Which of the following species does not show disproportionation reaction?

Options

A. `ClO_4^(-)`
B. `ClO_(3)^(-)`
C. `ClO_2^(-)`
D. `ClO^(-)`

Answer

A

Explanation

In a disproportionation reaction, an element in one oxidation state is simultaneously oxidized as well as reduced. This is possible provided the element (capable of existing in at least three oxidation states) is present in the intermediate oxidation state in the reacting species.
Among the oxo-anions of chlorine listed above, `ClI_(4)^(-)` does not disproportionate because in this oxoanion, ` Cl` is present in its highest oxidation state (+7). Thus it can be reduced only but cannot be oxidized. The disproportionation reactions for the other three oxoanions of chlorine are as follows :
`4overset(+5)(Cl)O_(3)^(-) rarr overset(-1)(Cl^(-))+3overset(+7)(Cl)O_(4)^(-)`
`6overset(+3)(Cl)O_(2)^(-) rarr 2overset(-1)(Cl^(-))+4overset(+5)(Cl)O_(3)^(-)`
`3overset(+3)(Cl)O^(-) rarr 2overset(-1)(Cl^(-))+overset(+5)(Cl)O_(3)^(-)`