330 ]VIE. Gr. GOEE ON THE PEOPEETIES OE ELECTEO-DEPOSITED ANTIMONY. 
cliiferent temperatures in the three substances, being at about 200°Fabr. in the chloride 
deposit, about 280° in the bromide, and about 340° in the iodide. The manifestations 
of heat evolved also vary, being considerable in the chloride deposit (73.), apparently 
less in the bromide one, and but very small in the iodide compound. They each become 
much less metallic in appearance by a gradual discharge of their heat, and the gradual 
discharge is also attended by an increase of cohesive force, most in the chloride and least 
(if any) in the iodide deposit. The iodide compound is also the most affected by solar 
light. 
123. The chloride deposit contains about 6*3 per cent, of saline matter, the bromide 
about 20, and the iodide about 22-2. The pseudo-electro-chemical equivalent (if I may 
apply this term to such cases) varies in each variety, and is dependent upon the amount 
of saline matter which unites with the true equivalent of metallic antimony deposited ; 
it is about 42 ‘5 with the chloride deposit, 50 with the bromide, and 51 with the iodide. 
Conclusion. 
124. A probably correct explanation of the formation and properties of these several 
metallic deposits is as follows : — The electric current in passing decomposes the salt of 
antimony, setting free 1 equivalent of chlorine, bromine, or iodine, and -^rd of an equi- 
valent of antimony for every single equivalent of zinc consumed (48. 102. 109.). The 
antimony in the act of depositing, being in what is termed the “ nascent ” state, unites 
chemically, in a comparatively feeble or unstable manner, with the elements of the 
electrolyte, combining with them in an indefinite and somewhat variable proportion. 
The -g-rd equivalent, or 40 parts of antimony, carry down from to 3 parts from the 
chloride solution, about 10 parts from the bromide liquid, and about 11 parts from the 
iodide solution, and thus occasion about 42’75 parts of deposit in the first liquid, about 
50 parts in the second, and 50 '5 parts in the third solution, for each equivalent of zmc 
consumed. 
125. Another explanation, which has nearly an equal weight of evidence in its favour, 
is that the antimony is deposited in the “ amorphous ” state, and the chloride or other 
salt is enclosed mechanically in it during the process of deposition, and that the change 
consists in the assumption by the metal of the crystalline state, whereby it is converted into 
an inconceivable number of crystals of insensible size, and the imprisoned salt is set ffee. 
126. Antimony is not the only metal that manifests this property of uniting dm-ing 
electrolysis with portions of the electrolyte ; several other metals also show it : it is well 
known that silver deposited by electrolysis from a solution of the double cyanide of 
silver and potassium containing a little bisulphide of carbon, is harder and very much 
brighter than that deposited from the same solution without that mgredient ; this bright 
deposit is not wholly metallic silver, but contains a small proportion (about 1 per cent.) 
of some other ingredients of the electrolyte. 
I have not examined the laws or conditions that regulate the proportions of the sub- 
stances that unite by this species of combination. 
