Chlorine Tetroxide
It has been claimed that the oxide ClO4 is produced by the reaction of silver perchlorate with iodine in
anhydrous ether, the concentrations of the reactants being about 1%:
2AgClO4 + I2 ----> 2AgI + 2ClO4
The presence of a small amount of unstable iodo-compound, not volatile in ether, and probably dimeric, (ClO4)2. It was believed to react with water
according to the following equation:
2ClO4 + H2O -----> HClO4 + HO.ClO4
It has also been regarded as an intermediate in the reaction between perchloric acid and fluorine. The following facts are submitted as evidence that
the solutions in ether contain chlorine tetroxide rather then perchloric acid: (a) the solution liberated iodine from hydroiodic acid, thogh not in
equivalent amount; (b) with zinc and magnesium metals, perchlorates were produced but no hydrogen was evolved. (The reaction could thus be explained
in terms of a single electron trasfer process: with iron, tin, and copper, perchlorates of the metals in more then one valency state were produced,
and with cadmium, bismuth, and silver, reaction was slow and incomplete). (c) The reactions of solutions of perchloric acid and of ethyl perchlorate
differed from those of the chlorine tetroxide solutions.
The evidence for the existence of this oxide was in no way conclusive, and an alternative interpretation of the experimental data has been proposed
involving the intermediate formation of iodine perchlorate.:
AgClO4 + I2 -----> AgI + IClO4
followed by iodination of ether to give an unstable iodo-ether:
C2H5.O.C2H5 + IClO4 -----> C2H5.O.C2H4I + HClO4
The iodo-ether slowly reacts with more silver perchlorate:
AgClO4 + C2H5.O.C2H4I -----> AgI + C2H5.O.C2H4.ClO4
The overall reaction therefore leads to the formation of equivalent amounts of perchloric acid and ether perchlorate. On this basis, the oxidizing
power of the solution should vanish towards the end of the reaction, as the iodine perchlorate is consumed in iodinating the solvent. This has been
found to be the case, although the obeservation has been contested. The second and third stages are difficult to confirm because of the instability
of the iodinated ether, but receive support from later work. When silver perchlorate and iodine react in the presence of an aromatic compound C6H5X
(e.g. chloro- or nitro-benzene) the reaction is exclusively:
C6H5X + I2 + AgClO4 -----> C6H5XI + AgI + HClO4
and there is no evidence of the formation of chlorine tetroxide. The aromatic iodo-compound is not affected by excess of silver perchlorate. However
alkyl iodides do react:
C2H5I + AgClO4 -----> C2H5ClO4 + AgI
When iodine and silver perchlorate react in ether solution, the initial precipitation corresponds to 1 mol. of silver iodide per mol. of iodine.
Reaction with the solvent is an essential step in the formation of the second molecule of silver iodide. This precipitation is slow and during the
process the oxidizing power of the solution dissappers. The original postulate that chlorine tetroxide was formed was based on the assumption that
ether behaved as an inert solvent: since this appers to be untrue there is no apparent justification for supposing that chlorine tetroxide is formed
in the reaction between iodine and silver perchlorate.
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