frishmuth's process ; Patent claims . . . .178
Other processes; Niewerth's method of reduction by nas-
cent sodium ; Grousillier's reduction under pressure . 179
PART X.
REDUCTION OF ALUMINIUM BY OTHER REDUCING AGENTS
THAN SODIUM.
Reduction by Cyanogen; Knowles's patent; Corbelli's
patent 180
Deville's and Watts' s comments ; Reduction by hydrogen ;
Process of F. W. Gerhard; Comment by Watts . 181
Reduction by carburetted hydrogen ; Process of A. L.
Fleury, of Boston 182
^Petitjean's process . . . . . . .183
Reduction by double reaction ; Processes of M. Comenge
and Johnson . . . . . . . . 1 84
Process of Niewerth . . . . . . .185
Reduction by carbon and carbon dioxide ; Process of J.
Morris, of Uddington 187
Reduction by carbon ; Article by M. Chapelle . .188
Statement of G. W. Reinar ; Cowles Bros.' process . 189
Patent claim of Messrs. Cowles 190
Prof. Charles F. Mabery's official account of Cowles Bros.'
process 191
Dr. T. Sterry Hunt's paper read before the American
Institute of Mining Engineers . . . . .194
CONTENTS. XV
PAOB
Dr. Hunt's address before the National Academy of
Science 196
W. P. Thompson's complete description of the process . 197
Illustrative description of the furnace ; Mode of operat-
ing furnace, and improvements thereon ; Amount re-
duced ; Ores used 199
Reduction by iron ; Lauterborn's process not new ; Pa-
tents of F. Lauterborn and of H. Niewerth . . 206
Preparation of aluminium and sodium in the Bessemer
converter; W. P. Thompson's experiments . .207
Calvert and Johnson's experiments .... 209
Reports of Fremy, Watts, Benzon, Evrard . . .211
Silicon bronze, by Evrard; Ostberg's statement of the
iron-aluminium alloy used in the mitis process ; Re-
duction with copper ; Calvert and Johnson's process . 212
Kerl and Stohman's account of Benzon's process . .213
Laboratory tests of this process ; Reduction by zinc ;
Dullo's observations . . . . . . .214
Patent of M. N. Basset 215
Wedding's remarks on Basset's process . . .217
Kagensbusch's singular proposition; Fred'k J. Seymour's
patent 218
Extraordinary claim in Seymour's second patent . . 220
American Aluminium Co., Detroit; Reduction by lead;
Wilde's invention 221
Reduction by manganese ; Claims of W. Weldon, Bur-
stow, England ; Reduction by electricity . . . 222
Deville's account of the process ..... 223
Sectional illustration of the crucibles .... 224
Bunsen and Deville on the subject 225
Mierzinski's practical remarks . . . . .226
Patented improvement by Richard Gratzel, Germany,
illustrated 228
Duvivier's experiment with electric current . . . 229
XVI CONTENTS.
PAGE
Kagensbusch's proposition ; Gaudin's " economic" reduc-
tion of aluminium ....... 230
Metals coated with aluminium by Thomas and Tilly ;
Depositing of aluminium by Corbelli and J. B.
Thompson 231
Patented process by J. A. Jeancon ; Experiments by M.
A. Bertrand, C. Winkler, and Sprague . . .232
Electrolyses of M. L. Senet, Gerhard, and Smith ; De-
composition of a solution of alum by J. Braun ; Moses
G. Farmer's patent for obtaining aluminium . . 233
Mierzinski's denial of the successful deposition of alu-
minium from an aqueous solution of its salt ; Alumin-
ium and nickel plating at Frishmuth's works . .234
PART XI.
WORKING IN ALUMINIUM.
Melting aluminium ; Deville's instructions . . . 235
Kerl and Stohman's instructions 236
Mierzinski's instructions; Casting aluminium; Deville's
instructions 237
Purification of aluminium ; Freeing from slag, Deville . 238
Process of Paul Morin 239
Watts' s suggestion ; Freeing from impurities, Deville . 240
Mierzinski's recommendation . . . . .242
Buchner's treatment of commercial aluminium to elimi-
nate silicon; Mallet's process of obtaining pure from
commercial aluminium ; Uses of aluminium . . 243
Aluminium plating and aluminium leaf . . . .246
Aluminium coins ; Soldering aluminium ; Deville's
views on . . . . . . . . .247
Hulot's process ; Monrey's solder 248
Mierzinski's statements as to Mourey's solder; Improve-
ments of Schwarz ; Formulae for these solders . .249
CONTENTS. XV11
PAGE
Frishmuth's solders; Kerl and Stohman on Mourey's
solders, with formulae ...... 250
Process of Bell Bros 252
Veneering with aluminium; Deville's account of- the
success of M. Sevrard in 1854 253
Dr. Clemens Winckler on this subject . . . .254
Gilding and silvering ahminium ; Failures of Deville
and Morin ; Success of Mourey and Christofle . . 256
Watts, and Kerl and Stohman, on this subject . .257
PART XII.
ALLOYS OF ALUMINIUM.
General remarks, Mierzinski ..... 258
Aluminium and silicon ; Tissier and Deville . . . 259
Aluminium and mercury ; Statements of Deville and
Watts ; Aluminium amalgam made by Caillet with the
battery 261
Joules' s method of electrolyzing 262
Properties of aluminium amalgam ; Fremy, Tissier,
Gmelin on this subject ...... 263
Aluminium and copper; Tissier Bros., 18e8 . . . 264
Deville, 1859 ; Use of the alloy by Christofle ; Alloy de-
scribed by Debray ; Composition of aluminium bronze 265
Properties of aluminium bronze ; M. Lechatelier's table
of its strength ; Experiments by A. Gordon . . 266
M. Boudaret on its malleability ; Mierzinski on points to
be attended to in making the aluminium bronze . .267
Directions to be observed in casting ; Comparative
strength of the bronze 268
Hulot's solder ; Fremy's instructions ; Kerl and Stohman's
directions 269
Bronze for philosophical instruments; Specific gravity
and strength ; Comparative strength of the alloys ;
Their specific gravities 270
XVlll CONTENTS.
PAOE
Melting point of 10 per cent, bronze ; B. S. Procter's ex-
periments . . . . . . . . .271
Thurston on the properties of aluminium bronze . . 272
Strange and Knight on the properties of aluminium
bronze 273
Alloys made by Cowles Bros. 274
Strength of these alloys by the testing machine . . 27G
Alloys of aluminium and copper with other metals;
Neogen made by F. H. Sauvage . . . .277
Minargent ; P. Baudrin's alloy ; James Webster's
patent bronze . . . . . . . .278
Phosphor aluminium bronze made by Thomas Shaw,
Newark, N. J.; Cowles Bros.' reports of the strength
of aluminium silver castings ; Solders for aluminium
bronze for jeweller's use ...... 279
Silicon and aluminium bronze, Cowles Bros.; Aluminium
and iron; Tissier Bros.' alloy; Deville, Rogers . 280
Fremy and Mierzinski on aluminium alloys . . . 282
Ostberg's mitis castings, with description of the process . 283
Alloy used by Ostberg, Worcester, llass. . . . 285
Ostberg's note to the Engineering and Mining Journal ;
Watts's note; Mr. Sellers's series of experiments . 286
Aluminium and zinc; Tissier Bros., Deville, Kerl and
Stohman, and Fremy on these alloys . . . .287
Aluminium and tin ; Tissier Bros., Deville, and Keii
and Stohman on this subject ..... 289
Fremy, Mierzinski, and M, Bourbouze . . . 290
Aluminium and lead; Tissier, Deville, Kerl and Stohman,
and Mierzinski . . . . . . . .291
Aluminium and antimony ; Tissier, and Kerl and Stoh-
man; Aluminium and bismuth ; Tissier and Watts . 292
Aluminium and nickel ; Tissier and Mierzinski . . 293
Argentan .....'.... 294
Minargent . . . 295
Aluminium and silver ; Tissier on this subject . . 295
CONTENTS. XIX
PAflB
Deville ; Kerl and Stohman ; Fremy .... 296
Mierzinski ; "Tiers Argent;" Cowles Bros, on "Alu-
minium silver" 297
Aluminium and gold ; Tissier, Fremy, and Mierzinski
on these alloys 298
Aluminium and platinum ; Tissier ; Aluminium and Cad-
mium, Deville; Aluminium and boron, Deville on this
subject 299
Aluminium and carbon, Deville and Cowles ; Aluminium
and gallium, Watts, Lecoq de Boisbaudran . .300
Aluminium and titanium, TVohler 301
Aluminium and tungsten, by Michel, in Wb'hler's labora-
tory ; Aluminium and molybdenum ; Experiments by
Michel; Aluminium and manganese ; Experiments by
Michel 302
Aluminium and sodium ; Deville and Fremy on these
alloys ; Aluminium and nitrogen, Dr. Hunt . . 303
APPENDIX.
Native sulphate of alumina ; Account of a deposit in
New Mexico 305
Decomposition of cryolite; F. Lauterborn's patent;
American aluminium ; Frishmuth's metal . . . 306
Analyses of same ; Specific gravity of aluminium ; Gravity
calculated from analyses ...... 307
Amalgamation of aluminium ...... 308
Theory of the rapid oxidation of aluminium amalgam ;
Reduction of alumina ; Experiment on reduction with
copper; Production and reduction of aluminium sul-
phide ; Fremy 's researches ..... 309
Investigations by Reichel . . . . . .312
Than's remarks 314
Reichel's experiments in reducing aluminium sulphide ;
Petitjean's patent . . . . . . 315
XX CONTENTS.
PAGE
Reich el* 8 summary . . . . . . .316
Aluminium chloride formed from the sulphide ; F. Laut-
erborn-'s patent 317
Niewerth ; Reichel ; A. Orlowski ; Experiments on mak-
ing aluminium sulphide . . . . . .318
Tabulated results ; Remarks and suggestions of a practical
process 321
Reducing the aluminium sulphide 322
Experiments with lead, copper, tin, antimony, and iron ;
Review of these experiments and suggestions of a prac-
, tical process 323
ADDENDA.
Additional details of Castner's sodium process . .324
New process for making aluminium chloride ; Remarks on
the mitis process . . . . . . .326
Production of aluminium in 1885; Low price of aluminium
in October, 1886 327
INDEX 328
ALUMINIUM
PART I.
HISTORY OF ALUMINIUM.
LAVOISIER* first suggested the existence of metal-
lic bases of the earths and alkalies. The first
researches in the preparation of aluminium date
back to 1807. Davy tried, but in vain, to decom-
pose A1208 by an electric current, or to reduce it
by vapor of potassium. Oerstedt, in 1824, believed
he had isolated aluminium. He decomposed anhy-
drous A12C16 by K amalgam, and he obtained,
along with some KC1, an amalgam which decom-
posed by heat furnished him a metal resembling
tin. It is probable that he employed either some
moist APC16 or K amalgam which contained KOH,
for it is only when wetted with a solution of KOH
that aluminium alloys with mercury; for, when
AVohler, later, wished to prepare aluminium by
this method, he found it impossible to obtain an
Al amalgam when he employed materials pure
* Fremy, Ency.
26 ALUMINIUM.
and dry. Nevertheless, the method of Oerstedt
marks an epoch in the history of the science, for
in 1827 Wohler isolated aluminium by decomposing
APC16 by K. The metal first isolated by Wohler
was a gray powder, taking under the polisher the
brilliancy of tin. It was very easily changed,
because of its extreme division, and also because
it was mixed with the K or A12C16 used in excess.
At that time no further use was made of these
facts. Later, in 1845, on making vapor of AP016
pass over potassium placed in platinum boats,
Wohler obtained the metal in small, malleable
globules of metallic appearance, from which he
was able to determine the principal properties of
aluminium. But the metal thus obtained was
scarcely as fusible as cast iron, without doubt
because of the platinum with which it had alloyed
during its preparation. In addition to this, it
decomposed water at 100°, from which we suppose
that it was still impregnated with K or APC16. It
is to H. St. Claire Devil le that the honor belongs
o
of having in 1854 isolated aluminium in a state of
almost perfect purity, determining its true proper-
ties. In commencing researches on aluminium,
Deville, while he applied the method of Wohler,
was ignorant of the latter's results of 1845. Besides,
he was not seeking to produce aluminium that he
might turn its valuable properties to practical ac-
count, but that it might serve for the production
of A10, which he believed could exist as well as
HISTORY OF ALUMINIUM. 27
FeO. The aluminium he wished to prepare would,
he thought, by its further reaction on APC16 form
A1C12, from which he might derive A1O and the
other proto-salts. But this proto-chloride was not
thus produced ; he obtained, enclosed in a mass of
A12C16.2KC1, fine globules of a brilliant substance, -
ductile, malleable, and very light, capable of being
melted in a muffle without oxidizing, attacked
by H^TO3 with difficulty, but dissolved easily by
HC1 or KOH with evolution of hydrogen. Recog-
nizing the importance of these properties, which
he proceeded to investigate and establish, and
fearing to see the honor of his discovery pass into
other hands, Deville immediately commenced
research for an economic process to produce alumi-
nium. The task was difficult, for the metal could
only be isolated from its chloride or fluoride by ~
potassium or sodium, of which only the former
was known at that time. Moreover, potassium I
cost then 900 fr. per kilo, was extremely dangerous, •
and gave only a small return of aluminium.
Deville succeeded in advantageously replacing \
potassium by sodium, and introduced such im-
provements into the manufacture of the latter that
he reduced the cost of a kilo from 2000 fr. in 1855
to 10 fr. in 1859. In order to produce aluminium
cheaply, he busied himself also in the economic
production of A1203, which gave later a lively
impulse to the cryolite and beauxite industries.
The researches of Deville, at first undertaken in I
28 ALUMINIUM.
the laboratory of the Normal School, Paris, were
afterwards continued on a larger scale, thanks to
the liberality of the Emperor Napoleon III., at
the chemical works of Javel. At this works were
made the ingots and divers objects of aluminium
which figured at the Paris Exhibition in 1855.
Later, after new experiments made together at the
Normal School, Deville, H. Debray, and P. Morin
set up a plant to make aluminium on a large scale
at Messrs. Rousseau Brothers' works at Glaciere.
The primary method there received many improve-
ments. Later on it was still further improved
under the direction of P. Morin at the works in
Nanterre. At last, in the works of Messrs. Merle
& Co., at Salindres, it has reached its present stage
^of advancement.
Tissier Bros, wrote and published a book entitled
' Recherches sur 1'Aluminium' in 1858. These
brothers were employed in the experiments which
Deville superintended at the laboratory of the
Normal School, Paris, and Deville charges that
after learning the important results of his experi-
ments they suddenly left him, taking drawings of
furnaces, details of processes, etc., and started works
themselves. Deville was very bitter against them,
and this ill-feeling was increased by the following
incident : Deville was collecting material to write
a book on the subject, which he almost regarded as
his prerogative, seeing that he had, so to speak,
created the industry ; but, before he had completed
HISTORY OF ALUMINIUM. 29
it, Tissier Bros, published theirs. In order not to
be too far behind, Deville hastened the comple-
tion of his book, by doing which he was unable
to make it as full as he had wished, and published
it in September, 1859. Several sharp letters passed
between Deville and the Tissiers, which may be
seen in the Compt. Rend, or Ann. de Chem. et de
Fhys. A. Tissier, in his book, thus describes the
formation and history of his works : In July, 1855,
Messrs. Maletra, Chanu, and Davey, of Rouen,
formed a company to produce aluminium, and we
were entrusted with the organization and special
charge of the industry. The commencement was
beset with difficulties, not only in producing, but
in using the metal. It then sold at §200 per kilo,
the price being an insurmountable obstacle to its
employment in the arts. The small capital at our
disposal was not enough to start the industry, to
pay general expenses, and the losses occasioned by
the many experiments necessary. On February
28, 1856, the society was dissolved. In April, the
same year, Mr. William Martin, struck by the
results already obtained, and sanguine of greater
success, united with us. From that time daily
improvements confirmed M. Martin's hopes, and
in 1857 the works at Amfreville-la-mi-Voie, near
Rouen, sold the metal at §60 per" kilo (§2.00 per
oz.). The laboratory of this works was devoted
to researches on everything concerning the produc-
tion and application of aluminium. M. Martin
3*
30 ALUMINIUM.
has our sincere gratitude for the kindness with
which he so willingly encouraged and contributed
to the progress of the manufacture of "this won-
derful metal."
Deville, as stated above, published his book in
September, 1859, and he concludes it with these
words : " I have tried to show that aluminium may
become a useful metal by studying with care its
physical and chemical properties, and showing the
actual state of its manufacture. As to the place
which it may occupy in qur daily life, that will
depend on the public's estimation of it and its
commercial price. The introduction of a new
metal into the usages of man's life is an operation
of extreme difficulty. At first, aluminium was
spoken of too highly in some publications, which
made it out to be a precious metal ; but later these
estimates have depreciated even to the point of
considering it attackable by pure water. The
cause of this is the desire which many have to see
taken out of common field mud a metal superior
to silver itself; the opposite opinion established
itself because of very impure specimens of the
metal which were put in circulation. It seems
now that the intermediate opinion, that which I
have always held and which I express in the firsf
lines of my book, is becoming more public, and
will stop the illusions and exaggerated beliefs
which can only be prejudicial to the adoption of
aluminium as a useful metal. Moreover, the in-
HISTORY OF ALUMINIUM. 31
dustry, established as it now is, can be the cause
of loss to no one ; as for myself, I take no account
of the large part of my estate which I have devoted,
but am only too happy, if my efforts are crowned
with definite success, in having made fruitful the
work of a man whom I am pleased to call my
friend — the illustrious Wohler."
As early as 1856 we find an article in an Ameri-
can magazine* showing that there were already
chemists in the United States spending time and
money on this subject. The following is the sub-
stance of the article alluded to: "Within the
last two years Deville has extracted 50 to 60 Ibs.
of aluminium. At the present time, M. Rousseau,
the successor of Deville in this manufacture, pro-
duces aluminium which he sells at §100 per pound.
Xo one in the United States has undertaken to
make the metal until recently Mons. Alfred Mon-
nier, of Camden, X. J., has, according to the
statement of Prof. James C. Booth in the c Penn.
Inquirer/ been successful in making sodium by a
continuous process, so as to procure it in large bars,
and has made aluminium in considerable quantity,
specimens of which he has exhibited to the Frank-
lin Institute. Mons. Monnier is desirous of forming
a company for tjie manufacture of aluminium, and
is confident that by operating in a large way he
can produce it at a much less cost than has hereto-
* Mining Magazine, 1856, vii. 317.
32 ALUMINIUM.
fore been realized. We would suggest the pro-
priety of giving aid to this manufacturer at the
expense of the government, for the introduction of
a new metal into the arts is a matter of national
importance, and no one can yet realize the various
and innumerable uses to which this new metal may
be applied. It would be quite proper and consti-
tutional for Congress to appropriate a sum of
money, to be expended under the direction of the
Secretary of the Treasury in the improvement of
this branch of metallurgy, and in testing the value
of the metal for coinage and other public use."
In the next volume of the ' Mining Magazine'*
there is a long article by Mr. W. J. Taylor, con-
taining nothing new in regard to the metallurgy
of aluminium, but chiefly concerned in calculating
theoretically the cost of the metal from the raw
materials and labor required by Deville's processes,
and concluding that it is quite possible to make it
for $1,00 per pound.
In 1874 we have the following resume by Kerl &
Stohman : " Deville first worked under the direc-
tion of the Paris Academy ; later, the Emperor
Napoleon gave him great encouragement, by means
of which he succeeded in producing several kilos
of aluminium, which were shown at the exhibition
in Paris, 1855. With the experience thus gained,
Deville took possession of Rousseau Bros.' cherni-
* Mining Magazine, viii. 167 and 228. Proc. Ac. Nat. Sci.,
Jan. 1857.
HISTORY OF ALUMINIUM. 66
cal works at La Glaciere, near Paris. It soon fol-
lowed that the price of aluminium was reduced
from 1000 fr. per kilo to 300 fr. After a short
time the undertaking was enlarged, and the manu-
facture removed to Nanterre and Salindres. The
last named works, under the management of
Usiglio, went into the possession of Merle. !N"ew
advances made a further reduction in price to
200 fr. possible. In 1862 the price was put down
to 130 fr. Another works was then established at
Amfrcville, near Rouen. This was on a larger
scale than that at Kauterre, for while in 1859 the
latter produced 60 kilos, the former produced 80.
In England the first manufactory was established in
1859, at Battersea, London ; and the next year Bell
Bros, started at Kewcastle-on-Tyne. Germany as
yet possesses no aluminium works."
The further we get away from an age the better
able are we to write the true history of that age.
And so, as years pass since the labors of AVohler,
Deville, and Tissier, we are now able to see better
the whole connected history of the development
of this art. Dr. Clemens Winckler gives us a
comprehensive retrospect of the field seen from the
standpoint of 1879, from which we condense the fol-
lowing :* The history of the art of working in alu-
minium is a very short one, so short that the present
generation, with which it is contemporary, is in
* Industrie Blatter, 1879 ; Sci. Am. Suppl., Sept. G, 1879.
34 ALUMINIUM.
danger of overlooking it altogether. The three
international exhibitions which have been held in
Paris since aluminium first began to be made on a
commercial scale form so many memorials of its
career, giving, as they did, at almost equal intervals,
evidence of the progress made in its application.
In 1855, we meet for the first time, in the Palais de
1'Industrie, with a large bar of the wonderful
metal, docketed with the extravagant name of the
" silver from clay." In 1867 we meet with it
again, worked up in various forms, and get a view
of the many difficulties which had to be overcome
in producing it on a large scale, purifying, and
moulding it. We find it present as sheets, wire,
foil, or worked-up goods, polished, engraved, and
soldered, and see for the first time its most impor-
tant alloy — aluminium bronze. After a lapse of
almost another dozen years we see at the Paris
exhibition of 1878 the maturity of the industry.
"We have passed out of the epoch in which the
metal was worked up in single specimens, showing
only the future capabilities of the metal, and we
see it accepted as a current manufacture, having a
regular supply and demand and being in some
regards commercially complete. The despair which
has been indulged in as to the future of the metal
is thus seen to have been premature. The manu-
facture of aluminium and goods made of it has
certainly not taken the extension at first hoped
for in its behalf; the lowest limit of the cost of
HISTORY OF ALUMINIUM. 35
manufacture was soon reached, and aluminium
remains as a metal won by expensive operations
from the cheapest of raw materials.
To France is due the merit of having been the
first country to carry out Wohler's process on a
practical scale, and to have created the aluminium
industry. France seems to be the only country in
which the industry is able to prosper. The English
establishment at Newcastle-on-Tyne by Bell & Co.
did not succeed, and has been shut up now for
about live years. The German manufactory, set
up in Berlin by Wirz & Co., cannot be said really
to have lived at all ; it drooped before it was well
started. In France, the great chemical works of
H. Merle & Co., Salindres, carries on the extraction
of aluminium, and the Societe Anonyme de 1'Alu-
rninium, at Nanterre, works up the metal. Both
firms were represented at the exhibition in 1878.
The most rational use indicated for aluminium
by reason of its low specific gravity is the making
of beams for balances. Sartorius, of Gottingen,
was the first to make these light and unalterable
beams of an alloy of 96 aluminium and 4 silver.
He has had but few imitators. There are several
reasons why the metal is shown so little favor by
mathematical instrument makers and others. First
of all, there is the price ; then the methods of
working it are not everywhere known ; and further,
no one knows how to cast it. Molten aluminium
attacks the common earthen crucible, reduces silicon
36 ALUMINIUM.
from it, and becomes gray and brittle. This incon-
venience is overcome by using Jirne crucibles, or
by lining an earthen crucible with carbon or strongly
burnt cryolite clay. If any one would take up the
casting of aluminium and bring it into vogue as a
current industrial operation, there is no doubt that
the metal would be more freely used in the finer
branches of practical mechanics. The prices per
kilo quoted in the last list issued by the Societe
Anonyme are as follows : —
ALUMINIUM.
Bars 130 fr.
Sheets (0.5 to 0.1 mm. thick) . 135 " to 160 fr.
Wire (2 to 3 mm. diam.) . . 170 " " 200 "
ALUMINIUM BRONZE (10 per cent, aluminium).
Bars 18 fr.
Sheets (2 to 0.5 mm. thick) . . 24 " to 30 fr.
Wire (7 to 1 mm. diam.) . . . 28 " to 39 "
The preceding paper of Dr. Winckler, as he re-
marks, chronicles the perfection of Deville's pro-
cesses, when aluminium was made as cheaply
as it could possibly be by these methods. But,
about this time an aluminium works was started
in Birmingham, England, by Mr. Webster, which
has grown to be one of the largest in the world.
Mr. Webster owns several patents on processes of
his own, which will be found described in their
proper places.
In the United States one of the most prominent
HISTORY OF ALUMINIUM.
chemists engaged on aluminium is Colonel William
Frishmuth, of Philadelphia. The following article
gives an account of his invention :* " Some months
ago, we published in the ' Star7 the fact that Colonel
"William Frishmuth, well known in this city for
many years, has discovered a method for producing
aluminium at reduced cost. Comments were made
in various quarters as to the real value of the discov-
ery, some of which even questioned the possibility
of producing the metal by this process, which is
stated to produce it from South Carolina corundum,
using sodium as a reagent. Meanwhile patents
have been taken out in this and foreign countries,
and preliminaries are fairly under way to test the
process practically. It did not seem too much to
hope when the publication was made that Ameri-
can capitalists would at once make investigation of
Colonel Frishmuth's discovery, learn whether the
results were even measurably up to the promise,
and in that event secure to themselves a commercial
plant so extremely important. It has, however,
fallen to capitalists abroad to obtain control of the
patent. At the present time Major Ricarde-Seaver,
F.R.S.E., late Government Inspector of Mines,
London, is in this city as an expert to examine the
process and its practicability on behalf of these
capitalists. A reporter endeavored to obtain from
Major Seaver his opinion of the process, but he
* Philadelphia Evening Star, November 15, 1884.
4
38 ALUMINIUM.
stated that his opinion could not be made public.
Mr. Seaver said in reference to aluminium : ' Some
of the best minds in Europe have been studying
for years the problem of producing the metal
cheaply. Scientists in France and Germany and one
in Geneva have been at work on it a long time.
As to the possibility of producing it so that it
could be used as an alloy for iron and steel, that is not
to be expected unless it could be produced at much
less than a dollar per pound. As to the possibility
of doing that by this process, I am not at liberty
to speak. The work here has so far been merely
on an experimental scale. As scientific men know
by many experiences, disappointments are some-
times met with when they leave the experimental
field and work is attempted on a commercial scale
for business purposes. I am, however, very much
pleased with what I have seen here, and, as I have
said, while scientific men all over Europe have been
investigating the problem, it seems to be solved
here. I am certainly satisfied that aluminium can
be produced by Frishmuth's process, there is some
metal made by it, and there will be a display of it
at the NQW Orleans exhibition. Even if it can be
made very cheap by this process, it is not probable
that anything more would be done by the parties I
represent than to supply the market at a fair price,
just as the Rothschilds, who own the great quick-
silver mines of the world, regulate the supply by
the demand.' "
HISTORY OF ALUMINIUM. 39
Colonel Frishmuth's works are at Rush and
Amber streets, near the Richmond coal wharves,
Philadelphia. lie seems to be kept busy, and his
metal is on the market ; an analysis of it will be found
in the Appendix. It can be bought from Bullock
& Crenshaw, Philadelphia. He cast the tip of the
AVashington Monument, which weighs one hundred
ounces, one of the largest single castings of alumin-
ium ever made. As far as is known, he is at pres-
ent the only producer of pure aluminium in the
United States. His metal is sold in bars at about
fifteen dollars per pound. In the Philadelphia city
census of 1884 he is placed as employing ten men,
and his annual product is valued at §18,000. Mr.
Frishmuth melts down quantities of aluminium
scrap, and the author has been unable to learn, ex-
cept from Mr. Seaver's statement, that Mr. Frish-
muth produces any aluminium by his process. Mr.
Seaver represented an English syndicate which
stands ready to buy out all patents of any value
which appear on aluminium ; they possess large
capital, and are said to be ready to pay an immense
sum for any practical, cheap process for producing
the metal.
In the Mineral Resources of the United States,
1883-4, we find a few statistics as to the amount
of aluminium made in recent years. It is there
stated that in 1882 there were 2350 kilos made in
France. The price of the American metal ranged
from §0.75 to §1.00 per troy ounce in 1883 ; and
40 ALUMINIUM.
from $0.50 to $1.00 per ounce in 1884, according
to quantity. The amount imported and entered for
consumption in the United States from 1870 to 1884
is as follows : —
Year ending June 30,
Quantity (pounds).
Value.
1870 .
$ 98
1871
• ....
341
1872
.
1873 .
2
22
1874
. 683
2125
1875 .
. 434
1355
1876 .
. . .139
1412
1877
. 131
1551
1878 .
. 251
2978
1879
. 284
3423
1880
. 341
4042
1881 . . .
. 517
6071
1882 .
. 566
6459
1883
. 436
5079
1884' .
. 590
8416
Until recently the aluminum sold in the United
States was entirely of foreign origin, but it is now
produced in this country by Colonel Frishmuth,
of Philadelphia, who turned out 1000 ounces of
the metal in 1883, and 1800 ounces in 1884. The
aluminium cap or apex of the Washington Monu-
ment was cast by him ; it is of pyramidal form,
10 inches high, 6 inches on a side of its base, and
weighs 8J pounds (see p. 53).
Within the last two years a process has been
invented and brought into practical use which has
served to bring the metallurgy of aluminium into
HISTORY OF ALUMINIUM. 41
very general attention. The Cowles' process, the
discovery and details of which will be given further
on, is due to two Cleveland gentlemen, and they
seem to be developing all that is in their process.
They make no pure metal, but sell the alloys,
principally aluminium bronze, the latter of good
quality, and at a much lower price than it was
ever sold before. If they can make it profitable
to sell the bronze at the price which they now
quote, the permanent success of their process is
assured. Mr. Charles F. Mabery, of the Case
School of Applied Science, Cleveland, is their con-
sulting chemist, and Dr. T. Sterry Hunt, of Mon-
treal, seems to be very much interested in the pro-
cess from a scientific point of view. Mr. Mabery
gives his views as to the present state of the alumi-
nium industry as follows: "The aluminium of
commerce has been made chiefly in France by
Deville's old method. Several patents have been
issued for its prod uction by electrolysis, and although
it can be deposited in small quantities from solu-
tions, there is but one electrolytic method that
can be worked on a commercial basis, and that is
Bunsen & Deville's method of electrolysing molten
Al2Cl6.2XaCl. Large works have recently been
erected in France for obtaining the metal by this
method, and it is claimed that it can be produced
for about $7 per pound. A company has recently
been formed in London to manufacture aluminium
alloys on the basis of the Webster patents. The
4*
42 ALUMINIUM.
chief improvement on the old process, according
to the patent specifications, is in the preparation of
the pure A1203. Frishmuth, of Philadelphia,
attempts to produce sodium in one retort, volatilize
aluminium chloride from another, and allow the
vapors to meet in a third. The assertion made by
him at first that he could place the metal on the
market at $1.25 per pound has not been verified."
Dr. Hunt, in reply to an inquiry as to the present
state of the industry, replies : " Webster, of Eng-
land, is the chief, perhaps the only, manufacturer
in that country of the metal and its alloys. Messrs.
Cowles manufacture the alloys, and they can now
make pure aluminium, but the method is not yet
perfected or made public. The process of Frish-
muth is not new, but is mentioned in Watts' Dic-
tionary. So far as I can learn, and so far as Messrs.
Cowles are informed, there has been no pure alu-
minium made commercially save from the chloride
by use of sodium. Messrs. Cowles' work with
their large new dynamo has been very satisfac-
tory."
PART II.
OCCURRENCE OF ALUMINIUM IN NATURE.
THERE is no other metal on the earth which is
so widely scattered and occurs in such abundance.
Al is not found metallic. Stocker* made the
statement that Al occurred as shining scales in an
alumina formation at St. Austel, near Cornwall,
but he was in error. But the combinations of Al
with oxygen, the alkalies, fluorine, silicon, and
the acids, etc., are so numerous and occur so abun-
dantly as not only to form mountain masses, but to
be also the bases of soils and clays. Especially
numerous are the combinations with Si and other
bases, which, in the form of felspar and mica,
mixed with quartz, form granite. Mierzinski
gives the formulae of a few of these silicates as: —
Orthoclase . . K2Si3O" +
Albite . . . Na2Si3O7 + Al2Si3O9
Anorthite . . CaSiOS-f Al2SiO5
K Mica . . (HK)*Al*Si*08+ (HK)2Al2Si4O'5
Na Mica . . (HNa)2Al2Si2O8-f- (HNa)2Al2Si4O«
Li Mica . . (Li^KXFe^.AlWSSiO2.
Mg Mica . . m(HK)4SiO4-f-n(Mg.Fe.H.)2SiO4-f
* Jrnl. fr. prakt. Chenu, 06, 470.
44 ALUMINIUM.
These combinations, by the influence of the
atmosphere, air, and water, are decomposed, the
alkali is replaced or carried away, and the residues
form clays. The clays form soils, and thus the
surface of the earth becomes porous to water and
fruitful. It is a curious fact that Al has never
been found in animals or plants, which would seem
to show that it is not necessary to their growth,
and perhaps would act injuriously, if it were present,
by its influence on the other materials. Most of the
Al compounds appear dull and disagreeable, such
as felspar, mica, pigments, gneiss, amphibole, por-
phyry, eurite, trachyte, etc. ; yet there are others
possessing extraordinary lustre, and so beautiful as
to be classed as precious stones. Some of these,
with their formulae, are —
Ruby . . . . A12Q3
Sapphire . . . A12O3
Garnet .... (Ca.Mg.Fe.Mn)3Al2Si3Oi2
Cyanite . . . APSiO5
Some other compounds occurring frequently
are —
Turquoise . . . A12P2O8.H6A12O6.2H20
Lazulite . . . (MgFe)Al2P2O9 + Aq
Wavellite . . . 2A12P2O8.H6AK)5.9H2O
Topaz .... 5Al2SiO5.Al2SiF10
Cryolite . . . Al2F3.6NaF
Diaspore . . . H2A12O4
Beauxite . . . H6A12O6
Aluminite . . . A12SO6.9H2O
Aluuite K*SO4.A1*S3012.2H2AKO3
OCCURRENCE OF ALUMINIUM IN NATURE. 45
One would suppose that since aluminium occurs
in such ahundance over the whole earth, since we
literally tread it under foot, that it would he ex-
tracted and applied to numberless uses, being
made as abundant and useful as iron ; but such is
not the case.
Beauxite and cryolite are the minerals most
used for producing aluminium, and their preference
lies mainly in their purity. Native alums gene-
rally contain Fe, which must be removed by ex-
pensive processes. Some observations on a native
alum deposited in New Mexico will be found in
the Appendix. WQ will here consider at greater
length only beauxite and cryolite.
BEAUXITE.
Beauxite is a combination between diaspor,
A1203.3H20, and brown hematite, Fe*0».3EPO ; or,
it is diaspor with Al replaced more or less by Fe ;
the larger the amount of Fe the more its color
changes from white to brown. It was first found
in France, near the town of Beaux, large deposits
occurring in the departments Yar and Benches du
Rhon, extending from Tarascon to Antibes. Seve-
ral of these beds are a dozen yards thick, and . 160
kilometres in length. Deposits are also found in
the departments of 1'Herault and 1'Arriege. Very
important beds are found in Styria, at Wochein,
and at Freibriss, in Austria, a newly discovered
46
ALUMINIUM.
locality where the mineral is called Wochehrite.
Here it has a dense, earthy structure, while that of
France is conglomerate or oolitic. Deposits similar
to those of France are found in Ireland at Irish
Hill, Straid, and Glenravel. Further deposits are
found in Hadamar in Hesse, at Klein-Steinheim,
Langsdorff, and in French Guiana.
The following analyses give an idea of the pecu-
liar composition of this mineral ; besides the in-
gredients given there are also traces of CaO, MgO,
SO3, P205, TiO2, and Ya203.
a.
b.
c.
d.
e.
/.
A12O3 . . .
60.0
75.0
63.16
72.87
44.4
54.1
Fe2O3 . . .
25.0
12.0
23.55
13.49
30.3
10.4
SiO2 . . .
3.0
1.0
4.15
4.25
15.0
12.0
K*0 and Na2O
...
...
0.79
0.78
...
...
H20 ...
12.0
12.0
8.34
8.50
9.7
29.9
9-
h.
i.
k.
L
m.
A12O3 . . .
Fe2O3 . . .
SiO2 . . .
K2O and Na2O
64.6
20
7.5
29.80
3.67
44.76
48.12
2.36
7.95
43.44
2.11
15.05
61.89
1.96
6.01
45.76
18.96
6.41
0 38
H20 . . .
24.7
13.86
40.33
35.70
27.82
27.61
.
n.
0.
P-
1-
r.
A1203 . . .
55.61
76.3
50.85
49.02
73.00
FC2O3 . . .
7.17
6.2
14.36
12,90
4.26
SiO2 . . .
4.41
11.0
5.14
10.27
2.15
K2O and Na2O
0.26
0.31
H20 ...
32.33
26.4
28.38
25.91
18.66
OCCURRENCE OF ALUMINIUM IN NATURE. 47
Index : —
a and b. from Beaux (Deville).
c. dark \ Woclieinite (Drechsler).
d. light J
e. red brown \
f. yellow > Beauxite from Feisstritz (Schnitzer).
g. white
h. white Wocheinite (L. Mayer and O. Wagner).
*. Beauxite from Irish Hill.
k. " " Co. Antrine (Spruce).
I " " Glenravel (F. Hodges).
raandw. " " Hadamar (Hesse) (Retzlaff).
o. from Klein-Steinheim (Bischof ).
p and q. from LangsdorfF (I. Lang).
r. Beauxite from Dublin, Ireland, brought to the Laurel
Hill Chemical Works, Brooklyn, L. I., and there
used for making alums. It is dirty white, hard,
dense, compact, and in addition to the ingredients
given above contains 0.59 percent. CaO, and some
TiO2. It costs $6 per ton laid down in the works.
The above analysis, made by Mr. Joiiet, is fur-
nished me by the kindness of the superintendent
of the works, Mr. Herreshoff.
As is seen from the above analyses, the percentage
of A1203 is very variable, and cannot be determined
at all simply by inspection but only by an analysis,
for often- the best-looking specimens are the lowest
in APO3. For instance, a beauxite containing 62.10
A1203, 6.11 Fe203, 5.06 SiO2, and 20.83 H*0 was
much darker and more impure looking than that
from Wochein (h) which contained only 29.8 per
cent. APO3.
48 ALUMINIUM.
CRYOLITE.
Cryolite was first found at Ivigtuk, in Arksut-
fiord, west coast of Greenland, where it constitutes
a large bed or vein in gneiss. It is a semi-trans-
parent, snow-white mineral. When impure it is
yellowish or reddish, even sometimes almost black.
It is shining, sp. gr. 2.95, and hardness 2.5 to 3.
It is brittle, not infrequently contains FeCO3, PbS,
SiO2, and sometimes columbite. It is fusible in
the flame of a candle, and on treatment with sul-
phuric acid yields hydrofluoric acid. As will be
seen further on, cryolite was first used by the soap-
makers for its soda; it is still used for making soda
and alumina salts,.and to make a white glass which
is a very good imitation of porcelain. The Penn-
sylvania Salt Company in Philadelphia import it
from Ivigtuk by the ship-load for these purposes ;
lately they have discontinued making the glass.
Cryolite is in general use as a flux. A very com-
plete description of the deposit at Ivigtuk can be
found in Hoffman's ' Chemische Industrie.'
The only known deposit of cryolite in the United
States is that found near Pike's Peak, Colorado,
and described by W. Cross and W. F. Hillebrand
in the ' American Journal of Science,' October,
1883. It is purely of mineralogical importance
and interest, occurring in small masses as a sub-
ordinate constituent in certain quartz and feld-
spar veins in a country rock of coarse reddish
OCCURRENCE OF ALUMINIUM IN NATURE. 49
granite. Zircon, astrophyllite, and columbite are
the primary associated minerals, the first only
being abundant.
There -is no duty on the imports of cryolite into
the United States, and they have varied from
10,000 tons in 1869 to 9000 in 1884, costing $9 to
$10 per ton.
CORUNDUM.
" Till 1869, the sole sources of corundum were
a few river washings in India and elsewhere.
It was found in scattered crystals, and cost twelve
to twenty-five cents per pound. In 1869, in
riding over a spur of the Alleghenies in northern
Georgia, I* found what has proven to be an
almost inexhaustible mine of corundum in the
crysolite serpentine, the first instance on record of
the mineral being found in situ. Previously it had
been washed out of debris at Cripp's Hill, N". C.,
and at a mine in West Chester, Pa., both on the
slopes of the crysolite serpentine. The clue being
thus obtained accidentally, about thirty mines were
shortly afterwards discovered in the same forma-
tion ; but of the thousands of tons thus far dug
out, the larger portion has come from the mines I
discovered.
" At present it can be bought at about ten dollars
per ton at the mines. It is nearly pure A12O3.
. W. P. Thompson.
50 ALUMINIUM.
Disapore, a hydrated alumina, is also found in the
same region and locality. Corundum will proba-
bly always be the principal source in America of
material from which to manufacture pure Al.
But in Great Britain, in all probability, manufac-
turers must look to alumina prepared artificially
from cryolite or from Mr. Kynaston's sulphate of
alumina."*
* Journal of the Society of Chemical Industry, April, 1886.
PART III.
PHYSICAL PROPERTIES OF ALUMINIUM.
COMMERCIAL aluminium is never chemically pure,
and therefore displays properties varying more or
less from those of the pure metal according to the
character and amount of impurities present. In
this treatise, whenever the properties of aluminium
are mentioned, they must be understood to refer to
the chemically pure metal, and not to the commer-
cial article, unless specifically stated. As prelimi-
nary to the presentation of these properties we will
here make some observations on the commercial
metal and the impurities generally found in it.
In whatever way aluminium may be reduced,
still it is always far from being pure, being con-
taminated with iron, silicon, or even sodium and
lead, as is shown by the following analyses : —
Al.
Si.
2149
0.454
1.270
0.2o
0.70
0.47
2.87
0.45
3.70
0.04
0.12
1.00
0.40
Fe.
<7tt.
P6.
Ara.
1 Parisian (Salvetat) . ...
92.969
96.253
96.890
97.200
92.500
96.160
8S.330
92.000
94.700
98.290
97.680
97.400
97.600
4.882
3.293
1.840
2.40
6.80
3.37
2.40
7.55
1.60
1.67
2.20
1.30
1.40
trace
63*8
o'l'o
0.40
trace
trace
0*20
0.20
trace
trace
trace
o' * Berlin (Mallet)
4. Mo fin & Co., Nanterre (Sauerwein) .
**' [ Parisian (Dumas)
7. Parisian (Salvetat) ... ...
9 Bonn (Kraut) . ... . .
}}• j Morin & Co., Nanterre, 1862 (Kraut)
12. ) (Hampe) the purest he could buy
13. $ Wagner's Jahresb., 1877 ....
52 ALUMINIUM.
According to Rammelsberg (Kerl's Handbuch)
the Si which is always found in aluminium is in
part combined with it, and this combined Si
changes by treatment with HC1 into either SiO2,
which remains, or into SiH4, which escapes ; while
another part of the Si is combined with the alu-
minium just as graphite is with Fe ; and this part
of the Si remains on treatment with acid as a black
mass, not oxidized by ignition in the air. Two
analyses of aluminium reduced from cryolite by
sodium in a porcelain crucible gave—
SiO2
1.
. 9.55
2.
1.85
Free Si .
Si in SiH4
. 0.17
. 0.74
0.12
0.58
One sample of aluminium analyzed by Professor
Rammelsburg contained as much as 10.46 percent.
Si, and another sample even 13.9 per cent. The
quantity of Fe varies from 2.9 to 7.5 per cent.
M. Dumas has found that aluminium usually
contains gases, about which he makes the follow-
ing statements :* " On submitting aluminium in
a vacuum to the action of a gradually increasing
temperature up to the softening point of porcelain,
and letting the mercury pump continue acting on
the retort until it was completely exhausted, con-
siderable quantities of gas were withdrawn. The
liberation of the gas from the metal seems to take
* Sci. Am. Suppl., Aug. 7, 1880.
PHYSICAL PROPERTIES OF ALUMINIUM. 53
place suddenly towards a red-white heat. 200
grammes of aluminium, occupying 80 c. c., gave
89.5 c. c. of gas, measured at 17° and 755 mm.
pressure. The gas consisted of 1.5 c. c. CO2 and
88 c. c. H. CO, £T, and 0 were absent,"
*The aluminium apex or cap of the Washington
Monument cast by Colonel Frishmuth,of Philadel-
phia, has the following composition : —
Al 97.75
Fe . . . . . . 1.70
Si 0.55
COLOR.
Deville: The color of aluminium is a beautiful
white with a slight blue tint, especially when it has
been strongly worked. Being put alongside silver,
their color is sensibly the same. However, common
silver, and especialh7 that alloyed with copper, has a
yellow tinge, making the aluminium look whiter by
comparison. Tin is still yellower than silver, so
that aluminium possesses a color unlike any other
useful metal.
Fremy : Aluminium has a fine white color, just
a little blue when compared with silver. When it
has been worked, or when it contains Fe or Si, its
blue tint acquires greater intensity. The commer-
cial aluminium resembles silver.
* Mineral Resources of the United States, 1883-84.
5*
54 ALUMINIUM.
Mallet: Absolutely pure aluminium is percepti-
bly whiter than the commercial metal ; on a cut
surface very nearly pure tin-white, without bluish
tinge, as far as could be judged from the small
pieces examined.
Mierzinski : The pure white color of aluminium
is very brilliant ; it has a tint lying between the
color of tin and zinc, although on account of its
usual blue shading, even in a poor light, it cannot
be confounded with them or with any white metal.
MAT.
Deville: Aluminium like silver is able to take a
very beautiful mat which keeps indefinitely in the
air. It is obtained easily by plunging the surface
for an instant in a very dilute solution of caustic
soda, washing in a large quantity of water and at
last dipping in strong nitric acid. Under these
conditions, all the foreign materials which might
contaminate it, except silicon in large proportion,
dissolve and leave the metal quite white and with
a very pleasing appearance.
Mierzinski: The peculiar lustre of aluminium,
however, is not permanent. With time, the objects
take on their plain faces an olive green coloration,
and look much less agreeably. Their former white
color can be restored by Mourey's receipt, by placing
them first in dilute hydrofluoric acid, 1000 parts
PHYSICAL PROPERTIES OF ALUMINIUM. 55
water to 2 of acid, and then dipping them in nitric
acid.
Bell Bros.: They recommend first washing the
objects in benzole or essence of turpentine, before
treating with NaOH and HNO3, as above.
POLISH AND LUSTRE.
Deville: Aluminium may be polished and bur-
nished easily, but it is necessary to employ as an
intermediate material between the stone and polish-
ing powder a mixture of stearic acid and essence of
turpentine, finishing with pure essence of turpen-
tine. In general, the polished surfaces are of a less
agreeable appearance than the mat, the blue tint of
the metal becoming more manifest. But, in this
work, the experience and practice of the workers
in aluminium is far from being complete ; each metal
requires a special way of working, and we may ex-
pect yet for a material so new that progress will be
made in this direction.
Bell Bros. : Aluminium is easily polished and
burnished. Use a mixture of equal parts of rum
and olive oil as an intermediate substance between
the polishing stone and the powder used. The
polishing stone is steeped in this mixture, and will
then burnish the metal as silver and copper are bur-
nished, care being taken not to press too heavily on
the burnishing instrument.
Kerl & Stohman : The use of the old means of
56 ALtMINIUM.
polishing and burnishing metals, such as soap, wine,
vinegar, linseed-oil, decoction of marshmallow, etc.,
is not effective with aluminium, but, on the contrary,
is even harmful ; because, using them, the blood
stone arid the burnishing iron tear the metal as
fine stone does glass. Oil of turpentine has also
been used, but with no good effect. Mourey found,
after many attempts, that a mixture of equal weights
of olive oil and rum, which were shaken in a bottle
till an emulsified mass resulted, gave a very bril-
liant polish. The polishing stone is dipped in this
liquid, and the metal polished like silver, except
that one must not press so hard in shining up.
The peculiar black streaks which form under the
polishing stone need cause no trouble ; they do not
injure the polish in the least, and can be removed
from time to time by wiping with a lump of cotton.
The best way to clean a soiled surface and remove
grease is to dip the object in benzine, and dry it in
fine sawdust. Hammered and pressed objects of
aluminium may, before polishing, be very easily
ground by using olive oil and pumice.
ODOR.
Deville: The odor of pure aluminium is sensibly
nothing, but the metal strongly charged with
silicon will exhale the odor of silicuretted hydro-
gen, exactly represented by the odor of cast iron.
But, even under these unfavorable circumstances,
PHYSICAL PROPERTIES OF ALUMINIUM. 57
the smell of the metal is only appreciable to persons
experienced in judging very slight sensations of
this kind.
"Watts: When pure, aluminium is quite desti-
tute of taste or odor.
TASTE.
Deville : Pure aluminium has no tast£, but the
impure and odorous metal may have a taste like
iron, in any case only very slight.
MALLEABILITY.
Deville: Aluminium may be forged or rolled
with as much perfection as gold or silver. It is
beaten into leaves as easily as they, and a very
experienced gold beater, M. Rousseau, has made
leaves as fine as those of gold or silver, which are
put up in books. I know of no other useful
metal able to stand this treatment. Before rolling
a bar of aluminium it is well to prepare the metal
by forging it on all sides, and commencing work
with a hammer. Aluminium is tempered at a
very low red heat ; or the plate is heated just until
the black trace left on its surface by a drop of oil
put there and which is carbonized has entirely dis-
appeared.
Mallet: With absolutely pure aluminium the
malleability was undoubtedly improved, the metal
58 ALUMINIUM.
yielding easily to the hammer, bearing distortion
well, and flattening in two or three directions
without cracking. It seemed to be sensibly less
hardened by hammering than the ordinary metal
of commerce.
'Chemical News,' 1859: M. Degousse has suc-
ceeded in beating aluminium into leaves as thin as
those obtained of gold or silver. The operation is
attended with a certain difficulty, and it is neces-
sary to temper the metal frequently. This can-
not be done, however, in the ordinary manner
as with gold or silver; only a very slight heat
must be employed. The beating is done as usual.
These thin aluminium leaves can be substituted for
silver leaf. They have a less brilliant color, but
are much more durable, and may be employed
advantageously for decorative purposes. A very
thin leaf will burn like paper when made into a
roll, with a brilliant white flame.
Kerl & Stohman : Aluminium may be rolled as
easily as other metals, but it must be annealed
oftener. The annealing of objects made of it is
not more difficult than that of other metals. The
moment the metal begins to glow its annealing is
complete. Those metal-workers who are anxious
about the exact point of time can rub the top of
the article to be annealed with a lump of fat, the
disappearance of the fat shows the moment in
which the object is to be removed from the anneal-
ing oven. Aluminium can also be pressed or
PHYSICAL PROPERTIES OF ALUMINIUM. 59
stamped into all forms of hollow and round vessels,
in a stamping press. But there must be used a
kind of varnish of 4 parts of oil of turpentine and
1 part of stearic acid.
Bell Bros. : Aluminium can be beaten out, hot
or cold, to the same extent and as perfectly as gold
and silver, and may be rolled in much the same
way. Thin leaves may be used in the same man-
ner as gold and silver leaf. Covered iron ingot
moulds serve best for casting bars of the metal to
be rolled. Aluminium quickly loses its temper,
and therefore requires frequent reheating at a dull
red heat ; when the plates are very thin this de-
mands great attention.
Mierzinski: The extensibility of aluminium is
quite high, standing near to gold and silver. It
may easily be beaten out or rolled without tearing.
In beating to leaf it should at first be warmed only
to 100° or 150°, an actual glowing heat has proved
to be very unsuitable. Such leaves are especially
suitable for showing the characteristic qualities of
the metal ; for instance, it dissolves with extraor-
dinary quickness in caustic alkali, leaving the iron,
which is always present. This leaf is also very
combustible, even in a gas flame, burning with a
brilliant, sparkling light ; the resulting A1203 is
melted, and as hard as corundum. While water
does not appear to be decomposed by aluminium
in compact masses at 100°, yet it does so when in
the extremely attenuated form of leaf. In pure,
60 ALUMINIUM.
boiling water the leaf slowly evolves hydrogen,
after several hours the leaves are half gone, being
changed into hydrated alumina. Aluminium leaf
was first made by C. Falk & Co., Vienna.
. DUCTILITY.
Deville : Aluminium behaves very well at the
drawing plate. M. Yangeois obtained in 1855,
with a metal far from being pure, wires of extreme
tenuity, which were used to make aluminium pas-
sementere. However, the metal deteriorates much
in the operation, and the threads become flexible
again only after an annealing very delicately per-
formed, because of the fineness of the threads and
the fusibility of the metal. The heat of the air
coming from the top of the chimney over an Ar-
gand burner is sufficient to anneal them.
Bell Bros. : Aluminium is easily drawn into
wire. Run the metal into an open mould, so as to
form a flat bar of about one-half inch section, the
edges of which are beaten very regularly with a
hammer. The diameter should be very gradually
reduced at first, with frequent heating. When the
threads are required very fine the heating becomes
a very delicate operation, on account of the fine-
ness of the threads and the fusibility of the metal.
PHYSICAL PROPERTIES OF ALUMINIUM. 61
ELASTICITY — TENACITY — HARDNESS.
Deville: The elasticity of aluminium, according
to M. Wertheirn, is sensibly the same as that of
silver; its tenacity is also nearly the same. The
moment after being cast it has the hardness of virgin
silver ; when it has been worked it resembles that
of soft iron, becomes elastic by becoming much more
rigid, and gives the sound of steel when dropped
on a hard body.
Mallet: Absolutely pure aluminium was dis-
tinctly softer than before purification. Hence its
fracture was not easily observed, but seemed to be
very fine grained with some appearance of fibrous
silkiness. It seemed to be sensibly less hardened
by hammering than the ordinary metal of com-
merce.
Fremy : Aluminium just cast is scratched by a
wire or edge of silver, but by hammering it be-
comes as hard as iron and elastic. The tenacity of
aluminium wire is between that of zinc and tin,
but by hammering it attains that of hardened cop-
per. When cast carefully it can be easily filed
without fouling the tool.
Kerl & Stohman : Aluminium resists the action
of the engraving tool, which slides upon the sur-
face of the metal as upon hard glass. But as soon
as one uses the varnish of 4 parts of oil of turpen-
tine and 1 of stearic acid, or some olive oil mixed
with rum, the tool cuts into it like pure copper.
62 ALUMINIUM.
Mierzinski : The tenacity of aluminium is very
remarkable, and, according to Barlow, is 1892 kilos
per square centimetre ; the extensibility 2.5 per cent.
W. H. Barlow :* A ba-r of aluminium three feet
long and one-quarter inch square was obtained, and
different parts of it subjected to tests for tension,
compression, and transverse strain, elasticity, elastic
range, and ductility. It will be seen on reference
to the results that the weight of a cubic inch was
0.0275 pound, showing a specific gravity of 2.688,
and its ultimate tensile strength was about twelve
tons per square inch. The range of elasticity is
large, the extreme to the yielding point being one-
two hundredth of the length. The modulus of
elasticity is 10,000. The ductility in samples two
inches long was 2.5 per cent. Taking the tensile
strength of the metal in relation to its weight, it
shows a high mechanical value. These results are
thus tabulated : —
Weight of Tensile Length of a
1 cubic foot strength bar able to sup-
in pounds, persq.in. port its weight,
in pounds. in feet.
Cast Fe . . . .444 16,500 5351
Bronze . . . .525 36,000 9893
Wrought Fe . 480 50,000 15,000
Steel 490 78,000 23,040
Al 168 26,800 23,040
It thus appears that taking the strength of alu-
minium in relation to its weight, it possesses a
* Rpt. Brit. A. A. S., 1882, p. 668.
PHYSICAL PROPERTIES OF ALUMINIUM. 63
mechanical value about equal to that of steel of
35 tons per square inch tensile strength.
Mierzinski: Kamarsch (Dingier 172, 55) obtains
the following results as the strength of aluminium
wire : —
DIAMETER. TBKSII.E STRENGTH, GRAMMES. TENACITY.
Millimetres. 1st trial. 2d trial. Mean. Kilos per sq. millimetre.
0.225 661 653 657 12.975
0.205 524 506 515 12.255
0.160 307 311 309 12.700
0.145 246 252 249 11.845
SONOROUSNESS.
Deville: A very curious property, which alumi-
nium shows the more the purer it is, is its excessive
sonorousness, so that a bar of it suspended by a
fine wire and struck sounds like a crystal bell.
M. Lissajous, who with me observed this property,
has taken advantage of it to construct tuning forks
of aluminium, which vibrate very well. I also
tried to cast a bell, which has been sent to the
Royal Institution at London at the request of my
friend Rev. J. Barlow, vice-president and secretary
of the institution. This bell, cast on a model not
well adapted to the qualities of the metal, gives a
sharp sound of considerable intensity, but which
is not prolonged, as if the clapper or support hin-
dered the sound, which, thus hindered, becomes
far from agreeable. The sound produced by the
ingots is, on the contrary, very pure and prolonged.
64 ALUMINIUM.
Ill the experiments made in Mr. Faraday's labora-
tory, this celebrated physicist has remarked that
the sound produced by an ingot of aluminium is
riot simple. One can distinguish, by turning the
vibrating ingot, two sounds very near together
and succeeding each other rapidly, according as one
or the other face of the ingot faces the observer.
Watts: Aluminium is highly sonorous, but a
bell cast of it gave a sound like a cracked pot.
DENSITY.
Deville : The density of aluminium is 2.56 ; by
rolling this is considerably increased, so as to become
2.67, indicating a considerable approaching of the
molecules to each other; which may explain the
differences existing in its properties after being
annealed or worked. Heated to 100° and cooled,
it changes very little, for its specific gravity is
still 2.65. The following table compares it with
the other metals : — •
Pt
Au
Pb
Hg
Cu
Fe
Sn
Zn
Al
Sp.Gr.
21.5
Sp.Gr. Al.=
8 6
19.3
11.4
7.7
4.8
10.5
8.9
4.2
3.6
7.8
7.3
2.9
2 8
7.1
2.5
2.8
1.0
PHYSICAL PROPERTIES OF ALUMINIUM. 65
Since the metal has been in commerce it has
been sold at a high price ; at present (1859) it can
be bought in large quantities at 300 fr. per kilo ;
it is, therefore, much dearer than silver. But,
because of the difference in their densities, for
equal volumes of aluminium and silver, the value
of the former must be divided by 4 in order to
compare them; making a volume of aluminium
much cheaper than an equal volume of silver,
while, besides, it is much stronger. So, to-day,
Al may be considered as costing 75 fr. to Ag
220 fr.
Mallet: The specific gravity of absolutely pure
aluminium was carefully determined at 4° C., and
the mean of three closely agreeing observations
gave 2.583.
FUSIBILITY.
Deville: Aluminium melts at a temperature
higher than that of zinc, lower than that of silver,
but approaching nearer to that of zinc than silver.
It is, therefore, quite a fusible metal.
Mallet : It seems that pure aluminium is a little
less fusible than the commercial metal.
Mierzinski: The melting point of aluminium
can be taken as about 700° C.
66 ALUMINIUM.
FIXITY.
Deville: Aluminium is absolutely fixed, and
loses no part of its weight when it is violently
heated in a forge fire in a carbon crucible.
Watts: Aluminium heated in a closed vessel
does not exhibit the slightest tendency to volatilize.
Fremy : Aluminium is fixed at all temperatures.
ELECTRIC CONDUCTIVITY.
Deville: Aluminium conducts electricity #rith
great facility, so that it may be considered as one
of the best conductors known, and perhaps equal
to silver. I found by Wheatstone's Bridge that
it conducts eight times better than iron. M. Buff*
has arrived at results evidently different from
mine because we have not taken the same ground
of comparison. The difference is due, without
doubt, to the metal which he employed containing,
as is easily found in many specimens, a little cryo-
lite and fusible materials, the density of which is
near that of the metal, and which were employed
in producing it. The complete separation of the
metal and flux is a difficult mechanical operation,
but which is altogether avoided by using a vola-
tile flux. This is a condition which must be sub-
mitted to in order to get the metal absolutely
pure.
' Jahresb. der Chemie,' 1881, p. 94: Aluminium
PHYSICAL PROPERTIES OF ALUMINIUM. 67
thus compares with copper and magnesium in elec-
tric conductivity : —
At 0°. At 100°.
Cu .... 45.74 33.82
Mg .... 24.47 17.50
Al .... 22.46 17.31
After Al come red brass, Cd, yellow brass, Fe,
Zn, Pb, Ag, Sb, Bi, in the order given.
Fremy : The electric conductivity of aluminium
is 51.5, copper being 100 ; or 33.74, silver being
100.
THERMAL CONDUCTIVITY.
Deville: It is generally admitted that conductiv-
ity for heat and electricity correspond exactly in
the different metals. A very simple experiment
made by Mr. Faraday in his laboratory seems to
place aluminium very high among metallic con-
ductors. He found that it conducted heat better
than silver or copper.
Watts: Aluminium conducts heat better than
silver.
4 Jahresb. der Chemie,' 1881, p. 94: Aluminium
has the following conductivity for heat: —
AtO°. At 100°.
Cu .... 0.7198 0.7226
Mg 0.3760 0.3760
Al .... 0.3435 0.3619
After Al come red brass, Cd, yellow brass, Fe,
Zn, Pb, Ag, Sb, Bi in the order given.
68 ALUMINIUM.
Mierzinski: No less remarkable than the con-
ductivity of aluminium for electricity is that for
heat. According to Calvert and Johnson (Dingier,
153, 285), that of silver being 1000, aluminium is
665.
SPECIFIC HEAT.
Deville: According to the experiments of M.
Regnault, the specific heat of aluminium corre-
sponds to its equivalent 13.75, from which we may
conclude that it must be very large when compared
with all the other useful metals. One can easily
perceive this curious property by the considerable
time which it takes an ingot of the metal to get
cold. We might even suggest that a plate of alu-
minium would make a good chafing dish. Another
experiment makes this conclusion very evident.
M. Paul Morin had the idea to use aluminium for
a plate on which to cook eggs,. the sulphur of which
attacked silver so easily ; and he obtained excellent
results. He noticed, also, that the plate kept its
heat a much longer time than the silver one. This
exceptional property should be utilized for some-
thing.
Mallet: The specific heat of absolutely pure
aluminium was 0.2253, therefore the atomic heat
is 0.2253 times 27.02 or 6.09.
Fremy : The specific heat of aluminium is
PHYSICAL PROPERTIES OF ALUMINIUM. 69
0.2181 ; larger than that of any other useful metal,
which accords with its small atomic weight.
MAGNETISM.
Deville: I have found, as also MM. Poggen-
dorfF and Reiss, that aluminium is very feebly
magnetic.
CRYSTALLINE FORM.
Deville : Aluminium often presents a crystalline
appearance when it has been cooled slowly. When
it is not pure the little crystals which form are
needles, and cross each other in all directions.
When it is almost pure it still crystallizes by
fusion, but with difficulty, and one may observe
on the surface of the ingots hexagons which ap-
pear regularly parallel along lines which centre in
the middle of the polygon. It is an error to con-
clude from this observation that the metal crystal-
lizes in the rhombohedral system. It is evident
that a crystal of the regular system may present a
hexagonal section ; while, on the other hand, in
preparing aluminium by the battery at a low tem-
perature, I have observed complete octahedrons,
which were impossible of measurement, it is true,
but their angles appeared equal.
PART IV.
CHEMICAL PROPERTIES OF ALUMINIUM.
REMARK: Unless specifically stated otherwise,
the properties here mentioned are those of the
pure metal and not of the commercial, the impuri-
ties of which generally modify the properties of
the aluminium more or less.
ACTION OF AIR.
Deville: Air, wet or dry, has absolutely no
action on aluminium. No observation which has
come to my knowledge is contrary to this assertion,
which may easily be proved by any one. I have
known of beams of balances, weights, plaques,
polished leaf, reflectors, etc., of the metal exposed
for months to moist air and sulphur vapors, and
showing no trace of alteration. We know that
aluminium may be melted in the air with impun-
ity. Therefore air and also oxygen cannot sensi-
bly affect it ; it resisted oxidation in the air at the
highest heat I could produce in a cupel furnace, a
heat much higher than that required for the assay
of gold. This experiment is interesting, especially
CHEMICAL PROPERTIES OF ALUMINIUM. 71
when the metallic button is covered with a layer
of oxide which tarnishes it, the expansion of the
metal causes small branches to shoot from its sur-
face, which are very brilliant, and do not lose their
lustre in spite of the oxidizing atmosphere. M.
Wbhler has also observed this property on trying
to melt the metal with a blowpipe. M. Peligot
has profited by it to cupel aluminium. I have
seen buttons of impure metal cupelled with lead
and become very malleable.
With pure aluminium the resistance of the metal
to direct oxidation is so considerable that at the
melting point of platinum it is hardly appreciably
touched, and does not lose its lustre. It is well
known that the more oxidizable metals take this
property away from it. But silicon itself, which
is much less oxidizable, when alloyed with it
makes it burn with great brilliancy, because there
is formed a silicate of aluminium.
Watts : Aluminium may be heated intensely in
a current of air in a muffle without undergoing
more than superficial oxidation. When heated as
foil with a splinter of wood in a current of oxygen
it burns with a brilliant, bluish-white light.
1 Chemical News,' 1859 : Wohler finds that alu-
minium leaf burns brightly in air and in oxygen
with a brilliant light. The A1203 formed is as
hard as corundum. Wire burns in oxygen like
iron wire, but the combustion cannot continue be-
cause the wire fuses.
72 ALUMINIUM.
Mterzinski: Aluminium does not change at a
somewhat high temperature in the air; hut if
heated to whiteness it burns, with the production
of strong light, to A1203, which covers the surface
of the bath.
ACTION OF WATER (H20).
Deville: "Water has no action on aluminium,
either at ordinary temperatures, or at 100°, or at
a red heat bordering on the fusing point of the
metal. I boiled a fine wire in water for half an
hour and it lost not a particle in weight. The
same wire was put in a glass-tube heated to red-
ness by an alcohol lamp and traversed by a current
of steam, but after several hours it had not lost its
polish, and had the same weight. To obtain any
sensible action it is necessary to operate at the
highest heat of a reverberatory furnace, a white
heat. Even then the oxidation is so feeble that it
develops only in spots, producing almost inappre-
ciable quantities of APO3. This slight alteration
and the analogies of the metal allow us to admit
that it decomposes water, but very feebly. If,
however, metal produced by M. Rose's method
was used, which is almost unavoidably contami-
nated with slag 'composed of chlorides of alumin-
ium and sodium, the A12C16, in presence of water,
plays the part of an acid towards aluminium, dis-
engaging hydrogen with the formation of a sub-
CHEMICAL PROPERTIES OF ALUMINIUM. 73
chlorhydrate of alumina, whose composition is not
known, and which is soluble in water. When the
metal thus tarnishes in water one may be sure to
find chlorine in the water on testing it with nitrate
of silver.
Mierzinski: Cold and warm water have no
influence on aluminium even if it is heated to
redness.
4 Chemical Xews,' 1859 : Aluminium leaf will
slowly decompose water at 100° ; at first it takes
a bronze color, and after boiling some hours it
becomes translucent.
ACTION OF HYDROGEN SULPHIDE AND SULPHUR
(H2S and S).
Deville: Sulphuretted hydrogen exercises no
action on aluminium, as may be proved by leaving
the metal in an aqueous solution of the gas. In
these circumstances almost all the metals, and
especially silver, blacken with great rapidity.
Sulph-hydrate of ammonia may be evaporated on
an aluminium leaf, leaving on the metal only a
deposit of sulphur which the least heat drives
away.
Aluminium may be heated in a glass tube to a
red heat in vapor of sulphur without altering the
metal. This resistance is such that in melting
together poly sulphide of potassium and some
aluminium containing copper or iron, the latter are
7
74 ALUMINIUM.
attacked without the aluminium being sensibly
affected. Unhappily, this method of purification
may not be employed because of the protection
which aluminium exercises over foreign metals.
Under the same circumstances gold and silver dis-
solve up very rapidly. However, at a high tempera-
ture I have observed that it combines directly with
sulphur to give A12S3. These properties varying
so much with the temperature form one of the
special characteristics of the metal and its alloys.
Fremy : H2S is without action on aluminium,
acting towards it as towards the sulphides of iron,
zinc, or copper. It is true that aluminium decom-
poses Ag2S, but it sets the sulphur at liberty and
combines with the silver. These facts are in ac-
cordance with the resistance the metal offers to
free sulphur.
SULPHURIC ACID (H2S04).
Deville : Sulphuric acid, diluted in the propor-
tion most suitable for attacking the metals which
decompose water, has no action on aluminium ; and
contact with a foreign metal does riot help, as with
zinc, the solution of the metal, according to M. de
la Rive. This singular fact tends to remove alu-
minium considerably from, those metals. To
establish it better, I left for several months some
globules weighing only a few milligrammes in con-
tact with weak H2S04, and they showed no visible
CHEMICAL PROPERTIES OF ALUMINIUM. 75
alteration; however the acid gave a faint precipi-
tate with aqua ammonia.
Fremy : H2S04, dilute or concentrated, exercises
in the cold only a very slight sensible action on
aluminium, the pure metal is attacked more slowly
than when it contains foreign metals. The presence
of silicon gives rise to a disengagement of Sill4,
which communicates to the hydrogen set free a
tainted odor. Concentrated H2S04 dissolves it
rapidly with the aid of heat, disengaging sulphurous
acid gas (SO2).
NITRIC ACID (UNO3).
Deville: Nitric acid, weak or concentrated, does
not act on aluminium at the ordinary temperature.
In boiling HXO3 the solution takes place, but with
such slowness that I had to give up this mode of dis-
„ solving the metal in my analyses. By cooling the
solution all action ceases. M. Hulot has obtained
good results on substituting aluminium for plati-
num in the Grove battery.
HYDROCHLORIC ACID (HC1).
Deville: The true solvent of aluminium is HC1,
weak or concentrated ; but, when the metal is per-
fectly pure, the reaction takes place so slowly that
M. Favre, of Marseilles, had to give up this way of
attack in determining the heat of a combination of
76 ALUMINIUM.
the metal. But impure aluminium is dissolved
very rapidly. At a very low temperature gaseous
HC1 attacks the metal and changes it into A12C16.
Under these circumstances iron does not seem to
alter; able, no doubt, to resist by covering itself
with a very thin protecting layer of FeCl2. This
experiment would lead me to admit that it is the
HC1 and not the water which is decomposed by
aluminium; and, in fact, the metal is attacked
more easily as the acid is more concentrated. This
explains the difference of the action of solutions of
HC1 and H2S04, the latter being almost inactive.
This reasoning applies also to tin.
When the metal contains silicon, it disengages
hydrogen of a more disagreeable smell than that
given out by iron under similar circumstances.
The reason of this is the production of that remark-
able body recently discovered by MM. Wohler
and Buff — Sill4. "When the proportion of silicon is
small, the whole is evolved as gas ; when in-
creased a little, some remains in solution with the
aluminium, and then it requires great care to
separate the metal exactly, even when the solution
is evaporated to dryness. If 3 to 5 per cent, of Si
is present, it remains insoluble mixed with a little
SiO2, as has been cleverly proven by Wohler and
Buff by the action of hydrofluoric acid, which dis-
solves the SiO2 with evolution of H without attack-
ing the Si itself. On dissolving commercial alu-
minium there is sometimes obtained a black,
CHEMICAL PROPERTIES OF ALUMINIUM. 77
crystalline residue, which, separated on a filter and
dried at 200° to 300° takes fire in places; this
residue is Si mixed with some SiO2. The presence
of Si augments very much the facility with which
Al is attacked by HC1.
Mierzinski: If HC1 is present in a mixture of
acids, it begins the destruction of the metal. HI,
HBr, and HF act similarly to HC1.
POTASH, SODA, AND LIME (KOH, ^"aOH, Ca(OH)2).
Deville : Alkaline solutions act with great energy
on the metal, transforming it into aluminate of
potash or soda, setting free hydrogen. However,
it is not attacked by KOH or !N"aOH in fusion ;
one may, in fact, drop a globule of the pure metal
into melted caustic st>da raised almost to a red
heat in a silver vessel, without observing the least
disengagement of hydrogen. Silicon, on the con-
trary, dissolves with great energy under the same
circumstances. I have employed melted £TaOH to
clean siliceous aluminium. The piece is dipped
into melted XaOH kept almost at red heat. At
the moment of immersion several bubbles of H
disengage from the metallic surface, and when they
have disappeared, all the Si of the superficial layer
of Al has been dissolved. It only remains to wash
well with water and dip it into nitric acid, when
the aluminium takes a beautiful mat.
Mallet : The pure metal presents greater resist-
7*
78 ALUMINIUM.
ance to the prolonged action of alkalies than the
impure.
Mierzinski : Lime-water acts similarly to NaOH
or KOH, with the difference that the resulting
calcium compound is precipitated.
I
AQUA AMMONIA (NH4OH).
Deville: Aqua ammonia acts only feebly on
aluminium, producing a little A1203, which, accord-
ing to a very curious observation of Wohler, has
the property of partly dissolving in the ammonia.
In an atmosphere in which ammonia was present,
the metal did not lose its lustre, which is easily
explained, because it is only in contact with water
that the oxidization of the metal takes place, with
disengagement of hydrogen.
ORGANIC ACIDS, VINEGAR, ETC.
Deville : Weak acetic acid acts oh aluminium in
the same way as H2S04, i. e., in an inappreciable
degree or with extreme slowness. I used for the
experiment acid diluted to the strength of strongest
vinegar. M. Paul Morin left a plaque of the metal
a long time in wine which contained tartaric acid
in excess and acetic acid, and found the action on it
quite inappreciable. The action of a mixture of
acetic acid and NaCl in solution in pure water on
pure aluminium is very different, for the acetic
CHEMICAL PROPERTIES OF ALUMINIUM. 79
acid replaces a portion of the HC1 existing in the
NaCl, rendering it free. However, this action is
very slow on the Al, especially if it is pure.
The practical results flowing from these observa-
tions deserve to be clearly defined, because of the
applications which may be made of aluminium to
culinary vessels. I have observed that the tin so
often used, and which each day is put in contact
with ivTaCl and vinegar, is attacked much more
rapidly than aluminium under the same circum-
stances. Although the salts of tin are very poison-
ous, and their action on the economy far from
being negligible, the presence of tin in our food
passes unperceived because of its minute quantity.
Under the same circumstances, aluminium dissolves
in less' quantity; the acetate of Al formed resolves
itself on boiling into insoluble APG3 or an insoluble
sub-acetate, having no more taste or action on the
body than clay itself. It is for that reason, and
because it is known that the salts of the metal have
no appreciable action on the body, that aluminium
may be considered as an absolutely harmless metal.
SOLUTIONS OF METALLIC SALTS.
Deville : The action of any salt whatever may
be easily deduced from the action of the acids on
the metal. We may, therefore, predict that in acid
solutions of sulphates and nitrates aluminium will
precipitate no metal, not even silver, as Wohler has
80 ALUMINIUM.
observed. But the hydrochloric solutions of the
same metals will be precipitated, as MM. Tissier
have shown. Likewise, in alkaline solutions, Ag,
Pb, and metals high in the classification of the
elements are precipitated.
It may be concluded from this that' to deposit
aluminium on other metals by means of the bat-
tery, it is always necessary to use acid solutions in
which IIC1, free or combined, should be absent.
For similar reasons the alkaline solutions of the
same metals cannot be employed, although they
give such good results in plating common metals
wnth gold and silver. It is because of these curious
properties that gilding and silvering aluminium
are so difficult. M. Paul Morin and I have often
tried a bath of basic sulphide of gold, or hyposul-
phite of silver, with a large excess of sulphurous
acid, with no good results. But M. Mourey, who
has already rendered great services in galvanoplasty,
readily gilds and silvers aluminium for commerce
with astonishing skill when we consider the short
time he has had to study this question. I know
also that M. Christofle has gilded it, but I am
entirely ignorant of the processes employed by these
gentlemen. The coppering of aluminium by the
battery is effected very easily by means of M. Hulot's
process. He uses simply a bath of acid sulphate
of copper. The layer of copper, if well prepared,
is very solid.
All that I have said on the subject of the action
CHEMICAL PROPERTIES OF ALUMINIUM. 81
of metallic salts is true only for pure aluminium.
Impure metal, especially if it contains iron or sodium,
acts then in producing in the copper salts with which
I operate a deposit of metallic Cu. But this phe-
nomenon, even in the most unfavorable cases, is
produced very slowly, and if a leaf of aluminium
is used one may see at the end of several weeks
the texture of the metal etched with red fibres, as
if the Fe and Al were only in juxtaposition, and
the ferruginous fibres acted alone. Moreover, the
deposit is only local, and little by little becomes
complete ; but it is slower as the metal is purer.
Mierziuski: Silver is precipitated by Al from a
nitrate solution, feebly acid or neutral, in dendrites ;
the separation begins after six hours ; from an am-
moniacal solution of AgCl or Ag2Cr04, Al precipi-
tates the metal immediately as a crystalline powder.
From CuSO4 or Cu(N03/ solution, Al separates
Cu only after two days, in dendrites or octahedra ;
from the latter it also precipitates a basic salt as a
green, insoluble powder; from a CuCl2 solution the
Cu falls immediately ; somewhat slower from solu-
tion of acetate of copper. The sulphate or nitrate
solution behaves similarly if a little KC1 is added
to it, and the precipitation is complete in presence
of excess of Al.
From Hg2Cl2, Hg2Cy2, and Hg2(X03)2, Hg sepa-
rates first, and then forms an amalgam with the
Al which decomposes water at ordinary tempera-
tures or oxidizes in the air with development of
82 ALUMINIUM.
much heat ; the same qualities are possessed by the
amalgam formed by warming the two metals to-
gether in an atmosphere of CO2.
From Pb(N03)2 and Pb(C2H302/ the metal sepa-
rates slowly in crystals ; from PbCl2 immediately ;
an alkaline solution of PbCrO gives Pb and Cr203.
From an alcoholic solution of HgCl2 the Hg is
precipitated much quicker with a gentle heat. Al
also reduces Hg from a solution of Hgl2 in KI.
Al separates Hg from HgCl2 vapors, and A12C16
deposits in the cooler part of the tube, the remain-
ing Al being melted by the heat of the reaction.
Al acts likewise toward melted As^Cl, the silver
£5 /
set free being melted by the heat of the reaction.
Zn is easily thrown down from alkaline solution.
Fremy: Aluminium decomposes a very large
number of metallic solutions, which takes place
especially easily if the solution is made alkaline
or ammoniacal. Acid, and especially neutral solu-
tions, are less favorable for the experiment. All
the chlorides, excepting KC1 and NaCl,are reduced
by it. A12C16 is no exception, for the solution is
decomposed with evolution of hydrogen. Alu-
minium easily resists solutions of Nad and alum
separately, but dissolves in a mixed solution of
these two salts. In alkaline solution, the metals
are precipitated because of the facility with which
aluminates of the alkalies are formed.
Watts (2d Supplement) : The action of alumin-
ium on metallic solutions is as follows : Cu is pre-
CHEMICAL PBOPERTIES OF ALUMINIUM. 83
cipitated from copper salts ; Pb is slowly precipi-
tated from lead salts ; Ag is precipitated from a
slightly acid or neutral solution of Ag^O3 ; Zn is
readily precipitated from zinc salts.
NITRE.
Deville: Aluminium may be melted in nitre
without undergoing the least alteration, the two
materials rest in contact without reacting, even at
a red heat, at which temperature the salt is plainly
decomposed, disengaging oxygen actively. But if
the heat is pushed to the point where nitrogen
itself is disengaged, there the nitre becomes potassa,
a new affinity becomes manifest, and the phenomena
change. The metal then combines rapidly with
the K2O to give aluminate of potash. The accom-
panying phenomenon of flagration often indicates a
very energetic reaction. Aluminium is continually
melted with nitre at a red heat to purify it by the
oxygen disengaged, without any fear of loss. But
it is necessary to be very careful in doing it in an
earthen crucible. The SiO2 of the crucible is dis-
solved by the nitre, the glass thus formed is decom-
posed by the aluminium, and the silicide of alu-
minium formed is then very oxidizable, especially
in the presence of alkalies. The purification by
nitre ought to be made in an iron crucible well
oxidized by nitre inside.
Fremy : At the melting point, aluminium is not
84 ALUMINIUM.
attacked by nitre ; this property has been at times
utilized to oxidize and then remove the metals
alloyed with it, but it is now demonstrated that
this mode of purification is very imperfect.
Mierzinski : Heated to redness with nitre, alu-
minium burns with a fine blue flame.
SILICATES AND BORATES.
Deville : By treating silicates and borates with
aluminium silicon and boron may be obtained.
The process is described at the end of Deville's
book, but is too long and foreign to the subject in
hand to be given here.
Tissier : Aluminium melted in an ordinary white
glass vessel oxidizes itself at the expense of the
SiO2, setting free silicon, and the alumina formed
combines with the alkali forming an alurninate.
In experiments which we have made, the metal
became covered with a thin layer of silicon, while the
metal which remained underneath was still malle-
able and did not appear to be combined with Si.
FLUORSPAR.
Tissier: This salt is without action on the metal
and makes its best flux, especially so because of the
property which it has of dissolving the alumina
with which the metal may be contaminated and
CHEMICAL PROPERTIES OF ALUMINIUM. 85
which encrusts little globules. The fluorspar, by
dissolving this crust, facilitates their reunion.
PHOSPHATE OF LIME.
Tissier : We have heated to white heat a mixture
of pure Ca3(P04)2 and aluminium leaf, without the
metal losing its metallic appearance. This material
thus appears to have no action on the metal.
SODIUM CHLORIDE (NaCl) AND CHLORIDES.
Deville : A solution of sodium or potassium
chloride, in which is put a pure aluminium wire,
seemed to me to exercise no sensible action on the
metal, either cold or warm. It is not the same
with the other metallic chlorides, and we may
state that, as a general rule, these are decomposed
by aluminium with greater facility as the metal
which they contain belongs to a higher order. The
chlorhydrate of A\ itself dissolves aluminium
forming a sub-chlorhydrate with evolution of hy-
drogen.
Tissier: KaCl is employed as a flux for Al in
remelting it. It does not possess the property, like
CaF2, of dissolving the A1203, and has the incon-
venience of producing with the clay of the crucible
a sensible quantity of A12C16, which may on con-
tact with the air act in promoting the loss of a
certain quantity of metal.
8
86 ALUMINIUM.
METALLIC OXIDES.
Tissier : We made our experiments in this way :
The Al leaf was mixed carefully with the oxide
on which we experimented, then the mixture was
placed in a small porcelain capsule and heated in a
small earthen crucible which served as a muffle.
Our results were as follows : —
MnO2 — Aluminium has no action on manganese
o
dioxide.
Fe203 — By heating to white heat 1 equivalent of
Fe203 and 3 of Al, the reaction took place with
detonation, and by heating sufficiently we obtained
a metallic button, well melted, and containing 69.3
per cent. Fe and 30.7 per cent. Al, being as hard
and brittle as cast-iron. Its composition is nearly
AlFe. It would thus appear that the decomposition
of Fe203 will not pas's the limit where the quantity
of iron reduced is sufficient to form with the alu-
minium the alloy AlFe.
ZnO: A mixture of aluminium leaf and zinc
oxide heated to whiteness did not appear to present
the least indication of decomposition.
PbO: We mixed 2 equivalents of litharge with 1
of aluminium, and heated the mixture slowly up to
white heat, when the Al reacted on the PbO with
such intensity as to produce a strong detonation.
We made an experiment writh 50 grammes of PbO
and 2.9 grammes of Al leaf, when the crucible was
CHEMICAL PROPERTIES OF ALUMINIUM. 87
broken to pieces and the doors of the furnace blown
off.
CuO : 3 grammes of black oxide of copper mixed
with 1.03 grammes of aluminium detonated pro-
ducing a strong explosion when the heat reached
whiteness.
Mierzinski: Aluminium reduces CuO and PbO
with explosion, Fe203 only in part, forming the
alloy AlFe. ZnO and MnO are not reduced by
aluminium.
Beketoff :* He reduced baryta (BaO) with metal-
lic aluminium in excess, and obtained alloys of
aluminium and barium containing in one case 24
per cent, in another 33 per cent, of Ba.
ANIMAL MATTERS.
Deville: Among the animal matters produced
by the organism, some are acid, as sweat. These
appear to have no sensible action on aluminium.
Alkaline materials, as the saliva, have a greater
tendency to oxidize it, but the whole effect produced
is insignificant. M. Charriere has made for a patient
on whom he practised tracheotomy a small tube
of the metal, which remained almost unaltered
although in contact with purulent matter. After
a long time a little alumina was formed on it,
hardly enough to be visible.
* Bull, de la Soc. Chem., 1857, p. 22.
88 ALUMINIUM.
MISCELLANEOUS AGENTS.
Tissier: Only 2.65 grammes of aluminium intro-
duced into melted red hot sodium sulphate (Na2S04)
decomposed that salt with such intensity that the
crucible was broken into a thousand pieces, and
the door of the furnace blown to a distance.
Heated to redness with alkaline carbonate, the
Al wTas slowly oxidized at the expense of the CO2,
C was set free, and an aluminate formed. The
reaction takes place without deflagration.
Mierzinski : Heated to redness with potassium
or sodium sulphate, aluminium gives a strong
detonation. Potassium carbonate quickly destroys
the metal with separation of carbon. Hydrogen,
nitrogen, sulphur, and carbon are without any
influence on aluminium, but chlorine, iodine, bro-
mine, and fluorine attack it rapidly.
GENERAL OBSERVATIONS ON THE PROPERTIES OF
ALUMINIUM.
Deville: Aluminium, at a low temperature, con-
ducts itself as a metal which can give a very weak
base ; in consequence, its resistance to acids, IIC1
excepted, is very great. It conducts itself with
the alkalies as a metal capable of giving a quite
energetic acid, it being attacked by K20 and Na20
O O v
dissolved in water. But, this affinity is still
insufficient to determine the decomposition of
CHEMICAL PROPERTIES OF ALUMINIUM. 89
melted KOH. For a stronger reason it does not
decompose metallic oxides at a red heat. This is
why, in the muffle, the alloy of aluminium and
copper gives black CuO, and this also accounts for
the alloy of aluminium and lead being capable of
being cupelled. But, by a strange exception, and
which does not appertain solely, I believe, to alu-
minium, as soon as the heat is above redness the
affinities are quickly inverted, and the metal takes
all the properties of silicon, decomposing the oxides
of lead and copper with the production of alumin-
ates.
From all the experiments which have been re-
ported and from all the observations which have
been made, we can conclude that aluminium is a
metal which has complete analogies with no one ot
the simple bodies which we consider metals. In
1855 I proposed to place it along side of chromium
and iron, leaving zinc out of the group with which
aluminium had been until then classed. Zinc is
placed very well beside magnesium, there being
intimate analogies between these two volatile
metals. There may be found at the end of a memoir
which M. AVohler and I published in the ' Compt
Rendue' and the ' Ami. de Chem. et de Phys.' the
reasons why we are tempted to place aluminium
near to silicon and boron in the carbon series, on
grounds analogous to those on which antimony and
arsenic are placed in the nitrogen series.
PART V.
METALLURGY OF ALUMINIUM.
As has been remarked in the historical section,
Davy was the first to try to isolate aluminium.
His attempts were unsuccessful. The next chemist
to publish an account of attempts in this direction
was Oerstedt, who published a paper in 1824 in a
Swedish periodical.* Oerstedt's original paper is
thus translated into Berzelius' ' Jahresbericht :'f
" Oerstedt mixes calcined and pure alumina, quite
freshly prepared, with powdered charcoal, puts it
in a porcelain retort, ignites and leads Cl gas
through. The coal then reduces the alumina, and
there results A12C16 and CO, and perhaps also some
phosgene, COC12 ; the A12C16 is caught in the con-
denser and the gases escape. The A12C16 is white,
crystalline, melts about the temperature of boiling
water, easily attracts moisture, and evolves heat
when in contact with water. If it is mixed with
a concentrated potassium amalgam and heated
quickly, it is transformed ; there results KC1, and
* Oversigt over clct K. Danske Videnskabemes Sclkabs
Forhandlingar og dets Medlemmers Arbeider. May, 1824, to
May, 1825, p. 15.
t Berz. Jahresb. der Chemie, 1827, vi. 118.
METALLURGY OF ALUMINIUM. 91
the aluminium unites with the mercury. The new
amalgam oxidizes in the air very quickly, and
gives as residue when distilled in a vacuum a lump
of metal resembling tin in color and lustre. In
addition, Oerstedt found many remarkable prop-
erties of the metal and of the amalgam, but he
holds them for a future communication after further
investigation."
I have not been able to find any other paper by
Oerstedt, but the next advance in the science is by
Wohler, and all agree in naming him as the true
discoverer of the metal. The following is taken
from Poggendorf.*
Wohler reviews the article which we have just
given, and then continues as follows: —
" I have repeated this experiment of Oerstedt,
but achieved no very satisfactory result. By heat-
ing potassium amalgam with APC16 and distilling
the product, there remained behind a gray melted
mass of metal, but which, by raising the heat to
redness, went off as green vapor and distilled as
pure potassium. I have therefore looked around
for another method or way of conducting the ope-
ration, but, unpleasant as it is to say it, the reduc-
tion of the aluminium fails each time. Since, how-
ever, Herr Oerstedt remarks at the end of his paper
that he did not regard his investigations in alu-
minium as yet ended, and already several years
* Pogg. Ann., 1827, ii. 147.
92 ALUMINIUM.
have passed since then, it looks as if I had taken
up one of those researches begun auspiciously by
another (but not finished by him) because it prom-
ised new and splendid results. I must remark, how-
ever, that Herr Oerstedt has indirectly by his silence
encouraged me to try to attain to further results my-
self. Before I give the art how one can quite
easily reduce the metal, I will say a few words
about APCl6 and its production.
" I based the method of reducing aluminium on
the reaction of A12C16 on potassium, and on the
property of the metal not to oxidize in water. I
warmed in a glass retort a small piece of APCl6
with some potassium, and the retort was shattered
with a strong explosion. I tried then to do it in a
small platinum crucible, in which it succeeded very
well. The reaction is always so violent that the
cover must be weighted down, or it will be blown
off'; and at the moment of reduction, although the
crucible be only feebly heated from outside, it sud-
denly glows inside, and the platinum is almost torn
by the sudden shocks. In order to avoid any
mixture of platinum with the reduced aluminium,
I next made the reduction in a porcelain crucible
and succeeded then in the following manner : Pat
in the bottom of the crucible a piece of potassium
free from carbon and oil, and cover this with an
equal volume of pieces of APCl6. Cover, and heat
over a spirit lamp, at first gently, that the crucible
be not broken by the production of heat inside,
METALLURGY OF ALUMINIUM.
and then heat stronger, at last to redness.
and when fully cold put it into a glass of cold water.
A gray powder separates out which on nearer ob-
servation, especially in sunlight, is seen to consist
of little flakes of metal. After it has separated,
pour off the solution, filter, wash with cold water,
and dry ; this is the aluminium."
In reality this powder possessed no metallic
properties, and, moreover, it contained potassium
and APC16, which gave to it the property of de-
composing water at 100°. To avoid the loss of
A12C16 by volatilization at the high heat developed
during the reaction, Liebig afterwards made the
vapor of APC16 pass slowly over some potassium
placed in a long glass tube. This device of Liebig
is nearly the arrangement which Wohler adopted
later, in 1845, and which gave him much better
results. The following is W6hler's second paper,
published in 1845 : — *
" On account of the violent incandescence with
which the reduction of A PCI6 by potassium is ac-
companied, this operation requires great precau-
tions, and can be carried out only on a small scale.
I took for the operation a platinum tube, in which
I placed A12C16 and near it some potassium in a
platinum boat. I heated the tube gently at first,
then to redness. But th£ reduction may also be
done by putting potassium in a small crucible
* Liebig's Annalen, 53, 422.
• 94 ALUMINIUM.
which is placed inside a larger one, and the space
between the two filled with APC16. A close cover
is put over the whole and it is heated. Equal
volumes of potassium and A12C16 are the best pro-
portions to employ. After cooling, the tube or
crucible is put in a vessel of water. The metal is
obtained as a gray, metallic powder, but on closer
observation one can see even with the naked eye
small tin-white globules some as large as pins' heads.
Under a microscope magnifying two hundred diam-
eters the whole powder resolves itself into small
globules, several of which may sometimes be seen
sticking together, showing that the metal was
melted at the moment of reduction. A beaten-out
globule may be again melted to a sphere in a bead
of borax or salt of phosphorus, but rapidly oxidizes
during the operation, and if the heat is continued,
disappears entirely, seeming either to reduce boron
in the borax bead or phosphorus or P205in the salt
of phosphorus bead. I did not succeed in melting
together the pulverulent aluminium in a crucible
with borax, at a temperature which would have
melted cast iron, for the metal disappeared entirely
and the borax became a black slag. It seems prob-
able that aluminium, being lighter than molten
borax, swims on it and burns. The white metallic
globules had the color and lustre of tin. It is per-
fectly malleable and can be hammered out to the
thinnest leaves. Its specific gravity, determined
with two globules weighing 32 milligrammes, was
METALLURGY OF ALUMINIUM. 95
2.50, and with three hammered-out globules weigh-
ing 34 milligrammes, 2.67. Ou account of their
lightness these figures can only be approximate.
It is not magnetic, remain's white in the air, de-
composes water at 100°, not at usual temperatures,
and dissolves completely in caustic potash (KOH).
When heated in oxygen almost to melting, it is
only superficially oxidized, but it burns like zinc
in a blast-lamp flame."
These results of Wbhler's, especially the deter-
mination of sp. gr., were singularly accurate when
we consider that he established them working with
microscopic bits of the metal. It was just such
work that established Wohler's fame as an investi-
gator. However, we notice that his metal differed
from aluminium as we know it in several important
respects, in speaking of which Deville says: "All
this time the metal obtained by Wohler was far
from being pure; it was very difficultly fusible,
owing without doubt to the fact that it contained
platinum taken from the vessel in which it had
been prepared. It is well known that these two
metals combine very easily at a gentle heat. More-
over, it decomposed water at 100°, which must be
attributed either to the presence of some potassium
or to APC16, with which the metal might have
been impregnated ; for aluminium in presence of
APCl6 in effect decomposes water with evolution of
hydrogen.
After AYohler's paper in 1845, the next improve-
96 ALUMINIUM.
ment is that introduced by Deville, in 1854-55,
and this is really the date at which aluminium, the
metal, became known and its true properties estab-
lished. He first read to the Academy an account of
his laboratory process, by which he obtained a
pencil of the metal. The following is his account:*
"The following is the best method for obtaining
aluminium chemically pure in the laboratory.
Take a large glass tube about four centimetres in
diameter, and put into it pure APC16 free from
iron, and isolate it between two stoppers of ami-
anthus (tine, silky asbestos). Hydrogen, well dried
and free from air, is brought in at one end of the
tube. The APC16 is heated in this current of gas
by some lumps of charcoal, in order to drive off
hydrochloric acid or sulphides of chlorine or of
silicon, with which it is always impregnated. Then
there are introduced into the tube porcelain boats,
as large as possible, each containing several grammes
of sodium, which was previously rubbed quite dry
between leaves of filter paper. The tube being full
of hydrogen the sodium is melted, the A12C16 is
heated and distils, and decomposes in contact with
the sodium with incandescence, the intensity of
which can be moderated at pleasure. The operation
is ended when all the sodium has disappeared, and
when the sodium chloride formed has absorbed so
much A12C16 as to be saturated with it. The Al
* Ann. de. Pays, et de Chem., xliii. 24.
METALLURGY OP ALUMINIUM. 97
which has been formed is held in the douhle
chloride of sodium and aluminium, Al2Cl6.2!N"aCl,
a compound very fusihle and very volatile. The
boats are then taken from the glass tube, and their
entire contents put in boats made of retort carbon,
which have been previously heated in dry chlorine
in order to remove all silicious and ferruginous
matter. These are then introduced into a large
porcelain tube, furnished with a prolongation and
traversed by a current of hydrogen, dry and free
from air. This tube being then heated to redness,
the Al2Cl6.2XaCl distils without decomposition
and condenses in the prolongation. There is found
in the boats, after the operation, all the Al which
had been reduced, collected in at most one or two
small buttons. The boats when taken from the
tube should be nearly free from Al2Cl6.2]N"aCl and
also from ^aCl. The buttons of aluminium are
united in a small earthen crucible which is heated
as gently as possible, just sufficient to melt the
metal. The latter is pressed together and skimmed
clean by a small rod or tube of clay. The metal
thus collected may be very suitably cast in an
ingot mould."
The later precautions added to the above given
process were principally directed towards avoiding
the attacking of the crucible, which always takes
place when the metal is melted with a flux, and the
aluminium thereby made more or less siliceous.
The next improvement was the introduction by
9
98
ALUMINIUM.
Deville of an application
on a large scale of the lab-
oratory method just de-
scribed. He first put it
up at the chemical works
of M. du Sussex, at Javel,
and later at the works of
MM. Rousseau Bros., at
Glaciere. It has at pre-
sent only an historic inter-
est, as it was soon modi-
fied in its details so as to
be almost entirely chang-
ed, but I give it here so
as to show the different
phases through which the
industry has passed. The
text is not given in full as
Deville describes it, which
would be unnecessary ; but
the condensed account
gives a clear idea of the
process. The full descrip-
tion may be found in De-
ville'shook, or in the 'Ann.
de Chem. et de Phys.' [3]
xlvi. 445, where it first
appeared.
The crude APC16, placed
in the cylinder A, is vap-
METALLURGY OF ALUMINIUM. 99
orized by the fire and passes through the tube to
the cylinder B containing 60 to 80 kilos of iron
nails heated to a dull-red heat. The iron retains
as relatively fixed ferrous chloride, the ferric
chloride and hydrochloric acid which contaminate
the APC16, and likewise transforms any sulphur
dichloride (SCI2) in it into ferrous chloride and sul-
phide of iron. The vapors on passing out of B
through the tube, which is kept at about 300°,
deposit spangles of ferrous chloride, which is with-
out sensible tension at that temperature. The
vapors then enter D, a cast-iron cylinder in which
are three cast-iron boats each containing 300 grms.
of sodium. It is sufficient to heat this cylinder
barely to a dull-red heat in its lower part, for the
reaction once commenced disengages enough heat
to complete itself, and it is often necessary to take
away all the fire from it. There is at first pro-
duced in the first boat some aluminium and some
sodium chloride, which latter combines with the
excess of .A12C1' to form the volatile chloride
Al2Cl6.2NaCl. These vapors of double chloride
condense on the second boat and are decomposed
by the sodium to aluminium and sodium chloride.
A similar reaction takes place in the third boat
when all the sodium of the second has disappeared.
When on raising the cover it is seen that the reac-
tions are over, the boats are taken out, immedi-
ately replaced by others, and are allowed to cool
covered by empty boats. In this first operation
100 ALUMINIUM.
the reaction is rarely complete, for the sodium is
protected by the layer of NaCl formed at its
expense. To make this disappear, the contents of
the hoats are put into cast iron pots or earthen
crucibles, which are heated until the APC16 begins
to volatilize. Then the pots or crucibles are cooled
and there is taken from the upper part of their
contents a layer of ISTaCl, almost pure, while under-
neath are found globules of aluminium, which are
separated from the residue by washing with water.
Unfortunately, the water in dissolving the A12C16
of the flux exercises on the metal a very rapid
destructive action, and only the globules larger
than the head of a pin are saved from this washing.
These are gathered together, dried, melted in an
earthen crucible, and pressed together with a clay
rod. The button is then cast in an ingot mould.
It is important in this operation to employ only well
purified sodium, and not to melt the aluminium if it
still contains any sodium, for in this case the metal
takes fire and burns as long as any of the alkaline
metal remains in it. In such a case it is necessary to
remelt in presence of a little Al2Cl6.2JSTaCl."
Deville says later, "Such was the detestable pro-
cess by means of which we made the ingots of
aluminium which were sent to the Exposition."
Deville, after this, tried some experiments in
which he used sodium vapor, and he thus reports
his results in his book: "This process, which I
have not perfected, is very easy to operate, and gave
METALLURGY OF ALUMINIUM. 101
me very pure metal at the first attempt. I operate
as follows : I fill a mercury bottle with a mixture
of chalk, carbon, and carbonate of soda, in the
proportions best for generating sodium. An iron
tube about ten centimetres long is screwed to the
bottle, and the whole placed in a wind furnace,
so that the bottle is heated to red-white and the
tube is red to its end. The end of the tube is
then introduced into a hole made in a large earthen
crucible about one-fourth way from the bottom,
so that the end of the tube just reaches the inside
surface of the crucible. The carbonic oxide (CO)
disengaged burns in the bottom of the crucible,
heating and drying it; afterwards the sodium flame
appears, and then pieces of A12C16 are thrown into
the crucible from time to time. The salt volatilizes
and decomposes before this sort of tuyere from
which issues the reducing vapor. APC16 is added
when the vapors coming from the crucible cease to
be acid, and when the flame of sodium burning in
the atmosphere of A12C16 loses its brightness. AV hen
the operation is finished, the crucible is broken and
there is taken from the walls below the entrance
of the tube a saline mass composed of N"aCl, a
considerable quantity of globules of aluminium,
and some sodium carbonate, which latter is in
larger quantity the slower the operation wras per-
formed. The globules are detached by plunging the
saline mass into water, when it becomes necessary
to notice the reaction of the water on litmus. If the
9*
102 ALUMINIUM.
water becomes acid, it is renewed often ; if alkaline.,
the mass impregnated with metal must be digested
in nitric acid diluted with three or four volumes of
water, and so the metal is left intact. The globules
are reunited by melting with the precautions before
given."
Deville modified these methods in various ways.
APC16 is a deliquescent salt, difficult of preservation,
and so was soon replaced by Al2Cl6.2NaCl, which
does not present these inconveniences. The double
chloride, however, does draw some moisture and
holds it energetically, from which it results that at
a high temperature it will give rise to some alumina,
which encloses the globules of metal with a thin
coating and so hinders their easy reunion into a
button. Deville remarked that the presence of
fluorides facilitated the reunion of these globules,
which he attributed to their dissolving the coat of
A1203 on them. Since then, the employment of a
fluoride as a flux is considered necessary to over-
come the effect produced primarily by the APC16.-
2NaCl holding moisture so energetically. The first
fluoride employed by Deville was fluorspar, which
was soon replaced by cryolite. This opens up the
subject of the reduction of aluminium from cryolite,
and since Percy and Rose both preceded Deville in
using it, I will first give their investigations, follow-
ing with those which Deville published in 1859.
METALLURGY OF ALUMINIUM. 103
REDUCTION FROM CRYOLITE.
We will here give H. Rose's entire paper, as an
account of this eminent chemist's investigations
written out by himself with great detail, describ-
ing failures as well as successes, cannot but be of
value to all interested in the production of alu-
minium.*
u Since the discovery of aluminium by Wohler,
Deville has recently devised the means of procuring
the metal in large, solid masses, in which condition
it exhibits properties with which we were previ-
ously unacquainted in its more pulverulent form
as procured by Wohler's method. While, for in-
stance, in the latter state it burns vividly to white
earthy alumina on being ignited, the fused globules
may be heated to redness without perceptibly oxi-
dizing. These differences may be ascribed to the
greater amount of division on the one hand and of
density on the other. According to Deville, how-
ever, Wohler 's metal contains platinum, by which
he explains its difficulty of fusion, although it
affords white alumina by combustion. Upon the
publication of Deville's researches I also tried
to produce aluminium by the decomposition of
Al2Cl6.2XaCl by means of sodium. I did not,
however, obtain satisfactory" results. Moreover,
Prof. Rammelsberg, who followed exactly the
* Pogg. Annalen, Sept. 1855.
104 ALUMINIUM.
method of Deville, obtained but a very small pro-
duct, and found it very difficult to prevent the
cracking of the glass-tube in which the experiment
was conducted by the action of the vapor of sodium
on A12C16. It appeared to me that a great amount
of time, trouble, and expense, as well as long prac-
tice, was necessary to obtain even small quantities
of this remarkable metal.
" The employment of A12C16 and its compounds
with alkali chlorides is particularly inconvenient,
owing to their volatility, deliquescence, and to the
necessity of preventing all access of air during
their treatment with sodium. It very soon occurred
to me that it would be better to use the fluoride of
aluminium instead of the chloride ; or rather the
combination of the fluoride with alkaline fluorides,
such as we know them through the investigations
of Berzelius, who pointed out the strong affinity
of A12F6 for NaF and KF, and that the mineral
occurring in nature under the name of Cryolite
was a pure compound of A12F6 and ]S"aF.
" This compound is as well fitted for the prepara-
tion of aluminium by means of sodium as A12C16
or Al2Cl6.2NaCl. Moreover, as cryolite is not vola-
tile, is readily reduced to the most minute state of
division, is free from water and does not attract
moisture from the air, it affords peculiar advan-
tages over the above-mentioned compounds. In
fact, I succeeded with much less trouble in prepar-
ing aluminium by exposing cryolite together with
METALLURGY OF ALUMINIUM. 105
sodium to a strong red heat in an iron crucible,
than by using A12C16 and its compounds. But the
scarcity of cryolite prevented my pursuing the ex-
periments. In consequence of receiving, however,
from Prof. Krantz, of Bonn, a considerable quan-
tity of the purest cryolite at a very moderate price
(S2 per kilo), I was enabled to renew the investi-
gation.
" I was particularly stimulated by finding, most
unexpectedly, that cryolite was to be obtained here
in Berlin commercially at an inconceivably low
price. Prof. Krantz had already informed me that
cryolite occurred in commerce in bulk, but could
not learn where. Shortly after, M. Rudel, the
manager of the chemical works of H. Kunheim,
gave me a sample of a coarse white powder, large
quantities of which were brought from Greenland,
by way of Copenhagen, to Stettin, under the name
of mineral soda, and at the price of $3 per centner.
Samples had been sent to the soap boilers, and a
soda-lye had been extracted from it by means of
quicklime, especially adapted to the preparation of
many kinds of soap, probably from its containing
alumina. It is a fact, that powdered cryolite is
completely decomposed by quicklime and water.
The fluoride of lime formed contains no alumina,
which is all dissolved by the caustic soda solution;
and this, on its side, is free from fluorine, or only
contains a minute trace. I found this powder to
be of equal purity to that received from Prof.
106 ALUMINIUM.
Krantz. It dissolved without residue in HC1 (in
platinum vessels); the solution evaporated to dry-
ness with H2S04, and heated till excess of acid was
dissipated, gave a residue which dissolved com-
pletely in water, with the aid of a little HC1.
From this solution, ammonia precipitated a con-
siderable quantity of alumina. The sol ution filtered
from the precipitate furnished, on evaporation, a
residue of sulphate of soda, free from potash.
Moreover, the powder gave the well-known re-
actions of fluorine in a marked degree. This
powder was cryolite of great purity: therefore the
coarse powder I first obtained was not the form
in which it was originally produced. It is now
obtainable in Berlin in great masses ; for the prepa-
ration of aluminium it must, however, be reduced
to a very fine powder.
" In my experiments on the preparation of alu-
minium, which were performed in company with
M. Weber, and with his most zealous assistance, I
made use of small iron crucibles, If inches high
and If inches upper diameter, which I had cast
here. In these I placed the finely divided cryolite
between thin layers of sodium, pressed it down
tight, covered with a good layer of potassium
chloride (KC1), and closed the crucible with a well-
fitting porcelain cover. I found KC1 the most
advantageous flux to employ; it has the lowest
specific gravity of any which could be used, an
important point when the slight density of the
METALLURGY OF ALUMINIUM. 107
metal is taken into consideration. It also increases
the fusibility of the sodium fluoride. I usually
employed equal weights of cryolite and KC1, and
for every five parts of cryolite two parts of sodium.
The most fitting quantity for the crucible was
found to be ten grammes of powdered cryolite.
The whole was raised to a strong red heat by
means of a gas-air blowpipe. It was found most
advantageous to maintain the heat for about half
an hour, and not longer, the crucible being kept
closely covered the whole time ; the contents were
then found to be well fused. When quite cold the
melted mass is removed from the crucible by means
of a spatula, this is facilitated by striking the
outside with a hammer. The crucible may be
employed several times, at last it is broken by the
hammer blows. The melted mass is treated with
water, when, at times only, a very minute evolu-
tion of hydrogen gas is observed, which has the
same unpleasant odor as the gas evolved during
solution of iron in HC1. The carbon contained in
this gas is derived from a very slight trace of
naphtha adhering to the sodium after drying it.
On account of the difficult solubility of ISTaF, the
mass is very slowly acted on by water, although
the insolubility is somewhat diminished by the
presence of the KC1. After twelve hours the mass
is softened so far that it may be removed from the
liquid and broken down in a porcelain mortar.
Large globules of aluminium are then discovered,
108 ALUMINIUM.
weighing from 0.8 to 0.4 or even 0.5 gramme,
which may be separated out. The smaller globules
cannot well be separated from the undecomposed
cryolite and the alumina always produced by
washing, owing to their being specifically lighter
than the latter. The whole is treated with UNO3
in the cold. The APO3 is not dissolved thereby,
but the little globules then first assume their true
metallic lustre. They are dried and rubbed on fine
silk muslin ; the finely-powdered, undecomposed
cryolite and A1203 pass through, while the globules
remain on the gauze. The mass should be treated
in a platinum or silver vessel, a porcelain vessel
would be powerfully acted on by the NaF. The
solution, after standing till clear, may be evapo-
rated to dryness in a platinum capsule, in order to
obtain the !NaF, mixed, however, with much KC1.
The small globules may be united by fusion in a
small, well-covered, porcelain crucible, under a
layer of KC1. They cannot be united without a
flux. They cannot be united by mere fusion, like
globules of silver, for instance, for, though they do
not appear to oxidize on ignition in the air, yet
they become coated writh a scarcely perceptible film
of oxide, which prevents their running together
into a mass. This fusion with KC1 is always at-
tended with loss of aluminium. Buttons weighing
0.85 grm. lost, when so treated, 0.05 grm. The
KC1 when dissolved in water left a small quantity
of A1203 undissolved, but the solution contained
METALLURGY OF ALUMINIUM. 109
none. Another portion of the metal had un-
doubtedly decomposed the KC1 ; and a portion of
the A12C16 and KC1 must have been volatilized
during fusion (other metals, as copper and silver,
behave in a similar manner — Pogg. Ixviii. 287).
I therefore followed the instructions of Deville,
and melted the globules under a stratum of
Al2Cl6.2NaCl in a covered porcelain crucible. The
salt was melted first, and then the globules of
metal added to the melted mass. There is no loss,
or a very trifling one of a few milligrammes of
metal, by this proceeding. "When the aluminium
is fused under KC1 its surface is not perfectly
smooth, but exhibits minute concavities; with
Al2Cl6.2XaCl this is not the case. The readiest
method of preparing the Al2Cl6.2]STaCl for this pur-
pose is by placing a mixture of alumina and carbon
in a glass tube, as wide as possible, and inside this a
tube of less diameter, open at both ends, and contain-
ing XaCl. If the spot where the mixture is placed
be very strongly heated, and that where the NaCl
is situated, more moderately, while a current of
chlorine is passed through the tube, the vapor of
A12C1* is so eagerly absorbed by the !N"aCl that no
A12C16, or, at most, a trace, is deposited in any other
part of the tube. If the smaller tube be weighed
before the operation, the amount absorbed is readily
determined. It is not uniformly combined with
the EaCl, for that part which is nearest to the
10
110 ALUMINIUM.
mixture of charcoal and alumina will be found to
have absorbed the most.
" I have varied in many ways the process for the
preparation of aluminium, but in the end have
returned to the one just described. I often placed
the sodium in the bottom of the crucible, the pow-
dered cryolite about it, and the KC1 above all. On
proceeding in this manner, it was observed that
much sodium was volatilized, burning with a strong,
yellow flame, which never occurred when it was cut
into thin slices and placed in alternate layers with
the cryolite, in which case the process goes on quietly.
When the crucible begins to get red hot, the tempera-
ture suddenly rises, owing to the commencement of
the decomposition of the compound ; no lowering
of the temperature should be allowed, but the
heat should be steadily maintained, not longer,
however, than half an hour. By prolonging the
process a loss would be sustained, owing to the
action of the KC1 on the aluminium. Nor does
the size of the globules increase on extending the
time even to two hours; this effect can only be
produced by obtaining the highest possible tempera-
ture. If the process be stopped, however, after five
or ten minutes of very strong heat, the production
is very small, as the metal has not had sufficient
time to conglomerate into globules, but is in a pul-
verulent form and burns to APO3 during the cooling
of the crucible. No advantage is gained by mixing
the cryolite with a portion of chloride before plac-
METALLURGY OF ALUMINIUM. Ill
ing it between the layers of sodium, neither did I
increase the production by using Al2Cl6.2NaCl to
cover the mixture instead of KC1. I repeatedly
employed Nad, decrepitated, as a flux in the
absence of KC1, without remarking any important
difference in the amount of metal produced, although
a higher temperature is in this case required. The
operations may also be conducted in refractory
unglazed crucibles made of stoneware, and of the
same dimensions, although they do not resist so
well the action of the sodium fluoride at any high
heats, but fuse in one or more places. The iron
crucibles fuse, however, when exposed to a very
high temperature in a charcoal fire. The product
of metal was found to vary very much, even when
operating exactly in the manner recommended and
with the same quantities of materials. I never
succeeded in reducing the whole amount of metal
contained in the cryolite (which contains only 13
per cent. Al). By operating on 10 grammes of
cryolite, the quantity I always employed in the
small Fe crucible, the most successful result was
0.8 grm. But 0.6 or even 0.4 grm. may be con-
sidered favorable ; many times I obtained only 0.3
grm., or even less. These very different results
depend on various causes, more particularly, how-
ever, on the degree of heat obtained. The greater
the heat the greater the amount of large globules,
and the less amount of minutely divided metal to
oxidize during the cooling of the crucible. I sue-
112 ALUMINIUM.
ceeded once or twice in reducing nearly the whole
of the metal to one single button, weighing 0.5
grm., at a very high heat in a stoneware crucible.
I could not always obtain the same heat with the
blowpipe, as it depended in some degree on the
pressure in the gasometer in the gasworks, which
varies at different hours of the day. The follow-
ing experiment will show how great the loss of
metal may be owing to oxidation during the
slow cooling of the crucible and its contents : In a
large iron crucible were placed 35 grms. of cryolite
in alternate layers with 14 grms. of sodium and
the whole covered with a thick stratum of KC1.
The crucible, covered by a porcelain cover, was
placed in a larger earthen one, also covered, and
the whole exposed to a good heat in a draft furnace
for one hour and cooled as slowly as possible. The
product in this case was remarkably small, for
0.135 grm. of aluminium was all that could be
obtained in globules. The differences in the amounts
reduced depend also in some degree on the more or
less successful stratification of the sodium with the
powered cryolite, as much of the latter sometimes
escapes decomposition. The greater the amount of
sodium employed, the less likely is this to be the
case ; however, owing to the great difference in their
prices, I never emploj^ed more than 4 grms. of
sodium to 10 grms. of cryolite. In order to avoid
this loss by oxidation I tried another method of
preparation : Twenty grms. of cryolite were heated
METALLURGY OF ALUMINIUM. 113
intensely in a gun-barrel in a current of hydrogen,
and then the vapor of 8 grms. of sodium passed
over it. This was effected simply by placing the
sodium in a little iron tray in a part of the gun-
barrel without the fire, and pushing it forward
when the cryolite had attained a maximum tempe-
rature. The operation went on very well, the
whole being allowed to cool in a current of hydro-
gen. After the treatment with water, in which
the sodium fluoride dissolved very slowly, I ob-
tained a black powder, consisting for the most part
of iron. Its solution in HC1 gave small evidence
of Al. The small amounts I obtained, however,
should not deter others from making these experi-
ments. These are the results of first experiments
on which I have not been able to expend much
time. Now that cryolite can be procured at so
moderate a price, and sodium, by Deville's improve-
ments, will in future become so much cheaper, it is
in the power of every chemist to engage in the
preparation of aluminium, and I have no doubt
that in a short time methods will be found afford-
ing a much more profitable result.
" For the rest, I am of opinion that cryolite is the
best adapted of all the compounds of aluminium
for the preparation of this metal. It deserves the
preference over Al2Cl6.2XaCl or A12C16, and it might
still be employed with great advantage even if its
price were to rise considerably. The attempts at
preparing aluminium direct from A1203 have as
10*
114 ALUMINIUM.
yet been unattended with success. Potassium and
sodium appear only to reduce metallic oxides when
the potash and soda produced are capable of forming
compounds with a portion of the oxide remaining
as such. Pure potash and soda, with whose pro-
perties we are very slightly acquainted, do not
appear to be formed in this case. Since, however,
alumina combines so readily with the alkalies to
form aluminates, one would be inclined to believe
that the reduction of APO3 by the alkali metals
should succeed. But even were it possible to ob-
tain the metal directly from A1203, it is very prob-
able that cryolite would long be preferred should
it remain at a moderate price, for it is furnished
by nature in a rare state of purity, and the alumi-
nium is combined in it with sodium and fluorine
only, which exercise no prejudicial influence on the
properties of the metal, whereas A1203 is rarely
found in nature in a pure state and in a dense,
compact condition, and to prepare A1203 on a large
scale, freeing it from those substances which would
act injuriously on the properties of the metal,
would be attended with great difficulty.
" The buttons of aluminium which I have pre-
pared are so malleable that they may be beaten
and rolled out into the finest foil without cracking
O
on the edges. They have a strong metallic lustre.
Some small pieces, not globular, however, were
found in the bottom of the crucible, and occasion-
ally adhering to it, which cracked on being ham-
METALLURGY OF ALUMINIUM. 115
mered, and were different in color and lustre from
the others. They were evidently not so pure as
the greater number of the globules, and contained
iron. On sawing through a large button weighing
3.8 grms., it could readily be observed that the
metal for about half a line from the exterior was
brittle, while in the interior it was soft and malle-
able. Sometimes the interior of a globule contained
cavities. AVith Deville, I have occasionally observed
aluminium crystallized. A large button became
striated and crystalline on cooling. Deville believes
he has observed regular octahedra, but does not
state this positively. According to my brother's
examination, the crystals do not belong to any of
the regular forms. As I chanced on one occasion
to attempt the fusion of a large, flattened-out but-
ton of rather impure aluminium, without a flux, I
observed, before the heat was sufficient to fuse the
mass, small globules sweating out from the surface.
The impure metal being less fusible than pure
metal, the latter expands in fusing and comes to
the surface."
Such were the results given to the world by H.
Rose. After their publication, many minds were
turned towards this field, and it was discovered
that some six months previously Dr. Percy had
accomplished the same results, and had even shown
them to the Royal Institution, but with the singu-
lar fact of exciting very little attention. These
facts are stated at length in the following paper,
116 ALUMINIUM.
written by Allan Dick, Esq., which appeared in
November, 1855, two months after the publication
of H. Rose's paper : — *
"In the last number of this magazine was the
translation of a paper by H. Rose, of Berlin, de-
scribing a method of preparing aluminium from
cryolite. Previously, at the suggestion of Dr.
Percy, I had made some experiments on the same
subject in the metallurgical laboratory of the
School of Mines, and as the results obtained agree
very closely with those of Mr. Rose, it may be
interesting to give a short account of them now,
though no detailed description was published at
the time, a small piece of metal prepared from
cryolite having simply been shown at the weekly
meeting of the Royal Institution, March 30, 1855,
accompanied by a few words of explanation by
Faraday.
" Shortly after the publication of Mr. Deville's
process for preparing aluminium from A12C16, I
tried, along with Mr. Smith, to make a specimen
of the metal, but we found it much more difficult
to do than Deville's paper had led us to antici-
pate, and had to remain contented with a much
smaller piece of metal than we had hoped to obtain.
It is, however, undoubtedly only a matter of time,
skill, and expense to join successful practice with
the details given by Deville. Whilst making
* Phil. Mag., Nov. 1855.
METALLURGY OF ALUMINIUM. 117
these experiments Dr. Percy had often requested
us to try whether cryolite could be used instead of
the chlorides, but some time elapsed before we
could obtain a specimen of the mineral. The first
experiments were made in glass tubes sealed at one
end, into which alternate layers of finely powdered
cryolite and sodium cut into small pieces were
introduced, and covered in some instances with a
layer of cryolite, in others by KaCl. The tube
was then heated over a gas blowpipe for a few
minutes till decomposition had taken place and
the product was melted. When cold, on breaking
the tube, it was found that the mass was full of
small globules of aluminium, but owing to the
specific gravity of the metal and flux being nearly
alike, the globules had not collected into a button
at the bottom. To effect this, long continued
heat would be required, which cannot be given in
glass tubes owing to the powerful action of the
melted fluoride on them. To obviate this difficulty
a platinum crucible was lined with magnesia by
ramming it in hard, and subsequently cutting out
all but a lining. In this, alternate layers of cryolite
and sodium were placed, with a thickish layer of
cryolite on top. The crucible was covered with a
tight-fitting lid, and heated to redness for about
half an hour over a gas blowpipe. When cold it
was placed in water, and after soaking for some
time the contents were dug out, gently crushed in
a mortar, and washed by decantation. Two or
118 ALUMINIUM.
three globules of aluminium, tolerably large con-
sidering the size of the experiment, were obtained,
along with a large number of very small ones.
The larger ones were melted together under KOI.
Some experiments made in iron crucibles were not
attended with the same success as those of Rose,
no globules of any considerable size remained in
the melted fluorides ; the metal seemed to alloy on
the sides of the crucible, which acquired a color
like zinc. It is possible that this difference may
have arisen from using a higher temperature than
Rose, as we made these experiments in a furnace,
not over the blowpipe. Porcelain and clay cruci-
bles were also tried, but laid aside after a tew ex-
periments, owing to the action of the fluorides
upon them, which in most cases was sufficient to
perforate them completely."
The above papers, Rose's and Dick's, contain all
the published researches with cryolite until Deville's
attention was turned towards it. He then took
up the subject with his accustomed thoroughness.
The following pages are taken from his ' De 1' Alu-
minium,' the subject not being given in its entirety,
but only the most important points. He published
the first account of these researches in ' Ann. de
Chem. et de Phys.' [3], xlvi. 451 :-
" I have repeated and confirmed all the experi-
ments of Dr. Percy and H. Rose, using the specimens
of cryolite which I obtained from London through
the kindness of MM. Rose and Hofmann. I have,
METALLURGY OF ALUMINIUM. 119
furthermore, reduced cryolite mixed with !N"aCl by
the battery, and I believe that this will be an ex-
cellent method of covering with aluminium all the
other metals, copper in particular. Anyhow, its
fusibility is considerably increased by mixing it
with A12C16.2KC1. Cryolite is a double fluoride of
aluminium and sodium, containing 13 per cent.
Al, 32.5 per cent. Xa, and 54.5 per cent. F. Its
formula is Al2F6.6NaF. I have verified these facts
myself by many analyses."
Deville then gives a description of methods of
making cryolite artificially, which is unnecessary
to repeat here, for natural cryolite is so cheap that
these methods are of no practical importance. He
continues : —
"In reducing the cryolite I placed the finely-pul-
verized mixture of cryolite and XaCl in alternate
layers with sodium in a porcelain crucible. The
uppermost layer is of pure cryolite, covered with
XaCl. The mixture is heated just to complete fu-
sion, and, after stirring with a pipe-stem, is let cool.
On breaking the crucible, the aluminium is often
found united in large globules easy to separate from
the mass. The metal always contains silicon, which
increases the depth of its natural blue tint and
hinders the whitening of the metal by nitric acid,
because of the insolubility of the silicon in that
acid. M. Rose's metal is very ferruginous. I have
verified all M. Rose's observations, and I agree
with him concerning the return of metal, which I
120 ALUMINIUM.
have always found very small. There are always
produced in these operations brilliant flames, which
are observed in the scoria floating on the alumin-
ium, and which are due to gas burning and
exhaling a very marked odor of phosphorus. In
fact, P206 exists in cryolite, as one may find by
treating a solution of the mineral in sulphuric acid
with molybdate of ammonia, according to H.
Rose's reaction.
"The facility with which aluminium unites in
fluorides is due without doubt to the property which
these possess of dissolving the alumina on the surface
of the globules at the moment of their formation,
and which the sodium is unable to reduce. I had
experienced great difficulty by obtaining small
quantities of metal poorly united, when I reduced
the Al2Cl6.2]N"aCl by sodium ; M. Ramrnelsberg, who
often made the same attempts, tells me he has had a
like experience. But, I am assured by a scrupulous
analysis that the quantity of metal reduced by the
sodium is exactly that which theory indicates,
although after many operations there is found only
a gray powder, resolving itself under the micro-
scope into a multitude of small globules. The fact
is simply that Al2Cl6.2NaCl is a very poor flux
for aluminium. MM. Morin, Debray, and myself
have undertaken to correct this bad eflect by the
introduction of a solvent for the A1203 into the
saline slag which accompanies the aluminium at
the moment of its formation. At first, we found
METALLURGY OF ALUMINIUM. 121
it an improvement to condense the vapors of A12C16,
previously purified by iron,-directly in NaCl, placed
for this purpose in a crucible and kept at a red
heat. We produced in this way , from highly colored
material, a double chloride very white and free from
moisture, and furnishing on reduction a metal of
fine appearance. We then introduced fluorspar
(CaF2) into the composition of the mixture to be
reduced, and we obtained good results with the
following proportions : —
Al*Cl6.2NaCl .... 400 grammes.
NaCl 200
CaF2 200 "
Na . . . . . . 75 to 80 "
The double chloride ought to be melted and heated
almost to low red heat at the moment it is em-
ployed, the NaCl calcined and at a red heat or
melted, and the CaF2 pulverized and well dried.
The double chloride, NaCl and CaF2 are mixed and
alternated in layers in the crucible with sodium.
The top layer is of the mixture, and the cover is
XaCl. Heat gently, at first, until the reaction ends,
and then to a heat about sufficient to melt silver.
The crucible, or at least that part of it which con-
tains the mixture, ought to be of a uniform red tint,
and the material perfectly liquid. It is stirred a
long time and cast on a well-dried, chalked plate.
There flows out first a very limpid liquid, colorless
and very fluid, then a gray material, a little more
pasty, which contains aluminium in little grains,
11
122 ALUMINIUM.
and is set aside, and finally a button with small,
metallic masses which of themselves ought to weigh
20 grms. if the operation has succeeded well. On
pulverizing and sieving the gray slag, 5 or 6 grms. of
small globules are obtained, wrhich may be pressed
together by an earthen rod in an ordinary crucible
heated to redness. The globules are thus reunited,
and when a sufficient quantity is collected the metal
is cast into ingots. In a well-conducted operation,
75 grms. of Na ought to give a button of 20 grms.
and 5 grms. in grains, making a return of one Al
from three of Na. Theory indicates one to two
and a half, or 30 grms. of Al from 75 of Na. But
all the efforts which have been made to recover from
the insoluble slag the 4 or 5 grms. of metal not
united but easily visible with a glass, have been so
far unsuccessful: There is, without doubt, a knack,
a particular manipulation on which depends the
success of an operation which would render the
theoretical amount of metal, but we lack it yet.
These operations take place, in general, with more
facility on a large scale, so that we may consider
fluorspar as being suitable for serving in the manu-
facture of aluminium in crucibles. We employed
very pure fluorspar, and our metal was quite exempt
from silicon. It is true that we took a precaution
which is necessary to adopt in operations of this
kind; we plastered our crucibles inside with a layer
of aluminous paste, the composition of which has
been given in ' Ann. de Chem. et de Phys.,' xlvi.
METALLURGY OF ALUMINIUM. 123
195. This paste is made of calcined alumina and
an aluminate of lime, the latter obtained by heating
together equal parts of chalk and alumina to a high
heat. By taking about four parts calcined alumina
and one of aluminate of lime well pulverized and
sieved, moistening with a little water, there is
obtained a paste with which the inside of 'an
earthen crucible is quickly and easily coated. The
paste is spread evenly with a porcelain spatula, and
compressed strongly until its surface has become
well polished. It is allowed to dry, and then heated
to bright redness to season the coating, which does
not melt, and protects the crucible completely
against the action of the aluminium and fluorspar.
A crucible will serve several times in succession
provided that the new material is put in as soon as
the previous charge is cast. The advantages of
doing this are that the mixture and the sodium are
put into a crucible already heated up, and so lose
less by volatilization because the heating is done
more quickly, and the crucible is drier than if a new
one had been used or than if it had been let cool.
A new crucible should be heated to at least 300°
or 400° before being used. The saline slag contains
a large quantity of calcium chloride, which can be
washed away by water, and an insoluble material
from which aluminium fluoride can be volatilized.
" Yet the operation just described, which was a
great improvement on previous ones, requires many
precautions and a certain skill of manipulation to
124 ALUMINIUM.
succeed every time. But, nothing is more easy or
simple than to substitute cryolite for the fluorspar.
Then the operation is much easier. The amount of
metal produced is not much larger, although the
-IT O 7 O
button often weighs 22 grammes, yet if cryolite can
only be obtained in abundance in a continuous sup-
ply, the process which I will describe will become
most economical. The charge is made up as before,
except introducing cryolite for CaF2. In one of
our operations we obtained, with 76 grrns. of sodi-
um, a button weighing 22 grms. and 4 grms. in
globules, giving a yield of one Al to two and ei^ht-
tenths parts sodium, which is very near to that
indicated by theory. The metal obtained was of
excellent quality. However, it contained a little
iron coming from the A12C16, W7hich had not been
purified perfectly. Bat iron does not inj ure the prop-
erties of the metal as copper does ; and, save a little
bluish coloration, it does not alter its appearance or
its resistance to physical and chemical agencies.
"Process with cryolite alone: The process adopted
in the works at Amfreville, near Rouen, directed
by Tissier Bros., is the same as that described by
Percy and Rose. The details which I give are
taken from MM. Tissier's own account of their pro-
cess." (Deville then gives the details of the process
outlined by Rose (see p. 103), of reducing in iron
crucibles ; which it is not necessary to repeat.)
" I obtained a good specimen of commercial alu-
minium thusextracted from cryolite ; and M. Demon-
METALLURGY OF ALUMINIUM. 125
deur has been so kind as to make an analysis of it,
with the following results: Si 4.4; FeO.8; A! 94.8.
" M. Rose has recommended iron vessels for this
operation, because of the rapidity with which alka-
line fluorides attack earthen crucibles and so intro-
duce considerable silicon into the metal. Unfortu-
nately, these iron crucibles introduce iron into the
metal. This is an evil inherent to this method, at
least in the present state of the industry. The
inconveniences of this method result in part from
the high temperature required to complete the ope-
ration, and from the crucible being in direct contact
with the fire, by which its sides are heated hotter
than the metal in the crucible. The metal itself,
placed in the lower part of the fire, is hotter than
the slag. This, according to my observations, is an
essentially injurious condition. The slag ought to
be cool, the metal still less heated, and the sides of
the vessel Avhere the fusion occurs ought to be as
cold as possible. The yield from cryolite, accord-
ing to Rose's and my own observations, is also very
small. M. Rose obtained from 10 of cryolite and
4 of Xa about 0.5 of Al. This is due to the
affinity of aluminium for fluorine, which must be
very strong not only with relation to its affinity
for sodium but even for calcium, and this affinity
appears to increase with the temperature, as was
found in my laboratory. Cryolite is convenient to
employ as a flux to add to the mixture which is
fused, especially when operating on a small scale;
11*
126 ALUMINIUM.
but it is fortunate that it is not indispensable, for
no one would wish to establish an industry on the
employment of a material wThich is of uncertain
supply."
We here close what Deville has written on the
use of cryolite. The process was that used by
Tissier Bros, at Rouen, but was finally abandoned
there and the works closed. We find a little
improvement on Deville's process suggested by
Wohler,* in which he shows how to perform the
reduction in an earthen crucible. The finely pul-
verized cryolite is mixed with an equal weight of
a flux containing 7 NaCI to 9 KC1. This mixture'
is then placed in alternate layers with sodium in
the crucible, 50 parts of the mixture to 10 of
sodium, and heated gradually just to its fusing
point. The metal thus obtained is free from
silicon, but only one-third of the aluminium in the
cryolite is obtained. In spite of the small yield,
this method was used for some time by Tissier
Bros. Cryolite has also been treated at ]^"anterre,
by a different process, but the aluminium produced
contained phosphorus. So, while the exclusive
use of cryolite in the preparation of aluminium is
now renounced, it has retained the office of a flux.
Watts gives the following paragraph in connec-
tion with the reduction of cryolite : "A peculiar
apparatus for effecting the reduction of aluminium,
* Ann. der Cbem. und Pharm. 99, 255.
METALLURGY OF ALUMINIUM. 127
either from Al2Cl6.2NaCl or from cryolite, the
object of which is to prevent loss of sodium by
ignition, has been invented and patented by W. F.
Gerhard.* It consists of a reverberatory furnace
having two hearths, or of two crucibles, or of two
reverberatory furnaces, placed one above the other
and communicating by an iron pipe. In the lower
is placed a mixture of sodium with the aluminium
compound, and in the upper a stratum of !NaCl, or
of a mixture of NaCl and cryolite, or of the slag
obtained in a previous operation. This charge,
when melted, is made to run into the lower furnace
•in quantity sufficient to completely cover the mix-
ture contained therein, and so to protect it from
the air. The mixture thus covered is reduced as
by the usual operation."
Watts thus summarizes the use of cryolite :
" The chief inducement for using it as a source of
aluminium is that it is a natural product obtained
with tolerable facility, and enables the manufact-
urer to dispense with the troublesome and costly
preparation of Al2Cl6.2^"aCl. But the metal thus
obtained is less pure than that obtained by other
processes. If earthenware crucibles are used, the
metal is contaminated with silicon, because the
sodium fluoride produced acts strongly on the
siliceous matter of the crucible, while if an iron
crucible be used, the metal takes up some iron.
* Eng. Pat. 1858, No. 2247.
128 ALUMINIUM.
The best use of cryolite is as a flux in the prepara-
tion of aluminium from Al2Cl6.2JN"aCl, in which
case the slag is not sodium fluoride but aluminium
fluoride, which acts but slightly on the containing
vessel."
GENERAL REMARKS.
I have now given the metallurgy of aluminium
through what may be called its experimental stage
up to its practical industrial manufacture. Up to
this period, which I will place at about 1859, the
object has been to produce the metal at any cost,
only produce it. " To learn how" engrossed the
attention of the investigators, who troubled them-
selves very little about the ultimate cost. They
must learn first how to do the thins: and afterwards
O
devote their energies to cheapening the process
discovered. But, in 1859, the works at Amfreville,
near Rouen, under the direction of the Tissiers, is
producing aluminium from cryolite; Morin & Co.,
at Nanterre, are making it, though not in such
large quantities as Tissier, but they soon after
move to Salindres, and set up so large a plant that
a year or so afterwards the Tissiers were driven
from the business. Such is then the state of the
industry. We iind that in the next fifteen or
twenty years very little advance is chronicled. At
Salindres, the processes given by Deville were used
somewhat improved and perfected, but yet the
METALLURGY OF ALUMINIUM. 129
same processes. It is only within the last ten
years that any improvements of a radical nature,
such as Webster's, Frishmuth's, and Cowles, have
been brought into the industry.
So, from now on we will treat the subject in the
order usually adopted in presenting it ; i. e., first
give a short sketch of the metallurgy of sodium
up to the present time, then a review of the manu-
facture of alumina and its conversion into
Al2Cl6.2XaCl, ending with a full description of the
process as now carried on at Salindres, and a fewr
attempts which have been made to improve it.
Afterwards, leaving the old Deville process and its
improvements, I will give as full an account as I
have been able to gather of the various methods
proposed to produce aluminium without the use of
sodium.
PART VI.
THE MANUFACTURE OF SODIUM.
As already observed, we will not go extensively
into the metallurgy of this metal. Some years
ago, in order to treat fully of the metallurgy of
aluminium, it would have been as necessary to ac-
company it with all the details of the manufacture of
sodium as to give the details of the reduction of the
aluminium, because the manufacture of the former
was carried on solely in connection with that of the
latter. But now sodium has come out of the list of
chemical curiosities and has become an article of
commerce, used for many other purposes than the
reduction of aluminium, though that is still its
chief use. So we regard the manufacture of sodium
as a separate metallurgical subject, still intimately
connected with that of aluminium, but yet so far
distinct from it as to deserve a metallurgical trea-
tise of its own. Moreover, the metallurgy of sodium
is very much as Deville left it, it has been very
little improved since then, and so almost all the
details of its manufacture are to be found in Eng-
lish in any good book on chemistry. To such
works I refer the reader for fuller accounts than are
THE MANUFACTURE OF SODIUM. 131
given here. The following summary is taken prin-
cipally from Mierzinski.
Sodium was first isolated by Davy by the use of
electricity in the year 1808.* Later, Gay Lussac
and Thenard made it by decomposing at a very
high temperature a mixture of Na2C03 and iron
filings/)- On April 30, 1808, Curaudau announced
that he had succeeded in producing potassium or
sodium without using iron, simply by decomposing
K2C03 or ^a2COs by means of animal charcoal.
Briinner continuing this investigation used instead
of animal charcoal the so-called black flux, the pro-
duct obtained by calcining crude tartar from wine
barrels. He was the first to use the w rough t-iron
mercury bottles. The mixture was heated white
hot in a furnace, the sodium volatilized and was
condensed in an iron tube screwed into the top of
the flask, which projected from the furnace and
was cooled with water. In Briinners experiments
he only obtained three per cent, of the weight of
the mixture as metallic sodium, the rest of the
metal being lost as vapor.
Donny and Mareskagave the condenser the form
which with a few modifications it retains to-day.
It was of iron, 4 millimetres thick, arid was made
in the shape of a book, having a length of about
100 centimetres, breadth 50, and depth 6 (see Fig.
2). This form is now so well known that a further
* Phil. Trans., 1808.
| Recherches Physico-chemiques, 1810.
132 ALUMINIUM.
description is unnecessary. With this condenser
the greatest difficulty of the process was removed,
and the operation could be carried on in safety.
Fig. 2.
This apparatus was devised and used by Donny and
Mareska in 1854, with the supervision of Deville,
and the whole process as used by them is the same
that the Tissier Bros, took with them and operated
at their works at Rouen, and their description ac-
cords with that given by Deville, which is as fol-
lows : —
The Na2C03 is first well dried at a high tempera-
ture, then mixed with well dried pulverized char-
coal and chalk, ground to the finest powder, the
success of the operation depending on the fineness of
this mixture. The proportions of these to use is
various. One simple mixture is of
Na2CO* 30
Coal . . . ' . . . .13
Chalk . . . . ".." . 5
Coke 5
THE MANUFACTURE OF SODIUM.
Devil le recommends taking —
Coal .
Chalk .
1000
450
175
The addition of chalk has the object of making the
mixture less fusible and more porous, but has the
disadvantage that the residue remaining in the re-
tort after the operation is very impure, and it is
impossible to add any of it to the succeeding charge ;
and also, some of it being reduced to caustic lime
forms caustic alkali with some Na'CO8, which is
then lost. When the mixture is well made it is
subjected to a preliminary calcination. This is
done in cast-iron cylinders, two of which are placed
side by side in a furnace and heated to redness (see
Fig. 3). This is continued till all the moisture,
Fig. 3.
carbonic acid, and any carburetted hydrogen rforn
the coal cease coming oft'. The mass contracts, be-
comes white and somewhat dense, so that a larger
12
134
ALUMINIUM.
amount of the mixture can now be treated in the
retorts where the sodium is evolved. As soon as
the outcorning gases burn with a yellow flame,
showing sodium coming off, the calcination is
stopped. The mixture is then immediately drawn
out on to the stone floor of the shop, wThere it cools
quickly and is then ready for the next operation.
This calcination yields a mixture which without
any previous reactions is just ready to evolve sodium
when brought to the necessary temperature. This
material is made into a sort of cylinder or cartridge
and put into the decomposition retorts (see Fig. 4).
Fig. 4.
The charging should be done quickly. The final
retorts are 120 centimetres long, 12 to 14 centime-
THE MANUFACTURE OF SODIUM. 135
tres diameter, with walls 10 to 30 millimetres thick.
These are of wrought iron, since cast iron would
not stand the heat. At each end this retort is
closed with wrought-iron stoppers and made tight
with fire-clay. Through one stopper leads the pipe
to the condenser, the other stopper is the one re-
moved when the retort is to be recharged. These
retorts are placed horizontally in rows in a furnace.
Usually four are placed in a furnace, preferably
heated by gas, such as the Siemens regenerative
furnace or Bicheroux's, these being much more eco-
nomical. In spite of all these precautions the re-
torts will be strongly attacked, and in order to pro-
tect them from the destructive action of a white
heat for seven or eight hours they are coated with
some kind of fire-proof material. The best for
this purpose is graphite, which is made into cylin-
ders inclosing the retorts, and which can remain in
place till the furnace is worn out. These graphite
cylinders not only protect the iron retorts, but pre-
vent the diffusion of the gaseous products of the
reaction into the hearth, and so support the retorts
that their removal from the furnace is easily ac-
complished. Instead of these graphite cylinders
the retorts may be painted with a mixture that
melts at white heat and so enamels the outside. A
mixture of alumina, sand, yellow earth, borax, and
water-glass will serve very well in many cases. We
would remark that the waste gases from this fur-
nace can be used for the calcining of the mixture, or
136 ALUMINIUM.
even for the reduction of the aluminium by sodium,
where the manufacture of the former is connected
with the making of the sodium. Donny and
Mareska's condenser is the best to use.
As for the reduction of the sodium, the retort is
first heated to redness, during which the stopper
at the condenser end of the retort is left off. The
charge is then rapidly put in, and the stopper at
once put in place. The reaction begins almost at
once and the operation is soon under full headway,
the gases evolved burning from the upper slit of
the condenser tube with a flame a foot long. The
gases increase in volume as the operation continues,
the flame becoming yellower from sodium and so
intensely bright as to be insupportable to look at.
Now has come the moment when the workman
must quickly adapt the condenser to the condenser
tube projecting from the retort, the joint being
greased with tallow or paraffine. The sodium
collects in this in a melted state and trickles out.
The length of the operation varies, depending on
the intensity of the heat and the quantity of the
mixture ; a charge may sometimes be driven over
in two hours, and sometimes it takes eight. We
can say, in general, that if the reaction goes on
quickly a somewhat larger amount of sodium is
obtained. The higher the heat used, however, the
quicker the retorts are destroyed. The operation
requires continual attention. From time to time,
a workman with a prod opens up the neck of the
THE MANUFACTURE OF SODIUM. 137
condenser. But, if care is not taken the metal
overflows : if this happens, the metal overflowing
is thrown into some petroleum, while another man
replaces the condenser with an empty one. The
operation is ended when the evolution of gas ceases
and the flame becomes short and feeble, while the
connecting tube between the retort and condenser
O
keeps clean and does not stop up. As soon as this
occurs, the stopper at the charging end is removed,
the charge raked out into an iron car, and a new
charge being put in, the operation continues.
After several operations the retorts must be well
cleaned and scraped out. The sodium thus ob-
tained is in melted bits or drops, mixed with carbon
and Na2C03. It must therefore be cleaned, which
is done by melting it in a wrought-iron kettle
under paraffin with a gentle heat, and then casting
it into the desired shapes. The sodium is kept
under a layer of oil or any hydrocarbon of high
boiling point containing no oxygen.
Deville says that the temperature necessary for
the reduction of sodium from Na2C03 and carbon
is not so high as is generally supposed. He says
that it was M. Bivot's opinion that the retorts were
not heated higher than the retorts at Veille-Mon-
tague used for reducing zinc. Tissier gives the
reaction as
:NTa2C03 -f 2C = SCO 4- 2^a.
The sodium is condensed, while the carbonic
12*
138 ALUMINIUM.
oxide, carrying over some sodium, burns at the
end of the apparatus. This would all be very
simple if the reaction of carbonic oxide on sodium
near the condensing point did not complicate
matters, producing a black, infusible deposit of
Na?0 and C, which on being melted always gives
rise to a loss of sodium.
The foregoing is the process as perfected by
Donny and Mareska, Deville, and Tissier. Only a
few improvements have been made, the most im-
portant are the following: —
R. Wagner* uses paraffin in preference to paraf-
fin oil in which to keep the sodium after making
it. Only pure paraffin which has been melted a
long time on a water bath and all its water driven
off can be used. The sodium to be preserved is
dipped in the paraffin melted on a water bath and
kept at no higher heat than 55°, and the metal is
thereby covered with a thick coat of paraffin
which protects it from oxidation, and may then be
put up in wooden or paper boxes. When the
metal is to be used, it is easily freed from paraffin
by simply warming it, since sodium melts at 95°
to 96° C. and the paraffin at 50° to 60°.
The reduction of K2CG3 by carbon requires much
less heat than that of Na2C03, and, therefore, many
attempts have been made to reduce potassium and
sodium together, tinder circumstances where so-
* Dingier, 1883, p. 252.
THE MANUFACTURE OF SODIUM. 139
dium alone would not be reduced. Dumas* added
some K2C03 to the regular sodium mixture ; and
separated the sodium and potassium from each
other by a slow, tedious oxidation. R. Wagnerf
made a similar attempt. He says that not only
does the reduction of both metals from a mixture
of K2C03, Xa2C03, and carbon work easier than
Xa2C03 and carbon, but even caustic soda (XaOH)
may be used with K2COS and carbon. Also, the
melting point of potassium and sodium alloyed is
much lower than that of either one alone, in con-
sequence of which their boiling point and the tem-
perature required for reduction are lower.
"W. Weldon calculated the cost of sodium as
seven to eight marks per kilo. The greater part
of this is for retorts in which the operation takes
place, and which are so quickly destroyed that the
replacing of them forms half the cost of the metal.
Compare with p. 172.
The latest announcement of advance in making
sodium is from New York City, and is thus de-
scribed in a New York paper: — %
" When sodium was reduced in price to $1.50 per
pound, it was thought to have touched a bottom
figure, and all hope of making it any cheaper seemed
fruitless. This cheapening was not brought about
* Handbuch der Angewandten Chemie, 1830, ii. 345.
t Dingier, 143, 343.
t New York World, May 16, 1886.
140 ALUMINIUM.
by any improved or new process of reduction, but
was owing simply to the fact that the aluminium
industry required sodium, and by making it in
large quantities its cost does not exceed the above-
mentioned price. The retail price is now $4.00
per pound. The process now used was invented
by Briinner, in 1808, and up to the present time
nothing new or original has been patented except
three or four modifications of his process which
have been adopted to meet the requirements of
using it on a large scale. Mr. H. Y. Castner, whose
laboratory is at 218 West Twentieth Street, New
York, has the first patent ever granted on this sub-
ject in the United States, and the only one taken
out in the world since 1808. Owing to negotia-
tions being carried on, Mr. Castner having filed
applications for patents in various foreign countries,
but not having the patents granted there yet, we
are not at liberty to state his process fully. The
metal is reduced and distilled in large iron cruci-
bles, which are raised automatically through aper-
tures in the bottom of the furnace, where they remain
until the reduction is completed and the sodium
distilled. Then the crucible is lowered, a new one
containing a fresh charge is substituted and raised
into the furnace, while the one just used is cleaned
and made ready for use again. The temperature
required is very moderate, the sodium distilling as
easy as zinc does when being reduced. Mr. Cast-
ner expects to produce it at 25 cents per pound,
THE MANUFACTURE OF SODIUM. 141
thus solving the problem of cheap aluminium, and
with it magnesium, silicon, and boron, all of which
depend on sodium for their manufacture. Thus
the production of cheap sodium means much more
than cheap aluminium. Mr. Castner is well known
in New York as a chemist of good standing, and
has associated with him Mr. J. H. Booth and Mr.
Henry Booth, both well known as gentlemen of
means and integrity."
Mr. Benjamin, in a letter to the ' Engineering
and Mining Journal,' gives the following details
in addition to those above:* The pots used are
cast iron, 8 inches in diameter and 14 inches deep.
They are kept at bright red, or about 1000°, at
which temperature the decomposition takes place.
Whereas, by previous processes only one-third of
the sodium in the charge is obtained, Mr. Castner
gets nearly all, for the pots are nearly entirely
empty when withdrawn from the furnace. Thus
the great items of saving are, two or three times
as much metal extracted from a given amount of
salt, and cheap cast-iron crucibles used instead of
expensive wrought-iron retorts.
• The following are the claims which Mr. Castner
makes in his patent : — f
Claim 1. In a process for manufacturing potas-
sium or sodium, performing the reduction by diflus-
* Eng. and Min. Journ., May 29, 1886.
t U. S. Pat. No. 342,897, June 1, 1886. Hamilton Y. Cast-
ner, New York.
142 ALUMINIUM.
ing carbon in a body of alkali in a state of fusion
at moderate temperatures.
2. Performing the reduction by means of the
carbide of a metal or its equivalent.
3. Mechanically combining a metal and carbon
to increase the weight of the reducing material,
and then mixing this product with the alkali and
fusing the latter, whereby the reducing material is
held in suspension throughout the mass of fused
alkali.
4. Performing the deoxidation by the carbide of
a metal or its equivalent.
We learn later that Mr. Castner cokes a mixture
of fine iron and gas-tar, grinds the coke, and uses
this as the reducing material ; caustic soda is used
on account of its low fusing point.
REDUCTION OF SODIUM BY ELECTRICITY.
Mierzinski : In order to lower the cost of sodium
efforts have been made to obtain it by means of
electricity. Davy has shown that its production
in this way is possible, for he first obtained the
metal by electrolizing a solution of Na2C03. P.
Jablochoff uses the following arrangement to de-
compose Nad or KC1 : —
The arrangement is easily understood. The salt
to be decomposed is fed in by the funnel into the
kettle heated by a fire beneath. The positive pole
evolves chlorine gas, and the negative pole evolves
THE MANUFACTURE OF SODIUM.
143
vapor of the metal, for, as the salt is melted, the
heat is sufficient to vaporize the metal liberated.
The gas escapes through one tube and the metallic
Fig. 5.
anrrm «•?**•
vapor by the other. The vapor is led into a con-
denser and solidified.
PAUT VII.
MANUFACTURE OF ALUMINA.
I DO not propose to give here all the methods
.which have been employed to get good clean alu-
mina (APO3), but only those which may be recom-
mended as being practical and economical on a
large scale, not repeating the methods used at Sal-
indres or by Mr. Webster, which will be found in
connection with the full description of the processes
used at Salindres and Birmingham. Most of the
O
following is from Mierzinski, and may be taken as
representing the present state of the industry.
By igniting an alum salt, as ammonia alum, there
remains either a white powder or shining, sticky
pieces which are very hard and dissolve with dif-
ficulty in weak acid or in concentrated solutions of
alkali. Large quantities of this alumina may be
obtained by calcining the salt in an oven similar in
its principal details to a soda furnace.
Mierzinski then gives Mr. Webster's process of
mixing the powdered alum with coal-tar, etc.,
which is given in full in Part IX.
Tilghman decomposes commercial sulphate of
alumina, AP(S04)3.18H20, by filling a red-hot fire-
MANUFACTURE OF ALUMINA. 145
clay cylinder with it. This cylinder is lined inside
with a magnesia fettling, is kept at a red heat, the
sulphate put in in large lumps, and steam is passed
through the retort, carrying with it vapor of XaCl.
This last arrangement is effected by passing steam
into a cast-iron retort in which ^N"aCl is kept melted,
and as the steam leaves this retort it carries vapor
of the salt with it. It is preferable, however, to
make a paste of the sulphate of alumina and the
sodium chloride, forming it into small hollow cyl-
inders, which are well dried, and then the fire-clay
cylinder filled with these. Then, the cylinder being
heated to whiteness, highly superheated steam is
passed over it. The HC1 which is formed is
caught in a condensing apparatus, and there remains
a mass of aluminate of soda, which is moistened
with water and treated with a current of carbon
dioxide and steam. By washing the mass, the soda
goes into solution and hydrated alumina remains,
which is washed well arid is ready for use.
Most of the alumina is now made from the
natural aluminous earths, beauxite and cryolite,
the occurrence and properties of which have been
already described. The manufacture from beauxite
is fully described in the account of the process used
at Salindres, on p. 158. "We will give here the
modern methods of making it from cryolite.
146 ALUMINIUM.
MANUFACTURE FROM CRYOLITE.
Dry Way. — The cryolite is pulverized, an easy
operation, and to every 100 parts, 130 to 150 parts of
chalk are added, and a suitable quantity of fluorspar
is also used, which remains in the residue on wash-
ing after ignition. More chalk is used than is theo-
retically necessary, in order to make the mass less
fusible and keep it porous. But, to avoid using
too much chalk merely for this purpose, a certain
quantity of coke may be put into the mixture. It
is of-the first importance that the mixture be very
intimate and finely pulverized. It is of greater
importance that the mixture be subjected to just
the proper wTell-regulated temperature while being
calcined. The cryolite will melt very easily, but
this is to be avoided. On this account, the calci-
nation cannot take place in an ordinary smelting
furnace, because, in spite of stirring, the mass will
rnelt at one place or another, while at another part
of the hearth it is not even decomposed, because
the heat at the fire-bridge is so much higher than
at the farther end of the hearth. Thomson con-
structed a furnace for this special purpose (see
Figs. 6 and 7), in which the flame from the fire
first went under the bed of the furnace, then over
the charge spread out on the bed, and finally in a
flue over the roof of the hearth. The hearth has
an area of nearly 9 square metres, being 4 me-
tres long and 2.5 metres wride. It is charged
MANUFACTURE OF ALUMINA.
147
twelve times each day, each time with 500 kilos of
mixture, thus roasting 6000 kilos daily, with a
Fig. 6.
consumption of 800 kilos of coal. The waste heat
of the gases escaping from the furnace is utilized
for drying the soda solution to its crystallizing
point, and the gases finally pass under an iron
plate on which the chalk is dried. In this fur-
148 ALUMINIUM.
nace the mass is ignited thoroughly without a hit
of it melting, so that the residue can be fully
washed with water. The reaction commences at
a gentle heat, hut is not completed until a red heat
is reached. Here is the critical point of the whole
process, since a very little raising of the tempera-
ture ahove a red heat causes it to melt. However,
it must not he understood that the forming of
lumps is altogether to be avoided. These lumps
would be very hard and unworkable when cold,
but they can be broken up easily while hot, so
that they may be drawn out of the furnace a few
minutes before the rest of the charge is removed,
and broken up while still hot without any trouble.
The whole charge, on being taken out, is cooled
and sieved, the hard lumps which will not pass the
sieve arc ground in a mill and again feebly ignited,
when they will become porous and may be easily
ground up. However, the formation of these
lumps can be avoided by industrious stirring of
the charge in the furnace. A well-calcined mix-
ture is porous, without dust and without lumps
which are too hard to be crushed between the
fingers. We would here remark that mechani-
cal furnaces of similar construction to those used
in the manufacture of soda, potash, sulphate of
soda, etc., are more reliable and give the best
results if used for this calcination. The mixture,
or ashes, as the workmen call it, is drawn still hot,
and washed while warm in conical wooden boxes
with double bottoms, or the box may have but one
MANUFACTURE OF ALUMINA. 149
bottom, with an iron plate about 76 millimetres
above it. A series of such boxes, or a large appa-
ratus having several compartments, may be so
arranged that the washing is done methodically,
i. £., the fresh water comes first in contact with a
residue which is already washed nearly clean, and
the fresh charge is washed by the strong liquor.
This is known as the " Lessiveur methodique,"
and an apparatus constructed especially for this
purpose is described in Dingier 186, 370, by P. J.
Havrez, but the subject is too general and the de-
scription too long to be given here. A very suit-
able washing apparatus is also that of Schank,
used in the soda industry for washing crude soda,
and described in ' Lunge's Handbook of the Soda
Industry,' Book II. p. 410. Since the ashes are
taken warm from the furnace the washing water
need not be previously heated, but the final wash-
water must be warmed as the ashes have been
cooled down by the previous washings. As soon
as the strong liquor does not possess a certain
strength, say 20° B., it is run over a fresh charge
and so brought up. The solution contains sodium
aluminate.
Xow, whether the sodium aluminate solution is
made from beauxite or cryolite, it is treated further
in the same way in either case to get the hyd rated
alumina and the soda solution. Carbon dioxide is
next passed through the solution.
The carbon dioxide necessary for precipitating the
13*
150 ALUMINIUM.
by d rated alumina may be made in different ways.
The gases coming from the furnace in calcining the
cryolite might be used if they were not contaminated
with dust ; and there is also the difficulty that ex-
hausting the gases from the furnace would interfere
with the calcination. It has also been recommended
to use the gases from the fires under the evapora-
ting pans, by exhausting the air from the flues and
purifying it by washing with water. This can
only be done where the pans are fired with wood
or gas. However, the lime-kiln is almost exclu-
sively used to furnish this gas. The kiln used is
shaped like a small blast furnace. Leading in at the
boshes are two flues from five fire-places built in
the brickwork of the furnace, and the heat from
these calcines the limestone. The gases are taken
off by a cast-iron down-take at the top. At the
bottom of the furnace, corresponding with the tap
hole in a blast furnace, is an opening, kept closed,
from which lime is withdrawn at intervals. A
strong blast is blown in just above the entrance of
the side flues, and by keeping up a pressure in the
furnace, leakings into it may be avoided. The
gas is sucked away from the top by a pump, which
forces it through a cleaning apparatus constructed
like a wash bottle, and it is then stored in a ga-
someter. Instead of the pump, a steam aspirator
may be used, which is always cheaper and takes up
less room.
The precipitation with CO2 is made by simply
MANUFACTURE OF ALUMINA. 151
forcing it through a tube into the liquid. The
apparatus used at Salindres is one of the most im-
proved forms. (See p. 163.) The precipitate is
granular, and settles easily. However, it is not
pure hydrated alumina, hut a compound of alumina,
soda, carbonic acid, and water, containing usually
about 45 per cent, APO3, 20 per cent, Na^O3, and
35 per cent, H20. The sodium carbonate can be
separated by long-continued boiling with water,
but by this treatment the alumina becomes very
gelatinous and very difficult of further treatment.
The precipitate was formerly separated on linen
filters, but centrifugal machines are now preferred.
The evaporated solution gives a high grade of car-
bonate of soda free from iron. The heavy residue
which is left after the ashes have been lixiviated
consists of Fe*03, CaO, undecomposed cryolite, and
aluminate of Na, and has not been used for any-
thing.
According to Lo wig's experiments, the solution
of sodium aluminate can be precipitated by cal-
cium, barium, strontium, or magnesium, hydrates,
forming caustic soda and hydrated alumina, the
latter being precipitated with the CaO, BaO, SrO,
or MgO. The precipitate is washed by decantation
and then divided into two portions, one of which
is dissolved in HC1, the other made into a mush
with water and gradually added to the solution of
the other half until the nitrate shows only a very
little APO3 in solution. CaCP, EaCP, SrCP, or
152 ALUMINIUM.
MgCl2 has been formed, and the alumina all pre-
cipitated.
Wet way. — The decomposition of cryolite in the
wet way is operated as follows: The finely
powdered cryolite is boiled with dried burnt lime
in the proportion of three parts cryolite to two of
lime. There results a precipitate of calcium fluor-
ide, CaF2, while sodium aluminate is in the
solution. The reaction takes place quite easily.
The solution is settled, washed by decaritation,
and these washings put with the strong solution
first poured off; the next washings are reserved
for the fresh wash-water of another operation.
The solution of sodium aluminate is then boiled
with a quantity of cryolite equal to the amount
first used, when sodium fluoride is formed and
alumina precipitated. This operation is in noway
difficult, only requiring a little more attention
than the first. The alumina thus made is very
finely divided. The reactions involved are : —
Al2F6.6^NTaF + 6CaO= AP03.3^"a20 4- 6CaF2.
Al2F6.6STaF + Al203.3£Ta20 + 6H20= 2(A1203.3H20)
+ 121STaF.
During this last operation it is best to add an
excess of cryolite, and keep the liquid in motion
to prevent the cryolite from caking at the bottom.
Lead is the best material to make these precipitat-
ing tanks of, since iron would contaminate the
alumina. The precipitate is washed as in the
MANUFACTURE OF ALUMINA. 153
previous operation. The solution of sodium fluor-
ide, XaF, is boiled with the requisite quantity of
burnt lime, which converts it into caustic soda,
KaOH, which is separated from the precipitated
CaF2 by decantation and washing. The solution
is evaporated down to a concentrated solution of
XaOH, or to dryness, as desirable. The lime used
should be as pure and free from iron as possible, to
avoid contaminating the alumina.
Alumina may also be obtained from alum stone
or alum shales; by converting these into alums or
into Al2(S04)3Aq. by any of the well-known
methods of alum-makers, and then the alumina
made by calcining this salt, as given on p. 144.
PART VIII.
MANUFACTURE OP THE DOUBLE CHLORIDE OF
ALUMINIUM AND SODIUM.
SINCE the cost of the aluminium chloride is
equal to the cost of the sodium used, in making
aluminium, many attempts have been made to
cheapen its manufacture from alumina, but with-
out much success. Mr. Frishmuth, of Philadel-
phia, claims that he has lowered the cost of alum-
inium principally by making the APCl6 much
cheaper than before. Mr. Webster's process,
which has been applied on such a large scale, is
altogether concerned with producing the APCl6
cheaply, not a word being said about improve-
ments in making the sodium. However, with
these exceptions, and possibly one or two others
which will be found further on, the making of
these chlorides has remained much as Deville
left it. The description of their manufacture as
conducted at Salindres is the only account given
by Mierzinski, and so that may be taken as the
process now in general use, especially in Europe.
It will be found on p. 166. I add here just a few
words to Fremy's description of the process, which
may serve to render his description more exact : —
CHLORIDE OF ALUMINIUM AND SODIUM. 155
Mierzinski says that when the double chloride
is to be made, special importance is to be attached
to using materials free from iron in preparing the
alumina, as iron cannot be removed from A12C16.-
2XaCl as easily as from A12C16. Mierzinski also
devotes some space to descriptions of chlorine
generators, but that is a separate subject, full de-
scriptions of which can be found in any good work
on practical chemistry.
There have been a few attempts to make these
chlorides in different ways from that used in
Deville's process. I find two such processes,
which, however, cannot have been much of an
improvement on Deville's, or else they would have
supplanted it.
M. Dullo makes the following observations on
the production of APC16 direct from clay: — *
"Up to the present time the A12C1* necessary to
the production of aluminium has been prepared by
treating cryolite or beauxite, calcining them with
carbonate of soda, and neutralizing directly with
HOI or CO2 the alu initiate of soda formed. This
process may be simplified, and the APC16 obtained
much more easily, by direct treatment of clay.
For this purpose a good clay, free from iron and
sand, is mixed with enough water to make a thick
pulp, to which is added !N~aCl and pulverized
carbon. For every 100 parts of dry clay there are
* Bull, de la Soc. Chem. 1860, vol. T. p. 472.
156 ALUMINIUM.
taken 120 parts XaCl and 30 of carbon. The mix-
ture is dried and broken up into small fragments,
which are then introduced into a red-hot retort
traversed by a current of chlorine. Carbonic
oxide is disengaged, while at the same time APC16
and a little SiCl4 are formed. It is not necessary
that the chlorine should be absolutely dry, it may
be employed just as it comes from the generator.
The gas is absorbed very rapidly, because between
the aluminium and silicon there are reciprocal
actions under the influence of which the chemical
actions are more prompt and energetic. The
aluminium having for chlorine a greater affinity
than silicon has, A12C16 is first formed, and it is
only when all the aluminium is thus transformed
that any SiCl4 is formed. When SiCl4 begins to
form the operation is stopped, the incandescent
mixture is taken out of the retort and treated
with water. The solution is evaporated to dryness
to separate out a small quantity of silica, SiO2,
which is in it, the-residue is taken up with water,
and the Al2ClV2NaCl remains when the filtered
solution is evaporated to dryness. These succes-
sive solutions and evaporations might probably be
suppressed, especially if only enough chlorine is
passed over the incandescent clay to just convert all
the aluminium into APC16, in which case no SiCl4
will be formed, and therefore no soluble silica can
exist in the solution to contaminate the APC16 or
CHLORIDE OF ALUMINIUM AND SODIUM. 157
impede its reduction. M. Dullo recommends re-
ducing the AlfClV2]$raCl by zinc. See Part X.
' Chemical News/ 1878, p. 307, contains a short
account of an improved method of producing
A1*C16, which consists essentially in passing vapors
of hydrochloric acid, HC1, and carbon disulphide,
CS*, simultaneously over heated alumina or clay*
The CS2 changes it into aluminium, sulphide,
A12S8, and the HC1 converts this into Al'Cl6,
which distils.
14
PART IX.
MANUFACTURE OF ALUMINIUM AT SALINDRES (GARD).
We will now give the actual preparation at Salin-
dres,* with the latest improvements which it has
received in practice. Aluminium is there regularly
prepared at the works of the Chemical Manufac-
turing Company of Alais and Camargue, the old
firm of Henry Merle & Co., new firm A. R. Pechi-
ney & Co.
The principal chemical reactions on which this
process rests are the following : —
Formation of aluminate of soda by calcining
beauxite with Na2C03 —
(AlFe)203.2H20 + 3¥a2C03= Al203.33Ta20 + Fe203
Formation of alumina by precipitating the alu-
minate of soda with a current of carbon dioxide —
Al203.3ISra20 + SCO2 + 3II20 = A1203.3H20 -h
Formation of Al2Cl6.2^sTaCl by the action of
* Fremy's Ency. Chem., M. Margottet.
REDUCTION OF THE ALUMINIUM. 159
chlorine on a mixture of alumina, carbon, and sodi-
um chloride —
APO3 + 30 + 2NaCl + 601= Al2CK2NaCl + SCO.
Reduction of this double chloride by sodium.
Al2CR2XaCl + 6¥a = 2 Al + SXaCl.
The primary material then to furnish the alumin-
ium is beauxite. It will be seen that to obtain
the metal it is necessary to proceed successively
through the following operations: —
I. Preparation of the aluminate of soda and so-
lution of this salt to separate it from the ferric
oxide contained in the beauxite.
II. Precipitation of hyd rated alumina from the
aluminate of soda by a current of carbon dioxide;
washing the precipitate.
III. Preparation of a mixture of alumina, car-
bon, and salt, drying it, and then treating with
gaseous chlorine to obtain the double chloride of
aluminium and sodium.
IV. Lastly, treatment of this chloride by sodium
to obtain aluminium.
We will now review these operations as practi-
cally carried out in detail. We will not consider
the preparation of the crude materials as chlorine,
sodium, etc., which is spoken of elsewhere.
I. Preparation of the Aluminate of Soda.
The aluminate to serve for the preparation of
Al2Cl6.2XaCl was first obtained by the calcination
160 ALUMINIUM.
of ammonia alum. At Salindres this was with-
drawn and beauxite used, a material consisting of
sesqui-oxide of iron aad aluminium in varying pro-
portions, with two molecules of water and a little
silica. It is redder the more iron it contains.
Beauxite is plentiful enough in the south of France,
principally in the departments of Herault, Bouches-
du-Rhone, and Yar. That used at Salindres comes
from Yar. It contains at least seventy-five per
cent, alumina. To separate the alumina from Fe203,
it is treated with carbonate of soda, under the in-
fluence of a sufficiently high temperature, the A1203
displacing the CO2 and forming alurninate of soda,
Al203.3N"a20, while the Fe203 remains unattacked.
A simple washing with water then permits the
separation of the Al203.31^a20 from the insoluble
Fe203. The beauxite is first finely pulverized by
means of a vertical mill-stone, then intimately
mixed with some Na2C03. The mixture is made
for one operation, of —
480 kilos beauxite.
300 " Na2CO3 of 90 alkali degrees.
This mixture is introduced into a reverberatory
furnace, resembling in form a soda furnace, and
which will 'bear heating strongly. The mass is
stirred from time to time, and it is kept heated
until all the carbonate has been attacked, which is
recognized by a test being taken which does not
effervesce with acids. The operation lasts from
five to six hours.
REDUCTION OF THE ALUMINIUM. 161
The aluminate thus obtained is separated from
Fe203 by a washing with warm wrater. This wash-
ing is made at first with a feeble solution which has
served for the complete exhaustion of the preceding
charge, which was last washed with pure water,
forming thus this feeble solution. This gives, on
the first leaching, solutions of aluminate concen-
trated enough to be called strong liquor, which are
next treated by the current of CO2 to precipitate
the hyd rated alumina. The charge is next washed
with pure water, wrhich completely removes the
aluminate ; this solution is the weak liquor, which
is put aside in a special tank, and used as the first
leaching liquor on the next charge treated. This
treatment takes place in the following apparatus
(see Fig. 8) : B is a sheet-iron vessel, in the middle
of which is a metallic grating>,F, on which is held
all round its edges, by pins^ a cloth, serving as a
filter. The upper part of this vessel is called sim-
ply the filter. A ought to be closed by a metallic
lid held on firmly by bolts. To work the apparatus,
about 500 kilos of the charge to be washed is
placed on the filter cloth, the lid is closed, then the
steam-cock / of the reservoir A is opened. In A
is the weak solution from the last washing of the
preceding charge. The pressure of the steam
makes it rise by the tube Tinto the filter; another
jet of steam, admitted by the cock 6, rapidly
warms the feeble liquor as it soaks into the charge.
After filtering through, the strong liquor is drawn
14*
162
ALUMINIUM.
off by turning the stopcock Cr. The weak solu-
tion of the reservoir A is put into the filter in
Fig. 8.
B
t.£VYTYf>£ (Ji
successive portions, and not all at once ; and after
each addition of solution has filtered through, its
strength in B.° is taken, before any more solution
is run in ; then, when the solution marks 3 to 4°,
it is placed in the special tank for weak liquor,
with all that comes through afterwards. Just
REDUCTION OF THE ALUMINIUM. 163
about this time, the weak liquor of the reservoir
A is generally all used up, and is replaced by pure
water introduced by the tube d. All the solutions
which filtered through, marking over 3 to 4° B.,
are put together, and form the strong liquor which
marks about 12° B. This extraction of the alu-
minate being completed by the pure wrater, the
residue on the filter is taken out, and a new opera-
tion may be commenced.
II. Preparation of the Alumina.
The strong liquor is introduced into a vessel
having an agitator, wThere a strong current of CO2
may precipitate the A1203 from it. The gas is
produced by small streams of hydrochloric acid
continuously falling on some limestone contained
in a series of earthenware jars. The precipitation
vessel is called a baratte. The CO2 after having
passed through a washing flask, is directed to a
battery of three barattes, where the precipitation
is worked methodically, so as to precipitate com-
pletely the alumina of each baratte, and utilize at
the same time all the carbon dioxide produced.
In order to do this, the gas always enters first into
a baratte in which the precipitation is nearest com-
pletion, and arrives at last to that in which the
solution is freshest. When the gas is not all ab-
sorbed in the last baratte, the first is emptied, for
the precipitation in it is then completed, and it is
164
ALUMINIUM.
made the last of the series, the current being now
directed first into the baratte which was previously
second, while the newly charged one is made the
last of the series. The process is thus kept on
Fig. 9.
a. Charging pipe.
Z>. Steam pipe.
c. Steam drip.
d. CO2 enters.
/. Discharge pipe.
A. Agitator, made of iron rods.
C. Tank in which the precipitate settles.
B. Baratte body.
D. Steam jacket.
REDUCTION OF THE ALUMINIUM. 165
continuously. The apparatus used is shown in
Fig. 9.
Each baratte holds about 1200 litres of solution,
and the complete precipitation of all the alumina
in it takes five to six hours. A mechanical agi-
tator stirs the contents continually, and a current
of steam is let into the double bottom so as to
keep the temperature of the solution about 70°.
The precipitated alumina and the solution of
Ka2C03 which remains are received in a vat
placed beneath each baratte. The solution is de-
canted off* clear, after standing, and then evapo-
rated down to dry ness, regenerating the Na*C03
used in treating the beauxite to make the alumi-
nate, less the inevitable losses inseparable from all
industrial operations. The deposit of alumina is
put into a conical strainer to drain, or else into a
centrifugal drying machine, which rapidly drives
out of the hydrated alumina the solution of Ka2C03
which impregnates it ; a washing with pure wrater
in the drier itself terminates the preparation of the
alumina. At the works at Salindres, a part of this
alumina is converted into sulphate of alumina,
which is sold, the remainder being used for the
aluminium manufacture. After washing in the
dryer, the alumina presents this composition:—
APO3 47.5
H*0 50.0
2.5
166 ALUMINIUM.
III. Preparation of the APCP.ZNaCl.
When a current of chlorine is passed through a
mixture of anhydrous alumina and carbon, APC16
is obtained. This simple chloride may be em-
ployed for obtaining aluminium ; it was first so
employed by Deville ; but it is deliquescent, its
preservation is difficult, and its employment very
inconvenient. Industrially, as indicated by De-
ville, the double chloride is always used, as it does
not present these inconveniences to so large a
degree. The double chloride may be obtained in
the same manner as the simple chloride ; it is suf-
ficient to put some common salt, NaCl, into a
mixture of alumina and carbon, and, on heating
this mixture strongly, there is formed, by the
action of the chlorine, Al2Cl6.2NaCl, which distils
at a red heat and condenses in a crystalline mass at
about 200°. The Irydrated alumina obtained in
the preceding operation is mixed with salt and
finely pulverized charcoal, in proper proportions,
the whole is sifted, and a mixture produced as
homogeneous as possible ; then it is agglomerated
with water and made into balls the size of the fist.
These balls are first dried in a drying stove, at
about 150°, then calcined at redness in retorts,
where the double chloride should commence to be
produced just as the balls are completely dried.
These retorts are vertical cylinders of refractory
earth, each one is furnished with a tube in its lower
REDUCTION OF THE ALUMINIUM.
167
part for the introduction of chlorine, and with
another towards its upper end for the exit of the
vapor of double chloride. (See Fig. 10.) A lid
Fig. 10.
carefully luted during the operation with a mix-
ture of fine clay and- horse dung serves for the
charging and discharging of the retort. The
double chloride is condensed in earthen pots like
flower pots, made of ordinary clay, and closed by a
well-luted cover, into which passes a pipe of clay
to conduct the gas resulting from the operation
into flues connected with the main chimney. Each
retort is heated by a fire, the flame of which circu-
lates all round it, and permits keeping it at a bright
red heat. An operation is conducted as follows :
168 ALUMINIUM.
The retort is filled with stove-dried balls, the lid-
is carefully luted, and the retort is heated gently
till all the moisture is driven off. This complete
desiccation is of great importance, and requires
much time. Then chlorine, furnished by a battery
of three generating vessels, is passed in. During
the first hours, the gas is totally absorbed by the
balls, and the double chloride distils regularly for
about three hours, and runs into the earthen pots
where it solidifies. Toward the end, the distilla-
tion is more difficult and less regular, and the
chlorine is then only incompletely absorbed. After
each operation there remains a little residue in the
retort, which accumulates and is removed every
two days, when two operations are made per day.
One operation lasts at least twelve hours, and a
retort lasts sometimes a month. The double
chloride is kept in the pots in which it was con-
densed until the time it is to be used in the next
operation ; it is almost chemically pure, save traces
of iron, and is easy to keep and handle.
IV. Reduction of the Double Chloride by Sodium.
The difficulty of this operation, at least from an
industrial point of view, is to get a slag fusible
enough and light enough to let the reduced metal
easily sink through it and unite. This result has
been reached by using cryolite, a white or grayish
mineral originally from Greenland, very easy to
REDUCTION OF THE ALUMINIUM.
169
melt, formula Al2F6.6XaF. This material forms
with the XaCl resulting from the reaction a very
fusible slag, in the midst of which the aluminium
collects well, and falls to the bottom. In one ope-
ration the charge is —
100 kilos
45 "
35 u
APF^GNaF.
Na.
The double chloride and cryolite are pulverized,
the sodium, cut into small pieces a little larger than
the thumb, is divided into three equal parts, each
part being put into a sheet-iron basket. The mixture
of double chloride and cryolite, being pulverized, is
divided into four equal parts, three of these are
respectively put in each basket with the sodium,
Fig. 11.
the fourth being placed in a basket by itself. The
reduction furnace (see Fig. 11) is a little furnace of
15
170 ALUMINIUM.
refractory brick, with an inclined hearth and a
vaulted roof. This furnace is strongly braced by
iron tie-rods, because of the concussions caused by
the reaction. The flame may at any given moment
be directed into a flue outside of the hearth. At
the back part of the furnace, that is to say, on that
side towards which the bed slopes, is a little brick
wall which is built up for each reduction and is
taken away in operating the running out of the
metal and slag. A gutter of cast iron is placed
immediately in front of the wall to facilitate run-
ning out the materials. All this side of the furnace
O
ought to be opened or closed at pleasure by means
of a damper. Lastly, there is an opening for charg-
ing in the roof, closed by a lid. At the time of an
operation the furnace should be heated to low red-
ness, then are introduced in rapid succession the
contents of the three baske'ts containing sodium,
etc., and lastly the fourth containing only double
chloride and no sodium. Then all the openings of
the furnace are closed, and a very vivid reaction
accompanied b3Tdull concussions immediately takes
place. At the end of fifteen minutes, the reaction
subsides, the dampers are opened, and the heat con-
tinued, meanwhile stirring the mass from time to
time with an iron poker. At the end of three
hours the reduction is ended, and the metal collects
at the bottom of the liquid bath. Then the run-
ning out is proceeded with in three phases : First.
Running off the upper part of the bath, which
REDUCTION OF THE ALUMINIUM. 171
consists of a fluid material completely free from re-
duced aluminium and constituting the white slag.
To run this out a brick is taken away from the
upper course of the little wall which terminates
the hearth. These slags are received in an iron
wagon. Second. Running out the aluminium.
This is done by opening a small orifice left in the
bottom of the brick wall, which was temporarily
plugged up. The liquid metal is received in a cast-
iron melting pot, the bottom of which has been
previously heated to redness. This aluminium is
immediately cast in a series of small rectangular
cast-iron moulds. Third. Running out of the rest
of the bath, which constitutes the gray slags.
These were, like the white slags, formed by the
XaCl and cryolite, but they contain in addition,
isolated globules of aluminium. To run these out
all the bricks of the little wall are taken away.
This slag is received in the same melting-pot into
which the aluminium was run, the latter having
been already moulded Here it cools gradually,
and after cooling there are always found at the
bottom of the pot several grains of metal. In a
good operation there are taken from one casting
10.5 kilos of aluminium, which is sold directly as
commercial metal.
The foregoing description from Fremy sets forth
in its perfection the production of aluminium by
means of sodium, and until very recently this was
the only successful commercial process. A large
172 ALUMINIUM.
amount of aluminium is now produced by this
process, and it, therefore, does not lack interest.
The following data as to the expense of this pro-
cess may he very appropriately inserted here, giving
the cost at Salindres in 1872.
In 1872, 3600 kilos of Al were made at Salindres
at the following average cost: —
a. Manufacture of one kilo of N"a.
Soda . . . 9.35 kilos (a) 32 fr. per 100 kilos = 3 fr. 9 cent.
Coal ... 74.32 " "1.40" " " " = 1" 4 "
Wages ... 1 " 73 "
Expenses . . 3 " 46 "
Total . . . . 11 " 32 "
p. Manufacture of one kilo of Al2Cl6.2NaCl.
Anhydrous A12O3
0.59 kilos @ 86 fr. per 100 kilos = 0 fr. 50.7 cent.
MnO2 . 3.74 " " 14 " " " " =0 " 52.3 "
HC1 . . 15.72 " " 3 " " " " =0 "47.1 "
Coal . . 25.78 " "1.40 " " " =0 "36.1 "
Wages . . . 0 " 23.8 "
Expenses . . 0 " 38.0 "
Total .... 2 " 48.0 '
y. Manufacture of one kilo of Al.
Na . .3.44 kilos @ 11.32 fr. per kilo = 38 fr. 90 cent.
Al2Cl6.2NaCl
10.04 " " 2.48" " " =24 " 90 "
Cryolite 3 87 " " 61.0 " " 100 kilos = 2 " 36 "
Coal 29.17 " " 1.4.0 " " " " = 0 " 41 "
Wages ... 1 " 80 "
Costs . 0 " 88 "
Total . 69 " 25
* A. Wurtz, Wagner's Jaresb., 1874, vol. xxi.
REDUCTION OF THE ALUMINIUM. 173
This must be increased ten per cent, for losses
and other expenses, making the cost of aluminium
80 fr. per kilo, and it is sold for 100.
According to a statement in the ' Bull, de la Soc.
de I'lndustrie Minerale,' ii., 451, made in 1882.
Salindres was then the only place in which alu-
minium was manufactured.
LATER IMPROVEMENTS IN DEVILLE'S PROCESSES.
The later improvements in this process have been
made principally by Mr. J. Webster, of Birming-
ham, England, and some are claimed by Frishmuth
of Philadelphia. We will examine the reports of
Webster's processes and the claims of Frishmuth.
WEBSTER'S PROCESS.
Recently the statement* has been current in a
number of journals that material improvements
have been made in the manufacture of aluminium at
the Aluminium Crown Metal Works at Hollywood,
near Birmingham, England, under the direction of
Mr. Webster. Mr. Webster describes one of his
improvements, which is patented,f as follows :
Three parts of alum are mixed with one part of
coal pitch, and the mixture heated to 200° or 260°.
* Dingier, 1883, cclix. 86.
f Austrian Pat. Sept. 28, 1882.
15*
174 ALUMINIUM.
In about three hours the pasty mass is spread upon
a stone floor, and after becoming cool is broken in
pieces. Hydrochloric acid of twenty to twenty-
five per cent, is poured upon these pieces placed in
piles which are turned over from time to time.
When the evolution of sulphuretted hydrogen,
IPS, has stopped, about five per cent, of charcoal
powder or lampblack, with enough water to make
a thick paste, is added. The mass is thoroughly
broken up and mixed in a mill, and then worked
into balls of about a pound each. These are bored
through to facilitate drying, and heated in a dry-
ing chamber at first to 40°, then in a furnace from
95 up to 150°. The balls are then kept for three
hours at a low red heat in retorts while a mixture
of two parts steam and one part air is passed
through, so that the sulphur and carbon are con-
verted into SO2 and CO2, and thus escape. The
current of gas carries over some K2S04, FeSO4, and
A1203, and is therefore passed through clay con-
densers. After these have been driven off the dry
residue is removed from the retort, again ground
in a mill to fine powder, which now consists of
A12C3 and K2304. This powder is treated with
about seven times its weight of water, then boiled
in a pan or boiler by means of steam for about one
hour, then allowed to stand till cool. The solution
containing the K2S04 is run off and evaporated to
dryness, the alumina is washed out and dried.
REDUCTION OF THE ALUMINIUM. 175
The product thus obtained contains 84.1 per cent.
A1203.
The ahove patent is seen to cover only the man-
ufacture of pure alumina. A later account thus
describes Mr. Webster's plant and processes. It
is taken from the Birmingham, England, ' Gazette,'
and was copied into an American journal* as fol-
lows : —
" There has been recently patented in most of
the leading countries of the world an invention of
great importance. The Aluminium Crown Metal
Co., at Hollywood, near Birmingham, now claim to
have perfected an improved process by which they
produce pure alumina from alum, convert it into
APC16, and reduce this by sodium. By this pro-
cess the two common impurities of aluminium,
silicon and iron, are avoided. The inventor is Mr.
James Webster, the founder and principal of the
company. Their works having been erected within
the last five years, the plant is of the most recent
date, comprising all the modern improvements in
calcining furnaces and retorts, sheet-rolling and
wire-drawing mills, together with the requisite
casting, fitting, and other shops.
" On retiring from business some years ago as a
metal manufacturer, Mr. Webster took up his resi-
dence at Hollywood, and while nominally engaged
* Bulletin of the Iron and Steel Association, Philadelphia,
January 3, 1883.
176 ALUMINIUM.
in farming carried on the experiments which he
had commenced as far back as 1851 for the inven-
tion of an expeditious and inexpensive mode of
producing aluminium. He designed all the vari-
ous buildings, appliances, and apparatus necessary
for the carrying on of experiments, upon which he
expended upwards of £3000, besides £2000 or
£3000 in procuring patent rights at home and
abroad. A French syndicate has just oifered him
£25,000 for the patent for France alone, while
parties in the United States, Belgium, and Ger-
many are arranging to purchase rights.
u The invention has only been perfected about
eighteen months, and the firm have but recently
begun to place the product on the market, yet such
is the demand, that though they are now working
day and night, they cannot execute one-quarter of
the orders accumulating on their books. By the
ordinary method of precipitation, 12 tons of alum
and 6 tons of K2C03 or Na2C03 are required to pro-
duce one ton of alumina, and the whole process
occupies nine weeks ; whereas, in Mr. Webster's
plan, no precipitant is used, and a ton can be manu-
factured in a week with the existing plant. The
cost of one ton of alumina by the ordinary method
is upwards of £1000, while it is less than £100 by
Mr. Webster's process.
" Mr. Webster's process consists in taking a given
quantity of alum and pitch, which are finely ground,
mixed together, and placed in a calcining furnace,
REDUCTION OF THE ALUMINIUM. 177
by which means 38 per cent, of water is driven off,
leaving the sulphur, potash, and alumina, with
some ferric oxide. The calcined mixture is then
put in vertical retorts, and steam and air are forced
through, which leaves a residue of K20 and A1203
only. This is then placed in a vat of warm water
heated by steam. The caustic potash liquor is then
run oft' and boiled down, while the residual APO3
is collected in sacks and dried. This deposit con-
tains about 84 per cent. APO3, while that obtained
by the old process of precipitation has only 65 per
cent. Thus a saving is effected of nine-tenths in
cost and 19 per cent, more alumina is obtained.
In addition to this, the whole of the bye products
are recovered, consisting of KOH,S (which is used
in making H2S04), and aluminate of iron. From
these bye products is made a blue dye, which is
sold for six shillings a pound, and is used in place
of indigo for dyeing calico and other materials.
The APC16 is reduced by sodium.
" ' The English Ironmonger' for April, 1886, con-
tains a long article describing the extensions which
this company have made, their works having now
attained a large size, wThile the number and variety
of their products, in aluminium and its alloys, as
ingots, wire, sheet, or worked up in "hundreds ot
different ways, is truly surprising. They have
monopolized this business in England, and are very
enterprising in introducing their manufactures else-
where."
178 ALUMINIUM.
FRISHMUTH'S PROCESS.
In the United States the only improvement in
the sodium process of reducing aluminium is
contained in the following patent: — *
Win. Frishmuth, of Philadelphia, in his patent
makes the following claims : —
1. The simultaneous generation of sodium vapor
and a volatile compound of aluminium in two
separate vessels or retorts, and mingling the
vapors thus obtained in a nascent (?) state in a third
vessel, wherein they react on each other.
2. The sodium vapor is produced from a mixture
of a sodium compound and carbon, or some other
reducing agent ; and the aluminous vapor from
aluminous material.
3. The simultaneous generation of sodium vapor
and vapor of A12C16 or A12F6 ; or of sodium vapor
and Al2Cl6.2NaCl.
4. Converting the aluminous material to a vapor
by heating it in a retort with NaCl,and subjecting
it at the same time to chlorine gas; mingling the
vapor of Al2Cl6.2Nad thus obtained with vapor
simultaneously generated from Na2C03 and carbon.
* U. S. Pat., 308,152. Nov. 18, 1884.
REDUCTION OF THE ALUMINIUM. 179
OTHER PROCESSES.
H. Niewerth, of Hanover, has patented in the
United States and other countries the following
process :* A compound of aluminium, with chlorine
or fluorine, is hrought by any means into the form
of vapor, and conducted, strongly heated, into
contact with a mixture of 62 parts Xa2C03, 28 coal
and 10 chalk, which is also in a highly heated con-
dition. This mixture disengages sodium, which
O O '
reduces the gaseous chloride or fluoride of alumin-
ium, the nascent sodium being the reducing agent.
In place of the above mixture other suitable mix-
tures which generate sodium may be employed, or
mixtures may also advantageously be used from
which potassium is generated.
Hector von Grousilliers, Springe, Hanover, pat-
ents the following improvement :f In order to
avoid the difficulties ordinarily met with in the
use of Al2Cl6.2XaCl to obtain aluminium, the
patentee raises the volatilizing point of APCl6 by
performing its reduction, either chemically or
electrolytically, under pressure in a strong, her-
metically-closed vessel lined with clay or magnesia
and provided with a safety valve.
* Sci. Am. Suppl., Nov. 17, 1883.
t Eng. Pat., June 29, 1885, No. 7858.
PART X.
REDUCTION OF ALUMINIUM BY OTHER REDUC-
ING AGENTS THAN SODIUM.
REDUCTION BY CYANOGEN.
ACCORDING to Knowles's patent,* aluminium
chloride, APC16, is reduced by means of potassium
or sodium cyanide, the APC16, either fused or in
the form of vapor, being brought in contact with
either the melted cyanide or its vapor. The
patent further states the strange fact that pure
alumina may be added to increase the product.
Corbelli, of Florence,f patented the following
method in England : Common clay is freed from
all foreign particles by washing, then well dried.
One hundred grammes of it are mixed with six
times its weight of concentrated sulphuric or
hydrochloric acid ; then the mixture is put in a
crucible and heated to 400 or 500°. The mass re-
sulting is mixed with 200 grammes of dry yellow
prussiate of potash and 150 grammes of N"aCl, and
this mixture heated in a crucible to whiteness.
* Sir Francis C. Knowles, Eng. Pat. 1857, No. 1742.
f Wagner's Jaliresb., 1858.
REDUCTION BY OTHER AGENTS THAN SODIUM. 181
After cooling, the reduced aluminium is found in
the bottom of the crucible as a button.
According to Deville's experiments, this process
will not give any results. Watts remarks that
any metal thus obtained must be very impure,
consisting chiefly of iron. The patent is dated
1858, No" 142.
REDUCTION BY HYDROGEN.
F. W. Gerhard* decomposes aluminium fluor-
ide, APF6, or Al2F6.6NaF — cryolite— by subjecting
it to hydrogen at a red heat. The aluminium
compound is placed in a number of shallow dishes
of glazed earthen ware, each of which is surrounded
by a number of other dishes containing iron
tilings. These dishes are placed in an oven pre-
viously heated to redness, hydrogen gas is then
admitted, and the heat increased. Aluminium
then separates, hydrofluoric acid, HF, being
formed, but immediately taken up by the iron
filings and thereby prevented from reacting on the
aluminium. To prevent the pressure of the gas
from becoming too great, an exit tube is provided,
which may be opened or closed at pleasure. This
process, patented in England in 1856, No. 2980, is
ingenious and was said to yield good results. The
inventor has, however, returned to the use of the
* Watts's Dictionary.
16
182 ALUMINIUM.
more costly reducing agent, sodium, which would
seem to imply that the hydrogen method has not
yet quite fulfilled his expectations.
REDUCTION BY CARBURETTED HYDROGEN.
Mr. A. L. Fleury,* of Boston, mixes pure
alumina with gas tar, resin, petroleum, or some
such substance, making it into a stiff paste which
may be divided into pellets and dried in an oven.
They are then placed in a strong retort or tube
which is lined with a coating of plumbago. In
this they are exposed to a cherry-red heat. The
retort must be sufficiently strong to stand a press-
ure of from 25 to 30 pounds per square inch, and
be so arranged that by means of a safety valve the
necessary amount of some hydro-carbon may be
introduced into the retort among the heated mix-
ture, and a pressure of 20 to 30 pounds must be
maintained. The gas is forced in by a force pump,
By this process the APO3 is reduced, while the
metal remains as a spongy mass mixed^vith car-
bon. This mixture is re-melted with metallic
zinc, and when the latter has collected the alumin-
ium, it is driven off by heat. The hydrocarbon
gas under pressure is the reducing agent. The
time required for reducing 100 pounds of alumina,
earth, cryolite, or other compound of aluminium,
* Chemical News, June, 1869, p. 332.
REDUCTION BY OTHER AGENTS THAN SODIUM. 183
should not be more than four hours. When the
gas can be applied in a previously heated condition
as well as being strongly compressed, the reduction
takes place in a still shorter period.
Xothing is now heard of this process, and it has
been presumably a failure. It is said that several
thousand dollars were expended by Mr. Fleury
and his associates without making a practical
success of it. We should be glad to hear in the
future that their sacrifices have not been in vain,
and that the process still has possibilities in it
which will some time be realized.
Petitjean* makes aluminium sulphide, APS3, by
one of Fremy's methods,f or makes a double sul-
phide of aluminium with potassium or sodium by
mixing alumina with a little tar or turpentine in
a carbon lined crucible, heating strongly, and then
mixing with a powder composed of Ka2C03, or
K2C03, and sulphur ; again heating a long time at
bright redness. The sulphide or double sulphide
thus made is put in a crucible or retort through
the bottom of which can be led a stream of carbu-
retted hydrogen, which separates the aluminium
from its combination with the sulphur. Alumin-
ium J can also be reduced from APS3 by mixing it
with iron filings or a pulverized rnetal having
* Kerl and Stohman, Poly. Central Blatt. 1858, 888.
f See Appendix.
J See Appendix.
184 ALUMINIUM.
similar qualities, and melting the mixture. A
metallic mixture may be used instead of carbu-
retted hydrogen in the above operation.
REDUCTION BY DOUBLE REACTION.
M. Comenge,* of Paris, obtains aluminium from
its sulphide either by heating it in an atmosphere
of hydrogen, or by heating it with A1203 or
A12(S04/ in such proportions that sulphur dioxide,
SO2, and aluminium may be the sole products; or
the sulphide may be decomposed by iron, copper,
or zinc. The reactions involved would be — •
A12S3 + 3H-H= 2 Al + 3H2S.
A12S3 + 2 A1203= 6 Al -f 3S02.
A12S3 + Al2(S04/= 4A1 + 6S02.
A21S3 + 3(Fe.Cu.Zn.)= 2A1 + 3(Fe.Cu.Zn.)S.
Johnsonf patented the following process: Alu-
minium sulphide is mixed with quite dry A12(S04)3
in such proportions that the sulphur and oxygen
present may evolve as SO2. The mixture is heated
to redness in an unoxidizing atmosphere, when
SO2 evolves and the metal remains. The reaction
is furthered by agitation. The aluminium in the
resulting mass can be treated in the way commonly
used in puddling spongy iron, and then either
pressed or hammered together. Or, the aluminium
* Eng. Pat. 1858, No. 461.
Kerl and S tollman's Handbucb.
REDUCTION BY OTHER AGENTS THAN SODIUM. 185
sulphide may be heated to redness in an unoxidiz-
ing atmosphere and dry hydrogen or water gas
conducted over it, and the metal separated from
the resulting mass by dressing.
Mr. Niewerth's* process may be operated in his
newly invented furnace, but it may also be carried
on in a crucible or another form of furnace. The
furnace alluded to consists of three shaft furnaces,
the outer ones well closed on top by iron covers,
and connected beneath by tubes with the bottom
of the middle one : the tubes being provided with
closing valves. These side shafts are simply water-
gas furnaces, delivering hot water-gas to the
central shaft, and by working the two alternately
supplying it with a continuous blast. The two pro-
ducers are first blown very hot by running a blast
of air through them with their tops open, then the
cover of one is closed, the blast shut oft', steam
turned on just under the cover, and water gas
immediately passes from the tube at the bottom of
the furnace into the central shaft. The middle
shaft has meanwhile been filled with these three
mixtures in their proper order: —
First. A mixture of sodium carbonate, carbon,
sulphur, and alumina.
Second. Aluminium sulphate.
Third. A flux, preferably a mixture of XaCl and
KOL
* Sci. Am. Suppl., Nov. 17, 1885.
16*
186 ALUMINIUM.
•
This central shaft must be already strongly
heated to commence the operation, it is best to fill
it with coke before charging, and as soon as that
is hot to put the charges in on the coke. Coke
may also be mixed with the charges, but it is not
necessary. The process then continues as follows:
The water-gas enters the bottom of the shaft at a
very high temperature. These highly heated
gases, carbonic oxide and hydrogen, act upon the
charges so that the first breaks up into a combina-
tion of sodium sulphide and aluminium sulphide,
from which, by means of the second charge of
A12(SG4)3, free aluminium is reduced. As the latter
passes down the shaft, it is melted and the flux
assists in collecting it, but is not absolutely neces-
sary. Instead, of producing this double sulphide,
pure aluminium sulphide might be used for the
first charge, or a mixture which would generate
APS3 ; or, again, pure iui2S, K2S, CuS, or any
other metallic sulphide which will produce the
effect alone, in which case aluminium is obtained
alloyed with the metal of the sulphide. Instead
of the first charge a mixture of alumina, sulphur,
and carbon might be introduced. Or, the A12(S04)3
of the second charge might be replaced by alumina.
So, one charge may be Na2S, K2S, or any other
metallic sulphide, and the second charge may be
either A1203 or A12(S04)3.
REDUCTION BY OTHER AGENTS THAN SODIUM. 187
REDUCTION BY CARBON AND CARBON DIOXIDE.
J. Morris'55' of Uddington claims to obtain alumin-
ium by treating an intimate mixture of alumina
and charcoal with carbon dioxide. For this pur-
pose, a solution of A12C16 is mixed with powdered
wood-charcoal or lampblack, then evaporated till
it forms a viscous mass which is shaped into balls.
During the evaporation hydrochloric acid is given
off. The residue consists of alumina intimately
mixed with carbon. The balls are dried, then
treated with steam in appropriate vessels for the
purpose of driving off all the chlorine, care being
taken to keep the temperature so high that the
steam is not condensed. The temperature is then
raised so that the tubes are at a low red heat, and dry
carbon dioxide,C02,is then passed through. This CO2
is said to be reduced by the carbon to carbonic oxide,
CO, which now, as affirmed by Mr. Morris, reduces
the alumina. Although the quantity of carbonic
oxide escaping is in general a good indication of the
progress of the reduction, it is, nevertheless, not
advisable to continue heating the tubes or vessels
until the evolution of this gas has ceased, as in con-
sequence of slight differences in the consistency of
the balls some of them give up all their carbon
sooner than others. The treatment with carbon
* Dingier, 1883, vol. 259, p. 86. German Pat. No. 221oO,
Aug. 30, 1882.
188 ALUMINIUM.
dioxide lasts about thirty hours when the substances
are mixed in the proportion of five parts carbon
to four parts alumina. Morris states further that
the metal appears as a porous spongy mass, and is
freed from the residual alumina and particles of
charcoal either by smelting it, technically " burn-
ing it out," with cryolite as a flux or by mechani-
cal treatment.
*
REDUCTION BY CARBON.
About the first attempt of this nature we can
find record of is the following article by M. Cha-
pelle : — *
" When I heard of the experiments of Deville,
I desired to repeat them, but having neither alu-
minium chloride nor sodium to use, I operated as
follows : I put natural clay, pulverized and mixed
with ground Nad and charcoal, into an ordinary
earthen crucible and heated it in a reverberatory
furnace, with coke for fuel. I was not able to get
a white heat. After cooling, the crucible was
broken, and gave a dry pulverulent scoria in which
were disseminated a considerable quantity of small
globules about one^half a millimetre in diameter,
and as white as silver, They were malleable, in-
soluble in nitric or cold hydrochloric acids, but at
60° dissolved rapidly in the latter with evolution
of hydrogen ; the solution was colorless and gave
* Compt. Bendus, 1854, yol, xxxyiij. p. 358.
REDUCTION BY OTHER AGENTS THAN SODIUM. 189
with ammonia a gelatinous precipitate of hydrated
alumina. My numerous occupations do not permit
me to assure myself of the purity of the metal.
Moreover, the experiment was made under condi-
tions which leave much to be desired, but my in-
tention is to continue my experiments and especially
to operate at a higher temperature. In addressing
this note to the Academy I but desire to call the
attention of chemists to a process which is very
simple and susceptible of being improved. I hope
before many days to be able to exhibit larger glob-
ules than those which my first experiment fur-
nished."
M. Chapelle never did address any further com-
munications to the Academy on this subject, and
•we must presume that further experiments did not
confirm these first ones.
G. W. Keinar* states that the pyrophorous mass
which results from igniting potash or soda alum
with carbon, contains a carboniferous alloy of alu-
minium with potassium or sodium, from which the
alkaline metal can be removed by weak nitric acid.
COWLES BROS.' PROCESS.
This process, which reduces alumina by carbon
in the presence of another metal to take up the
aluminium, using the electric furnace, is the nov-
* Wagner's Jaliresb. 1859, p. 4.
190 ALUMINIUM.
elty which is attracting widespread attention to the
metallurgy of aluminium. Its history has already
been sketched, and will be still further developed
in the following pages. It properly comes under
the heading of " Reduction by Carbon."
" Early in the present century, Sir H. Davy,
Berzelius, and Oerstedt, all famous chemists, at-
tempted unsuccessfully to reduce alumina by elec-
tricity. Likewise, many learned scientists have
striven to decompose it by carbon, as other metals
are smelted from their ores, but without success,
and the opinion has become profound and wide-
spread among chemists that alumina could not be
reduced by carbon and heat. But this is exactly
what the Cowles process accomplishes, and by its
means the Cowles Electric Smelting and Alumin-
ium Company is enabled to supply the alloys of
aluminium with other metals at one-quarter to one-
third their former price. * As to the details of the
process, we refer to the papers of Professor Hunt
and the one read by Mr. Mabery."*
The following is the patent claim of Messrs.
Cowles : U. S. Pat. 324,658 and 324,659, August
18, 1885. Electric smelting of aluminium. To
Cowles Bros., Cleveland, Ohio. Claim: Reducing
the aluminium compound in company with a metal
in a furnace heated by electricity in presence of
* Cowles Bros. ' Pamphlet.
REDUCTION BY OTHER AGENTS THAN SODIUM. 191
carbon. The alloy of aluminium and the metal
formed is treated to separate the aluminium.
The following paper is the first official and sci-
entific account of Cowles Bros/ process, and was
read before the American Association for the Ad-
vancement of Science by Professor Charles F. Ma-
bery of the Case School of Applied Science, Cleve-
land.*
" The application of electricity to metallurgical
processes has hitherto been confined to the reduc-
tion of metals from solution, while few attempts
have been made to effect dry reductions by means
of an electric current. Some time since Eugene H.
Cowles and Alfred H. Cowles, of Cleveland, con-
ceived the idea of obtaining a continuous high
temperature on an extended scale by introducing
into the path of an electric current some material
that would afford the requisite resistance, thereby
producing a corresponding increase in the tempera-
ture. After numerous experiments, coarsely pul-
verized carbon was selected as the best means for
maintaining an invariable resistance, and at the
same time as the most available substance for the
reduction of oxides. When this material mixed
with the oxide to be reduced was made a part of
the electric circuit, enclosed in a fire-clay retort,
and subjected to the action of a current from a
powerful dynamo, not only was the oxide reduced,
* Ann Arbor Meeting, August 28, 1885.
192 ALUMINIUM.
but the temperature increased to such an extent
that the whole interior of the retort fused com-
pletely. In "other experiments lumps of lime,
sand, and corundum were fused, with a reduction
of the corresponding metal ; on cooling, the lime
formed large, well-defined crystals, the corundum
beautiful red-green and blue octahedral crystals.
Following up these results with the assistance of
Prof. Mabery, who became interested at this stage,
it was soon found that the intense heat thus pro-
duced could be utilized for the reduction of oxides
in large quantities,, and experiments were next
tried on a large scale with the current from a fifty
horse-power dynamo. For the protection of the
walls of the furnace, which were of fire-brick, a
mixture of ore and coarsely pulverized gas carbon
was made a central core, and was surrounded on
the side and bottom by fine charcoal, the current
following the lesser resistance of the core from
carbon electrodes inserted in the ends of the fur-
nace in contact with the core. The furnace was
charged by first filling it with charcoal, making a
trough in the centre, and filling this with the ore
mixture, the whole being covered with a layer of
coarse charcoal. The furnace was closed on top
with fire-brick slabs containing two or three holes
for the escape of the gaseous products of the reduc-
tion, and the whole furnace was made air tight by
luting with fire clay. Within a few minutes after
starting the dynamo, a stream of carbonic oxide
REDUCTION BY OTHER AGENTS THAN SODIUM. 193
issued through the openings, burning usually with
a flame eighteen inches high. The time required
for complete reduction was ordinarily about an
hour. Experience has already shown that alu-
minium, silicon, boron, manganese, sodium, and
potassium can be reduced from their oxides with
ease. In fact, there is no oxide that can withstand
the temperature attainable. in this furnace. Char-
coal is changed to graphite ; does this indicate
fusion ? As to wrhat can be accomplished by con-
verting enormous electrical energy into heat within
narrow limits it can only be said that it opens the
way into an extensive field of pure and applied
chemistry. It' is not difficult to conceive of
temperature limited only by the power of carbon
to resist fusion.
" Since the motive power is the chief expense in
accomplishing reductions by this method, its
commercial success is closely connected with ob-
taining power cheaply. Realizing the importance
of this point, Messrs. Cowles have purchased at
Lockport, !N". Y., a water-power where they can
utilize 1200 horse-power. An important feature
in the use of these furnaces from a commercial
standpoint is the slight technical skill required in
their manipulation. The four furnaces operated
in the experimental laboratory at Cleveland are in
charge of two young men, who six months ago
knew absolutely nothing of electricity. The pro-
ducts at present manufactured are the various
17
194 ALUMINIUM.
grades of aluminium bronze^ made from a rich
furnace product obtained by adding copper to the
charge of ore. Aluminium silver is also made ;
and a boron bronze may be prepared by the re-
duction of boracic acid in contact with copper,
while silicon bronze is made by reducing silica in
contact with copper. As commercial results may
be mentioned the production in the experimental
laboratory, which averages 50 pounds of 10 per
cent, aluminium bronze daily, which can be sup-
plied to the trade in large quantities on the basis
of $5 per pound for the aluminium contained, the
lowest market quotation of aluminium being now
$15 per pound."
Dr. T. Sterry Hunt has written and read several
papers on this furnace and process, and we extract
from them anything not mentioned in Prof. Ma-
be ry's paper.
The following paper was read before the Am.
Ins. of Mining Engineers by Dr. T. Sterry Hunt,
of Montreal : — *
" The application of electricity in the extraction
of metals has hitherto been chiefly confined to the
electrolysis of dissolved or fused compounds by
various methods. The power of electric currents
to generate intense heat in their passage through
a resisting medium has long been known, and the
late Sir Wm. Siemens thereby succeeded in melting
* Halifax Meeting, Sept, 1C, 1885.
REDUCTION BY OTHER AGENTS THAN SODIUM. 195
considerable quantities of steel. Messrs. Cowles took
a new step in the metallurgic art by making the
heat thus produced a means of reducing, in presence
of carbon, the oxides not only of the alkali metals,
but of calcium, magnesium, manganese, aluminium,
silicon, and boron, with an ease which permits the
production of these elements and their alloys with
copper and other metals on a commercial scale.
" If alumina, in the form of granular corundum,
is mixed with the carbon in the electric path,
aluminium is rapidly liberated, being in part car-
ried off with the escaping gas and in part con-
densed in the upper layer of charcoal. In this way
are obtained considerable masses of nearly pure
aluminium, and others of a crystalline compound
of the metal with carbon. When, however, some
granular copper is placed with the corundum, an
alloy of aluminium and copper is obtained, which
is probably formed in the overlying stratum, but
at the close of the operation is found in fused
masses below. In this way there is obtained, after
the current has passed an hour and a half through
the furnace, four or tive pounds of an alloy con-
taining 15 to 20 per cent, of aluminium and free
from iron. On substituting this alloy for the
copper in a second operation, an alloy with over
30 per cent, aluminium is obtained. The diffi-
culties in the way of gathering together the reduced
metal without the aid of copper promise to be
overcome at an early day, so that we may expect
196 ALUMINIUM.
a cheap production of such alloys and of the pure
metal. The present plant at Cleveland is but an
experimental one, and has been in operation only
a few months. The company will soon put in
operation at Loekport a 125 horse-power dynamo,
and nine more of equal power will be added, per-
mitting the establishment of the electric furnace
on a large scale,"
Paper read before the National Academy of
Science by Dr. Hunt: — *
uDr. Hunt showed some alloys of aluminium
with carbon and silicon, and a peculiar alloy be-
lieved to consist entirely of aluminium and nitro-
gen. As yet, the pure metal has only been
produced direct from the furnace in small lumps,
but it may be obtained by melting an alloy of
aluminium and tin with lead, when the latter
takes up the tin and separates from the aluminium,
sinking beneath it. Or, we get aluminium by sub-
liming either its alloy with carbon or with copper,
when the pure aluminium is carried over. The
maximum amount of aluminium which copper can
tolerate is 10 per cent., until we approach the
other end of the scale, when alloys with 70 to 80
per cent, of aluminium, or more, give valuable work-
able alloys. In the early experiments with the
Cowles furnace, an engine of 30 horse-power running
a dynamo yielded a daily output of 50 pounds of
* Washington Meeting, April 30, 1886.
REDUCTION BY OTHER AGENTS THAN SODIUM. 197
10 per cent, aluminium bronze. Brush has now
constructed an engine running 900 revolutions per
minute, which for every 35 horse-power developed
reduces one pound of the alloy per hour. The
expense of working is now covered by one-half
cent per horse-power per hour; thus the cost of
the alloy is about 17 cents per pound. Within the
past week, the gases given off by the furnace have
been analyzed. In the first part of the process it
is found that a large amount of nitrogen is given
off, showing that air leaks into the furnace. After
an hour and a half this gas is much diminished.
The Cowles at first used moist carbon for packing,
but have now overcome the necessity of dampen-
ing it, thereby saving the waste of heat in driving
out the water."
The latest and most complete description of the
process is a paper read by Mr. W. P. Thompson
before the Liverpool Section of the Society of
Chemical Industry.* Mr. Thompson has been
Cowles Bros.' agent in taking out their patents in
England. The paper is as follows : —
" That this invention is a new departure will be
acknowledged by every one when they learn that
chromium, titanium, silicon, aluminium, calcium,
and the other alkaline earth metals are obtained
by direct reduction of their oxides by carbon — till
* Jrnl. of the Soc. of Chcm. Industry, April 29, 1886.
198 ALUMINIUM.
a year ago almost universally considered a prac-
tical impossibility.
"Conduction of the current of the large dynamo
to the furnace and hack is accomplished by a com-
plete metallic circuit, except where it is broken by
the interposition of the carbon electrodes and the
mass of pulverized carbon in which the reduction
takes place. The circuit is of 13 copper wires,
each 0.3 inch in diameter. There is likewise in
the circuit an ampere meter, or ammeter, through
whose helix the whole current flows, indicating
the total strength of the current heing used^Cfhis
is an important element in the management of the
furnace, for, hy the position of the finger on the
dial, the furnace attendant can tell to a nicety
what is being done hy the current in the furnace.
Between the ammeter and the furnace is a resist-
ance coil of German silver kept in water, throwing
-more or less resistance into the circuit as desired.
This is a safety appliance used in changing the
current from one furnace to another, or to choke
off the current before breaking it by a switch.
"The furnace (see Figs. 12, 13, 14) is simply a
rectangular box, A, one foot wide, five feet long
inside, and fifteen inches deep, made of firebrick.
From the opposite ends through the pipes BB the
two electrodes CC pass. The electrodes are im-
mense electric-light carbons three inches in diam-
eter and thirty inches long. If larger electrodes
are required, a series this size must be used
REDUCTION BY OTHER AGENTS THAN
Fig 12. [( UNIVERSITY
Longitudinal section.
Fig. 14.
Transverse section.
instead, as so far all attempts to make larger car-
bons that will not disintegrate on becoming
200 ALUMINIUM.
incandescent have failed. The ends of the carbons
are placed within a few inches of each other in the
middle of the furnace, and the resistance coil and
ammeter are placed in the circuit. The ammeter
registers 50 to 2000 amperes. These connections
made, the furnace is ready for charging.
•"The walls of the furnace must first be pro-
tected, or the intense heat would melt the fire
brick. The question arose, what would be the
best substance to line thewalls? Finely powdered
charcoal is a poor conductor of electricity, is con-
sidered infusible and the best non-conductor of
heat of all solids. From these properties it would
seem the best material. As long as air is excluded
it will not burn. But it is found that after
usin^ pure charcoal a few times it becomes value-
less ; it retains its woody structure, as is shown in
larger pieces, but is changed to graphite, a good
conductor of electricity, and thereby tends to
diffuse the current through the lining, heating it
and the walls. The fine charcoal is therefore
washed in a solution of lime-water, and after dry-
ing, each particle is insulated by a fine coating of
lime. The bottom of the furnace is now filled
with this lining about two or three inches deep.
A sheet-iron gauge is then placed along the sides
of the electrodes, leaving about two inches between
them and the side walls, in which space more of
the charcoal is placed*. The charge J5/, consisting
of about 25 pounds of alumina, in its native form as
REDUCTION BY OTHER AGENTS THAN SODIUM. 201
corundum, 12 pounds of charcoal and carbon, and
50 pounds of granulated copper, is now placed
within the gauge and spread around the electrodes
to within a foot of each end of the furnace. In
place of granulated copper, a series of short copper
wires or bars can be placed parallel to each other
and transverse to the furnace, among the alumina
and carbon, it being found that where grains are
used they sometimes fuse together in such a way
as to short-circuit the current. After this, a bed
of charcoal, -F, the granules of which vary in size
from a chestnut to a hickory, is spread over all,
and the gauge drawn out. This coarse bed of
charcoal above the charge allows free escape of the
carbonic oxide generated in the reduction. The
charge being in place, an iron top, 6r, lined with
h're-brick, is placed over the whole furnace and
the crevices luted to prevent access of air. The
brick of the walls insulate the cover from the
current.
" Xow that the furnace is charged and the cover
luted down, it is started. The ends of the electrodes
were in the beginning placed close together, as
shown in the longitudinal section, and for this
cause the internal resistance of the furnace may be
too low for the dynamo, and cause a short circuit.
The operator, therefore, puts sufficient resistance
into the circuit, and by watching the ammeter and
now and then moving one of tfie electrodes out a trifle,
he can prevent undue short circuiting in the begin-
202 ALUMINIUM.
ning of the operation. In about ten minutes, the
copper between the electrodes has been melted and
the latter are moved far enough apart so that the
current becomes steady. The current is now in-
creased till 1300 amperes are going through,
driven by 50 volts. Carbonic oxide has already
commenced to escape through the two orifices in
the top, where it burns with a white flame. By
slight movements outwards of the electrodes during
the coming five hours, the internal resistance in
the furnace is kept constant, and at the same time
all the different parts of the charge are brought in
turn into the zone of reduction. At the close of
the run the electrodes are in the position shown in
the plan, the furnace is shut down by placing a
resistance in the circuit and then the current is
switched into another furnace charged in a similar
manner. It is found that the product is larger if
the carbons are inclined at angles of 30° to the
horizontal plane.
" This regulating of the furnace by hand is rather
costly and unsatisfactory. Several experiments
have therefore been tried to make it self-regulating,
O O '
and on January 26, 1886, a British patent was
applied for by Cowles Bros., covering an arrange-
ment for operating the electrodes by means of a
shunt circuit, electro-magnet, and vibrating arma-
ture. Moreover, if the electrodes were drawn back
and exposed to the air in their highly heated state,
they would be rapidly wasted away. To obviate
REDUCTION BY OTHER AGENTS THAN SODIUM. 203
this, Messrs. Cowles place what may be called a
stuffing box around them, consisting of a copper
box tilled with copper shot. The wires are attached
to the boxes instead of the electrodes. The hot
electrodes as they emerge from the furnace first
encounter the shot, which rapidly carry off the
heat, and by the time they emerge from the box
they are too cool to be oxidized by contact with
the air.
uXinety horse-power have been pumped into
the furnace for five hours. At the beginning of
the operation the copper first melted in the centre
of the furnace. There was no escape for the heat
continually generated, and the temperature in-
creased until the refractory corundum melted, and
being surrounded on all sides by carbon gave up its
oxygen. This oxygen, uniting with the carbon to
form carbonic oxide, has generated heat which
certainly aids in the process. The copper has had
nothing to do with the reaction, as it will take
place in its absence. Whether the reaction is due
to the intense heat or to electric action it is difficult
to say. If it be electric, it is Messrs. Cowles's im-
pression that we have here a case where electrolysis
can be accomplished by an alternating current,
although it has not been tried as yet. Were the
copper absent, the aluminium set free would now
absorb carbon and become a yellow, crystalline
carbide of aluminium ; but, instead of that, the
copper has become a boiling, seething mass, and
204 ALUMINIUM.
the bubblings of its vapors may distinctly be heard.
The vapors probably rise an inch or two, condense
and fall back, carrying with them the freed alumin-
ium. This continues till the current is taken otf
the furnace, when we have the copper charged
with 15 to 30 per cent., and in some cases as high
as 40 per cent, of its weight of aluminium, and a
little silicon. After cooling the furnace this rich
alloy is removed. A valuable property of the fine
charcoal is that the metal does not spread and run
through its interstices, but remains as a liquid mass
surrounded below arid on the sides by fine charcoal
which sustains it just as flour or other fine dust
will sustain drops of water for considerable periods,
without allowing them to sink in. The alloy is
white and brittle. This metal is then melted in
an ordinary crucible furnace, poured into large
ingots, the amount of aluminium in it determined
by analysis, again melted, and the requisite amount of
copper added to make the bronze desired.
"Two runs produce in ten hours' average work
100 pounds of white metal, from which it is esti-
mated that Cowles Bros., at Lockport, are producing
aluminium in its alloys at a cost of about forty cents
per pound. The Cowles Co. will shortly have 1200
horse-power furnaces. With a larger furnace there
is no reason why it should not be made to run con-
tinuously like the ordinary blast furnace.
" In place of the copper any non-volatile metal
may be used as a condenser to unite with any
REDUCTION BY OTHER AGENTS THAN SODIUM. 205
metal it may be desired »to reduce, provided, of
course, that the two metals are of such a nature
that they will unite at this high temperature. In
this way aluminium may be alloyed with iron,
nickel-silver, tin, or cobalt. Messrs. Cowles have
made alloys containing 50 Al and 50 Fe, 30 Al,
and 70 Cu, 25 Al and 75 ]^i. Silicon or boron
or other rare metals may be combined in the same
way, or tertiary alloys may be produced ; as, for
instance, where tire clay is reduced in presence of
copper we obtain an alloy of aluminium, silicon,
and copper. This alloy is white and brittle if it
contains over ten per cent, of aluminium and sili-
con together. With from two to six per cent, of
these two, in equal proportions, the alloy is stronger
than gun-metal, has great toughness, does not
oxidize when heated in the air, and has a fine gold
color. I hear to-day that an aluminium-silicon
bronze wire made by Cowles has shown a tensile
strength of 200,000 pounds, hitherto unprecedented
in any metal.
"As to the ores of aluminium. For Mitis cats-
ings, where iron and silicon are not prejudicial,
beauxite or various clays may be used to advantage.
For bronze making, alumina containing silica in
considerable quantities is as available as the pure
earth and is indeed superior to it." To manufacture
pure aluminium, pure alumina is necessary.
Cowles Bros, use corundum obtained from Xorthern
Georgia. (See p. 49.)
18
206 ALUMINIUM.
REDUCTION BY IRON.
The statement has been made* that aluminium
sulphide, APS3, is to be obtained from powdered
cryolite by treating it with water, which dissolves
out sodium fluoride, NaF, and the residual A12F6
being calcined with sulphide of lime, CaS, there
results A12S3 and CaF2. The A12S3 is then decom-
posed by heating to redness with iron turnings.
According to a patent given to F. Lauterborn,f
Germany, Aug. 14, 1880, if pulverized cryolite is
boiled with water, NaF is set free and A12F6
remains. Likewise, calcium fluoride, CaF2, boiled
with APC16 gives CaCP and APF6. The aluminium
fluoride by heating with sulphide of lime will be
converted into APS3. Finally, the APS3, by heat-
ing red hot with iron gives, it is claimed, metallic
aluminium.
The above are all the details of this process to
be found. See in the Appendix an experiment on
thus decomposing cryolite.
H. Niewerthij: has patented the following pro-
cess: "Ferro-silicumis mixed with APF6 in proper
proportions and the mixture submitted to a suit-
able red or melting heat by which the charge is
decomposed into volatile silicon fluoride, SiF4, iron,
and aluminium, the two latter forming an alloy.
* Chemical News, 1860.
t Dingier, 242, p. 70.
•\. Sci. Am. Suppl. Nov. 17, 1883.
REDUCTION BY OTHER AGENTS THAN SODIUM. 207
In order to obtain the valuable alloy of aluminium
and copper from this iron-aluminium alloy, the
latter is melted with metallic copper, which will
then by reason of greater affinity unite with the
aluminium, while the iron will retain but an
insignificant amount of it. On cooling the bath,
the bronze and iron separate in such a manner that
they can readily be kept apart. In place of pure
APF6, cryolite may advantageously be employed,
or A12C16 may also be used, in which case silicon
chloride volatilizes instead of the fluoride. Or,
again, pure silicon may be used with APF6, cryo-
lite, or APC16, in which case pure aluminium is
obtained."
Preparation of Aluminium and Sodium im the
Bessemer Converter.
According to the experiments of Mr. W. P.
Thompson,* sodium and aluminium may be advan-
tageously prepared by means of a Bessemer con-
verter. The same process it seems should serve
equally well for the preparation of the other
difficultly reducible metals, such as calcium, stron-
tium, barium, magnesium, etc.
Mr. "W. P. Thompsonf has taken out a patent in
England^ for the manufacture of aluminium and
similar metals, which is carried out as follows:
The inventor employs as a reducing agent iron,
* Bull, de la Soc. Chcm. de Paris, 1880, xxiv. 128.
f Idem. p. 719. \ Mar. 27, 1879. No. 2101.
208 ALUMINIUM.
either alone or conjointly with carbon or hydrogen.
The operation is effected in an apparatus similar to
a Bessemer converter, divided into two compart-
ments. In one of these compartments is placed
melted iron, "or an alloy of iron, which is made to
run into the second by turning the converter.
This last compartment has two tuyeres, one of
which serves to introduce hydrogen, while by the
other is introduced either A12C16, APF6, APC16.-
2NaCl, or Al2F6.6NaF, in liquid or gaseous state.
In presence of the hydrogen the iron takes up
chlorine or fluorine, chloride or fluoride of iron is
diseno-ao-ed, and aluminium mixed with carbon
£D O '
remains as a residue. Then this mixture of iron,
aluminium, and carbon is returned to the other
compartment where the carbon is burnt out by
means of a current of air. The mass being then
returned to the chamber of reduction, the operation
described is repeated. When almost all the iron
has been consumed, the reduction is terminated by
hydrogen alone. There is thus obtained an alloy
of iron and aluminium. (The preparation of sodium
does not require the intervention of hydrogen. A
mixture of iron with an excess of carbon and
caustic soda, N"aOH, is heated in the converter,
when the sodium distils off.* "When all the
carbon has been burnt, the iron remaining as a
residue may be converted into Bessemer steel. As
iron forms an alloy with potassium, the method
* Compare with p. 141.
REDUCTION BY OTHER AGENTS THAN SODIUM. 209
would scarcely serve for the production of that
metal.) To obtain the pure aluminium, sodium is
first prepared by the process indicated, the chlo-
ride or fluoride of aluminium is introduced into
the apparatus in the other chamber, when the
metal is reduced by the vapor of sodium. The
chambers ought to be slightly inclined, and an
agitator favors the reaction. The inventor intends
to apply his process to the manufacture of mag-
nesium, strontium, calcium, and barium.
Calvert and Johnson* made experiments on the
reduction of aluminium by iron, and the produc-
tion thereby of iron-aluminium alloys. We give
the report in their own words : —
"We shall not describe all the fruitless efforts
we made, but confine ourselves only to those which
gave satisfactory results. The first alloy we ob-
tained was by heating to a white heat for two
hours the following mixture :—
8 equivalents of A12C16 . . . 1076 parts.
40 " " iron filings . . 1120 *'
8 u " lime . . .224 "
"The lime was added to the mixture with the
view of removing the chlorine from the APC16, so
as to liberate the metal and form fusible calcium
chloride, CaCl2. Subtracting the lime from the
above proportion, we ought to have obtained an
alloy having the composition of 1 Equivalent Al
* Phil. Mag., 1855, x. 240.
18*
210 ALUMINIUM.
to 5 Equivalents of Fe, or with 9.09 per cent,
aluminium. The alloy we obtained contained 12
per cent., which leads to the formula AlFe4. This
alloy, it will be noticed, has an analogous com-
position to the one we made of iron and potas-
sium, and like it was extremely hard, and rusted
when exposed to a clamp atmosphere. Still it
could be forged and welded. We obtained a
similar alloy by adding to the above mixture some
very finely pulverized charcoal and subjecting it
to a high heat in a forge furnace for two hours.
This alloy gave on analysis 12.09 per cent.* But, in
the mass of CaCl2 and carbon remaining in the cruci-
ble there was a large amount of globules varying
in size from a pin head to a pea, as white as silver
and extremely hard, which did not rust in the air
or in hyponitric fumes. Its analysis gave 24.55
per cent, aluminium ; the formula APFe3 would
give 25 per cent. Therefore this alloy has the
same composition as A1203, iron replacing oxygen.
"We treated these globules with weak sulphuric
acid, which removed the iron and left the alumin-
ium, the globules retaining their form, and the
metal thus obtained had all the properties of the
pure aluminium.
"We have made trials with the following mix-
ture, but, although they have yielded results, still
they are not sufficiently satisfactory to describe in
* In the original paper it is given as 12.09 per cent. iron.
The inference is unavoidable that this was a misprint, but it
is not corrected in the Errata at the end of the volume.
REDUCTION BY OTHER AGENTS THAN SODIUM. 211
this paper, which is the first of a series we intend
publishing on alloys. This mixture was : —
Kaolin 1750 parts.
NaCl 12CO "
Fc 875 "
" From this we obtained a metallic mass and a
few globules which we have not yet analyzed."
Fremy: Alloys of aluminium and iron have
been prepared by Benzon by calcining a mixture
of alumina, carbon, and iron or Fe203. (See p. 214.)
Watts : E. L. Benzon* reduces aluminium by
heating alumina with the oxide of another metal,
as of copper, iron, zinc, or a mixture of alumina
with carbon and the other metal in a free state,
the materials being all finely divided and mixed
in atomic proportions, or rather with the carbon
slightly in excess.
M. Evrard,f in order to make aluminium
bronze, makes use of an aluminous pig iron. (It
is not stated how this aluminous pig iron is made.)
This is slowly heated to fusion, and copper is
added to the melted mass. Aluminium, having
more affinity for copper than for iron, abandons
the latter and combines with the copper. After
the entire mass has been well stirred, it is allowed
to cool slowly so as to permit the bronze, which
is heavier than iron, to find its way to the bottom
* Eng. Pat., 1858, No. 2753.
t Annalesdu Genie Civil, Mars, 1867, p. 189.
212 ALUMINIUM.
of the crucible. M. Evrard makes silicon bronze
in the same way by using siliceous iron.
< Eng. and Mining Journal,' May 15, 1886 : " The
iron-aluminium alloy used in the Mitis process, we
are informed by Mr. Ostberg, is made in Sweden
by the addition of clays in iron smelting, a patented
process producing alloys with 7 to 8 per cent,
aluminium very cheaply. Mr. Ostberg adds that
he purchased a small quantity of Cowles Bros.'
alloy, which gave rise to our previous unqualified
statement that he used Cowles' alloys." (See
'Mitis Castings,' Part XL).
REDUCTION WITH COPPER.
Calvert and Johnson* obtained copper alloyed
with aluminium by recourse to a similar chemical
reaction to that employed to get their iron-alu-
minium alloy. Their mixture was composed of—
20 equivalents of Cu . . . . 640 parts.
8 " " A12C16 .... 1076 "
10 " " CaO . . . . 280 "
" We mixed these substances intimately together,
and after having subjected them to a high heat for
one hour we found at the bottom of the crucible a
melted mass covered with cuprous chloride, Cu2Cl2,
and in this mass small globules, which on analysis
contained 8.47 per cent, aluminium, corresponding
to the formula —
* Phil. Mag. 1855, x. 242.
REDUCTION BY OTHER AGENTS THAN SODIUM. 213
5 equivalents of Cu . . 160 . . 91.96 per cent.
1 " " Al . . 14 . . 8.04 "
174 100.00
" We made another mixture of A12C16 and copper
in the same proportions as above, but left out the
lime. We obtained an alloy in this case also,
which contained 12.82 per cent, aluminium, corres-
ponding to the formula —
3 equivalents of Cu . . 96 . . 87.27 per cent.
1 " " Al . . 14 . . 12.73 "
110 100.00
Kerl and Stohman give the following account of
Benzon's process: "Benzon* has patented the
reduction of aluminium with copper, forming an
aluminium-copper alloy. He mixes copper, or
oxidized copper, or cupric oxide, in the finest
possible state, with fine, powdered, pure alumina
and charcoal, preferably animal charcoal. The
alumina arid copper or copper oxide are mixed in
equivalent proportions, but an excess of charcoal
is used. The mixture is put in a crucible such as
is used for melting cast steel, which is lined inside
with charcoal. The charge is covered with char-
coal, and the crucible subjected first to a tempera-
ture near the melting point of copper, until the
alumina is reduced, and then the heat is raised
high enough to molt down the alloy. In this way
can be obtained a succession of alloys, whose hard-
* Eng. Pat, 1858, No. 27C3.
214 ALUMINIUM.
ness and other qualities depend on the percentage
of aluminium in them. In order to obtain alloys
of a certain composition, it is best to produce first
an alloy of the highest attainable content of alu-
minium, to analyze it, and then melt it with the
required quantity of copper. The same process
can be used for the reduction of alumina with iron
or Fe203, only the carbon must in this case be in
greater excess, and a stronger heat kept up longer
must be used than when producing the copper-
aluminium alloy. In contact with Fe203 the
alumina is more easily reduced than with metallic
iron."
Kerl and Stohman remark that were these
methods practicable, then at once there is the
possibility of producing copper-aluminium alloys
at a low price, and, on the other hand, of easily
producing pure aluminium from the iron alloy.
According to researches conducted in the labora-
tories at Zurich and Augsburg, it was found that
the melted-down copper contained either no alu-
minium or at most a trace. (See Appendix.)
Aluminium-bronze is also made by Mr. Evrard's
process given on p. 211.
REDUCTION BY ZINC.
M. Dullo* observes that the double chloride of
aluminium and sodium, which he makes directly
* Bull, dc la Soc. Chem. 1860, v. 472.
REDUCTION BY OTHER AGENTS THAN SODIUM. 215
from clay, may be reduced by zinc. He says,
" The reduction by zinc presents no difficulties,
but it is less easy tban with sodium. An excess
of zinc should be employed, which may be got rid
of afterwards by distillation. The metal thus pre-
pared possesses all the characteristics and all the
properties of that obtained from beauxite with
sodium."
M. IS". Basset,* a chemist in Paris, has recently
patented a new process for obtaining aluminium.
If the statements are correct they are of great value.
The paper is as follows: All the metalloids and
the metals which form by double decomposition
proto-chlorides or sesqui-chlorides more fusible or
more soluble than A12C16 may reduce A12C16 or
even Al'Cr^NaCl. Thus, As, Bi, Cu, Zn, Sb, Hg,
or even Sn, or amalgam of Zn, Sb, or Sn may be
employed to reduce the single or double chloride.
The author employs zinc in preference to the others
in consequence of its low price, the facility of its
employment, its volatility, and the property which
it has of metallizing easily the aluminium as it is
set free. When metallic zinc is put in the presence
of Al2Cl6.2XaCl at 250 to 300°, zinc chloride,
ZnCl2, is formed and aluminium is set free. This
dissolves in the zinc present in excess, the ZnCl2
combines with the I^aCl, and the mass becomes
little by little pasty, then solid, while the alloy
* Le Genie Industrie], 1862, p. 152.
216 ALUMINIUM.
remains fluid. If the heat is now raised, the mass
melts anew, the zinc reduces a new portion of the
double chloride, and the excess of zinc enriches
itself in aluminium proportionately. These facts
constitute the basis of the following general pro-
cess : One equivalent of A12C16 is melted, two of
KaCl added, and when the vapors of hydrochloric
acid are dissipated, four equivalents of zinc, in
powder or grain, is introduced. The zinc melts
rapidly, and by agitation the mass of chloride
thickens and solidifies. The mass is now composed
of A12C16, NaCl, and ZnCl2, and remains in a pasty
condition on top of the fluid zinc containing alu-
minium. This pasty mass is removed, piled up in
a crucible or in a furnace, and bars of the fluid
alloy of zinc and aluminium obtained from a pre-
vious operation are placed on top of it. This is
gradually heated to bright redness, and kept there
for an hour. The melted mass is then stirred with
a rake and poured out. It is an alloy of the two
metals in pretty nearly equal proportions. This
alloy, melted with some chloride from the first
operation furnishes aluminium containing only a
small per cent, of zinc, which disappears by a new
fusion under chloride mixed with a little A12F6,
providing the temperature is raised to a white
heat and maintained till the cessation of the vapors
of zinc, air being excluded.
The metal is pure if the zinc employed contained
no foreign materials or metals. It is melted and
REDUCTION BY OTHER AGENTS THAN SODIUM. 217
cast into ingots. In case the zinc contains iron, or
even if the A1*C16 contains some, the metallic pro-
duct of the second operation may be treated with
dilute sulphuric acid to remove it. The insoluble
residue is washed and melted layer by layer with
fluorspar or cryolite and a small quantity of APC16.-
2$"aCl, intended solely to help the fusion."
Mr. Wedding* makes the following remarks on
this process : —
" It is some time since Mr. Basset established the
possibility of replacing sodium by zinc in the
manufacture of aluminium. Operating on A12C16.-
2XaCl with granulated zinc, the reduction takes
place towards 300°. The reduced aluminium dis-
solves in the excess of zinc, while the ZnCl2 formed
combines with the ]S"aCl, forming a pasty mass if
the heat is not raised. Under the action of heat
the alloy enriches itself in aluminium, because the
zinc volatilizes. The zinc retained by this alloy is
completely eliminated by fusion with Al2Cl6.2KaCl
and a little fluorspar. The temperature ought to
be pushed at last to a white heat, and maintained
till no vapor of zinc escapes, air being excluded
during the operation. These results I have con-
firmed, having submitted the experiments of Mr,
Basset to an attentive examination, and I recom-
mend its use. However, the process demands very
much precaution because of the high temperature
* Journal de Pharm. L4] iii. p. loo (1866).
19
218 ALUMINIUM,
which it necessitates. Another chemist, Mr.
Spccht, even in 1860 decomposed APC16 by zinc,
and has the same report to make — that he thinks
the process will be some time advantageously prac-
tised on a large scale."
However, this method has not succeeded in being
established in practice, probably on account of the
high temperature which is necessary to drive off
the zinc, in which operation some aluminium is
lost.
Kagensbusch,* in Leeds, makes the singular
proposition to melt clay with fluxes ; then, by add-
ing zinc or lead, to decompose it by an electrical
current and isolate an aluminium-zinc or alu-
minium-lead alloy, from which the zinc may be
volatilized or the lead cupelled.
Mr. Fred. J. Seymourf patents the reduction of
aluminium by zinc, and makes the following claim :
An improvement in extracting aluminium from
aluminous earths and ores by mixing them with
an ore of zinc, carboniferous material and a flux,
and subjecting the mixture to heat in a closed
retort, whereby the zinc is liberated, is caused to
assist in bringing or casting down the aluminium
in a metallic state, and an alloy of aluminium and
zinc is obtained.
The only information outside of the patent claims
* Eng. Pat., 1872, No. 4811.
t U. S. Pat., No. 291,631, Jan. 8, 1884.
REDUCTION BY OTHER AGENTS THAN SODIUM. 219
which I could find in regard to this process is con-
tained in the following newspaper article, which,
although wordy and indefinite, will have to be
taken in the absence of a more precise account.
"Mr. F. J. Seymour,* a well-known practical
metallurgist, late of Bridgeport, Conn., has, as the
result of several years' study, succeeded in producing
aluminium at a low cost, and by the novel furnace
just designed asserts that he can extract the metal
on a commercial basis in large quantities. Not to
go into all the technical details, which are ex-
tremely interesting to metallurgists, it is sufficient
to say that Mr. Seymour has discovered that the
close affinity existing between aluminium and zinc
can be utilized in vaporizing, capturing, and deposit-
ing the aluminium, the separation being effected
by the aid of heat in a furnace, or rather a series of
furnaces, of peculiar construction. The charge for
each furnace is zinc ore 100 parts, koalin 50, carbon
(either anthracite coal or its equivalent in hydro-
carbon gas) 125, pearl ash or its equivalent 15,
XaCl 10 ; all intimately mixed. The retorts are of
steel, 36 inches long, 12 inches diameter, sides J
inch thick. The heat necessary to produce the
result is about 2500° F., or 1400° C. Properly
handled, one furnace should make two charges in
24 to 30 hours. Four men can operate 50 retorts.
* Cleveland Letter to the ' New York Times,' April 14,
1884.
220 ALUMINIUM.
The number of retorts can be increased to several
hundred in a single system. Capitalists are already
interested in this new process, and the prospects are
that operations on an extensive scale will soon
follow. Independent investigations in the same
line in this city have resulted in the recent incor-
poration of a company for the extraction of alu-
minium by electricity. Thus far the secret of the
process has been strictly guarded, and no details
can be given."
Mr. Seymour has quite recently taken out another
patent, the claims of which are hardly reconcilable
with those of the former patent. The claim is as
follows : —
Patent to Fred. J. Seymour,* Wolcottville, Conn.,
assignor of one-half to Mr. Henry Brown, New
York. The following is the claim : u The process
of extracting aluminium from aluminous earths,
consisting in subjecting such ore or earth with an
ore of zinc, carbonaceous matter, and a flux, to
heat, in a retort; wherein the oxides of aluminium
and zinc are vaporized ; collecting and condensing
the vapors in a condenser, and afterwards subject-
ing the condensed product to heat with carbo-
naceous matter, substantially as herein described."
If Mr. Seymour can make a process work accord-
ing to the details of the above extraordinary claim,
* U. S. Pat. No. 337,996, filed March, 1885, granted March
16, 1886.
REDUCTION BY OTHER AGENTS THAN SODIUM. 221
he will certainly have a claim on the admiration
of all scientific men. The idea of vaporizing the
oxides of zinc and aluminium is certainly unique.
I wrote to Mr. Seymour, asking for further details
of his process, and if he was making any alu-
minium, but have received no further informa-
tion than has already been given.
4 The American Machinist,' August, 1886, con-
tains the statement that the American Aluminium
Company has been organized at Detroit with a
capital stock of §2,500,000 ; to use the patents of
Dr. Smith for the United States, Great Britain and
France. I was informed- by a gentleman in the
aluminium industry that this company were to
operate Mr. Seymour's zinc process.
REDUCTION BY LEAD.
Accord ing to the invention of Mr. A. E.Wilde,* of
Xotting Hill, lead or sulphide of lead, or a mixture
of the two, is melted and in a molten state poured
upon dried or burnt alum. The crucible in which
the mass is contained is then placed in a furnace
and heated, with suitable fluxes. The metal, when
poured out of the crucible, will be found to contain
aluminium. The aluminium and lead can be sub-
sequently separated from each other by any known
means, or the alloy or mixture of the two metals
* Sci. Am. Suppl., Aug. 11, 1877.
19*
222 ALUMINIUM.
can be employed for the various useful purposes for
which lead is more or less unsuited.
Kagensbusch's process, using lead, is described
on p. 218 under the reduction by zinc.
REDUCTION BY MANGANESE.
"W. Weldon,* of Burstow, Eng., claims to melt
together cryolite with CaCl2 or another non-metal-
lic chloride or sulphide, and then to reduce the
APC16 or APS3 produced with manganese, which
he claims is even powerful enough to reduce
sodium.
REDUCTION BY ELECTRICITY.
The reduction of A12C16 or APCl6.2^aCl by
sodium is the only process by which the pure
metal is now made. However, many attempts
have been made to isolate it by means of the elec-
tric current. The reduction may take place in
either the dry or wet way. The reduction of
fused APCl6.2XaCl by the battery was accidentally
discovered simultaneously by Deville in France
and Bunsen in Germany, in 1854, and is nothing
else but an application of the process already an-
nounced by Bunsen of decomposing magnesium
* Eng. Pat., 1883, No. 97. Wagner's Jahresb., 1884.
REDUCTION BY OTHER AGENTS THAN SODIUM. 223
chloride, MgCl2, by the battery. Deville's account
of the process is as follows: — *
"It appears to me impossible to obtain alumin-
ium by the battery in aqueous solutions. I should
believe this to be an impossibility if the brilliant
experiments of Mr. Bunsen in the preparation
of barium did not shake my convictions. Still
I must say that all the processes of this de-
scription which have recently been published for
the preparation of aluminium have failed to give
me good results. To prepare the bath for decom-
position in the dry way, I heated a mixture of 2
parts APC16 and 1 part NaCl, dry and pulverized,
to about 200° in a porcelain capsule. They com-
bine with disengagement of heat, and the resulting
bath is very fluid. The apparatus which I use for
the decomposition comprises a glazed porcelain
crucible, which as a precaution is placed inside a
larger one of clay. The wrhole is covered by a
porcelain cover pierced by a slit to give. passage to
a large, thick leaf of platinum, w7hich serves as the
negative electrode ; the lid has also a hole through
which is introduced, fitting closely, a well-dried
porous cylinder, the bottom of which is kept at
some distance from the inside of the porcelain
crucible. This porous vessel incloses a pencil of
retort carbon, which serves as the positive electrode.
Melted Al2Cl6.22s"aCl is poured into the porous jar
and into the crucible so as to stand at the same
* Ann. de CUem. et de Phys. [3J. 46, 452.
224
ALUMINIUM.
height iu both vessels; the whole is heated just
enough to keep the bath in fusion, and there is
passed through it the current from several Bunsen
cells, two cells being strictly sufficient. The an-
nexed diagram shows the crucibles in section.
Fig. 15.
" The aluminium deposits with some JS"aCl on
the platinum leaf; the chlorine, with a little
APC16, is disengaged in the porous jar, and forms
white fumes, which are prevented from rising by
throwing into the jar from time to time some dry,
DEDUCTION BY OTHER AGENTS THAN SODIUM. 225
pulverized XaCl. To collect the aluminium, the
platinum leaf is removed when sufficiently charged
with the saline and metallic deposit; after letting
it cool the deposit is rubbed off and the leaf placed
in its former position. The material thus detached,
melted in a porcelain crucible, and after cooling
washed with water, yields a gray, metallic powder,
which is melted under a layer of Al2Cl6.22>TaCl and
reunited into a button."
Bunsen* adopted a similar arrangement. The
porcelain crucible containing the bath of A12C16.
2XaCl kept in fusion was divided into two com-
partments in its upper part by a partition, in order
to separate the chlorine liberated from the alumin-
ium reduced. He made the two electrodes of
retort carbon. To reunite the pulverulent alumin-
ium, Bunsen melted it in a bath of Al2Cl6.2XaCl,
continually throwing in enough XaCl to keep the
temperature of the bath about the fusing point of
silver.
Deville,f without being acquainted with Bun-
sen's investigations, employed the same arrange-
ment, but he abandoned it because the retort
carbon slowly disintegrated in the bath, and a
considerable quantity of Al2Cl'.2^"aCl was lost by
the higher heat necessary to reunite the globules
of aluminium after the electrolysis. Deville also
* Pogg, 97, 648.
t Ann. de Phys. et de Chem. [3], 43, 27.
226 ALUMINIUM.
observed that by working at a higher tempera-
ture, as Bunsen has done, he obtained purer metal,
but in less quantity. The effect of the high heat
is that silicon chloride is formed and volatilizes, and
the iron which would have been reduced with the
aluminium is transformed to FeCl2 by the A12C16,
and thus the aluminium is purified of silicon and
iron.
Mierzinski makes the following practical remarks
on the use of electricity in producing aluminium :—
"An important factor which we must notice in
the present production of aluminium is the appli-
cation of electricity. On all sides the greatest
efforts are being made to apply electricity to
chemical technology ; in the future the importance
of electricity will centre on its application to reduc-
ing metals. Even in the year 1807 Davy succeeded
in decomposing caustic potash by means of a current
from a 400 element Wollaston battery. But we
now have magneto-electric and dynamo-electric
machines which are much lighter and cheaper than
they were in Davy's time. The application of
electricity for producing metals also possesses the
advantage not to be ignored, that a degree of heat
may be attained with it such as cannot be reached
by a blowpipe or regenerative gas furnace. The
highest furnace temperature attainable is 2500 to
2800° C., but long before this point is reached the
combustion becomes so languid that the loss of
heat by radiation almost equals the production of
REDUCTION BY OTHER AGENTS THAN SODIUM. 227
heat by combustion, and hinders a further elevation
of temperature. But in applying electricity, the
degree of heat attainable is theoretically unlimited.
A further advantage is that the smelting takes
place in a perfectly neutral atmosphere, the whole
operation goes on without much preparation and
under the eyes of the operator. Finally, in ordi-
nary furnaces the refractory material of the vessel
must stand a higher heat than the substance in it,
whereas by smelting in an electrical furnace the
material to be fused has a higher temperature than
the crucible itself.
" The manufacture of aluminium is effected now
either by separating out the metal itself directly
from the solutions of its salts or by reducing it
with sodium. However, in spite of numerous
attempts, sodium has not been replaced as a reduc-
ing agent. In the production of aluminium, the
making of A1203 from beauxite costs 9.7 per cent.,
making the Al2Cl6.2XaCi 33.4 per cent,, and de-
composing by sodium 56.9 per cent, of the whole
cost. The attempt to reduce alumina directly by
carbon Mr. W. Weldon considers as impossible
because he could not produce the temperature
required for the reaction to take place. Hence
appears the great importance of utilizing the
temperature attainable by the electric current.
The separation of aluminium by electrolysis is now
done only by the use of anhydrous Al2Cl8.2!N"aCl,
melting at 200° C. The anodes are made of plates
228 ALUMINIUM.
of alumina and carbon pressed together, having the
conducting wire leading through their whole
length in order to lessen the resistance as much as
possible. The metal is obtained as a granular
powder mixed with Js"aCl. Where possible, vessels
of chalk or magnesia should be used, since alu-
minium takes up silicon from siliceous crucibles
and becomes brittle."
There have been some improvements made in the
form of apparatus over those used by Bunsen and
Deville, designed to produce the metal on a com-
mercial scale. The best one is that patented in
Germany by Richard Gratzel.* He uses melting-
pots of porcelain, alumina, or aluminium, which
serve also as negative electrodes. A number of
these are placed in one furnace. The following
section shows the arrangement (Fig. 16). The
positive electrode K can be made of a mixture of
anhydrous alumina and carbon pressed into shape
and ignited. A mixture of alumina and gas-tar
answers very well ; or it can even be made of gas-
tar and gas-retort carbon. During the operation
little pieces of carbon fall from it and would con-
taminate the bath, but are kept from doing so by
the mantle (7. This isolating vessel G is perforated
around the lower part at #, so that the chlorine gas
liberated at K may escape through the tube 0',
while reducing gases can be brought into the cruci-
* D. R. Pat. No. 26,962.
REDUCTION BY OTHER AGENTS THAN SODIUM. 229
ble by the tube O2. To lessen the electrical resist-
ance and to renew the bath of chloride or fluoride,
Fig. 16.
bars of carbon, alumina, or magnesia are placed
inside the isolating mantle G.
This process is now being worked on a large
scale in Germany, being also used for producing
magnesium. There are works at Bremen and
Hamburg.
M. Duvivier* states that by passing an electric
20
* The Chemist, Aug. 1854.
230 ALUMINIUM.
current from eighty Bunsen cells through a small
piece of laminated disthene between two carbon
points, the disthene melted entirely in two or three
minutes, the elements which composed it were
partly disunited by the power of the electric cur-
rent, and some aluminium freed from its oxygen.
Several globules of the metal separated, one of
which was as white and as hard as silver.
Kagensbusch,* of Leeds, makes the singular
proposition to melt clay with fluxes, then add zinc
or a like metal, pass an electric current through
the fused mass, isolating an alloy of aluminium and
the metal, from which the foreign metal may be
removed by distillation, sublimation, or cupella-
tion.
Gaudinf reduces aluminium by a process to
which he applies the somewhat doubtful title of
economic. He melts together equal parts of cryo-
lite and NaCl, and traverses the fused mass by an
electric current. Fluorine is evolved at the positive
pole, while aluminium accumulates at the negative.
Thus far we have given the methods based on
elect rolyzing fused salts. These seem to be the
operations best suited to throwing down aluminium
in mass. The electrolysis of aqueous solutions
seems so far to have succeeded only in depositing
very thin films of metal. We will now give the
* Eng. Pat. 1872, No. 4811.
f Moniteur Scieutifique, xi. 62.
REDUCTION BY OTHER AGENTS THAN SODIUM. 231
various methods proposed for electrolyzing alu-
minium in the wet way.
Messrs. Thomas and Tilly* coat metals with
aluminium and its alloys by using, for depositing
the pure metal, a solution of freshly precipitated
alumina dissolved in boiling water containing
potassium cyanide, or a solution of freshly calcined
alum in aqueous potassium cyanide ; also from
several other liquids. Their patent covers the
deposition of the alloys of aluminium with silver,
tin, copper, iron, silver and copper, silver and tin,
etc. etc.
M. Corbelli, of Florence,f deposits aluminium
by electrolyzing a mixture of rock alum or sulphate
of alumina with CaCl2 or UaCl, in aqueous solu-
tion, the anode being mercury placed at the bottom
of the solution and connected to the battery by an
iron wire coated with insulating material and
dipping its uncovered end into the mercury. The
zinc cathode is immersed in the solution. Alu-
minium is deposited on the zinc, and the chlorine
which is liberated at the anode unites with the
mercury, forming calomel.
J. B. Thompson^ reports that he has for over
two years been depositing aluminium on iron, steel,
and other metals, and also depositing aluminium
* Eng. Pat., 1855, No. 2756.
f Eng. Pat., 1858, No. 507.
J Chem. News, xxiv. 194.
232 ALUMINIUM.
bronze of various tints, but declines to state his
process.
J. A. Jeancon* has patented a process for de-
positing aluminium from an aqueous solution of a
double salt of aluminium and potassium of specific
gravity 1.161 ; or from any solution of an alumin-
ium salt, such as sulphate, nitrate, cyanide, etc.,
concentrated to 20° B. at 50° F. He uses a battery
of four pairs of Smee's or three Bunsen's cells,
with elements arranged for intensity, and electro-
lyses the solutions at 140° F. The first solution
will decompose without an aluminium anode, but
the others require such an anode on the negative
pole. The solution must be acidulated slightly
with acid corresponding to the salt used, the tem-
perature being kept at 140° F. constantly.
M. A. Bertrandf states that he deposited alu-
minium on a plate of copper from a solution of
double chloride of aluminium and ammonia, by
using a strong current, and the deposit was capable
of receiving a brilliant polish.
C. W inkier J states that he has spent much time
and tried all methods so far proposed, and comes
to the conclusion that aluminium cannot be de-
posited by electro-deposition in the wet way.
* Annual Record of Science and Industry, 1875.
t Chera. News, xxxiv. 227.
t Journal of the Chem. Soc., x. 1134.
REDUCTION BY OTHER AGENTS THAN SODIUM. 233
Sprague* also states his inability to deposit alumin-
ium electrically from solution.
M. L. Senetf electrolyzes a saturated solution of
AP(S04)3, separated by a porous septum from a
solution of NaCl. A current is used of four
amperes. The double chloride, Al2Cl6.2NaCl, is
formed, then decomposed, and the aluminium
liberated deposited on the negative electrode.
Gerhard and Smith:): patented a process for de-
positing electrically aluminium and its alloys.
John Braun§ decomposes a solution of alum, of
specific gravity 1.03 to 1.07, at the usual tempera-
ture, using an insoluble anode. In the course of
the operation, the sulphuric acid set free is neu-
tralized by the continual addition of alkali ; and,
afterwards, to avoid the precipitation of alumina,
a non-volatile organic acid is added to the solution.
Moses Gr. Fanner) has patented an apparatus for
obtaining aluminium electrically consisting of a
series of conducting cells in the form of ladles,
each ladle having a handle of conducting material
extending upwards above the bowl of the next
succeeding ladle ; each ladle can be heated sepa-
rately from the rest ; the anodes are hung in the
ladles, being suspended from the handles of the
* Sprague's Electricity, p. 309.
f Cosmos les Mondes, Aug. 10, 1885.
\ Eng. Pat., 1884, No. 16,653.
§ German Pat., No. 28,760.
II U. S. Pat., No. 315,266, Apr. 1885.
20*
234 ALUMINIUM.
preceding ladles, the ladles themselves being the
cathodes.
Mierzinski says that the deposition of aluminium
from an aqueous solution of its salt has not yet
been accomplished, and declares Gore to have been
in error when he stated that he had covered copper
with a film of aluminium by using a feeble current
and a solution of APC16 in water.
Several years ago, the writer was in Mr. Frish-
muth's works, in Philadelphia, and observed that
he was then doing a large amount of plating, de-
positing an alloy of aluminium and nickel. Nickel
plating is known to be very hard and lasting, but
it has a dark-bluish color, not agreeable to many.
The presence of aluminium with it whitens it so
that the plating is a very close imitation of silver,
and wears much better than silver plating. He
was depositing with a twenty horse-power dynamo.
The articles were previously cleaned in a hot pot-
ash solution, and then hung in the plating bath.
I do not know the composition of his solution, he
keeps that secret, but it was green and strongly
arnmoniacal.
PART XL
WORKING IN ALUMINIUM.
MELTING ALUMINIUM.
DEVILLE : To melt aluminium it is necessary to
use an ordinary earthen crucible and no flux.
Fluxes are always useless and almost always harm-
ful. The extraordinary chemical properties of the
metal are the cause of this ; it attacks very actively
borax or glass with which one might cover it to
prevent its oxidation. Fortunately this oxidation
does not take place even at a high temperature.
When its surface has been skimmed of all impuri-
ties it does not tarnish. Aluminium is very slow
to melt, not only because its specific heat is consid-
erable, but its latent heat appears very large. It
is best to make a small fire and then wait patiently
till it melts. One can very well work with an un-
covered crucible. When it is desired to melt
pieces together, they can be united by agitating the
crucible or compressing the mass with a well-cleaned,
cylindrical bar of iron. Clippings, filings, etc., are
melted thus : Separate out first, as far as possible,
foreign metals, and to avoid their combining with
236 ALUMINIUM.
the aluminium heat the divided metal to as low
a heat as possible, just sufficient to melt it. The
oil and organic matters will burn, leaving a cinder,
which hinders the reunion of the metal if one does
not press firmly with the iron bar. The metal may
then be cast very easily, and there is found at the
bottom of the crucible a little cinder which still
contains a quantity of aluminium in globules.
These may be easily separated by rubbing in a
mortar and then passing through a sieve, which
retains the flattened globules.
Kerl & Stohman : To be able to melt well and
pour aluminium, the whole quantity of metal which
is to be melted at one time must not be put into
the crucible at once, but little by little, so increas-
ing the mass from time to time as the contents
become fully melted. The necessary knack for
attaining a good clean melt consists in dipping the
pieces which are to be melted together in benzine
before putting in the crucible. Mourey even pours
a small quantity of benzine into the crucible after
the full melting of the metal, and he recommends
the employment of benzine in the melting of all
the noble metals. Turning to the cases arising in
the employment of aluminium in the different in-
dustrial arts, one must as far as possible separate
out first the pieces which have been soldered, in
order that the newly melted aluminium may riot
be contaminated by the solder. The solder adher-
ing to these pieces can be removed by treating them
WORKING IN ALUMINIUM.
with, nitric acid, by which the aluminium is not
attacked.
Mierzinski : To melt aluminium one cannot heat
it in common clay crucibles, because it reduces sil-
icon from them, by which the metal becomes gray
and brittle. This difficulty can be removed by
lining the crucible with carbon, or better, with well-
burnt cryolite-clay. Moreover, in practice, it is
only in the rarest cases that pure aluminium is
obtained to be melted up, but, as a rule, it is al-
loyed with four to eight per cent, of silver.
CASTING ALUMINIUM.
Deville : Aluminium can be cast very easily in
metallic moulds, but better in sand for complicated
objects. The mould ought to be very dry, made of
a porous sand, and should allow free exit to the air
expelled by the metal, which is viscous when
melted. The number of vents ought to be very
large, and a long, perfectly round git should be
provided. The aluminium, heated to redness,
ought to be poured rather quickly, letting a little
melted metal remain in the git till it is full, to pro-
vide for the contraction of the metal as it solidifies.
In general, this precaution ought to be taken even
when aluminium is cast in iron ingot moulds or
moulds of any other metal. The closed ingot
moulds give the best metal for rolling or hammer-
ing. By following these precautions, castings of
238 ALUMINIUM.
great beauty may be obtained, but it is not advisa-
ble to conceal tbe fact that to be able to succeed
completely in all these various operations requires
for aluminium, as for all other metals, a special
familiarity with the material which practice alone
is able to give.
In the fusion of impure aluminium, very different
phenomena are observed according to the nature of
the foreign metal which contaminates it. Ferru-
ginous material often leaves a skeleton less fusible
and pretty rich in iron ; a liquation has taken
place, increasing the purity of the melted material.
When the aluminium contains silicon this liquation
is no longer possible, or at least it is very difficult,
and I have sometimes seen some commercial alu-
minium so siliceous that the workmen were unable
to remelt it. But the aluminium which is made
at present is much purer than that.
PURIFICATION OF ALUMINIUM.
Freeing from Slag. — Deville gives the following
information on this important subject: —
"It is of great importance not to sell any
aluminium except that which is entirely free from
the slag with which it was produced and with
which its whole mass may become impregnated.
We have tried all sorts of ways of attaining this
end, so as to obtain a metal which would not give
any fluorides or chlorides upon boiling with water,
WORKING IN ALUMINIUM. 239
or give a solution which would be precipitated by
silver nitrate. At Glaciere, we granulated the
metal by pouring it while in good fusion into
water acidulated with H2S04 ; this method par-
tially succeeded. But the process which M. Paul
Morin uses at present, and which seems to give
the best results, is yet simpler. Three or four
kilos of aluminium are melted in a plumbago cru-
cible without a lid, and kept a long time red hot
in contact with the air. Almost always acid
fumes exhale from the surface, indicating the
decomposition by air or moisture of the saline
matter impregnating the metal. The crucible
being withdrawn from the fire, a skimmer is put
into the metal. This skimmer is of cast iron ; its
surface ought not to be rough and it will not be
wetted by the aluminium in the least during the
skimming. The white and slaggy matters are
then removed, carrying away also a little metal,
and are put aside to be remelted. So, in this
purification, there is really no loss of metal. After
having thus been skimmed, the aluminium is cast
into ingots. This operation is repeated three or
four times until the metal is perfectly clean, which
is, however, not easily told by its appearance, for,
after the first fusion, the crude aluminium when
cast into ingots has a brilliancy and color such as
one would judge quite irreproachable, but the
metal would not be clean when it was worked,
and especially when polished would present a mul-
240 ALUMINIUM.
titude of little points called technically 'piqures,'
which give to its surface, especially with time, a
disagreeable look. Aluminium, pure and free
from slag, improves in color on using. It is the
contrary with the impure metal or with alumin-
ium not freed from slag. When aluminium is
submitted to a slow, corroding action, its surface
will cover itself uniformly with a white, thin
coating of alumina. However, any time that this
layer is black or the aluminium tarnishes, we may
be sure that it contains a foreign metal and that
the alteration is due to this impurity."
Watts suggests that the iron skimmer be oxi-
dized on its surface.
Freeing from Impurities. — Again Deville is the
authority, and we quote his advice on the sub-
ject :—
" A particular characteristic of the metallurgy
of aluminium is that it is necessary, in order to get
pure metal, to obtain it so at the first attempt.
When it contains silicon, I know of no way to
eliminate it, all the experiments which I have
made on the subject have had a negative result ;
simple fusion of the metal in a crucible, permitting
the separation by liquation of metals more dense,
seems rather to increase the amount of silicon than
to decrease it. When the aluminium contains iron
or copper, each fusion purifies it up to a certain
limit, and if the operation is done at a low heat
there is found at the bottom of the crucible a
WORKING IN ALUMINIUM. 241
metallic skeleton containing much more iron and
copper than the primitive alloy. At first I made
this liquation in the muffle of a cupel furnace, in
which process the access of air permitted the par-
tial oxidation of these two metals. The little lead
which aluminium may sometimes take up may
thus be easily separated. Unfortunately, the pro-
cess does not give completely satisfactory results.
It is the same in fusing impure aluminium under
a layer of potassium sulphide, K3S3; there is a
partial separation of the lead, copper, and iron.
That which has succeeded best with us is the pro-
cess which we have employed for a long time at
Glaciere, and which consists in melting the alu-
minium under nitre in an iron crucible. We have
in this way improved the quality of large quanti-
ties of aluminium. The operation is conducted as
follows: Aluminium has generally been melted
with nitre in order to purify it by means of the
strong disengagement of oxygen at a red heat, no
doubts being entertained as to the certainty of the
result. But it is necessary to take great care
when doing this in an earthen crucible. The
silica of the crucible is dissolved by the nitre, the
glass thus formed is decomposed by the aluminium,
and the siliceous aluminium thus formed is, as we
know, very oxidizable, and especially in the pres-
ence of alkalies. So, the purification of aluminium
by nitre ought to be done in a cast-iron crucible
well oxidized itself by nitre on the inside.
21
242 ALUMINIUM.
" On melting aluminium containing zinc in con-
tact with the air and at a temperature which will
volatilize the zinc, the largest part of the latter
burns and disappears as flaky oxide. To obtain a
complete separation of the two metals it is neces-
sary to heat the alloy to a high temperature in a
brasqued crucible. This experiment succeeds very
W7ell,but it is here shown that the aluminium must
oxidize slightly on its surface, for some carbon is
reduced by the aluminium from the carbonic
oxide with w?hich the crucible is filled. This
carbon thus separated is quite amorphous."
This phenomenon may not appear so extraor-
dinary if we consider the case in this way : The
aluminium is dissolved in the fluid zinc in a man-
ner strictly analogous to the aluminium dissolved
in mercury. Kow, it will be seen that alumin-
ium-amalgam decomposes easily, the mercury ap-
pearing to impart to the aluminium the ability to
combine easily with oxygen, so that .in the
amalgam aluminium is said to play the part of an
alkali metal, with which it is so closely related in
its compounds. Considering the case of the alu-
minium dissolved in melted zinc instead of in
mercury, it appears probable that the zinc imparts
in the same manner as the mercury, though not
necessarily in the same degree, the alkali charac-
teristics to the metal, causing it to oxidize even at
the expense of carbonic oxide.
Mierzinski recommends the purification with
WORKING IN ALUMINIUM. 243
nitre to be made in a crucible made of alumina or
aluminate of soda.
Gr. Bucbner* states that commercial aluminium
contains considerable quantities of silicon, which
by treatment, when melted, with hydrogen, evolves
hydrogen silicide. This does not result if arsenic
is present.
Mallet made chemically pure aluminium by treat-
ing the commercial metal with bromine, purifying
the resulting APBr6 by fractional distillation, and
then reducing it with pure sodium. By repeatedly
melting the metal upon aluminium leaf, he obtained
it chemically pure. Although this method is quite
applicable when studying the properties of the
pure metal, yet it cannot serve on an industrial
scale.
USES OF ALUMINIUM.
" Since aluminium was prepared by Devillef on a
large scale it has received numerous applications.
Its beautiful color, its lightness, its unoxidizability
in contact with air or sulphuric acid, its harmless-
ness to the health, the ease with which it may be
worked, are some of the properties which assure for
it a place among the useful metals. On account of
its very high price the first articles made of it were
those of ornament and luxury. The very first article
* Wagner's Jahresb., 1884.
t Fremy's Ency., 1883.
244 ALUMINIUM.
made of it was a baby rattle, intended for the young
Prince Imperial in 1856. Afterwards there were
made of it jewelry, medals, inlaid work, and carved
mouldings for inlaid work and rich furniture. It is
very well suited for fine jewelry by reason of its
adaptability to being cast and carved, the beautiful
reflections from a chased surface, its color, which
matches well with gold, and its absence of all odor.
Later on, the lightness of aluminium leads to its
use for telescope tubes, marine glasses, eye-glasses,
and especially sextants. In delicate physical ap-
paratus, where it is necessary to avoid the inertia
of large masses, aluminium replaces the other
metals with advantage. It is used for beams
for delicate balances and for very small weights.
There have been made of it sabre sheaths, sword
handles, and the imperial eagles for the French
army. Finally, made into fine wire, it is worked
into lace, embroidery, etc. For all these purposes
aluminium answers better than silver, for the
objects are much lighter and do not tarnish. The
resistance of aluminium to most of the agents
which attack the useful metals has led to its em-
ployment for culinary articles ; a large number of
which were seen at the London Exhibition in 1862.
But the advantages of aluminium vessels have not
yet been sufficiently comprehended, and this use
of it has at present been entirely discontinued.
Likewise, aluminium jewelry is not seen any
more; so that the metal seems reserved for little
WORKING IN ALUMINIUM. 245
more than optical and surgical instruments. But
the aluminium industry is nevertheless established
on a permanent basis and will continue, because of
the numerous applications of its alloys."
M. Dumas made a helmet of aluminium, gilded
' o
and ornamented, which weighed complete only one
and one-fifth pounds.
Aluminium leaf, beaten very thin, may be used
anywhere in place of silver leaf. It is applied in
the same manner, and is more durable.
Aluminium wire has been proposed for telegraph
lines. The conductivity of aluminium is double
that of iron, and as it is so much lighter, thinner
wire can be used. As its high price is a practical
difficulty, an alloy of iron and aluminium has been
suggested.
" One of the most likely applications of alu-
minium is probably as a material for statuettes and
small works of art of this description, especially if
the means could be found of giving to it a richer
color and appearance either by a kind of bronzing
or some alloy.
" Aluminium makes very bright reflectors, not
tarnished by the products of combustion, while the
slight bluish tinge of the metal corrects the yel-
lowish tinge of the flame. For culinary uses it is
well adapted, because of its lightness and the little
tendency it has to become corroded by any of the
liquids likely to come in contact with it. It is
necessary to observe, however, that this power of
21*
246 ALUMINIUM.
resisting the action of corroding agencies, and
more especially the atmosphere of large towns, is
exhibited only by the pure metal. Most of the
metal of commerce is very impure with iron and
silicon, not having been properly freed from slag.
Aluminium thus contaminated soon becomes tar-
nished, and much disappointment has been experi-
enced from this cause by those who have used it
for ornamental purposes. According to Deville, the
impurities just mentioned are found to the greatest
amount in the metal obtained from cryolite."
In the ' Scientific American/ vol. xii. pp. 31 and
51, is a long article on plating with a luminium,
giving complete directions for preparing articles,
solutions, etc.
A large collection of articles of aluminium was
shipped from England to Calcutta in Oct. 1883,
intended for exhibition there. The exhibit con-
sisted of wire, pens, pencil-cases, railway-carriage
fittings, locks and bolts, harness furniture in great
variety, chandeliers, cutlery, and ships' fittings,
and illustrated very well the various uses to which
the metal can be put. It is being used for the
lighter parts of such instruments as galvanometers,
etc., for suture wire, and perhaps its most promis-
ing field is for engineering, astronomical, and
optical instruments.
" Aluminium is sold as leaf in books, like gold
leaf, for decorations, at from 40 to 50 cents per
book, and is being experimented with by manu-
WORKING IN ALUMINIUM. 247
facturers of jewelry. In Germany, experiments
have been made with it as a coating for iron, to be
applied for ornamental purposes, and as an improve-
ment on tin plate. Its use is extending slowly but
surely, its cost being at present the principal
obstacle to its wider employment."*
Experiments were made in the U. S. Mint in
1865, on alloys of aluminium for coins. The
results wrere not sufficiently successful to induce
the Government to adopt the metal for that purpose.
SOLDERING ALUMINIUM.
At the time Deville wrote his book, the difficulty
of soldering aluminium properly was one of the
greatest, if not the greatest, obstacle to the employ-
ment of the metal. His views on the question may
be, therefore, very interesting ; they are as follows : —
"Aluminium may be soldered, but in a very
imperfect manner, either by means of zinc or
cadmium, or alloys of aluminium with these
metals. But a very peculiar difficulty arises here,
wre know no flux to clean the aluminium which
does not attack the solder, or which, protecting the
solder, does not attack the aluminium. There is also
an obstacle in the particular resistance of aluminium
to being wetted by the more fusible rnetals, and
on this account the solder does not run between
* Mineral Resources of the U. S. 1883-4.
248 ALUMINIUM.
and attach itself to the surfaces to be united. .M-
Christofle and M. Charriere made, in 1855, during
the Exposition, solderings with zinc or tin. But
this is a weak solder and does not make a firm
seam. MM. Tissier, after some experiments made
in my laboratory, proposed alloys of aluminium
and zinc, which did not succeed any better. How-
ever, M. Denis, of Nancy, has remarked that when-
ever the aluminium and the solder melted on its
surface are touched by a piece of zinc, the adhesion
becomes manifest very rapidly, as if a particular
electrical state was determined at the moment of
contact. But even this produces only weak solder-
ings, insufficient in most cases.
" A long time ago, M. Hulot proposed to avoid
the difficulty by previously covering the piece
with copper, then soldering the copper surfaces.
To effect this, plunge the article, or at least the
part to be soldered, into a bath of acid sulphate of
copper. Put the positive pole of a battery in com-
munication with the bath, and with the negative
pole touch the places to be covered, and the copper
is deposited very regularly. M. Mourey has suc-
ceeded in soldering aluminium by processes yet
unknown to me ; samples which I have seen looked
excellent. I hope, then, that this problem has
found, thanks to his ingenuity, a solution ; a very
important step in enlarging the employment of
aluminium."
WORKING IN ALUMINIUM. 249
Mierzinski gives the following statements about
M. Mourey's solder: —
" Mourey, who first made a practicable solder
for aluminium, used two kinds of solder, soft and
hard. The first was used for the usual soldering
up of flasks or pieces of metal. He made solders
of five different alloys, the composition of which
were as given in the table below : —
I. II. III. TV. V.
Al ... 20 15 12 8 6
Zn ... 80 85 88 92 94
These solders have varying melting points, and
thus there results the hard and soft solders. One
can take a soft solder, as IV., for brazing, and one
like II. for ordinary soldering."*
Schwarzf improved these solders by adding
copper to the alloy. His solders have the follow-
ing composition : —
I. II. III. IV. V.
Al ... 12 9 7 6 4
Cu ... 8 6 5 4 2
Zn ... 80 85 88 90 94
MoureyJ recommends improved solders of some-
what similar composition. They are : —
I.
II.
III.
IV.
V.
VI.
VII.
Al . . .
30
20
12
9
7
6
4
Cu . .
20
15
8
...
...
...
2
Brass .
...
...
...
6
5
4
...
Zn . . .
50
65
80
85
88
90
94
* It is usual to employ hard solder for brazing, and No. II.
would be harder than No. IV.— J. W. R.
t Dingier, 157, 445. \ Dingier, 166, 205.
250 ALUMINIUM.
Col. "Wm. Frishmuth* recommends a solder con-
taining : —
Al . . . . . . . .20
Cu 10
Zn 30
Sn 60
Ag 10
Col. Frishmuthf states that the solder just given
is used for fine ornamental work , while for lower-
grade work he uses the following : —
I. n. in.
Sn .... 95 97 98-99
Bi .... 5 3 2-1
Frishmuth recommends for a flux, in all cases,
either paraffin, stearin, vaseHn, copaiva balsam, or
benzine. In the solder for fine work, if aluminium
is used in larger quantity than recommended, the
solder becomes brittle.
Kerl and Stohman give the following practical
observations on this subject:—
" At first, the soldering of aluminium appeared
impossible. But Ph. Mourey, a gold and silver
worker in Paris, invented a new method by which
he could solder any kind of object of this metal.
The following are his receipts:—
" There are needed, according to the objects to be
soldered, five different solders, which are composed
of aluminium, copper, and zinc, in different propor-
tions : —
* Teclmiker, vi. 249. f Wagner's Jahresb., 1884.
WORKING IN ALUMINIUM. 251
I. II. III. IV. V.
Al. . . 12 9 7 6 4
Cu. . . 8 6 5 4 2
Zn . . . 80 85 88 90 94
"To make the solder, first pat the copper in the
crucible. When it is melted, then add the alu-
minium in three or four portions, thereby some-
what cooling the melted mass. When both metals
are melted, the mass is stirred with a small iron
rod, and then the required quantity of zinc added,
free from iron, and as clean as possible. It melts
very rapidly. The alloy is then stirred briskly
with an iron rod for a time, some fat or benzine
being meanwhile put in the crucible to prevent
contact of the metal with air and oxidation of the
zinc. Finally the whole is poured out into an in-
got mould previously rubbed with benzine. After
the addition of zinc, the operation must be finished
very rapidly, because the latter will volatilize and
hum out. As soon as the zinc is melted, the cru-
cible is taken out of the fire.
"The separate pieces of metal to be soldered
together are first well cleaned, then made some-
what rough with a file at the place of juncture,
and the appropriate solder put on it in pieces about
the size of millet grains. The objects are laid on
some hot charcoal, and the melting of the solder
effected by a blast lamp or a Rochemont turpentine-
oil lamp. During the melting of the solder, it is
rubbed with a little soldering iron of pure alumin-
252 ALUMINIUM.
ium. The soldering iron of pure aluminium is
essentially a necessity for the success of the opera-
tion, since an iron of any other metal will allo}7
with the metals composing the solder, while the
melted solder does not stick to the iron made of
aluminium.
" The method just described differs from the one
described by Mourey in so far that he used, at first,
alloys of aluminium and zinc only, with no copper.
He used one of the more fusible alloys to first unite
the pieces, and then used a less fusible one to finish
with. In order to avoid the oxidation of the sol-
der he added while using the hard solder, which
must be worked with a hotter iron, a quantity of
copaiva balsam and turpentine, which acts just as
borax in working silver. With these new solders
of aluminium, copper, and zinc the process is much
simpler, the work is done wTith one solder and the
moistening with balsam is unnecessary. The sol-
derings may be done so perfectly that plates soldered
together never break at the joint when bent back
and forth, but always give way in other places ;
which is a result not always possible in the best
soldering of plates of silver."
Bell Bros, used to operate the works at N"ewcas-
tle-on-Tyne, and their description may contain a
few points not yet brought forward : — *
"In order to unite pieces of aluminium, small
* Chem. News, iv. 81.
WORKING IN ALUMINIUM. . 253
tools of the same metal are used, which facilitate
at the same time the fusion of the solder and its
adhesion to the previously prepared surfaces. Tools
of copper or brass must be strictly avoided, as they
would form colored alloys with the aluminium and
the solder. The use of the little tools of alumin-
ium is an art which the workman must acquire by
practice. At the moment of fusion the work needs
the application of friction, as the solder suddenly
melts very completely. In soldering it is well to
have both hands free and to use only the foot for
the blowing apparatus. The solders used are of
aluminium, copper, and zinc. (See the ones given
by Kerl & Stohman, p. 250.) No. IY. is the one
generally preferred, particularly for small objects.
In order to make the solder, the copper is first
melted, the aluminium added, and the whole
stirred with an unpolished iron rod, just as it
comes from the forge, adding also a little tallow.
The zinc is then added, avoiding too much heat,
which would drive it off. In soldering, also, too
high a heat should be avoided for the same reason.
VENEERING WITH ALUMINIUM.
Deville is the first writer to make mention of
this art : —
" M. Sevrard succeeded in 1854 in plating alumin-
ium on copper and brass with great perfection.
The two metallic surfaces being prepared in the
22
254 ALUMINIUM.
ordinary manner and well scoured with sand, they
are placed one on the other and held tightly be-
tween two iron plates. The packet is then heated
to dark redness, at which temperature it is strongly
compressed. The veneer becomes very firmly at-
tached, and sheets of it may be beaten out. I have
a specimen of such work perfectly preserved. The
delicate point of the operation is to just heat the
packet to that point that the adherence may be
produced without fusing the aluminium, for when
it is not heated quite near to this fusing point, the
adherence is incomplete. Experiments of this
kind with copper and aluminium foil did not suc-
ceed, for as soon as any adherence manifested itself
the two metals combined and the foil disappeared
into the copper. In an operation made at too low a
temperature, the two metals, as they do not behave
similarly on rolling, become detached after a few
passes through the rolls. Since then, the experi-
ments in veneering aluminium on copper, with or
without the intervention of silver, have succeeded
very well."
The only other article to be found on this subject
is Dr. Clemens Winckler's paper, from which we
extract the following : — *
uThe question demands attention whether it is
not possible to coat certain metals and alloys writh
aluminium, and thereby impart to them, superfi-
* Industrie Blatter, 1873.
WORKING IN ALUMINIUM. 255
cially at least, the advantageous properties of that
metal. The present high price of the metal does
not stand in its way for this purpose ; and it only
remains now to decide whether it is practicable to
coat our common metals, iron, copper, etc., with it.
The question must at present be answered in the
negative. Two methods can be used for covering
one metal with another, galvanoplasty and plating
or veneering. The separation of aluminium by
the galvanic current succeeds only by the use of a
bath of molten anhydrous Al2Cl6.2^N"aCl, melting
at 165° C. (329° F.), but the metal is deposited as a
non-coherent powder, mixed with ISTaCl, and there-
fore the object of plating is not attained in this way.
Ko one has yet been able to throw down aluminium
in a metallic state from aqueous solution, and it was
an error when Grore stated that he had coated cop-
per with aluminium by means of a solution of A12C16
in water and a weak galvanic current. Concerning
the coating of metals by the so-called plating
method, it is indeed, according to my own experi-
ence, possible to a certain degree, but the product .
is entirely useless, every plating requiring an incip-
ient fusing of both metals and their final intimate
union by rolling. The ductility of aluminium is,
however, greatly injured by even a slight admixture
with other metals ; iron makes it brittle and copper,
in small per cent, makes it fragile as glass. If now
it were possible in any way to fuse a coating of
aluminium upon another metal, there would be
256 ALUMINIUM.
formed an intermediate alloy between the two
metals from which all ductility would be gone and
which would crumble to powder under the pressure
of the rolls, thus separating the aluminium surface
from the metal beneath. But even if it were pos-
sible in this way to coat a metal with a thin plate,
it is still doubtful if anything would be attained
thereby. For, while compact aluminium resists
oxidizing and sulphurizing agencies, the divided
metal does not. In powder or leaves aluminium is
readily oxidized, as is shown by its amalgam be-
coming heated in the air and quickly forming alu-
mina. In the form of a coating upon other metals
it must necessarily be in a somewhat finely divided
state, and hence would probably lose its durability."
GILDING AND SILVERING ALUMINIUM.
Deville says: "The gilding and silvering of
aluminium by electricity is very difficult to do
satisfactorily and obtain the desirable solidity. M.
Paul Morin and I have often tried it by using a
bath of acid sulphide of gold or of nitrate of silver
with an excess of sulphurous acid. Our success
has only been partial. However, M. Mourey, who
has already rendered great services in galvano-
plasty, gilds and silvers the aluminium of com-
merce with a surprising perfection considering the
little time he has had to study the question. I
also know that Mr. Christofle has gilded it, but I
WORKING IN ALUMINIUM. 257
am entirely ignorant of the methods employed by
these gentlemen."
Watts's Dictionary : " Eight grammes of gold are
dissolved in aqua regia, the solution diluted with
water and left to digest twenty-four hours with an
excess of lime. The precipitate, with the lime, is
well washed, and then treated with a solution ot
twenty grammes of hyposulphate of soda. The
liquid resulting serves for the gilding of aluminium
without the aid of heat or electricity, the metal
being simply immersed in it after being previously
well cleaned by the successive use of caustic potash,
nitric acid, and pure water."
Kerl and 8 tohmau : " Gilding and silvering
aluminium galvanically does not offer the least
difficulty. One can, by using a proper ground,
coat it with silver and gold in six different colors,
by employing the correct combination, such as
shining or matt gold and silver or lead gray."
22*
PART XII.
ALLOYS OF ALUMINIUM.
General Remark. — Mierzinski : —
"Aluminium unites easily with most metals, the
combination being usually accompanied by a lively
disengagement of heat. Quite homogeneous alloys
can be made, which for the most part are easily
worked and have important applications. The
alloys in general become harder the greater the
proportion of aluminium, and become brittle if this
proportion passes a certain limit, which with gold
and copper is very low. On addition of a larger
amount of aluminium than this limit allows, gold
and copper become whiter, and at last entirely lose
their color. The addition of other metals to alu-
minium imparts to it the same new properties. It
becomes brighter and somewhat harder, but, united
with small quantities of zinc, tin, gold, or silver,
remains malleable. Iron and copper impart to it
no specially prejudicial qualities, if they are not
present in too large quantities. The alloys most
frequently used are those of copper, silver, and tin.
These owe their numerous uses to their fine color,
their resistance to most chemical agents, and the
facility with which they may be worked."
ALLOYS OF ALUMINIUM. 259
ALUMINIUM AND SILICON.
Tissier: "As Deville has observed, silicon is far
from injurious to the malleability of aluminium,
the latter bearing it much as iron and copper do.
We have had occasion to analyze a specimen of
aluminium, which, although it worked with diffi-
culty, was yet employed to make various objects,
and yet, attacked by HC1, it left an insoluble resi-
due of no less than 15.67 per cent. But, even
admitting that this residue still retained some alu-
o
minium with the silicon, we think that there was
at least 10 per cent, of the latter in this specimen."
Deville : " Any siliceous material whatever, put
in contact with aluminium at a high temperature,
is always decomposed ; and if the metal is in excess
there is formed an alloy or a combination of silicon
and aluminium in which the two bodies may be
united in almost any proportions. Glass, clay, and
the earth of crucibles act in this way. However,
aluminium may be melted in glassware or earthen
crucibles without the least contamination of the
metal if there is no contact between the metal and
the material ; the aluminium will not wet the
crucible if put into it alone. But, the moment that
any flux whatever facilitates immediate contact,
even sodium chloride does this, the reaction begins
to take place, and the metal obtained is always
more or less siliceous. It is for this reason that I
have prescribed in melting aluminium not to add
260 ALUMINIUM.
any kind of flux, even when the flux would not be
attacked by the metal. Among the fusible ma-
terials which facilitate the me] ting of aluminium,
it is necessary to remark of the fluorides that they
attack the siliceous materials of the crucible, dis-
solving them with* great energy, and then the
siliceous materials thus brought into solution are
decomposed by the aluminium with quite remark-
able facility. Aluminium charged with silicon
presents quite different qualities according to the
proportion of the alloy. When the aluminium is
in large excess, there is obtained what I have called
the ' cast-iron' state of aluminium, by means of which
I discovered crystallized silicon in 1854. This
4 cast' aluminium, gray and brittle, contains accord-
ing to my analysis 10.3 per cent, of silicon and
traces of iron. When siliceous aluminium is at-
tacked by hydrochloric acid, the hydrogen which
it disengages has an infected odor, which I formerly
attributed to the presence of a hydrocarbon, but
which we now know is due to hydrogen silicide, Sill4,
thanks to the fine experiments of MM. Wohler
and Buff. It is by the production of this gas that
may be explained the iron smell which is given
out by aluminium more or less contaminated with
silicon. But aluminium may absorb much larger
proportions of silicon, for, on treating fluo-silicate
of potash with aluminium, M. Wohler obtained a
material still metallic containing about 70 per cent,
of silicon, sometimes occurring as easily separable
ALLOYS OF ALUMINIUM. 261
crystals. Since I had the occasion in a work which
I published on silicon to examine a large number
of these combinations, I found that they were much
more alterable than pure aluminium or silicon,
without doubt because of the affinity which exists
between silica and alumina. I have, therefore,
dwelt on and tried to explain the importance
of this point in obtaining perfectly pure alumin-
ium. I should say, in addition, that the metal
now sold in commerce may contain either iron or
silicon, according to the method of preparation.
These two impurities are hurtful to most of the
qualities of the aluminium, and everything ought
to be done to avoid their presence."
ALUMINIUM AND MERCURY.
Deville : " Mercury is not able to unite with
aluminium. Experiments of this nature which I
have made myself, and which Mr. Wollaston has
confirmed, prove it most clearly."
Watts : " According to Caillet, aluminium may
be amalgamated by the action of ammonium or
sodium amalgam, with water; also when it is con-
nected with the negative pole of a voltaic battery
and dipped into the mercury moistened with acid-
ulated water, or into a solution of mercuric nitrate.
Tipsier* confirms this statement respecting the
* Compt. Rend., xlix. 56.
262 ALUMINIUM.
battery method, and adds that if the aluminium
foil is not very thick it becomes amalgamated
throughout and very brittle." Tissier also finds
that aluminium may be made to unite with mer-
cury merely by the intervention of a solution of
caustic potash or soda, without the intervention of
the battery. If the surface of the metal be well
cleaned, or moistened with the alkaline solution, it
is immediately melted by the mercury, and a shin-
ing amalgam forms on its surface. The amalgam
of aluminium instantly loses its lustre when ex-
posed to the air, becoming heated and rapidly
converted into alumina and mercury. It decom-
poses water with evolution of hydrogen and forma-
tion of alumina and mercury. Nitric acid attacks
it with violence.
Watts (First Supplement) states that aluminium
amalgam may be formed either by bringing the
aluminium in contact with mercury containing a
small quantity of sodium, or by Joules's method of
electrolyzing the solution of an aluminium salt,
with mercury for the negative pole ;* but the best
method is to heat the two metals together in a gas
which does not act on either of them. To do this,
a piece of aluminium foil is placed at the bottom
of a thick-walled test-tube, and well-dried mercury
is poured on it, the tube having been previously
drawn out at the middle to prevent the foil rising
* Chem. Gazette, 1850, p. 339.
ALLOYS OF ALUMINIUM. 263
to the surface. The air is then expelled by a
stream of carbonic acid gas and the tube is heated,
without interrupting the current of gas, till the
metal is all dissolved.
Aluminium amalgam decomposes in contact
with air or water more quickly than sodium amal-
gam. When a few drops of an amalgam contain-
ing but a small proportion of aluminium are left
in contact with moist air, gelatinous, opalescent
excrescences of pure hydrated alumina are seen to
form on their surfaces, exhibiting both in their
form and mode of growth considerable resemblance
to the so-called Pharoah's serpents. This hydrated
alumina is perfectly soluble in acids and alkalies.
Water has the same effect as moist air. Watts, in
vol. viii., states that aluminium oxidizes when
its surface is rubbed with a piece of soft leather
impregnated with mercury. The rubbed surface
becomes warm, and in a few seconds whitish ex-
crescences appear, consisting of pure alumina.
The presence of mercury appears necessary to
produce the result.
Fremy says that Tissier has proven that alumin-
ium previously contaminated with caustic potash
or soda combines easily with mercury. The alloy
which results is very brittle, the aluminium in it
decomposes water, oxidizes easily in the air, and
behaves as a metal of the alkaline earths.
Gmelin* states that potassium amalgam intro-
* Hand Book, vi. 3.
264 ALUMINIUM.
duced into a hole bored in a crystal of alum
immediately acquires a rotary motion, which lasts
sometimes half an hour. At the same time, it
takes up a considerable quantity of aluminium and
becomes more viscid.
ALUMINIUM AND COPPER.
Tissier Bros., 1858 : " Just as copper increases
the hardness of aluminium, so aluminiu'm in small
proportions increases the hardness of copper. How-
ever, aluminium does not injure its malleability,
but makes it susceptible of taking a beautiful
polish, and, according to the proportions, varies its
color from red gold to pale yellow. These facts
were announced some time back by Dr. Percy, in
England, who made the alloy by introducing
copper into the mixture of cryolite and sodium
which he was reducing. We have made large
quantities of these alloys, and we may say that
they leave nothing to be desired in regard to lustre
or color to make them perfect imitations of gold.
They alter much less by successive fusions than
the alloys of copper with zinc and tin employed
for the same object. A ten per cent aluminium
alloy was harder than our gold coin, took a fine
polish by burnishing, and had the color of pale
jeweller's gold ; it could be forged and worked the
same as copper. The five per cent, aluminium
alloy was less hard than the preceding, but, like
ALLOYS OF ALUMINIUM. 265
it, takes a fine polish, and in tint approaches
nearly to pure gold. The twenty per cent, alumin-
ium alloy much resembles bismuth, having a
whitish-yellow tint. This alloy crystallizes in
large leaves and pulverizes in the mortar like bis-
muth or antimony. Alloys with five to ten per
cent, of aluminium may have their color changed
at will, either by leaving in nitric acid, which
takes away the copper and leaves the aluminium,
or in hydrochloric, which leaves the copper. The
resistance, hardness, and elasticity, which are
communicated to copper by introducing small
quantities of aluminium, will certainly make these
important industrial alloys."
Deville, 1859: "The aluminium and copper
alloys with two to three per cent, aluminium are
used by M. Christofle, who employs them for large
castings of objects of art. They are harder than
aluminium, and work well under the burin and
chisel. The alloy with ten per cent, aluminium
had its useful properties first described by M.
Debray. It is very hard, can be beaten out cold,
but with remarkable perfection when hot, and may
be well compared to iron, which it resembles in all
these physical properties. It is also very ductile.
This ten per cent, aluminium alloy is usually
known as aluminium bronze. It behaves as a true
alloy, and, in consequence, will not liquate into
different combinations. It is formed of —
23
266 ALUMINIUM.
9 equivalents of Cu . . . 275 9
1 " " Al . . . 28 1
303 10
This is proven by the fact that, when in making
the alloy the pure copper is in the crucible and a
bar of aluminium is added, the combination takes
place with such disengagement of heat that if the
crucible is not of good quality it will be fused, for
the whole becomes white hot.
" The color of the ingot of bronze is exactly that
of c green gold,' an alloy of gold and silver. The
bronze receives a beautiful polish, being comparable
in this regard only to steel. Its chemical proper-
ties do not differ much from those of most of the
allo3rs of copper. However, in numerous experi-
ments, we have noticed that it resists most chemical
agents much better than these, especially sea-water
and sulphuretted hydrogen. Its tenacity is equal
to that of steel. M. Lechatelier made the follow-
ing determinations on the metal cast into cylinders:
Per cent, of Diarn. of
aluminium. cylinder.
10 -10.0m. m.
Breaking strain.
4627 kilos.
Strength per
sq. m. m.
58.36 kilos.
10
10.1 "
4432 "
55.35 "
8
10.1 "
2657 "
33.18 "
5
10.1 "
2582 "
32.20 "
5
10.1 u
2517 "
31.43 "
French wrought iron . . 35.00 "
" A. Gordon made some experiments recently, in
which the strength of the aluminium bronze which
ALLOYS OF ALUMINIUM. 267
he tested was 84.00 kilos per square millimetre.
I made the test on some wire, and the result I
reached was 85.00 kilos ; under the same condi-
tions iron gave 60.00 and best steel 90.00 kilos.
According to experiments as to its wear as journal
boxes, it is found to wear away less than any other
journal metal yet tried.
" Its malleability is almost perfect, as is seen by
the following report of M. Boudaret, a practical
engineer: First, aluminium bronze is malleable at
all temperatures, from bright red to cold ; second,
it is perfectly malleable at red heat, breaking less
and elongating more than pure copper ; third, it is
hard to roll in the cold, after several passes it
ceases to elongate and must then be annealed very
often or it will break quickly; fourth, it results
from the foregoing that it is best to roll it at as
high a heat as possible below fusion ; fifth, anneal-
ing and tempering render it softer than simple
annealing. If after having annealed at bright red
heat it is let cool in still air to redness arid then
plunged into cold water, it is ductile and malleable
enough in the cold to stand all industrial working."
Mierzinski, 1885: "Two points are to be at-
tended to in making aluminium bronze. First, a
very pure copper must be used, the best is that
electrically deposited, but it generally costs too
much. The next best is the Lake Superior brand.
The usual commercial copper gives all sorts of poor
results, owing to the antimony, arsenic, tin, zinc,
268 ALUMINIUM.
or iron contaminating it. The bronze loses by being
alloyed with zinc or tin. Second, the alloy must
be remelted two or three times to remove its brittle-
ness. In all probability, the percentage of alu-
minium increases by remelting. The usual alloys
are those with 1, 2, 5, and 10 per cent, aluminium.
The 5 per cent bronze is golden in color, polishes
well, casts beautifully, is very malleable cold or
hot, and has great strength, especially after ham-
mering ; its defect is that it easily oxidizes or
tarnishes. The 7.5 per cent, bronze is to be recom-
mended as superior to the 5 per cent. ; it has a
peculiar greenish-gold color, which makes it very
suitable for decoration. All these good qualities
are possessed by the 10 per cent, bronze. It is
bright golden, keeps its polish in the air, may be
easily engraved, shows an elasticity much greater
than steel, and can be soldered with hard solder.
It gives good castings of all sizes and runs in sand
moulds very uniformly. Thin castings come out
very sharp, but if a casting is thin and suddenly
thickens, small offshoots must be made at the
thick place into which the rnetal can run and then
soak back into the casting as it cools and shrinks,
thus avoiding cavities by shrinkage at the thick
part. Its sp. gr. is 7.689, that of soft iron. Its
strength, when cast, is between that of iron and
steel ; but when hammered it is equal to best steel.
It may be forged at about the same heat as cast
steel, and then hammered until it is almost cold
ALLOYS OF ALUMINIUM. 269
without breaking or ripping. Tempering makes
it soft and malleable. It does not foul a file, and
may be easily drawn into wire. Any part of a
machine which is usually made of steel can be re-
placed by this bronze. As a solder for it, Hulot uses
an alloy of the usual half-and-half lead-tin solder
with 12.5, 25, or 50 per cent of zinc amalgam."
Fremy : " By the addition of a small amount of
copper, aluminium becomes hard, brittle, and takes
a bluish-white color. The alloy with 5 per cent,
aluminium is very malleable, but if over 10 per
cent. Al is present the alloy cannot be used.
The 10 per cent, bronze is now replacing ordinary
bronze in the manufacture of articles which are to
stand great resistance, such as axle bearings,
weavers' shuttles, etc. Reflectors are also made of it,
for the smoke of oil, like illuminating gas, does not
tarnish it. By whatever method these bronzes are
made, they are at first very brittle, but by a series
of successive fusions and solidifications they may be
made to acquire the necessary solidity and tenacity."
Kerl and Stohman : "Most of the copper-alu-
minium alloys are very brittle and easily oxidized.
Only the 5 to 10 per cent, aluminium alloys are
fixed, forgeable, tenacious, and of fine color.
Alloys with much aluminium and little copper are
not forgeable, and are bluish or grayish-white.
AVith 60 to 70 per cent, aluminium they are very
brittle, glass hard, and beautifully crystalline.
23*
270 ALUMINIUM.
With 50 per cent, the alloy is quite soft, but under
30 per cent, of aluminium the hardness returns."
4 Chemical News,' vii. p. 220, contains a long
paper on testing aluminium bronze (10 per cent.)
as to its suitability for the construction of astro-
nomical and philosophical instruments, the work
of an English Royal Engineer. He concludes his
observations with these words : " It appears from
these experiments that the 10 per cent, bronze is
far superior, not in one or in some but in every
respect, to any metal hitherto used for these instru-
ments. Its sp. gr. is 7.689, strength 73,185 pounds
per square inch, to that of gun metal 35,000 ; it is
malleable almost to its melting point, and can be
soldered with either brass or silver solder.'7
' Chemical News,' v. p. 138, contains a number
of experiments on the relative strengths of these
alloys. The results are as follows, the numbers
expressing the results being merely relative :—
Strength.
Ordinary gun metal, 11 per cent tin and
89 per cent, copper . . . . . .10
Copper, with 10 per cent, aluminium . . .19
Drawn copper- wire ...... 7
Drawn brass-wire . . . . . .8
( Cu Sn Al
I 96 4 0 . . . .4
Tertiary alloys <| 96 4 l ^ _ w
( 96 4 2 . . . .16
Bell Bros., Newcastle, give the specific gravity
of the aluminium bronzes as being — •
ALLOYS OF ALUMINIUM. 271
3 per cent, aluminium . . . 8.091
4 " " ... 8.621
5 " " ... 8.369
10 " " , . 7.689
' Wagner's Jahresb.' vol. x., contains a long article
on aluminium bronze, ten per cent., most of the
facts in which have been already given. We may
note that the melting-point of this alloy is there
stated as about 650°.
Bernard S. Procter,* after describing thirty-one
experiments comparing aluminium bronze and
brass, sums up the conclusions as follows : —
" From the above experiments it appears that
aluminium bronze has a little advantage over ordi-
nary brass in power to withstand corrosion, and its
surface, when tarnished, is more easily cleaned.
This should give it general preference where cost
of material is not an important consideration, es-
pecially if strength, lightness, and durability are
at the same time desirable. It is out of my power
to say anything about its fitness for delicate ma-
chinery, except that its chemical examination has
revealed nothing which can detract from the pre-
ference its mechanical superiority should give it.
Being so much less acted on by ammonia and coal-
gas suggests its suitability for chemical scales,
weights, scoops, etc. Its resistance to the action of
the weather and the ease with which tarnish is.
removed render it especially applicable for door-
* Chem. News, 1861, vol. iv. p. 59.
272 ALUMINIUM.
plates, bell-handles, etc. Its mechanical strength
and chemical inactivity together recommend it for
hinges exposed to the weather. In experiments 18,
22, etc., the tendency of brass to corrode on the
edges and at any roughness on its surface will be
observed, while the bronze is free from this defect.
In several cases the bronze seemed to be more
quickly covered with a slight tarnish which did
not increase perceptibly, probably the tarnish act-
ing as a protection to the metal ; but the brass,
though less rapidly discolored, continued to be
corroded and apparently with increased speed as
the action was continued. The bronze is more
easily cleaned. For culinary vessels its superiority
to metals now in use appears questionable. Vari-
ous philosophical instruments are among the pur-
poses for which the use of the bronze appears
advantageous. Undoubtedly, the great obstacle to
its extensive application is its high price, resulting
partly from the difficulty of getting sufficiently
pure copper, the presence of a small amount of iron
being very prejudicial." The author states that he
wrote the article with a home-made pen of alumin-
ium bronze, and suggests that it is well worthy of
the attention of pen-makers.
Thurston* says: "The ten per cent, bronze has
a tenacity of about 100,000 pounds, compressive
strength 130,000 pounds, and its ductility and
* Materials for Engineering.
ALLOYS OF ALUMINIUM. 273
toughness are such that it does not even crack
when distorted by this load. It is so ductile and
malleable that it can be drawn down under a ham-
mer to the fineness of a cambric needle. It works
well, casts well, holds a fine surface under the tool,
and when exposed to the weather it is in every
respect considered the best bronze yet known. Its
high cost alone has prevented its extensive use in
the arts. The alloys are very uniform in character.
Even one per cent, of aluminium added to copper
causes a considerable increase in ductility, increases
its fusibility, and enables it to cast well ; two per
cent, gives a mixture used for castings which are
to be worked with a chisel. It is softened by sud-
den cooling from a red heat. Its coefficient of ex-
pansion is small at ordinary temperatures. It has
great elasticity when made into springs."
Guettier makes the following remarks : — *
" Mr. Strange's experiments in regard to the
relative rigidity of brass, ordinary bronze, and alu-
minium bronze showed that the latter was about
forty times as rigid as soft brass and three times
as rigid as ordinary bronze. Under the tool, alumin-
ium bronze produces long and resisting chips, and
although not entirely unoxidizable, it is not so
easily tarnished by air as brass, bronze, or steel."
Knight :f "Aluminium bronze is more difficult
* Metallic Alloys, by Guettier.
f American Mechanical Dictionary.
274 ALUMINIUM.
to cut than brass, but cuts very smooth and clean.
If less costly it would replace red and yellow brass.
In contact with fatty matters or juice of fruit, no
soluble metallic salt is formed, which highly recom-
mends it for various articles of table use."
Cowles Bros.* thus describe the alloys of alumin-
ium and copper which they make :—
" In England the Aluminium Crown Metal Co.
has for the past three or four years been turning
out large quantities of aluminium alloys based on
the price of $14.60 per pound for the aluminium
in them. Even at the high prices charged, these
Webster alloys have attained a great popularity,
and are replacing German silver, brass, bronze, etc.
Aluminium added to any of the common alloys,
such as brass, German silver, or Britannia metal,
adds greatly to all their desirable qualities. Alu-
minium bronze cannot only be used in all places
where brass or bronze are now used, but it will
likewise soon supersede iron and steel in many
places; as for artillery. The maximum standard
of strength demanded by the British and German
governments in their wrought-steel guns, which
cost from 50 cents to $1 per pound, is at present
70,000 pounds tensile strength and 15 per cent,
elongation. These guns could be cast of aluminium
bronze, giving a greater strength and elongation,
at far less cost, being made in one-quarter of the
* Cowles' Pamphlet, April, 1886.
ALLOYS OF ALUMINIUM. 275
time and with a comparatively inexpensive plant.
The melting-point of the bronze is somewhat below
that of copper and its specific gravity is 7.23. It
is without rival as an anti-friction metal, besides
having the hardness, tenacity, and wearing quali-
ties of the best steel. It has also the peculiar
uiictuousness of copper and lead, being so strong
and tough that very small quantities of the rolled
bronze may be used to bush boxes of cast or
wrought iron, so that its first cost is less than that
of the thick masses of brass or phosphor-bronze
now used. The five per cent, bronze makes beauti-
ful wearing plumbers' goods, and can be used also for
table articles, being free from the offensive smell
and taste peculiar to brass. Aluminium in almost
all proportions up to eight per cent, improves all
brasses. Some it makes more ductile, in others it
improves the color, and all are greatly increased in
strength and power to resist corrosion. The alloy
copper 67, zinc 26, aluminium 7 has a strength of
96,000 pounds, while that of copper 67, zinc 30,
aluminium 3 has a strength of 65,000 pounds with
12 per cent, elongation. When we understand
that ordinary brass rarely has a tensile strength
over 30,000 pounds, the extraordinary value of the
aluminium can be appreciated. The strength of
these alloys on the testing machine is as follows : —
276 ALUMINIUM.
Alloy, Tensile strength per Elongation,
Al brass castings. sq. in., pounds. per cent.
Al Cu Zn
5.8 67.4 26.8 95,712 1
3.3 63.3 33.3 85,867 7.6
3.0 67.0 80.0 67,341 12.5
1.5 77.5 21.0 32,356 41.7
1.5 71.0 27.5 41,952 27.0
1.25 70.0 28.0 35,059 25.0
2.5 70.0 27.5 40,982 28.0
1.0 57.0 42.0 68,218 2.0
1.15 55.8 43.0 69,520 4.0
Average commercial cast brass 23,000 Less than 10.0
" The second alloy is made by mixing two parts
five per cent, aluminium bronze with one part zinc.
" The aluminium bronzes gave the following
results : —
Al Cu Tensile strength, Elongation in
pounds. per cent.
2.5 97.5 42,770 53
5.0 95.0 68,480 7.8
6.6 93.4 55,038 80
7.5 92.5 54,636 16
7.5 92.5 60,520 22
91 9 87,783 5
90 10 108,966
90 10 99,931 1.5
90 10 97,103 3.0
90 10 105,336 7.8
90 10 110,657 5.4
16.8 83.2 29,369 (Sp. gr. 3.23)
" The two 10 per cent, bronzes last given were
plunged while red hot into water. Cowles Bros.
ALLOYS OF ALUMINIUM. 277
are now selling 10 per cent, bronze at forty cents
per pound."
In regard to some alloys of aluminium and
copper in which other metals are present, we Would
notice the following alloys which have been made in
addition to those already incidentally mentioned.
Aluminium can be melted with brass, argentan,
etc., by which new bronzes are made of beautiful
color, great hardness, and polish, unalterable in the
air, easily cast, etc. One per cent, of aluminium
is sufficient to modify the qualities of brass or tin
bronze, while 2 per cent, shows a decided change.
By taking ordinary bronze with 1 to 2 per cent, of
zinc or tin, and adding 1 to 2 per cent, of alu-
minium, alloys are obtained possessing additional
qualities to those of aluminium bronze, and which
can replace it in places and for purposes where the
latter's qualities are not so well suited.
Besides these simple alloys we have those of
copper with nickel, tin, zinc, bismuth, and alu-
minium, in such quantities as to make any desired
color or degree of hardness. The following has a
beautiful white polish, which is a close imitation
of silver : —
Copper . 100
Nickel 23
Aluminium 7
F. H. Sauvage makes a metal resembling pure
silver, which he calls Neogen. It contains —
24
278 ALUMINIUM.
Cu . . . . . . . 58
Zn ....... 27
Ni ....... 12
Sn ....... 2
Al .......
" Minargent" is a similar alloy, containing —
Cu ....... 100
Ni ....... 70
Sb ....... 5
Al ...... .2
To make this last alloy, the directions are first to
melt together the copper, nickel, and antimony,
and then granulate the resulting alloy in water.
The dried granules are mixed with the aluminium
and with 1.5 per cent, of a flux consisting of 2 parts
horax and 1 part fluorspar, and then remelted.
P. Baudrin makes an alloy very much resembling
silver in color, malleability, ring, and even sp. gr.,
of the following composition : —
Cu ....... 75
Ni ....... 16
Zn ....... 2.25
Sn ....... 2.75
Co ....... 2
Fe .... 1.5
Al ....... 0.5
Jas. Webster* patents the following bronze:
copper is melted, and aluminium added so as to
* German Pat., 11,577.
ALLOYS OF ALUMINIUM. 279
make a 10 per cent, bronze, which is then mixed
with 1 to 6 per cent, of an alloy of —
Cu 20
Ni 20
Sn 30
Al 7
Thos. Shaw, of Newark, N. J.,* pa tents a phosphor
aluminium bronze, making the following claims:
First, an alloy of copper, aluminium, and phos-
phorus containing 0.83 to 5 per cent, of aluminium,
0.05 to 1 per cent, of phosphorus, and the remainder
copper. Second, its manufacture by melting a bath
of copper, adding to it aluminium in the proportion
stated, the bath being covered with a layer of palm
oil to prevent oxidation, and then adding a small
proportion of phosphorus.
Cowles Bros, in their pamphlet give the follow-
ing tests of the strength of aluminium-silver cast-
Tensile strength, Elongation,
pounds. per cent.
5 p. ct. Al broiize, 1 part ; Ni 2 parts 79,163 33.0
" 4 parts ; Ni 1 part 118,000
German silver without aluminium 44,242 24.0
" " with " 92,849 1.0
Solders for Al Bronze. — Cowles give the follow-
ing jeweller's solder for aluminium bronze:—
* U. 8. Pat., 303,236. Aug. 1884.
280 ALUMINIUM.
Hard solder for 10 per cent, bronze—
Au ....... 88.88
Ag ....... 4.68
Cu ....... 6.44
Middling hard solder for 10 per cent, bronze—
Au ....... 54.40
Ag ....... 27.00
Cu . . ..... 18.00
Soft solder for Al bronze —
Au .... 14.30
Ag .... 57.10
Cu .... 14.30
Silicon and Aluminium Bronze. — Cowles Bros.
have, by reducing fire clay in presence of copper,
obtained alloys of aluminium, silicon, and copper.
This alloy is white and brittle if it contains over
10 per cent, of aluminium and silicon together.
With from 2 to 6 per cent, of these in equal pro-
portions, the alloy is stronger than gun metal, is
very tough, does not oxidize when heated in the
air, and has a fine color. Cowles report that a
silicon-aluminium bronze wire has shown a tensile
strength of 200,000 pounds, a strength hitherto
unprecedented in any metal.
ALUMINIUM AND IRON.
Tissier Bros., 1858 : " An alloy of aluminium
and iron with 5 per cent, iron was made by
ALLOYS OF ALUMINIUM. 281
placing very fine iron wire with fragments of alu-
minium in a crucible containing melted XaCl.
Under these circumstances the iron could not oxi-
dize, and the alloy was easily formed. We have
in this way been able to discover that small quan-
tities of iron give to aluminium the property of
crystallizing, and much impair its malleability.
When aluminium has become low in price, it will
be interesting to see what qualities it can com-
municate to iron as cast iron or steel, introduced
in large or small quantities. Iron raises the fusing
point of the aluminium, for we have melted alu-
minium free from iron on a plate of aluminium
containing 4 to 5 per cent. iron.
Deville, 1859 : . " Iron and aluminium combine
in all proportions. These alloys are hard, brittle,
and crystallize in long needles, when the propor-
tion of iron reaches 7 or 8 per cent. The alloy
containing 10 per cent, iron much resembles sul-
phide of antimony. It liquates, however, with
some facility, leaving a less fusible skeleton, while
less ferruginous aluminium runs down. But this
method of purifying aluminium is not exact. The
presence of a large quantity of iron in aluminium
alters both its chemical and physical properties."
Rogers :* " By melting a steel high in carbon
with aluminium, alloys of steel and aluminium
may be obtained. I have one containing 6.4 per
* Moniteur Industrie!, 1859, No. 2379.
24*
282 ALUMINIUM.
cent, of the latter. I melted 67 parts of this alloy
with 500 of steel, so that the resulting steel con-
tained 0.8 per cent, aluminium. This metal had
the qualities of the best Bombay wootz. A small
per cent, of aluminium makes steel hard, strong,
and brittle, a larger quantity makes it very dense,
without impairing its peculiar polish or detracting
from its qualities."
Fremy, 1883: "Aluminium unites with iron
with the greatest facility. To form an alloy it is
sufficient to stir a rod of iron in melted aluminium,
when it covers itself with a layer of aluminium
and takes on the aspect of being amalgamated.
The alloy with 5 per cent, iron is hard, brittle,
and more difficult to fuse than aluminium. The
7 per cent, iron alloy possesses the same proper-
ties, with a crystalline structure. The 10 per
cent, iron alloy, according to Deville, resembles
sulphide of antimony, Sb2S3. On the other hand,
M. Debray affirms that 7 to 9 per cent, of
iron in aluminium causes no appreciable change in
its properties. By melting ten parts aluminium,
five parts ferric chloride, and twenty parts KC1
and !NaCl, Michel obtained on cooling a mass
which, treated with very dilute sulphuric acid,
left six-sided prisms having the color of iron and
the formula Al2Fe, containing 51 per cent. Fe.*
Calvert and Johnson obtained the alloy Al2Fe3,
* Ann. Cheni. und Pharm. 115, 102.
ALLOYS OF ALUMINIUM. 283
containing twenty-four per cent, aluminium and
seventy-six per cent, iron, which was unalterable
in moist air (see p. 210). The alloy AlFe4, con-
taining 10.8 per cent, aluminium, has been pre-
pared by melting two parts aluminium, five parts
sheet iron, and one part of chalk. It is easily
worked and rolled, but rusts on contact with the
air."
Mierzinski : " A few per cent, of aluminium is
useful in making cast steel, to which it imparts
greater hardness and a bright silver-like polish ;
0.8 per cent, aluminium gives steel all the qualities
of best Bombay wootz, and objects made of it,
treated with dilute sulphuric acid, give the undu-
lating markings generally found only on Damascus
steel. Stoddart and Faraday found in wootz
steel 0.013 to 0.690 per cent, of aluminium. An
alloy of 24.5 per cent, aluminium is silver white,
extraordinarily hard, and does not rust in the air.
Mitis castings :* " The subject of the use of alu-
minium in wrought-iron castings was discussed at
the meeting of the American Society of Mining
Engineers, Pittsburgh meeting, on Feb. 16. It
was described by the inventor, Mr. Peter Ostberg,
of Stockholm, and as his paper has not yet appeared
we give a few particulars which may be of interest.
u Wrought-iron scrap is melted in plumbago
crucibles in a special reverberatory furnace fired
* Eng. and Mining Journal, Feb. 27, 1886.
284 ALUMINIUM.
with petroleum. The crucible is covered, while a
'hole in a cover corresponds with and is directly
under a hole in the roof of the furnace. Wrought
iron fuses at about 4000° F., and it would be neces-
sary to heat it far beyond its point of fusion before
it would be fluid enough to cast into line moulds
and to make it possible to handle it before it would
solidify. Now it is in this superheating that the
iron absorbs gases, and consequently it is impossible
to make solid castings in this way. In order to
obviate this difficulty, Mr. Ostberg has made use
of the well-known fact that certain alloys of metals
possess a fusing point much less than that of the
metals composing them, among which aluminium
alloys are very noticeable. In making w rough t-
iron or mitis castings a very small quantity of alu-
minium, about 0.05 per cent., is added to the charge
in the crucible the moment it has been melted.
The charge is about sixty pounds. The aluminium
is added in the form of an iron-aluminium alloy
containing 7 to 8 per cent, of aluminium. The
fusing point of the whole is at once lowered
some 500 degrees, and the charge being then
nearly 500 degrees above its new .fusing point be-
comes extremely fluid and can be cast into the
finest moulds ; while the great difference between
its temperature and its reduced fusing point gives
all the time necessary for manipulating it without
danger of solidifying. This extreme fluidity
allows the ready escape of gases which would
ALLOYS OF ALUMINIUM. 285
otherwise make the casting porous, and the result
appears to be a remarkably fine, solid, and tough
casting of wrought iron.
" These mitis castings are said to be 30 to
50 per cent, stronger than the iron from which
they are made; but, although aluminium undoubt-
edly increases the strength of most metals with
which it alloys, it is not credited with the increase
of strength in this case ; for it is said that after
hammering, the mitis metal loses its increase in
strength and returns to the fibrous appearance and
strength of the original iron.
" The alloys of iron and steel with aluminium
have long been known, and reference is made to
the addition of such an alloy to steel by Faraday,
only a few years after the discovery of aluminium ;
but this application to wrought iron castings
appears to be new and is certainly very interest-
ing.
" The alloy used by Mr. Ostberg at his works in
"Worcester, Mass., is made by the Cowles Electric
Smelting Co., and contains 6 to 8 per cent,
aluminium and 1 to 1.25 per cent, of silicon. It
costs about fort}T cents per pound, but as only 0.05
per cent, aluminium is required in the iron,
the addition to its cost is very slight. This utili-
zation of the well-known property of aluminium
to lower the fusing point of the iron is a very neat
and clever application of a curious phenomenon,
and it is said to succeed very well. Whether it.
286 ALUMINIUM.
will also facilitate the making of small steel cast-
ings is not stated, but it would probably in this
case make the metal more fluid and obviate the
necessity of using those extremely high heats
which are necessary to cause the steel to melt and
run well into the moulds."
Mr. Ostberg sent a note to the ' Engineering and
Mining Journal/ stating that he used only a small
sample of Cowles' alloys, but that he uses almost
altogether a 7 to 8 per cent, aluminium alloy,
made in Sweden by a very simple and cheap
patented process, which consists in adding clays in
iron smelting.
The following note, bearing on this subject, is
from Watts: "The 'London Mining Journal'
states that if common kaolin is added to iron when
being smelted in a crucible to convert it into steel,
an improved product is the result." Aside from
this note, the author has been unable to find any
reference to the process suggested by Mr. Ostberg.
Mr. Sellers, of Philadelphia, remarked after the
reading of Dr. Hunt's paper on the Cowles furnace
at the Washington meeting of the National Acad-
emy of Sciences, April, 1886 (see p. 196), that he
had made a series of experiments on the use of
aluminium with iron in casting, and obtained
what is technically called a " dead melt" in two or
three minutes, instead of an hour as required by
previous methods. The result is very fine castings,
ALLOYS OF ALUMINIUM. 287
and without the flaws which so often vex the
founder.
A company has been incorporated in New Jersey
within the last month to regulate the use and sell
rights to use Mr. Ostberg's patents. Mr. Fritz, of
the Bethlehem Iron Works, is one of the heads of
the company, which includes other prominent
Bethlehem capitalists.
ALUMINIUM AND ZINC.
Tissier Bros., 1858: "An alloy with 10 per
cent, aluminium is brittle, has the appearance of
zinc, is more fusible than aluminium, and less
so than zinc. An alloy with 25 per cent,
aluminium has a tine even grain, and is still more
fusible than aluminium and less so than zinc. An
alloy with 50 per cent, did not appear to be
homogeneous ; heated on an aluminium plate it
separated into a fusible portion and a part which
did not melt till the plate did. These alloys have
been tried as solders for aluminium, and so far
have succeeded better than any other alloys, but,
unfortunately, when, melted they are thick and
cast with difficulty, so much so that it is necessary
to spread them over the joint as a plumber does
when he wipes the joints of lead pipes. Joints
thus made stand hammer blows or rough usage
very poorly." •
Deville, 1859 : " The alloys of aluminium and
288 ALUMINIUM.
zinc are brittle, at least unless the zinc is in small
proportion. Several specimens of zinciferous alu-
minium were put into commerce by a singular
accident ; the retorts used for making the alumin-
ium were made at the Vielle Montague Zinc Works,
and having in their mixture some ground-up old
zinc retorts, the new retorts contained zinc, which
got into the aluminium and altered its properties
in a very evident manner. Some analyses of this
metal having been made in England, some asserted
that French aluminium was only an alloy to which
zinc gave a fusibility which might be wanting in
pure aluminium. The alloys of zinc and alumin-
ium have been used in experiments to solder alu-
minium solidly, but so far with little success.
Zinc unites easily with the aluminium, altering its
properties when exceeding a few per cent."
Kerl and Stohman, 1874 : " Zinc and alumin-
ium melted together in atomic proportions under
a cover of Nad and KC1 unite with incandescence,
forming a silver-white, very brittle, crystalline alloy,
with a specific gravity of 4.532."
Fremy, 1883: "The alloys of zinc and alu-
minium are employed to solder aluminium. They
will take a very fine polish. The alloy with three
per cent, zinc is yet malleable, but that with thirty
per cent, aluminium is white, crystalline, and very
brittle."
ALLOYS OF ALUMINIUM. 289
ALUMINIUM AND TIN.
Tissier Bros., 1858 : An alloy with 3 per cent,
tin is very brittle, a little more fusible than
aluminium. It was made by combining the metals
under a cover of NaCl, then remelted alone, and
cast. Its grain is very fine and crossed, and it
breaks at the first blow of the hammer. If tin,
even in small quantities, injures the qualities of
aluminium, the latter, on the contrary, gives to tin
hardness and tenacity, if it is not present in too
large an amount. The alloy with 5 per cent,
aluminium possesses these desirable qualities. The
alloy with 10 per cent, is not homogeneous, for it
arranges itself in the ingot in two layers, an upper
brittle one, a little more fusible than aluminium,
another lower one containing nearly all the tin but
rendered harder and less fusible by a small quan-
tity of aluminium. These alloj^s have been used
to solder aluminium because of their fusibility and
the ease with which they adhere to a clean surface,
but they have the same inconveniences as the zinc
solders, tney run thick and are fragile.
Deville : Tin unites easily with aluminium,
altering its properties as soon as the proportion
has passed a few per cent. These alloys may be
used to solder aluminium, but they answer imper-
fectly.
Kerl and Stohman : The aluminium-tin alloys
with over 30 per cent, of the former are silver-
25
290 ALUMINIUM.
white, but porous and brittle. The 19 per cent.
and especially the 7 per cent, aluminium alloys
are, on the contrary, malleable and workable at a
red heat.
Fremy : A small quantity of tin renders alu-
minium brittle, but a small percent, of aluminium
alloyed with tin renders it harder and more elastic.
Such an alloy, besides being easy to work, may
advantageously replace tin in many of its uses.
The alloys most recommended are those with 5, 7,
and 19 per cent, of aluminium.
Mierzinski: Aluminium and tin unite in cer-
tain proportions, but the tin will not combine with
more than 7 per cent, of aluminium, for the 10
per cent, aluminium alloy is no longer homogeneous
but on cooling liquates away a more fusible and
leaves a less fusible alloy, the latter being richer
in tin. An alloy with 3 per cent, aluminium is
harder than tin and less acted on by acids. The
7 per cent, aluminium alloy is especially recom-
mended as being easy to work, capable of being
polished, but possessing the drawback that it can-
not be melted without a part of the tin separating
from the aluminium.
M. Bourbouze,* a French physicist, employs an
alloy of aluminium and tin for the interior parts
of optical instruments, in place of brass. The
alloy contains 9 per cent, of tin. It is white, like
* Iron Age, July 29, 1886.
ALLOYS OF ALUMINIUM. 291
aluminium, and has a density of 2.85. This light-
ness is of great advantage. It can be soldered as
easily as brass, without special apparatus, and is
more resistant to reagents than aluminium. It
would be very useful for electrical instruments,
especially those of a portable character.
ALUMINIUM AND LEAD.
Tissier: As Deville has remarked, these two
metals have such little tendency to combine that
there may be recovered intact in the bottom of an
ingot of aluminium any small pieces of lead which
may accidentally have got into the metal.
Deville: Lead unites only imperfectly with
aluminium. However, an alloy may exist in cer-
tain proportions, especially at the temperature
necessary to the cupellatiou of aluminium. The
cupellation of aluminium with lead is quite pos-
sible.
Kerl and Stohman : Aluminium does not unite
with lead.
Mierzinski : Aluminium and lead do not unite.
By melting the metals together and cooling down,
they are found separated from each other, the
aluminium above and the lead beneath. This
property suggests the possibility of using it to
separate silver from work lead, as soon as its price
allows.
;292 ALUMINIUM.
ALUMINIUM AND ANTIMONY.
Tissier: Aluminium also appears to have as
little tendency to unite with antimony as with
lead ; we did not succeed in getting a homoge-
neous alloy of the two metals.
Kerl and Stohman : Aluminium does not unite
with antimony.
ALUMINIUM AND BISMUTH.
Tissier : The combination of these two metals
takes place easily and gives rise to very fusible
alloys, which oxidize very rapidly when melted.
They are also very alterable in the air at ordinary
temperatures when the bismuth is in large per
cent. However, these metals do not appear able
to unite in all proportions, as the following experi-
ment seems to prove. We melted together 10
grms. aluminium and 20 grms. bismuth. The
combination took place under NaCl, and although
it was stirred carefully the button appeared to be
of two layers, the lower one composed of almost
pure bismuth, and the upper one more malleable,
detachable from the lower by a blow of the
hammer, and weighing 13.45 grms. Supposing
that this latter contained all the aluminium (there
appeared to be none in the other layer), then the
alloy was composed of nearly 75 per cent, alumin-
ium and 25 per cent, bismuth. Thus the aluminium
did not appear able to take up over 25 per cent, of
ALLOYS OF ALUMINIUM. 293
bismuth. The alloy containing 10 per cent, bis-
muth is hard, malleable, takes a fine polish, is
unattaoked by nitric acid, and not blackened by
sulphuretted hydrogren. We say it was malleable
because it could be worked to a certain extent under
the hammer, and we thought it could be easily
drawn out, but in spite of frequent annealings it
split in all directions and we had to stop working
it. We tried, by diminishing the per cent, of
bismuth, to take away this bad quality, and to
this end prepared alloys with 5, 3, 2.5, and 0.5 per
cent, of the latter, but without obtaining satisfac-
tory results.
Watts : One-tenth of one per cent, of bismuth
renders aluminium so brittle that it cracks under
the hammer after being repeatedly annealed.
ALUMINIUM AND NICKEL.
Tissier: The alloy with 50 per cent, nickel was
made by melting together the metals in equal pro-
portions under XuCl ; the heat evolved was suffi-
cient to raise the mass to incandescence. This alloy
remained pasty at the temperature of melting
copper. It is so brittle that it pulverizes under
the hammer. By melting proper proportions of
this alloy with more aluminium, an alloy with 25
per cent, nickel was produced. This is less fusible
than aluminium, and as brittle as the 50 per cent,
alloy. By melting some 25 per cent, nickel alloy
25*
294 ALUMINIUM.
with aluminium, a 5 per cent, nickel alloy was
obtained. This is much less brittle than the pre-
ceding, but is still very far from being easy to
work. From the 5 per cent, alloy one with 3 per
cent, was made. With this amount of nickel the
aluminium acquired much hardness and rigidity,
and was easy to work. A curious fact with this
alloy is that it may be melted on a plate of alu-
minium, showing its fusion point to be less than
that of pure aluminium, the reverse effect to what
iron produces, which if present in the same pro-
portion would diminish the fusibility of the
aluminium. To sum up, the action of nickel on
aluminium is much analogous to that of iron, for
nickel, like iron, produces crystalline alloys with
aluminium, and if employed with care gives to it
certain desirable qualities such as hardness, elas-
ticity, etc.
Mierzinski : To alloy aluminium with nickel a
certain limiting quantity of nickel must not be
exceeded. When the latter is present less than 3
per cent., it behaves similarly to iron in improving
the qualities of the aluminium in many ways,
especially in hardness and elasticity. More than
3 per cent, makes the aluminium brittle and un-
workable.
Argentan has a beautiful color, and takes a high
polish, it contains —
Cu 70
Ni 23
Al . 7
ALLOYS OF ALUMINIUM.
Minargent contains —
Cu .
Ni .
Sb . .
Al .
100
70
5
2
ALUMINIUM AND SILVER.
Tissier: Silver is the metal which seems most
useful in improving aluminium. Five per cent,
silver gives to aluminium elasticity which is want-
ing in pure aluminium, increases its hardness and
its capability of being polished, and does not injure
its malleability. We have sold a quantity of these
alloys, the properties of which we will describe.
All the alloys up to 50 per. cent of silver are more
fusible than aluminium, the fusibility increasing
with the amount of silver. The alloy with 33 per
cent, silver is fusible enough to serve for a solder ;
but, like the alloys of aluminium with zinc and
tin, it casts with difficulty and makes a brittle
joint. With 10 per cent, silver the aluminium
will not stand under the hammer. The 50 per
cent, alloy breaks like those of copper. The pres-
ence of silver in aluminium can always be recog-
nized by the action of the alloy on a moderately
concentrated solution of caustic potash. Alumin-
ium whitens in this solution, but, if it contains
silver, this being exposed by the dissolving away
of the aluminium gives the surface a black color.
By introducing 5 per cent, of aluminium into silver
296 ALUMINIUM.
the latter acquires the hardness of silver coin, the
alloy takes a beautiful polish, does not contain as
alterable a metal as copper, and contains 95 per
cent, of silver instead of 90. This alloy is easily
distinguished from the alloy into which copper
enters by the test with nitric acid, which whitens
instead of blackening it.
Deville: A few per cent, of silver will take
away from aluminium all its malleability. How-
ever, the alloy with 3 per cent, is used by M.
Christofle for casting objects of art ; and the alloy
with 5 per cent, to make knife blades, and it may
be worked like pure aluminium. It has, moreover,
the color and lustre of silver, and is not tarnished
by sulphuretted hydrogen.
Kerl and Stohman : According to Hirzel, the
alloy containing 20 per cent, aluminium is very
porous, silver-white, tarnishing in the air, sp. gr.
6.733. AlAg2, containing 11.11 per cent, alumin-
ium is also silver-white, a little porous, tarnishes
in the air, sp. gr. 8.744. AlAg4, containing 5.9 per
cent, aluminium is pure silver-white, very malle-
able, forgeable, tarnishing in the air, sp. gr. 9.376.
Fremy : The alloys of aluminium and silver are
easy to form by direct fusion of the two metals ;
their hardness is generally superior to that of
aluminium, but, nevertheless, they are quite as easy
to work, and in some cases more fusible than it.
Debray states that the 50 per cent, alloy is as hard
as bronze.
ALLOYS OF ALUMINIUM. 297
Mierzinski : Five per cent, of silver makes alu-
minium elastic and as hard as coin silver, but not
brittle. Tbis alloy is workable like pure alumin-
ium, takes a fine polisb, is light, not magnetic,
does not rust, and has the color of pure silver,
whose place it can take for many purposes. How-
ever, the assertion that this or any other alloy of
silver and aluminium is not attacked by hydrogen
sulphide is incorrect and untenable, since, according
to careful experiments, these alloys are attacked
quicker and more actively by it than pure silver.
This alloy is used for watch-springs, dessert-spoons,
etc., on account of its hardness and elasticity. The
alloy with 3 per cent, silver has a very fine silver
color. The 50 per cent, alloy is as hard as bronze,
but so brittle that it cannot be pressed ; all the
alloys with over 10 per cent, silver up to the 50 per
cent, alloy are brittle and cannot be worked with a
hammer.
" Tiers Argent" is an alloy of two-thirds alumin-
ium and one-third silver, which was made homo-
geneous at first with some difficulty but is now
easily made. Spoons, forks, and salvers of this
alloy leave nothing to be desired. It possesses a
hardness superior to silver, and can be easily en-
graved.*
Cowles Bros, state that what is generally known
and sold as aluminium silver is an alloy of alu-
* Cbem. News, xvi. 289.
298 ALUMINIUM.
minium, nickel, and copper; or, in effect, it is alu-
minium added to German silver. The great
advantage of this metal is that it will keep its
beautiful white lustre for all time, and permits of
objects being made from it in an enduring and sub-
stantial manner. It requires no plating of any kind.
ALUMINIUM AND GOLD.
Tissier : Aluminium endures a large quantity of
gold without its ductility being impaired. We have
prepared an alloy with 10 per cent, of gold which
works at a red heat as well as aluminium, is a little
harder but scarcely polishes any better than it. Its
color, for some cause, is darkish brown, like that
of tin lightly sulphurized. The alloy containing
15 per cent, gold can no longer be forged. As to
the effect of small quantities of aluminium on gold,
5 per cent, of it gives to the latter a white color
and makes it brittle as glass.
Fremy : The alloy with one percent, aluminium
possesses the color of " green gold ;" it is very hard
but yet malleable. The alloy with 10 per cent,
aluminium is white, crystalline, and brittle; the
alloy with 5 per cent, is brittle as glass.
Mierzinski : Aluminium can take up as much as
10 per cent, of gold without its malleability de-
creasing. This alloy can be forged, but not well
polished. The color of the gold has entirely dis-
appeared, seeming to have no effect on the alumin-
ium.
ALLOYS OF ALUMINIUM. 299
ALUMINIUM AND PLATINUM.
Tissier : Aluminium unites with platinum with
great ease, forming with it alloys more or less fusi-
ble according to the proportions of aluminium.
Five per cent, of platinum makes an alloy not mal-
leable enough to be worked ; it is probable that by
diminishing the amount of platinum a suitable
alloy might be produced. In color it approaches
that of gold containing 5 per cent of silver.
ALUMINIUM AND CADMIUM.
Deville : Cadmium unites easily with alumin-
ium. The alloys are all malleable and fusible, and
may be used to solder aluminium, though imper-
fectly.
ALUMINIUM AND BORON.
Deville: "By melting aluminium with borax,
boracic acid, or fluo-borate of potassa, an alloy
very rich in boron was obtained. This alloy, like
siliceous aluminium, possesses the singular prop-
erty that the boron diminishes all its useful qualities.
The alloy is very white, only able to bear slight
bending, and tears under the rolls. It exhales a
very strong odor of hydrogen silicide, SiH4, with-
out doubt due to the silica of the vessel which was
attacked at the same time as the borax. M.
300 ALUMINIUM.
Wohler and I have shown that the boron may be
extracted from this alloy in two different forms,
the graphitoidal and the diamantine boron." De-
ville gives at the end of his volume on aluminium
the mode of preparation of this diamantine boron.
ALUMINIUM AND CARBON.
Deville : I was not able, by any effort I made,
to combine carbon with aluminium. On decom-
posing carbon tetrachloride, CC14, by aluminium,
there is formed ordinary carbon, while the alumin-
ium which remains has undergone no change.
Cowles: Specimens of alloys of aluminium and
carbon, yellow and crystalline, have been exhibited,
which were made in the Cowles furnace. (See
p. 195.)
ALUMINIUM AND GALLIUM.
Watts : Lecoq de Boisbaudran makes the fol-
lowing remarks : " If the proportion of aluminium
is to be considerable, the two metals are melted
together at dull redness. The alloys thus obtained
remain brilliant, arid do not sensibly absorb the
oxygen of the air in their preparation. After
cooling they are solid but brittle, even when the
excess of aluminium has raised the melting point
to incipient redness. They decompose water iu
the cold, but better at 40°, with rise of tempera-
ALLOYS OF ALUMINIUM. 301
ture, evolution of hydrogen, and formation of a
chocolate-brown powder, which is ultimately re-
solved into white flakes of alumina."
ALUMINIUM AND TITANIUM.
"Wohler* fused in a clay crucible 10 grms. of
titanic acid, 30 grms. cryolite, 15 grms. each of
Nad and KC1, and 5 grms. of aluminium. This
was kept at the melting point of silver for one
hour and then opened. The aluminium had
become lammelar, and when dissolved in caustic
soda left a quantity of brilliant, crystalline plates,
found to be a compound of aluminium, titanium,
and silicon. The elements of the compound appear
to be able to unite in various proportions. Its
density was 3.3. It was infusible before the blow-
pipe, but heated to redness in chlorine it burnt,
giving chlorides of the three metals present.
Another experiment, heated only to the melting
point of nickel, gave a white compound richer in
silicon, sp. gr. 2.7.
Alloysf of aluminium with wolfram, molybde-
num, and manganese were made by Michel in
Wohler's laboratory, on which the following report
is made : —
* Chcm. News, 1860, p. 310.
t Ibid.
26
302 ALUMINIUM.
ALUMINIUM AND TUNGSTEN.
A14W was made by fusing together 15 grms.
tungstic acid, 30 grms. cryolite, 15 grms. each of
KC1 and ]N"aCl, and 15 grms. aluminium, at a strong
red heat. The excess of aluminium was removed
from the regulus by HC1. The alloy is an iron-
gray powder, crystalline, single crystals were
several millimetres long, brittle and hard rhombic
prisms. Sp. gr. 5.58. Hot caustic soda extracts
all the aluminium from these crystals, leaving
behind pure tungsten.
ALUMINIUM AND MOLYBDENUM.
Molybdic acetate is dissolved in hydrofluoric
acid, the solution evaporated to dry ness, and the
.residue mixed with cryolite, flux, and alumin-
ium, in the same proportions as given for tungsten.
Excess of aluminium is dissolved from the product
with caustic soda, and there remains a black,
crystalline powder consisting of iron-gray rhombic
prisms, soluble in hot nitric or hydrochloric acid,
and consisting entirely of aluminium and molyb-
denum.
ALUMINIUM AND MANGANESE.
We fused together 10 grms. anhydrous manganese
chloride, 15 grms. each of KC1 and NaCl, and 15
ALLOYS OF ALUMINIUM. 303
grms. aluminium. The excess of aluminium was
removed by HC1. There remained a dark-gray,
crystalline powder consisting of square prisms, spe-
cific gravity 3.4. Dilute caustic soda extracts all
the aluminium from these, leaving the manganese.
ALUMINIUM AND SODIUM.
Deville : Aluminium unites easily with sodium,
especially in small proportions. From this it fol-
lows that the properties of the metal made care-
lessly by using sodium are completely altered.
The last traces of sodium can be removed only with
great trouble, especially when the aluminium has
been produced in presence of fluorides, because of
the marked affinity of aluminium for fluorine at
the temperature at which aluminium fluoride,
A12F6, commences to volatilize.
Fremy: Aluminium easily combines with so-
dium. If the combination contains 2 per cent, of
sodium, it easily decomposes water, which circum-
stance gave cause to the notable loss of aluminium
when it was first being manufactured.
ALUMINIUM AND NITROGEN.
Dr. Hunt,* in reading a paper on the Cowles
furnace (see p. 196), showed a specimen of a pecu-
liar alloy believed to consist entirely of aluminium
and nitrogen.
* Washington Meeting, Nat. Acad. Sciences, April, 1886.
APPENDIX.
NATIVE SULPHATE OF ALUMINA.
IN the summer of 1884, a large deposit of rock called
" native alum" was discovered on the Gila River, Sorocco
Co., New Mexico, about two miles below the fork of the
Little Gila and four miles below the Gila Hot Springs.
The deposit is said to extend over an area one mile square
and to be very thick in places. The greater part of the
mineral is impure, as is usual with native occurrences, but
it is thought that large quantities are available. A com-
pany formed in Sorocco has taken up the alum-bearing
ground. Through the kindness of Mr. W. B. Spear, of
Philadelphia, I was enabled to get a specimen of it.
It is white, with a yellowish tinge. On examining
closely it is seen to consist of layers of white, pure-looking
material arranged with a fibrous appearance at right
angles to the lamination. These layers are about one-
quarter of an inch thick. Separating them are thin layers
of a material which is deeper yellow, harder and more
compact. The whole lump breaks easily and has a strong
alum taste. On investigation, the fibrous material was
found to be hydrated sulphate of alumina, the harder
material sulphate of lime.
It is probable that this deposit was the bed of a shallow
26*
306 APPENDIX.
lake in which the alum-bearing water from the hot springs
concentrated and deposited the sulphate of alumina.
Periodically, or during freshets, the Little Gila, flowing
through a limestone country, bore into this lake water
containing lime, which, meeting the A12(S04)3 solution,
immediately caused a deposit of CaSO*. When the dry
season came, the Little Gila dried up, the deposit of alum
was made, and thus were formed the succession of layers
through the deposit.
Analysis showed 7 to 8 per cent, insoluble material,
and the remainder A12(SO4)3.18H2O. A small amount of
iron was present.
DECOMPOSITION OF CRYOLITE.
According to a patent given to F. Lauterborn (see p.
206), cryolite can be decomposed by boiling with water ;
sodium fluoride going into solution arid aluminium fluor-
ide remaining as residue.
To test the accuracy of this statement, I boiled 250
grms. of the mineral in 5 litres of water for 3 hours. The
solution was filtered hot and evaporated to dryness.
There was no residue. The material on the filter ap-
peared to be undecomposed cryolite.
The experiment does not prove that the decomposition
is impossible, but makes it appear extremely improbable.
AMERICAN ALUMINIUM.
I bought some of Mr. Frishmuth's aluminium from
Bullock & Crenshaw, Philadelphia. The surface was
slightly whitened by oxidation, resembling, though not
GRAVITY OF ALUMINIUM. 307
to such a degree, the oxidation which takes place on slabs
of zinc when exposed to the air. The wire was not per-
fectly smooth, being at places slightly rough and scaly.
It was quite soft and malleable. Its color was nearly white,
but with a slight blue tinge, which, if intensified, would
have made it resemble zinc more than any other metal.
Duplicate analyses of it gave me the following results : —
Si 0.65 0.56
Fe 1.94 1.87
Al (by diff.) . . . 97.41 97.57
After making these analyses, I came across the analysis
of Mr. Frishmuth's metal given on p. 53.
SPECIFIC GRAVITY OF ALUMINIUM.
The sp. gr. of the metal whose analysis was just given
I determined very accurately on a Becker balance. Com-
pared with water at 4° C., it was 2.735. I wished to see
if this would correspond to the sp. gr. calculated from the
analysis. The data were as follows : —
Si .
Fe .
Al .
Calculated sp. gr 2.757
The correspondence being so close has suggested that
the sp. gr. of commercial aluminium, carefully taken, gives
the approximate amount of iron present ; for the sp. gr.
of silicon is so near to that of aluminium, that 10 per
cent, of the former, an amount never found in commercial
aluminium at present, would only affect the sp. gr. 0.03.
Average
sp. gr.
2.34
Average per
cent, present.
0.60
Products.
0.014
7.7
1.80
0.138
2.67
97.60
2.605
308 APPENDIX.
So then, within the limits usually found in commercial
aluminium, i. e., silicon less than 5 per cent, and iron
anywhere less than 10 per cent., a careful determination
of the sp. gr. should, hy a little calculation, give the amount
of iron present within a limit of error of 0.5 per cent, at
most, thus saving a wet determination of iron.
AMALGAMATION OF ALUMINIUM.
Wishing to observe the effect of mercury on metallic
aluminium, I took a clean, bright piece of aluminium foil
of Mr. Frishmuth's make, and put on it a small globule
of mercury, which I rubbed in with the finger. Almost
immediately a white powder appeared and the foil felt
warm from the heat generated. On brushing away this
powder, the foil underneath appeared white and unattacked.
By letting the mercury remain on the foil, it very soon
eat a hole through it. Compare with p. 261.
It thus appears that mercury unites with a clean sur-
face of aluminium, forming an amalgam, and the alumin-
ium in the amalgam oxidizes in the air to alumina. The
question arises, why does aluminium oxidize so easily ?
We know how the properties of this metal depend much
on its state of division ; its foil will burn in the air, where-
as the metal in bulk will not. The mercury serves, as it
amalgamates the aluminium, to draw apart even the mole-
cules of the metal, and so this extremely minute, even
molecular division of the aluminium permits it to exhibit
in an intensified degree the principle just stated, which
was illustrated by the burning of the foil, t. e., the finer its
state of division the more easily is it acted on by oxidiz-
ing agents. Translating this into the language of chemi-
cal affinities, in metallic aluminium the atoms are united
AbUMINIUM SULPHIDE. 309
two by two by a mutual exchange of affinities, and the
oxygen of the air is not able to break this molecular bond
at ordinary temperatures. But by the intervention of
the mercury this bond is broken, and the atoms of alu-
minium become united with atoms of mercury, which
weakens the bond holding the molecule together. The
strong affinity which oxygen has for aluminium is now
able to break up the new molecule, the metal is rapidly
oxidized and the mercury set free.
REDUCTION OF ALUMINA.
I experimented on reducing alumina by carbon in pres-
ence of copper. (See p. 213.) I took for a charge —
40 grms CuO and Cu.
5 " . . . . A12O3.
5 " . . . . Charcoal.
These were intimately mixed and finely powdered, put in a
white-clay crucible and covered with cryolite. The whole
was slowly heated to bright redness, and kept there for two
hours. A bright button was found at the bottom of the
crucible. This button was of the same sp. gr. as pure
copper, and a qualitative test showed no trace of aluminium
in it.
This is the same result that other experimenters have
reached, and the conclusion seems to be that the process
gives no practical results.
PRODUCTION AND REDUCTION OF ALUMINIUM
SULPHIDE, AL2S3.
Until the reseai ches of M. Fremy, no other method of
producing A12S3 was known save by acting on the metal
310 APPENDIX.
with sulphur at a very high heat. Fremy was the first
to open up this new field, and it may be that his discover-
ies will yet be the basis of successful industrial processes.
Fremy is often quoted in connection with APS3, and in
order to understand just how much he discovered we here
give all that his original paper contains concerning this
sulphide.*
" We know that sulphur has no action on silica, boric
oxide, magnesia, or alumina. I thought that it might be
possible to replace the oxygen by sulphur if I introduced
or intervened a second affinity, as that of carbon for
oxygen. These decompositions produced by two affinities
are very frequent in chemistry, it is thus that carbon and
chlorine, by acting simultaneously on silica or alumina,
produce silicon or aluminium chloride, while either alone
could not decompose it ; a similar case is the decomposi-
tion of chromic oxide by carbon bisulphide, producing
chromium sesquisulphide. Reflecting on these relations,
I thought that carbon bisulphide ought to act at a high
heat on silica, magnesia, and alumina, producing easily
their sulphides. Experiment has confirmed this view. I
have been able to obtain in this way almost all the sul-
phides which until then had been produced only by the
action of sulphur on the metals.
" To facilitate the reaction and to protect the sulphide
from the decomposing action of the alkalies contained in
the porcelain tube which was used, I found it sometimes
useful to mix the oxides with carbon and to form the mix-
ture into bullets resembling those employed in the prepa-
ration of APC16. I ordinarily placed the bullets in little
* Ann. de Chem. et de Phys. [3] xxxviii. 312.
ALUMINIUM SULPHIDE. 311
carbon boats, and heated the tube to whiteness in the
current of vaporized carbon bisulphide. The presence of
divided carbon does not appear useful in the preparation
)hide.
.12S3 formed is not volatile; it remains in the car-
bon boats and presents the appearance of a melted vitre-
ous mass. On contact with water it is immediately de-
composed.
Al2S3-f3H2O=Al2O3+3H2S.
" The alumina is precipitated, no part of it going into
solution. This precipitated AFO3 is immediately soluble
in weak acids. The clear solution, evaporated to dryness,
gives no trace of alumina. It is on this phenomenon that
I base a method of analysis as will be seen below.
"Analysis of the product. A12S3 being non-volatile, it
is always mixed with some undecomposed alumina. It is,
in fact, impossible to entirely transform all the alumina
into A12S3. I have heated less than a gramme of alumina
to redness five or six hours in carbon bisulphide vapor,
and the product was always a mixture of Al2O3and A12S3.
The reason is that the sulphide being non-volatile and fusi-
ble coats over the alumina and prevents its further decompo-
sition. The A12O3 thus mixed with the A12SS, and which
has been exposed to a red heat for a long time, is very
hard, scratches glass, and is in grains which are entirely
insoluble in acids. By reason of this property I have
been able to analyze the product exactly, for on treating
the product with water and determining on the one hand
the sulphuretted hydrogen evolved, and on the other the
quantity of soluble alumina resulting, I have determined
the two elements of the compound. One gramme of my
312 APPENDIX.
product contained 0.365 grm. of A12S3, or 36.5 per cent.,
the remainder being undecomposed alumina." The com-
position of this APS3 was —
Al 0.137 grm. = 37.5 per
S ... 0.228 " = 62.5 "
0.365 " 100.0 "
The formula APS3 requires —
Al 36.3 per cent.
8 63.7 "
The above is the substance of Fremy's remarks on
APS3. The next investigation in this field was made by
Reichel. His paper is on the sulphides of magnesium and
aluminium and he proceeded in methods so similar with
both metals that he sometimes describes a process only for
magnesium sulphide, MgS, with details, and merely states
his results in working the same way for APS3, which will
account for the frequent allusion in his paper to MgS.
The paper is very lengthy, but only what bears directly on
the subject in hand is extracted.
" I wished* to obtain more definite knowledge of MgS
and APS3, and I also had a practical end in view ; for,
depending on the small affinity of sulphur for magnesium
and aluminium, I hoped, if not to isolate them from the
sulphide, at least to try the possibilities of this method."
(As preliminary, Reichel here gives extended remarks on
the behavior of aluminium and magnesium towards sul-
phur, and a description of the sulphides.)
" APS3 appears yellow, at least that made from the
metal and sulphur with exclusion of air always has this
* Jrnl. fr. Prak. Chem. xi . 55.
ALUMINIUM SULPHIDE. 313
color. It is only by heating the metal with sulphur vapor
with admittance of air that the product is of a darker
experiments to determine if the preparation
MgS was not possible in the same way as
K2S, Na2S, and BaS are made. For example, by melting
potassium oxide with sulphur some K2S is formed. How-
ever, on doing this with alumina and magnesia, it became
evident that magnesium and aluminium have less affinity
for sulphur than for oxygen, and the experiment failed*
But, matters were changed when a reducing agent was
introduced with the sulphur. If a mixture of carbon,
magnesia, and sulphur are heated, MgS results, which by
treating the product with water goes into solution un-
changed. Alumina under similar treatment gave no
APS3. In place of carbon as a reducing agent I next
used hydrogen. By igniting magnesia in a stream of
hydrogen and sulphur vapor some little MgS was formed,
but the mass of the magnesia was unchanged. The next
step was to substitute sulphuretted hydrogen for hydrogen
and sulphur separately, but only a little MgS was formed
in this way.
" Since the sulphates of calcium and barium are reduced
to sulphides with very little trouble, it appeared probable
that magnesium sulphate, MgSO4, should be convertible
into MgS by a reducing agent. The attempts to do this
were unsuccessful. I heated MgSO4 in vapor of ammon-
ium sulphide, but it underwent no change. Since accord-
ing to Stammer* K2SO, CaSO4, and BaSO4 may be re-
duced to sulphides by carbonic oxide, CO, I tried to
* Pogg. Ixxxii. 135.
27
314 APPENDIX.
reduce MgSO4 by this means. The following reaction
apparently took place- —
MgSO4+ 4CO=MgO+COS, + 3CO2.^^^
" I then took pure magnesia, filled a porcelain tube
with it, and passed carbon bisulphide vapor througnrt.
The apparatus was first filled with hydrogen, then as soon
as the tube was bright red the carbon bisulphide flask was
warmed, and sulphuretted hydrogen and carbonic oxide
began to issue from the tube. The heating was continued
till carbon bisulphide condensed in the outlet tube, then
the fire was removed and hydrogen passed through the
tube till it was cold. The MgS resulting was of a gray
color, not melted, but as a crumbly powder. The reaction
which took place was probably
MgO+ 2CS2-f-6H=MgS + 3H'S-|-CO+ C.
" The carbon was left with the MgS; and, to get rid of
it I heated the tube up as before but passed hydrogen and
carbonic oxide through, when the hydrogen took up the
carbon forming probably some hydrocarbon.
" Than* says that carbon oxysulphide, COS, is formed
by leading carbonic oxide and sulphur vapor through a
red-hot tube. The reactions made to take place are
=3COS.
" The product obtained thus contained 58 per cent.
MgS and 42 per cent, undecomposed magnesia. In act-
ing on alumina in the same way, the product obtained is
a mixture of APS3 and aluhiina."
* Jahresb. der Chein., 1867, 155.
ALUMINIUM SULPHIDE. 315
Reichel next tried the different methods which have
been proposed to reduce these sulphides to metal, and
thus records his results (see p. 183) : —
" Petitjean* patented a process in England for reducing
APS3 by hydrogen acting at a high temperature, or by
melting it with iron filings. MgS, heated a long time
in a current of hydrogen, remained unchanged. I mixed
MgS with iron filings, put it in a porcelain crucible,
covered with fresh, dry, fine NaCl, and filled the crucible
to the rim with carbon. To keep out all oxygen, I put
the crucible inside a larger Hessian crucible, filling in
between with pulverized charcoal. After heating several
hours in a wind furnace, I found a half-sintered mass
under the NaCl. This material, on being boiled with
water, evolved no trace of hydrogen sulphide but only
pure hydrogen. This showed that the iron had taken the
sulphur from the MgS. Still, I did not succeed in ex-
tracting the free magnesium from it by amalgamation.
In the same manner, A12S3 appeared to be decomposed by
iron and heat, but it was also impossible in this case to
separate the metallic aluminium out of the mass. Copper
effects the reduction as well as iron, forming CuS.
" Since magnesium is not sulphurized on ignition in a
current of hydrogen sulphide, it appeared probable that
MgS might be reduced by ignition in a stream of hydrogen.
I first tried a current of illuminating gas, well dried and
freed from hydrogen sulphide by a potash tube. In spite
of long ignition, the MgS was unaltered. Then I tried
hydrogen, but that also was unsuccessful, the MgS would
not give up its sulphur to hydrogen at a bright red heat.
Since hydrogen alone does not act on MgS, it is hardly
* Dingier, 148, 371.
316 APPENDIX.
to be expected that a hydrocarbon can remove any sulphur
from it.
" To find how carbonic oxide acted towards MgS, I ig-
nited the latter in a stream of this gas. The magnesium
sulphide used contained 56.5 per cent, sulphur and 33.0
per cent, magnesium, or 12.47 per cent, more sulphur
than the formula MgS allows. Under these circumstances
COS was evolved, recognized by forming barium sulphide
and sulphate, when led into baryta water. As soon as
these gases ceased coming off, I cooled the tube in a current
of carbonic oxide. The material had retained its former
color and still readily evolved hydrogen sulphide in moist
air or water. But it had lost 12.23 per cent, of its weight.
The gas, it appears, had united only with the sulphur in
excess of that required to form MgS, and the polysulphide
was thus changed to the monosulphide."
Reichel makes the following summary: —
" The above researches show that magnesium and alu-
minium can unite with sulphur directly at a high temper-
ature. Also, that MgS and Mg2OS will be formed when
magnesia is similarly treated. Alumina is unattacked by
sulphur. Alumina and magnesia are changed by ignition
in carbon bisulphide to sulphides. When carbon bisulphide
and oxide act on magnesia, Mg2OS remains ; alumina is un-
changed. Magnesia is changed by ignition in hydrogen
sulphide to MgS, but the operation is tedious and imper-
fect. By melting the oxides with sulphur no sulphides can
be obtained ; with alumina the contemporaneous action of
a reducing agent is necessary, while magnesia melted with
carbon and sulphur or heated in hydrogen and sulphur
vapor becomes MgS.
" APS3 possesses a yellow color, is with difficulty fusi-
ALUMINIUM SULPHIDE. 317
ble, but fuses to a hard crystalline mass. Usually it is
obtained as a sintered yellow powder. In damp air or
water the following reaction takes place: —
APS3+6H2O==A12(OH)6 + 3H2S.
" It burns in the air to alumina and sulphur dioxide.
MgS forms a polysulphide, as we have seen, but APS3 does
not.
" Also, APS3 and MgS appear to be reduced at a high
heat by metals which have a greater affinity for sulphur,
yet it remains to be seen whether this property is techni-
cally valuable."
Leaving these two experimenters, Fremy and Reichel,
we have very few allusions to the subject. Those who
have proposed to produce aluminium from APS3 state
merely that they use Fremy 's process for preparing the
APS3.
We have found an article* in which it is proposed to pass
vapor of carbon bisulphide and hydrochloric acid together
over ignited alumina, APS3 being formed as an intermedi-
ate product , and APC16 ultimately formed by the action of
the acid. The writer states that by passing the first alone
over the ignited alumina the gas evolved is mostly COS,
though a portion of it is decomposed to sulphur and car-
bonic oxide. He further states that APS3 is only slightly
acted on by sodium chloride, is unaffected by calcium or
magnesium chlorides, slightly acted on by potassium chlor-
ide, but readily chloridized by hydrochloric acid.
F. Lauterborn (see p. 206) claims in a patented process
that by calcining aluminium fluoride with calcium sulphide
* Chem. News, Dec. 19, 1873.
27*
318 APPENDIX.
APS3 results. I cannot find any corroboration of this
statement.
Mr. Niewerth's process for reducing aluminium, in which
he either uses APS3 or else makes it as an intermediate
product, will be found in full on p. 185, it being too long
to repeat here. I cannot find any outside testimony as to
the possibility of his schemes.
Reichel has probably proven the possibility of reducing
APS3 by a metal having more affinity for sulphur. From
a chemical standpoint its reduction by copper, iron, etc.,
should be under the proper conditions a very easy opera-
tion. These conclusions follow from the relative affinity
of sulphur for the metals, which is set forth in the follow-
ing investigation : —
" A. Orlowsky* has studied the affinity of sulphur
for the metals. From his researches it was found that
it usually possesses the greatest affinity for the alkaline
metals, with which it forms polysulphides. Among the
other metals, copper possesses the greatest affinity for sul-
phur, then follow in order mercury, silver, iron, lead, and
after these platinum, chromium, aluminium, and magne-
sium, whose affinities for sulphur are quite insignificant."
EXPERIMENTS ON AL2S3.
Taking the data given in the foregoing papers, I made
a series of experiments on first making APS3 and then
on reducing it.
Experiment L
Took pure, white alumina, made by calcining pure sul-
* Jahresb. der Chemie, 1881, p. 24.
ALUMINIUM SULPHIDE. 319
phate of alumina, put it in porcelain boats in a hard glass
tube, and passed vapor of carbon bisulphide, CS2, over it
at bright redness for forty-five minutes. The product was
cooled out of contact with the air. The result was a gray-
ish-black powder, not sintered together in the least. On
analyzing the product by Fremy's method, it showed 12.65
per cent, of A12S3.
Experiment II.
Took equal parts of alumina, sulphur, and charcoal,
ground intimately together in a mortar, and served as in
Experiment I, prolonging the action of CS2 to an hour and
a half. The product was a grayish-black powder, similar
in appearance to the former product. It contained 38.51
per cent. APS3.
Experiment III.
Repeated Experiment I, but used a porcelain tube, thus
allowing a higher heat than the glass tube would stand.
The treatment lasted an hour and a half. The product
was of similar appearance to the previous ones, and con-
tained 39.54 per cent. Ai2S3.
Experiment IV.
I placed some ordinary aluminium sulphate, A12(SO4)3.-
18H2O, in the porcelain tube, and heated it gradually up
to bright redness with the tube open at both ends, cal-
cining it thus for two hours. The result was that the tube
was filled with very porous alumina. CS2 was then passed
over it for two hours, the whole being kept at redness.
The product was dirty-white, but lemon-yellow in places,
and at the yellow parts sintered together, Analyzing an
320 APPENDIX.
average specimen, it showed 31.16 per cent, APS3. It is
probable that if a yellow piece had been singled out it
would have shown much 'more APS3 than this average
sample.
Experiment V.
I placed some pure alumina in small hollows cut in
pieces of charcoal, and placed these in the tube instead of
the porcelain boats. The tube was then placed in an
assay furnace and heated almost to whiteness for an hour
and half, CS2 being passed through. The product was
small, black, fused buttons melted down into the bottoms
of the cavities in the charcoal. These lumps were black
outside, brittle, compact fracture, and the broken surfaces
mottled, dirty-white, and yellow. They had a strong smell
of hydrogen sulphide, and when dropped into water this
gas was evolved so actively as to make quite a buzz, resem-
bling the action of a piece of zinc dropped into acid. In
one or two minutes the button was resolved into a black
powrder. This product contained 40.43 per cent. APS3.
Experiment VI.
Repeated Experiment V, but used porcelain boats. The
product was still dark, and contained 38.80 per cent. APS3.
Experiment VII.
Wishing to make a quantity of the substance, I filled
the tube with alumina, put it in a hot fire, and passed CS2
over it three hours. The product was grayish-black, with
here and there touches of yellow, with lumps of consider-
able size sintered together. An average sample of it con-
tained 32.32 per cent. APS3.
ALUMINIUM SULPHIDE. 321
Tabulating these results we have —
Experiment I. II. III. IV. V. VI. VII.
Al*S3(p.ct.) 12.65 38.51 39.54 31.16 40.43 33.80 32.32
First I would notice that, as remarked by Fremy, the
APS3 formed incloses the particles of alumina and prevents
further action. It seems highly probable that a stirring
apparatus to keep the alumina agitated would greatly im-
prove the product. Experiment I gave poor results because
the heat was not sufficient ; Experiment II was done at a
higher heat, with addition of carbon, and Experiment III
at a still higher heat, without carbon. It appears from
this that the presence of carbon had very little influence
on the amount of A12S3 produced. Experiment V, giving
the best results, was worked, I think, at a higher heat than
any of the others ; but Experiment VI was conducted
under as nearly as possible the same conditions ; however,
we may consider the products as being nearly enough
alike, the carbon does not appear to have made a marked
difference in the product.
To establish such a process on a practical scale, a
wrought-iron or fire-clay retort would be necessary, with
arrangements to heat it almost to whiteness. Boats of
charcoal, holding ample charges of alumina, are made to
fit in the retort. Some sort of stirring apparatus to agi-
tate the alumina from time to time should be provided.
The CS2 could be brought in superheated by waste heat
from the furnace and passed out into a condenser. Or, to
economize still further, the retort might be lengthened, its
forepart made a producer of CS2, by passing sulphur vapor
over carbon, and the rear part be filled with the alumina to
utilize this CS2. Many other devices will occur to the
322 APPENDIX.
practical chemist in running such a process, the above
being mere suggestions.
REDUCING THE AL2S3.
Experiment VIII.
I took about half a gramme of product of VII, and
wrapping it tightly in lead-foil placed it on a cupel and
heated in a muffle. Air was kept from the metal by a
close-fitting porcelain cover. On removing the lid after a
few minutes, there appeared a button of lead with some
powder on its surface. I then cupelled the lead at as
low a temperature as possible. The metal cupelled away
entirely, leaving no aluminium. On repeating with every
precaution the result was the same.
Experiment IX.
About one gramme of product VII was wrapped in
copper foil, put in a porcelain crucible, and covered with
NaCl and a little charcoal. A close cover was put on,
the whole placed in the middle of a Hessian crucible, the
latter filled up with fine charcoal, and a cover luted on.
On heating this an hour at bright redness, hardly white-
ness, there resulted a large button of copper. However, its
specific gravity was that of pure copper, and a qualitative
test showed no trace of aluminium. It occurs to me now
that probably the NaCl reacted on the APS3, forming alu-
minium chloride and sodium sulphide, preventing the
action of the copper.
Experiment X.
Repeated Experiment IX with tinfoil, and heating only
twenty minutes. The tin resulting showed some alumin-
ALUMINIUM SULPHIDE. 323
him on a qualitative test, and on analyzing it I found 0.52
per cent. Considering the small amount of sulphide and
the rather large amount of tin used, it is probable that
nearly all the aluminium present as APS3 was reduced.
Experiment XL
Repeated the same, but using powdered antimony to
mix with the APS3. The resulting button was pure anti-
mony with no aluminium in it.
Experiment XII.
Repeated the experiment, employing fine iron filings and
using a high heat for one and a half hours. The product
was a loose mass in which were small buttons of metal.
These buttons were bright, yellower than iron, and con-
tained 9.66 per cent, aluminium.
Lack of time and opportunity prevented my extending
these experiments on reduction. I had intended trying
copper filings, zinc filings, mercury — excluding air by
using a vacuum or an atmosphere of hydrogen — or its re-
duction by hydrogen gas.
On reviewing the experiments reported above, those with
tin and iron succeeded best. Knowing the great affinity
of copper for sulphur, I cannot but think that an experi-
ment with very fine copper filings intimately mixed with
the APS3 would give satisfactory results.
In closing I would remark that a process such as sug-
gested on p. 321 could be easily arranged on a large scale,
the undecomposed CS2 being caught and so no more of it
used than is necessary to supply sulphur for the A12S3.
The product could be mixed with fine metallic filings, 'put
into a crucible, surrounded by charcoal, and the alloy
324 ADDENDA.
made. The metal changed to sulphide could be recovered
by reducing the slags. These processes have been covered
by patents, but have never been made successful. It ap-
pears that if rightly managed they will give good results
and produce aluminium alloys cheaply.
ADDENDA.
ADDITIONAL DETAILS OF CASTNER'S SODIUM
PROCESS.
" In the ordinary sodium process,* lime is added to the
reducing mixture to make the mass refractory, otherwise
the alkali would fuse when the charge is highly heated,
and separate from the light, infusible carbon. The carbon
must be in the proportion to the sodium carbonate as four
is to nine, as is found needful in practice, so as to assure
each particle of soda in the refractory charge having an
excess of carbon directly adjacent or in actual contact.
Notwithstanding the well-known fact that sodium is
reduced from its oxides at a degree of heat but slightly
exceeding the reducing point of zinc oxide, the heat
necessary to accomplish reduction by this process and to
obtain even one-third of the metal in the charge, closely
approaches the melting point of wrought iron.
** In my process, the reducing substance, owing to its
composition and gravity, remains below the surface of the
molten salt, and is, therefore, in direct contact with the
* Journal of the Franklin Institute, Nov. 1886.
325
fused alkali. The metallic coke of iron and carbon con-
tains about 30 per cent, carbon and 70 per cent, iron,
equivalent to the formula FeC2. I prefer to use caustic
soda, on account of its fusibility, and mix with it such
quantity of so-called ' carbide' that the carbon contained
in the mixture shall not be in excess of the amount theo-
retically required by the following reaction : —
SXaOH + FeC2 = 3Na + Fe + CO+ CO2 + 3H ;
or, to every 100 pounds of pure caustic soda, seventy-
five pounds of * carbide,' containing about twenty-two
pounds of carbon.
" The necessary cover for the crucible is fixed station-
ary in each chamber, and from this cover a tube projects
into the condenser outside the furnace. The edges of the
cover are convex, those of the crucible concave, so that
when the crucible is raised into position and held there
the tight joint thus made prevents all leaking of gas or
vapor. Gas is used as fuel, arid the reduction begins
towards 1000° C. As the charge is fused, the alkali and
reducing material are in direct contact, and this fact,
together with the aid rendered the carbon by the fine
iron, in withdrawing oxygen from the soda, explains \vliy
the reduction is accomplished at a moderate temperature.
Furthermore, by reducing from a fused mass, in which
the reducing agent remains in suspension, the operation
can be carried on in crucibles of large diameter, the
reduction taking place at the edges of the mass, where
the heat is greatest, the charge flowing thereto from the
the centre to take the place of that reduced.
" I am enabled to obtain fully ninety per cent, of the
metal in the charge, instead of thirty per cent, as formerly.
28
326 ADDENDA.
The crucibles, after treatment, contain a little carbonate
of soda, and all the iron of the ' carbide' still in a fine
state of division, together with a small percentage of. car-
bon. These residues are treated with warm water, the
solution evaporated to recover the carbonate of soda, while
the fine iron is dried, and used" over again for ' carbide."'
NEW PROCESS FOR MAKING ALUMINIUM CHLORIDE.
Mr. Cha's. F. Mabery has patented and assigned to
Cowles Bros, a new process for making anhydrous alu-
minium chloride. The patent was granted Oct. 26, 1886.
The first claim is for producing it by passing chlorine gas
over an alloy of aluminium and some other metal kept in
a closed vessel at a temperature sufficient to volatilize the
APC16 formed, which is caught in a condenser. The
second claim is for passing hydrochloric acid gas through
the electric furnace in which alumina is being decomposed
by carbon, a condenser being attached as before.
REMARKS ON THE MITIS CASTINGS.
Mr. W. H. Wahl, Secretary of the Franklin Institute,
Phila., makes the following remark on this subject: — *
" The simplicity of this process, the certainty with
which it can be operated, the uniformity of the product,
and its good qualities in respect to strength and ductility,
indicate an extended field of usefulness for it. The mitis
castings threaten to seriously incommode the manufac-
turers of malleable castings, for which they not only offer
* Journal of the Institute, Nov. 1886.
PRODUCTION OF ALUMINIUM. 327
a perfect substitute, but one which, in respect to strength
and ductility, is distinctly superior, while for many pur-
poses mitis castings can be employed for which malleable
castings could not be made. The mitis process has also
been applied to the production of steel castings, and with
promising results. In one of the methods experimentally
tested, the sheet castings were from wrought iron scrap
as raw material, with the addition of the proper propor-
tion of cast iron to bring the percentage of carbon to the
point required for each special purpose."
PRODUCTION OF ALUMINIUM.
From advance proof-sheets of vol. iii. 'Mineral Re-
sources of the United States,' we learn* that the produc-
tion of metallic aluminium in the United States increased
from 1800 troy ounces in 1884 to 3400 ounces in 1885,
valued at $2550. Aluminium bronze, ten per cent., was
made to the amount of about 4500 pounds, valued at
$1800.
In October, 1886, a Philadelphia instrument maker
accepted the offer, from the maker, of a large amount of
European aluminium at the price of 50 cents per ounce,
the lowest at which aluminium has yet been sold.
* Sci. Am., Nov. 13, 1886.
INDEX.
Academy, Paris, patronage of, i Alloys of aluminium and mer-
towardfi Deville, 32
Acetic acid, action of, on alu-
minium, 78
Acid, acetic, action of, on alu-
minium, 78
hydrochloric, action of, on
aluminium, 75
muriatic, action of, on alu-
minium. ?.">
nitric, action of, on alu-
minium, ~~)
sulphuric, action of, on alu-
minium, 74:
tartaric, action of, on alu-
minium, 78
Acids, organic, action of, on alu-
minium, 78
Air. action of, on aluminium,
70
Albite, formula of, 43
Alkalies, caustic, action of, on
aluminium, 77
Alkaline carbonates, action of,
on aluminium, 88
Alloys, aluminium, made by
Cowh's Bros., 205
of aluminium, 258-303
and antimony. 21'2
and bismuth' 292
and boron, 1199
and cadmium, 299
and carbon. Moo
and copjXT, 204:
and gallium, 300
and gold.
and iron, 280
, and lead, -J'. > L
and mangan
cury, 201
and molybdenum, 302
and nickel, 293
and nitrogen, 303
and platinum, 299
and silicon, 259
and silver, 295
and sodium, 303
and tin, 289
and titanum, 301
and tungsten, 302
and zinc, 287
with steel, 281
of brass and aluminium. 276
of German silver and alu-
minium, 277
Alumina, composition of, pre-
cipitated, 105
crucibles, use of, for obtain-
ing aluminium, 228
in purifying alumin-
ium, 243
extracted from alum stone
or shale, 153
manufacture of, 144-153
manufactured from cryolite,
28*
dry way, 14/>
wet way, 152
precipitation of, by carbonic
acid gas, 149
reduction of, by carbon in
presence of copper, 309
sulphate of, Tilghman's pro-
cess for decomposing, 144
Aluminate of soda crucibles, use
of, in purifying alu-
minium. 24:?'
330
INDEX.
Aluminate of soda precipitation
by Lovvig, 151
precipitation of, at Sal-
indres, 159, 103
Aluminite, formula of, 44
Aluminium, alloys of, 258-303
amalgam, properties of, 263
bronze, solders for, 279
chemical properties of, 70-
89
Crown Metal Co.'s, 173
makers of alumin-
ium bronze, 274
crucibles, use of, for obtain-
ing aluminium, 228
history of, 25-42
manufacture at Salindres
(Gard), 158-171
metallurgy of, 90-257
occurrence in nature, 43-50
physical properties of, 51-70
plate as a substitute for tin
plate, 247
protoxide, 26
reduction of, by other agents
than sodium, 180
silver, 297
sodium, double chloride,
making of, 154-157
uses of, 243-247
working in, 235-257
Alum-shale, use of, for making
alumina, 153
Alum-stone, use of, for making
alumina, 153
Alums, native, impurities in, 45
Alunite, formula of, 44
Amalgam, potassium, used in
isolating aluminium, 25
Amalgamation of aluminium,
261, 308
Wohler's efforts, 25
American aluminium, 306
Co., Detroit, 221 ,
price of, 1883-84, 39
cryolite, 48
Amfreville-la-mi-Voie, alumin-
ium works at, 29, 33
process used at, 124
Ammonia, aqua, action of, on
aluminium, 78
Analyses of beauxite, 46
Analyses of commercial alumi-
nium, 51, 52
of Mr. Frishmuth's metal,
307
Analysis of aluminium sulphide,
311
of Bombay Wootz for alu-
minium, 283
Animal matters, action of, on
aluminium, 87
Animals, aluminium never found
in, 44
Annealing of aluminium, 58
Anorthite, formula of, 43
Antimony, alloys of aluminium
with, 292
reduction of aluminium sul-
phide by, 323
Argentan, a serviceable alloy, 294
Artistic purposes, use of alumin-
ium for, 245
Balance beams, special value of
aluminium for, 35
Barattes for precipitating alu-
mina, 163
Barium, alloys with aluminium,
87
oxide, action on aluminium,
87
Barlow, W. H., on the tensile
strength of aluminium, 62
Basset, M. N., reduction of alu-
minium by zinc, by, 215
Battersea, London, first alumin-
ium works in England, 33
Battery, use of aluminium in
the, 75
to deposit aluminium, 80
Baudrin, P., on a new aluminium
alloy, 278
Beating of aluminium, 57
Beaux, analysis of beauxite from,
47
Beauxite, 45-47
analyses of, 46
and cryolite, chief source of
aluminium, 45
stimulated production
of, 27
deposits in Ireland, France,
etc., 46
INDEX.
331
Beauxite. formula of, 44
treatment of, at Saliudres,
100
where principally found in
France, 100
Beketoff, on the action of oxide
of barium on aluminium, 87
Bell Bros., directions for solder-
ing aluminium, 252
makers of aluminium at
Newcastle-on-Tyne, 33
stoppage of their alu-
minium works, 35
Bells, aluminium, 63
Benjamin, Mr., additional details
of Castner's sodium process,
Benzine, use of, in melting alu-
minium, 230
Benzon, iron process of, 211
Berlin, aluminium works in, 35
Bertrand, M. A., deposition of
aluminium by electricity, 232
Berzelius, investigation on the
composition of cryolite, 104
Bessemer converter, reduction of
aluminium in the, 207
reduction of sodium and
potassium in, 208
Birmingham, England, Webster's
aluminium works at, 36
Bismuth, alloys of aluminium
with.
Blast furnace, reduction of alu-
minium in a, 185-204
Books on aluminium, Tissier
Bros., 28
Deville's. 20
Mierzinski's, £9
Borates, action of, on aluminium,
84
Boron, alloys of aluminium with,
299
Boudaret, M., report on the mal-
leability of aluminium bronze,
2or
Bourbouze, M., on an aluminium
tin alloy, 290
Brass, aluminium, strength of,
276
compared with aluminium
bronze, 27 1
Braun, John, deposition of alu-
minium by electricity, 2^53
Bremen, aluminium works at.
229 '
Bromide of aluminium used for
making pure aluminium, 243
Bromine, action on aluminium, 88
Bronze, aluminium, 264
a true alloy, 265
compared with brass, 271
compressive strength of,
•jr.'
Cowles Bros., 274
first exhibited at Paris,
1867, 34
making of, 267
malleability of, 267
manufactured by M.
Evrard, 211
melting point of, 271
phosphorized. 279
price in 1878, by the So-
ciete Anonyme, 36
production in the United
States in 1885, 327
specific gravity of, 271
tenacity of, 266, 267, 270,
276
silicon-aluminium, 205,280
silicon, manufactured by M.
Evrard, 211
B runner, reduction of sodium by,
131
Buchner, G., purification of alu-
minium from silicon, by, 243
Buff and Wbhler on the solution
siliceous aluminium, 260
Bunsen and Deville's electrolytic
method of separating alumin-
ium, 41
Bunsen, electrical process of, for
depositing aluminium, 222, 225
Burnishing of aluminium, 55
Cadmium, alloys of aluminium
with, 299
Caillet, on the amalgamation of
aluminium, 261
Calcination furnace for sodium
mixture, 133
Thomson's, for cryolite,
146
332
INDEX.
Calcination retorts for alumi-
nium-sodium chloride at Sa-
- lindres, 166
Calcutta, aluminium at the ex-
hibition of, in 1883, 246
Calvert and Johnson, making of
iron aluminium alloys,
282
reduction of aluminium
by iron, 209
Camden, N. J., aluminium made
at, 31
Carbon, action on aluminium, 88
alloys of aluminium with,
300
and aluminium, alloy of, 203
and carbon dioxide, reduc-
tion of aluminium by, 187
as lining for earthen cruci-
bles, 36
changed to graphite, 193
dioxide and carbon, reduc-
tion of aluminium by, 187
disulphide, use of, for making
aluminium chlo-
ride, 317
for making alumin-
ium sulphide, 310
reduction of aluminium by,
188-206
Carbonates of alkalies, action on
aluminium, 88
Carbonic acid gas, lime-kiln for
producing, 150
used for precipitat-
ing aluminium,
149, 163
Carburetted hydrogen, reduction
of aluminium by, 182
Casting of aluminium, 237
its importance, 36
the largest ever
made, 39
Castings, Mitis, alloy used for
making, 212
Castner, claims made in his pat-
ent, 141
process for reducing sodium
by, 324
reduction of sodium by, 131
Chalk, object of using, in the
reduction of sodium, 133
Chanu, aluminium plant at
Rouen, 29
Chapelle, M., on the reduction
of aluminium by carbon, 188
Charridre, on soldering alumin-
ium, 248
use of an aluminium tube in
tracheotomy, 87
Chemical classification of alu-
minium, 88
properties of aluminium,
70-89
reactions in the sodium pro-
cess, 158
Chemically pure aluminium, di-
rections for making, 243
Chlorhydrate of aluminium, 85
Chloride of aluminium, a new
process for producing,
326
Dullo's process for mak-
ing, 155
improved method for
producing, 157
Chlorides, metallic, action on
aluminium, 85
Chlorine, action on aluminium,
88
Christofle, M., castings of alu-
mipium bronze, 265
gilding of aluminium, 80
on soldering aluminium, 248
on the use of aluminium-
silver alloy, 296
Classification, chemical, of alu-
minium, 88
Clay, cryolite, as lining for
earthen crucibles, 36
Clays, alumina the base of, 43
Cleaning of tarnished alumin-
ium, 54
Cleveland, manufacture of alu-
minium in, 41, 190
Coating of metals with alumin-
ium, 231
iron with aluminium, 247
Coins, use of aluminium for.
247
Color of aluminium, 53
Combinations of aluminium, 43
Combustion of aluminium leaf,
71
INDEX.
333
Comenge, M., double reaction
method of,
Commercial aluminium, analyses
of, 51
made chiefly by Deville's
process, 41
Compressive strength of alu-
minium bronze, 2~2
Condenser for sodium, 131
Conductivity of aluminium for
heat, 67
electric, of aluminium, 66
Converter, the Bessemer, reduc-
tion of aluminium in,
807
reduction of sodium and
potassium in, 208
Cooking, aluminium utensils for,
245
utensils, valuable property
of aluminium for, 68
Copper, alloys of aluminium
with, 264-280
deposition of, by aluminium,
81
freeing of aluminium from,
240-
oxide, action on aluminium,
87
reduction of aluminium by,
212
of aluminium-sulphide
by, 322
the quality suitable for alu-
minium bronze, 267
Coppering of aluminium, 80
Corbelli, of Florence, cyanogen
process of, 180
process of, for deposit-
ins: aluminium elec-
trolytically, 231
Cornwall, supposed discovery of
native aluminium at, 43
Corundum, 49, 50
discovery in Georgia, 49
from Georgia, used by
Cowles Bros., 205
price at the mim->. 40
use of, for making alumin-
ium, 37
Cost of aluminium at Salindres
in is;:.', 172
Cowles's aluminium process, his-
tory of, 41
Cowles Bros.' agent in England,
197
aluminium bronze made
by, 274
aluminous materials used
by, 205
owners of a patent for
producing aluminium
chloride,^326
patent claims, 190
process for the reduction
of aluminium by car-
bon, 189-205
Cross, W., description of Ame-
rican cryolite, 48
Crucible clay, action on alumin-
ium, 84
Crucibles, action of aluminium
on siliceous, 259
alumina, use of, for obtain-
ing aluminium, 228
in purifying alumin-
ium, 243
aluminate of soda, use of,
in purifying aluminium,
243
aluminium, use of, for ob-
taining aluminium, 228
earthen, action of aluminium
on, 35
iron, used by Rose, 106
use of, in purifying alu-
minium, 241
lime, for melting alumin-
ium, 36
lining for, 35, 123
porcelain, use of, for obtain-
ing aluminium. 228
used in electrolyzing alu-
minium, 224
Cryolite, Allen Dick's experi-
ments on reduction of, 115
and Beauxite, chief source
of aluminium, 45
stimulated production
of, 27
Berzelius's investigation of
its composition, 104
clay as lining for earthen
crucibles, 36
334
INDEX.
Cryolite, composition of, 119
decomposition of, 306
by electricity, 230
Deville's process for reduc-
ing, 119-126
Dr. Percy's experiments on
reducing, 115
formula of, 44
general use as a flux, 48
H. Rose's paper on reduction
of, 103-1 15
importation of, by the Penn-
sylvania Salt Co., 48
imports into the United
States, 49
in the United States, 48
manufacture of alumina
from, 146-153
occurrence of, 48, 49
reduction of, 103-129
at Nanterre, 126
by ferro-silicum, 207
Watts's summary of its use,
127
Crystalline form of aluminium,
69
Crystallization of aluminium , 115
Crystallized silicon, 260
Culinary articles, use of alumin-
ium for, 68, 245
Cupellation of aluminium, 71
from lead, 291
Curaudau, reduction of sodium
by, 131
Cyanite, formula of, 44
Cyanogen, reduction of alumin-
ium by, 180
Davy, reduction of sodium by,
131
unsuccessful efforts to isolate
aluminium, 25
Debray, H., aluminium plant at
Glaciere, 28
Debray, M., statement of, in re-
gard to iron in aluminium, 282
Decomposition furnace for so-
dium mixture, 134
of aluminium sulphide by
water, 311, 317
Degousse, first successful beater
of aluminum leaf, 58
De la Rive, on the action of sul-
phuric acid on aluminium, 74
Denis, M., of Nancy, remark on
the soldering of aluminium,
248
Density of aluminium, 64
Deposition of aluminium by elec-
tricity, 255
by the battery, 80
electrolytically, 222-234
Deville, aluminium plant at Gla-
cidre, 28
analysis of beauxite by, 47
book on aluminium, 1859,29
charges against Tissier Bros.,
28
conclusion of his book, 30
description of the reduction
of sodium, 132
experiments on gilding and
silvering aluminium, 256
H. St. Claire, first to isolate
pure aluminium, 26
on soldering of aluminium,
247
on the aluminium obtained
by Wbhler, 95 .
on the casting of aluminium,
237
on the electrolytic reduction
of aluminium, 223, 225
on the melting of alumin-
ium, 235
on veneering with alumin-
ium, 253
purification of aluminium,
238
researches of, at the Normal
School, Paris, and at
Javel, 28
on cryolite by, 118
review of Percy's and Rose's
investigations of cryolite,
118
treatment of silicates and
borates with aluminium, 84
Deville's cryolite process, Wo li-
ter's improvement on, 126
improvements in 1854 for ob-
taining pure aluminium, 96
processes, later improve-
ments on, 173
INDEX.
335
Deville's sodium vapor process,
100
Diaspore, formula of, 44
where found, 50
Dick, Allan, paper on reducing
cryolite, 116
Disthene, reduction of, by an
electric current, 229
Donny and Mareska, condenser
for making sodium, 131
Double reaction, reduction of
aluminium by, 1*4
Drawing of aluminium into wire,
60
Drecbsler, analysis of beauxite
by, 47
Dublin, analysis of beauxite
from, 47
Ductility of aluminium, 60
Dullo, M., process for making
aluminium chloride, loo
remark on the reduction of
aluminium by zinc, 214
Dumas, on gases in aluminium,
52
Duvivier. M., on reduction of
aluminium by electricity, 229
Dynamo used in Cowles Bros.'
process, 204
Elastic rangre of aluminium, 62
Elasticity of aluminium, (U
Electric conductivity of alumin-
ium. »5H
furnace, Cowles Bros., 199
suggested by Miefzinski,
226
use of, for producing
aluminium chloride,
326
Electrical furnace, gases from
the, 197
separation of aluminium, 255
Electricity applied to melting
* steel, 194
to the extraction of
metals, 1J»4
reduction of aluminium by,
222
of sodium by, 131
un.-uccessful efforts of Davy
to i>olatc aluminium by. '!•)
Electrolytic methods of separat-
ing aluminium, 41
Enamelling mixture to protect
sodium retorts, 135
England, Cowles Bros.' agent in.
197
failure of aluminium manu-
facture in, 35
first aluminium wrorks in, 33
Webster perhaps the only
maker of aluminium in, 42
Engraving of aluminium, 61
Evrard, M., making of alumin-
ium bronze by, 211
Falk & Co., makers of alumin-
ium leaf, 60
Faraday's experiments on the
sonorousness of aluminium, 64
Farmer, Moses G.. patented ap-
paratus of, for electrolytically
obtaining aluminium, 233
Favre, M., on solution of alu-
minium in hydrochloric acid,
75
Feisstritz, analysis of beauxite
from, 47
Ferro-silicum, reduction of alu-
minium by, 206
Fixity of aluminium, 66
Fleury, A. L., carbu retted hy-
drogen process of, 182
Fluoride of aluminium, Ger-
hard's process of re-
ducing, 181
Lauterborn's process of
reducing, 206
reduction by ferro-sili-
cum, 206
Fluorides as fluxes, 260
use of, as flux, 102-120
Fluorine, action on aluminium,
88
Fluorspar, action on aluminium.
84.
Flux, fluorspar as, 84
use of fluorides as a, 102-120
Fluxes for aluminium, 259
Formulae of aluminous minerals,
4:;
France, deposits of beauxite in,
46
336
INDEX.
France, production of aluminium
in, 1882, 39
successful manufacture of
aluminium in, 35
Fremy, original paper on alu-
minium sulphide, 310
Frishmuth, aluminium works in
Philadelphia, 37
analyses of the metal of, 306
improvement of, in making
aluminium-sodium double
chloride, 154
plating with aluminium-
nickel, 234
production of aluminium,
1883, 1884, 40
solders for aluminium by,
250
Frishmuth's first assertions not
verified, 42
patent claims, 178
owners of, 37
process mentioned in Watts's
Dictionary, 42
works, annual production
of, 39
Fritz, Mr., of Bethlehem, Pa.,
interest of, in the mitis process,
287
Fusibility of aluminium, 65
Furnace, Thomson's, 146
Gallium, alloys of aluminium
with, 300
Garnet, formula of, 44
Gases in aluminium, 52
from the electrical furnace,
197
Gaudin, electric process of, 230
Gay Lussac, reduction of sodium
by, 131
Gerhard & Smith, patent process
of, for depositing aluminium,
233
Gerhard, W. F., furnace for re-
ducing aluminium, 127
German silver, aluminium, 277
Germany, aluminium works in,
33
failure of aluminium manu-
facture in, 35
reduction of aluminium in,
228
Gila River, N. M., native sul-
phate of alumina on the, 305
Gilding of aluminium, 80, 256
Glaci£re, process for making alu-
minium, as used at, 98
purification of aluminium
from slag at, 239
Rousseau Bros., aluminium
works at, 28
Glass, action of, on aluminium,
84
Gmelin, an observation on alu-
minium amalgam, 263
Gold, allo\'s of aluminium with,
298
Gordon, A., on the tensile
strength of aluminium bronze,
266
Gore, deposition of aluminium
on copper, 234
Granite, composition of, 43
Graphite, carbon changed to,
193
cylinders, use of, to protect
retorts in sodium reduc-
tion, 135
Gratzel, Richard, electrolytic pro-
- cess of, 228
Gravity, specific, of commercial
aluminium, 307
Greenland, cryolite in, 48
Grousilliers's improvement of re-
ducing under pressure, 179
Guettier, remarks on aluminium
bronze, 273
Guiana, deposits of beauxite in,
46
Hadamar, analysis of beauxite
from, 47
Hamburg, aluminium works at,
229
Hardness of aluminium, 61
Harmlessness of aluminium salts
to the body, 79
Havrez, P. J., washing appara-
tus of, 149
Heat, conduction of, by alumin-
ium, 07
specific, of aluminium, 68
Helmet, an aluminium, 245
Herreshoff', importer of beauxite
into the United States, 47
INDEX.
337
Hesse, analysis of beauxite frora,
47
deposits of beauxite in, 46
Hillebrand, description of Amer-
ican cryolite, 48
Hirzel, on alloys of aluminium
and silver, 296
History of aluminium, 25-42
Hodges, F., analysis of beauxite
by, 47
Hulot, coppering of aluminium,
80
method of soldering alu-
minium, 248
on the use of aluminium in
the battery, 75
Hunt, Dr. T. Sterry, paper on
Cowles's process, 194
second paper on Cowles's
process, 196
views on the aluminium
industry, 42
Hydrochloric acid, action of, on
aluminium, 75
Hydrogen, action on aluminium,
88
reduction of aluminium -by,
181
sulphide, action of, on alu-
minium, 73
use of, to purify aluminium,
243
Imports of aluminium, 1870 to
1884, 40
Impurities, freeing of aluminium
from, 240
Instruments, mathematical, etc.,
suitability of aluminium
bronze for, 268
optical and portable electric,
a suitable alloy for, 290 .
Iodine, action on aluminium,
88
Ireland, analysis of beauxite
from, 47
deposits of beauxite in, 46
Iron, alloys of aluminium with,
280
with aluminium, 209
aluminium alloy, production
of, :;-j:]
29
Iron, aluminium alloy, used in
the mitis process, 212
coated with aluminium, 247
crucibles, use of, in purify-
ing aluminium, 241
used by Rose, 106
freeing of aluminium from,
240
in commercial aluminium,
estimation of, 307
oxide, action on aluminium,
86
reduction of aluminium by,
206
sulphide by, 323
Ivigtuk, Greenland, cryolite beds
at, 48
Jablochoff, reduction of sodium
by, 131
Javel, chemical works at, 28
process for making alumin-
ium as used at, 98
Jeancon, J. A., patented process
for depositing aluminium,
232
Jewelry, aluminium, 247
Johnson, double reaction method
of, 184
Jouet, Mr., analysis of beauxite
by, 47
j Joules, on the amalgamation of
aluminium, 262
_
Kagensbusch, electric process of,
230
of Leeds, on reduction of
aluminium by zinc, 218
on reduction of aluminium
by lead, 222
Kamarsch, on the tensile strength
of aluminium, 63
Kerl and Stoh man, directions for
soldering aluminium,
by, 250
historical r6sum6 by, 32
on the melting of alu-
minium, 236
Klein Steinheim, analysis of
beauxite from, 47
Knight, remarks on aluminium
bronze, 273
338
INDEX.
Knowles, Sir F. C., cyanogen
process of, 180
Lang, I., analysis of beauxite'
by, 47
Langsdorff, analysis of beauxite
from, 47
Lauterborn, iron reduction, pro-
cess of, 206
Lauterborn's process for decom-
posing cryolite tested,
remark on, 317
Lavoisier, first to suggest the
existence of aluminium, 25
Lazulite, formula of, 44
Lead, action on an aluminium-
tin alloy, 196
alloys of aluminium with,
291
deposition of, by aluminium,
82
freeing of aluminium from,
241
oxide, action on aluminium,
86
reduction of aluminium by,
221
sulphide by, 322
Leaf aluminium, 245
beating of, 57
combustion of, 71
decomposition of water
by, 73
Lechatelier, M., on the tensile
strength of aluminium bronze,
266
Lecoq de Boisbaudran, on alu-
minium-gallium alloys, 300
"Lessiveur methodique," 149
Liebig, experiments to reduce
aluminium, 93
Lime, action of, on aluminium,
77
crucibles for melting alu-
minium, 36
kiln , use of, to furnish car-
bonic acid gas, 150
phosphate of, action on alu-
minium, 85
Lining for crucibles, 123
Liquation of aluminium, 238-240
Lissajous, M., aluminium tuning
fork made by, 63
Litharge, action on aluminium,
86
LIthia mica, formula of, 43
Lockport, N. Y., Cowles Bros.,
plant at, 193-196
Lbwig, experiments of, in pre-
cipitating alumina, 151
Lustre of aluminium, 55
Mabery, Prof. Chas. F., official
announcement of Cowles
Bros.' process, 191-194
on a new process for pro-
ducing aluminium chlo-
ride, 326
views on the aluminium
industry, 41
Magnesia mica, formula of, 43
Magnesium sulphide, production
and reduction of, 312-317
Magnetism of aluminium, 69
Mal^tra, aluminium plant at
Rouen, 29
Malleability of aluminium, 57
bronze, 267
Mallet, directions for making
chemically pure alumin-
ium, 243
on the resistance of pure alu-
minium to alkalies, 77
on the specific heat of pure
aluminium, 68
gravity of aluminium,
65
Manganese, alloys of, with alu-
minium, 302
oxide, action on aluminium,
86
reduction of aluminium by,
222
Manufacture of aluminium
bronze, 267
Martin, Wm., aluminium plant
at Rouen, 29
Mat, production of, on alumin-
ium, 54
Mayer, L., analysis of beauxite
by, 47
Mel ting of aluminium scraps, 235
point of aluminium, 65
INDEX.
339
Mercury, action on aluminium,
25
alloys of aluminium with,
261
deposition of, by aluminium,
81
Merle & Co., aluminium works j
at Salindres, 28, 35
Metallic aluminium not found :
native, 43
chlorides, action on alumin-
ium, 85
oxides, action on aluminium,
86
Metallurgy of aluminium, 90, 257
general remarks on the,
128
of sodium, 130-143
Metals, coating of, with alumin-
ium, 231
comparative density of, 64.
electric conductivity of, '
67
thermal conductivity of, ,
67
plating on, with aluminium,
255
precipitation of, from solu-
tion by aluminium, 79
relative affinity of sulphur
for, 318
Michel, experiment on alumin-
ium and molybdenum, 302
making of iron-aluminium
allo\> by, 383
Mierzinski, formulas of some alu-
minium minerals as given
by. 43
general remarks on alloys
of aluminium, 258
on making aluminium
bronze, 207
on the manufacture of alu-
minium-sodium chloride,
154
on the melting of alumin-
ium, 237
on the reduction of alumin-
ium by electricity, 226
remark on the electrolysis of
aqueous solutions o"f alu-
minium salts, 2: 54
Mierzinski, report on the present
state of the alumina industry,
144
Minargent, composition of, and
method of making, 278
Mineral soda, 105
Mitis castings, 283
ores suitable for, 205
W. H. Wahl's remarks
on, 326
process, iron-aluminium al-
loy used in the, 212
Molten aluminium, viscidity of,
237
Molybdenum, alloys of, with alu-
minium, 302
Monnier, Alfred, maker of
aluminium at Camden, N. J.,
31
Morin and Deville, experiments
in gilding and silverjng alu-
minium, 80
Morin, P., aluminium plant at
Glaciere, 28
experiments on gilding and
silvering aluminium, 256
improvements by, at Nan-
terre, 28
on the action of wine on alu-
minium, 78
on the specific heat of alu-
minium, 68
Morris. J.. carbon and carbon
dioxide, method of, 187
Mourey, method of soldering alu-
minium, 248
receipt for removing tarnish
from aluminium, 54
success in gilding and silver-
ing aluminium, 80, 256
Muriatic acid, action of, on alu-
minium, 75
Nanterre, aluminium works at,
28, 35
production of aluminium at,
1859, 33
reduction of cryolite at, 126*
Napoleon III., liberality of, 28
Native aluminium, 43
sulphate of alumina, 305
Neogen, composition of, 277
340
INDEX.
Newcastle-on-Tyne, Bell Bros.,
aluminium works at, 33
New York City, manufacture of
sodium in, 139-141
Nickel, alloys of aluminium with,
293
aluminium plating by Frish-
muth, 234
experiment on aluminium
aud tungsten, 302
Niewerth, double reaction,
method of, 185
iron reduction, process of,
206
Niewerth's nascent sodium pro-
cess, 179
process, remark on, 318
Nitre, action of, on aluminium,
83
purification of aluminium
by, 241
Nitric acid, action of, on alu-
minium, 75
Nitrogen, action on aluminium,
88
alloys of, with aluminium,
303
Normal School, Paris, experi-
ments at the, 28
Occurrence of aluminium in
nature, 43-50
Odor of aluminium, 56
Oerstedt, first published paper
on aluminium, 90
isolation of aluminium by, 25
Oerstedt's paper reviewed by
Wohler, 91
Ores of aluminium used by
Cowles Bros., 205
Organic acids, action of, on alu-
minium, 78
Orlowsky, A., on the relative
affinity of sulphur for the
metal, 318
Orthoclase, formula of, 43
Ostberg, Peter, inventor of mitis
castings, 283
remark on the reduction of
aluminium by iron, 212
Oxidation of aluminium, 71
Oxide of barium, action on alu-
minium, 87
Oxide of copper, action on aln-
minium, 87
of iron, action on alumin-
ium, 86
of lead, action on alumin-
ium, 86
of manganese, action on alu-
minium, 86
of zinc, action on alumin-
ium, 86
sub, of aluminium, 26
Oxides, metallic, action on alu-
minium, 86
Palais de ^Industrie, Paris, 1855,
aluminium bar exhibited at,
34
Paraffin, Wagner's use of, to pre-
serve sodium, 138
Paris Exhibition of 1855, alumin-
ium objects presented at, 28
Passemeutere, aluminium, 60
Peligot, on cupelling alumin-
ium, 71
Pennsylvania Salt Co., importers
of cryolite, 48
Pens, suitability of aluminium
bronze for, 272
Percy, Dr., experiments in mak-
ing aluminium bronze, 264
reduction of cryolite prior to
Rose, 115
Petitjean, carburetted hydrogen,
process of, 183
Petitjean's process tested by Rei-
chel,315
Philadelphia, Col. Wm. Frish-
inuth's aluminium works in,
37
Phosphate of lime, action on
aluminium, 85
Phosphorized aluminium bronze,
Phosphorus in aluminium, 126
Photo-salts of aluminium, efforts
to produce, 27
Physical properties of alumin-
ium, 51-70
Plants, alumina never found in,
44
Plating, aluminium, 231
aluminium-nickel, 234
with aluminium, 246
INltKX.
341
Platinum, alloys of aluminium
with. •-'.»'.'
Poggendorff and Reiss on the
nuiiriu'tisin of aluminium, 69
Polish of aluminium, 55
Porcelain crucibles, use of, for
obtaining: aluminium, 22><
imitation of, made with cryo-
lite, 48
Potash, action of, on aluminium, !
77
Production of aluminium bronze
in the United States in
1885,
by Col. Frishmuth,1883-
"lS8t, 40
in France, 18S2, 39
in the United States in
188"), 327
Properties of aluminium sul-
phide, 311, 316
mica, formula of, 43
Potassium, aluminium first iso-
lated by the use of, 26
amalgam, experiment with.
by Gmelin. 26:}
used in isolating alu-
minium, 'J5
and sodium, reduction to-
gether of, 138
carbonates, action on alu-
minium, 8S
chloride, action on alumin-
ium, 85
decomposition of, by
electricity, 142
cyanide as a reducing agent,
180
reduction in the Bessemer
converter, 208
in the electric furnace,
193
replaced by sodium by De-
vill.
sulphate, action on alumin-
. ium, 88
vapor of, Davy's efforts to
isolate aluminium with,
25
Precious stones, formula} of, 44
Precipitation of alumina at Sal-
indres. UW
of metals from solution by
aluminium, 79
Price of aluminium in 1857, 29
in 1878, by the Socie.6
Anonyme, 36
in 1883-84, 39
in October, 1886, 327
Proctor, Bernard S., comparison
of brass with aluminium bronze
by. 271
29*
Pure aluminium, chemically, di-
rections for making,
243
only made by using so-
dium, 42
requirement for making,
205
Purification of aluminium, 74,
238
by nitre, 83
Rammelsberg, on silicon in com-
mericial aluminium, 52
Rammelsberg, Prof., experi-
ments in reducing cryolite, 103
Rattle, baby, first article made
of aluminium, 244
Reduction furnace, Deville's, for
sodium, 134
for reducing aluminium
by sodium, 169
Gerhard's, 127
of alumina by carbon in
presence of copper, 309
of aluminium at Salindres,
168
by carbon, 188
and carbon dioxide,
187
by carburetted hydro-
gen, ISii
by copper, 212
by cyanogen. 180
by double reaction, 184
by electricity.
by feiTo-silicum, 206
by hydrogen, 181
by iron, 206
by lead, 221
by manganese, 222
by other agents than so-
dium, 180
342
INDEX.
Reduction of aluminium by sili- !
con, 207
by zinc, 214
sulphide, 315, 322
of sodium by Castner, 324
under pressure, 179
Reflectors, advantages of alu-
minium for, 245
Regnault, M., on the specific heat
of aluminium, 68
Reichel, paper on sulphides of
aluminium and magnesium, j
312-317
Reinar, G. W., on the reduction j
of aluminium by carbon, 189 ;
Reiss and Poggendorff, on the
magnetism of aluminium, 69 i
Retorts for reducing sodium,
134
Retzlaff, analysis of beauxite by, i
47
Ricarde-Seaver, Major, views on j
aluminium, 37
Rollins: of aluminium, 57
Rose, H., paper on reduction of j
cryolite, 103-115
Rouen, aluminium works near, I
29, 83
process used at, 124
Rousseau Bros., aluminium
works at Glaciere, 28
Ruby, formula of, 44
St. Austel, supposed discovery of j
native aluminium at, 43
Salindres, aluminium works at,
28, 35
cost of aluminium at, 172
manufacture of aluminium
at, 158-174
of aluminium-sodium j
chloride at, 154-166
Salt, common, action on alumin-
ium, 85
Salts, metallic, action of solu- .
tions of, on aluminium, 79 |
Sapphire, formula of, 44
Sartorius of Gottingen, first j
maker of aluminium balance I
beams, 35
Sauvage, F. H., inventor of neo- '
gen, 277
Schank, washing apparatus of.
149
Schnitzer, analysis of beauxite
by, 47
Schwarz, improvenent on Mou-
rey's solders by, 249
Scraps, aluminium, melting of,
235
melting of, by Col.
Frishmuth, 39
Sellers, Mr., of Philadelphia, on
the use of aluminium in cast-
ing iron, 284
Senct, M. L., on depositing alu-
minium by electricity, 233
Sevrard, M., success of, in ve
neeriug aluminium, 253
Seymour, Fred. J., patent for the
reduction of aluminium
by zinc, 218
second patent of, 220
Shaw, T., patented phosphor
aluminium bronze, 279
Siemens's furnace, used in reduc-
ing sodium, 135
Siemens, Sir Wm., melting of
steel with electricity, 194
Silicates, action of, on alumin-
ium, 84
of aluminium, formulae of, 43
Siliceous aluminium, 238
on the gases evolved
du ring sol ution of, 260
Silicon, alloys of aluminium
with, 259
aluminium bronze, 205
extraordinary strength
of, 280
bronze manufactured by M.
Evrard, 211
crystallized, 260
disengagement of, as si lieu-
retted hydrogen in dissolv-
ing aluminium, 76
facilitates the oxidation of
aluminium, 71
freeing of aluminium from,
243 -
its state of combination in
aluminium, 52
use of, to reduce aluminium,
207
INDEX.
343
Silieu rotted hydrogen, formation
of, 011 dissolving aluminium,
260
Silver, allovs of aluminium with,
295 "
aluminium, 297
comparative value with alu-
minium, 65
deposition of, by aluminium.
81
from clay, exhibited at Paris,
1855, 34
sulphide, decomposition of.
by aluminium. 74
Silvering1 of aluminium, 256
difficulty in, 80
Smith, Dr., patents on reduction
of aluminium, 221
Soci£:e Anonyme de 1'alumin-
ium, 35
prices of aluminium and
aluminium bronze, 36
Soda, action of, on aluminium,
77
mica, formula of, 43
mineral, 105
Sodium, alloys of, with alumin-
ium, 303
aluminate, precipitation of,
by Lowig, 151
amount necessary to reduce
aluminium from cryolite,
122
and potassium, reduction
together of, 138
calcination furnace, 133
carbonates, action on alu-
minium, 88
chloride, action on alumin-
ium, 85
decomposition of, by
electricity, 142
cvanide as a reducing agent,
*180
Gerhard's furnace to prevent
loss of, 120
great reduction of its price
in 1859, 27
its manufacture, 130-143
manufacture in New York
City, 1886, 139-141
mixture for reduction, 132
Sodium, nascent, as a reducing
agent, 179
preservation of, by Wagner's
method. 138
reaction for the reduction of,
137
reduction by Briinner, 131
by Castner, 139
additional details
of, 324
by Curaudau, 131
by Davy, 131
by electricity, 142
by Gay Lussac, 131
by Jablochoff, 142
by Thenard, 131
furnace for, 134
in the Bessemer conver-
ter, 208
in the electric furnace,
193
of aluminium by other
agents than, 180
of the double chloride
by, 168
process, the perfection
of the, 171
substituted for potassium by
Deville, 27
sulphate, action on alumin-
ium, 88
temperature of the reduction
of, 137
use of chalk in the reduction
of, 133
vapor process as used by
Deville, 100
of Frishmuth, 178
Weldon's calculation of the
cost of, 139
Soils, alumina the base of, 43
Soldering liquor for aluminium,
250
of aluminium, 247-253
Solders for aluminium, 248-251
bronze, 279
Sonorousness of aluminium, 63
Spear, Mr. W. B., in connection
with native sulphate of alu-
mina, 305
Specht, on the reduction of alu-
minium by /inc, 218
344
INDEX.
Specific heat of aluminium, 68
gravity of aluminium, 64
bronze, 271
of commercial alumin-
ium, 307
Sprague, remarks on electrolysis
of aluminium salts, 232
Spruce, Mr., analysis of beauxite
by, 47
Stamping of aluminium, 58
Stearic acid used for burnishing
aluminium, 55
Steel, alloys with aluminium,
281
Stocker, on native aluminium, 43
Stoddart and Faraday, analysis
of Bombay wootz, 283
Stones, precious, formulae of, 44
Strange, Mr., experiments with
aluminium bronze, 273
Strength, compressive, of alu-
minium, 62
aluminium bronze, 272
tensile, of aluminium, 62, 63
of aluminium bronze,
266, 267, 270, 276
of aluminium-silicon
bronze, 205
transverse, of aluminium, 62
Sulphate of alumina, decomposi-
tion of, by electricity,
231, 233
native, 305
Tilghman's process for
decomposing, 144
of potash, action on alu-
minium, 88
of soda, action on alumin-
ium, 88
Sulphide appearance, properties
and analysis of, 311
a practical process for
producing, 321
experiments on produc-
ing, 318
on reducing, 322
production and reduc-
tion of, 309-324
reduction of, by Co-
menge's method,
184
by manganese, 222
Sulphide appearance, reduction
of, by Petitjean's me-
thod, 183
remark by Than on, 314
researches of Fremy on,
310
of Reichel, 312
carbon di-, use of, for making
aluminium chloride,
317
use of, for making alu-
minium sulphide, 310
Sulphides of aluminium and
magnesium, Reichel's
paper on, 312-317
Sulphur, action on aluminium,
73, 88
its relative affinitv for. the
metals, 318
Sulphuretted hydrogen, action
of, on aluminium, 73
Sulphuric acid, action of, on
aluminium, 74
Surgery, use of aluminium in, 87
Sweat, action on aluminium, 87
Syndicate, an English, to control
patents on aluminium, 39
Tanks, precipitating, 152
Tarnish, Mourey's receipt for re-
moving, from aluminium, 54
Tarnishing of aluminium, cause
of, 240
Tartaric acid, action of, on alu-
minium, 78
Taste of aluminium, 57
Taylor, W. J., calculated cost of
aluminium, 32
Telegraph wire, aluminium, 243
Temperature necessary to reduce
sodium, 137
Tempering of aluminium, 58
Tenacity of aluminium, 61
Tensile strength of aluminium,
62, 63
of aluminium bronze,
266, 267, 270, 276
of aluminium-silicon
bronze, 205
Than, remark by, on the forma-
tion of aluminium sulphide,
314
INDEX.
345
Thenard, reduction of sodium
by, 131
Thermal, conductivity of alu-
minium, 67
Thomas and Tilly, process for
aluminium plating, 231
Thompson, J. B., deposition of
aluminium from solution, 231
Thompson, W. P., paper on the
Cowles's process, 197-205
Thompson, W. P., reduction of
aluminium by, 207
Thomson's calcination furnace
for cryolite, 146
" Tiers Argent/' an alloy of alu-
minium and silver, 297
Tilghman's process for decom-
posing sulphate of alumina,
144
Tin, alloy of aluminium and, 196
alloys of aluminium with,
289
aluminium alloy, action of
lead on, 196
production of. 322
its injurious effects in food,
79
plate, aluminium plate a
substitute for, 247
reduction of aluminium sul-
phide by, 322
Titanum, alloys of aluminium
with, 301
Tissier Bros., Deville's charges
against, 28
experiments on solder-
ing aluminium, 248
history of their works, 29
process, 124
"Recherches sur 1'Alu-
minium," 1858, 28
Tissier, on the amalgamation of
aluminium, 262
Topaz, formula of, 44
Tracheotomy, aluminium tube
used in, 87
Tungsten, alloys of aluminium
with, 302
Tuning forks, aluminium, 63
Turquois, formula of, 44
Uses of aluminium, 243-247
Usiglio, manager of the works at
Saliudres, 33
Vanadium, occurrence in beaux-
ite, 46
Vangeois, first maker of alumin-
ium wire, 60
Veneering with aluminium, 253
Vielle Mcntagne Zinc Works, on
the use of retorts from, 288
Viscidity of molten aluminium,
237
Volatilization of aluminium, 66
Wagner, 0., analysis of beauxite
by, 47
Wahl, W. H., remarks on mitis
castings, 326
Wasellite, formula of, 44
Washing apparatus, 149
used at Salindres, 161
methodical, 149
Washington monument, cast-
aluminium tip of, 39
composition of the alu-
minium in the tip of,
53
description of the apex
of, 40
Water, action of, on aluminium,
72
sulphide, 311, 317
decomposition of, by alu-
minium leaf, 73
Watts's Dictionary, Frishmuth's
process mentioned in, 42
Watts, on the use of cryolite for
producing aluminium, 127
Webster, aluminium works of,
at Birmingham, 36
improvement of, in making
aluminium sodium double
chloride, 154
James, patented alloy of, 278
process of, only one used in
England, 42
Webster's patent, 175
process, 173-177
Wedding. M., remarks on Bas-
set's zinc process, 217
Weldon, W., of Burstow, Eng-
land, manganese process of, 222
346
INDEX.
Wertheim, on the elasticity of
aluminium, 61
Wilde, A. E., on reducing alu-
minium by lead, 221
Winckler, Dr. Clemens, histori-
cal retrospect to 1879,
33
on coating metals with
aluminium, 254
remarks on electrolysis
of aluminium salts,
232
Wine, acid action of, on alumin-
ium, 78
Wire, aluminium, drawing of, 60
strength of, 63
Wirz & Co., Berlin, stoppage of
their aluminium works, 35
Wochein, analysis of beauxite
from, 47
Wocheinite, local .name for
beauxite, 46
Wohler and Buff, on the solution
of siliceous aluminium,
260
and Deville, on the extrac-
tion of Boron, 300
Deville's opinion of, 31
discovery of aluminium,
1827, 26, 91
experiments to obtain alu-
minium amalgam, 25
first paper of, 91
improvement on Deville's
cryolite process, 126
method used in 1845, 26
observation on melting alu-
minium with a blowpipe,
71
Wohler and Buff on the resist-
ance of aluminium to aqua
ammonia, 78
review of Oerstedt's paper,
91
second paper of, 93
Working of aluminium, 235-257
Works, aluminium, at Amfre-
ville, near Rouen, 29,
124, 128
at Battersea, London, 33
at Berlin, 35
at Birmingham, England, 36,
173
at Camden, N. J., 31
at Cleveland, Ohio, 4.1, 189
at Glacidre, 28, 98
at Javel, 28, 98
at Nanterre, 28, 35, 126, 128
at Newcastle-on-Tyne, 33
at Philadelphia, 37, 178
at Salindres, 28, 33, 128, 168
in England, 33, 35, 42
in France, 35, 128
in Germany, 33, 35
Zinc, alloys of aluminium with,
287
deposition of, by aluminium,
83
expelling from aluminium
by heat, 218
freeing of aluminium from,
242
oxide, action on aluminium,
86
reduction of aluminium by,
214
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