Which of the following species will not exhibit disproportionation reaction?

C l O^{-}

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C l O_{2}^{-}

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C l O_{3}^{-}

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C l O_{4}^{-}

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Solution

The correct option is B $C l O_{4}^{-}$
A substance can exhibit disproportionation reaction if it can increase as well as decrease its oxidation state.
Maximum oxidation number of $C l$ is +7 and minimum oxidation number is $- 1$ .
In $C l O^{-}$ , chlorine is present in +1 oxidation state so it can increase as well as decrease its oxidation state.
In $C l O_{2}^{-}$ , chlorine is present in +3 oxidation state so it can increase as well as decrease its oxidation state.
In $C l O_{3}^{-}$ , chlorine is present in +5 oxidation state so it can increase as well as decrease its oxidation state.
In $C l O_{4}^{-}$ , chlorine is present in +7 oxidation state so it cannot increase its oxidation state.
So only $C l O_{4}^{-}$ will not exhibit disproportionation reaction.

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Similar questions

Cl O^{-}, {ClO}_{2}^{-}, {ClO}_{3}^{-} and {ClO}_{4}^{-}

Also, write the reaction for each of the species that disproportionate.

C l O^{-}, C l O_{2}^{-}, C l O_{3}^{-}

C l O_{4}^{-}

{N a}_{2} S_{2} O_{7}

{K I}_{3}

{C l O}_{3}^{-}

{C l O}_{4}^{-}

3 C l O_{(a q)}^{-} \to C l O_{3}^{-} + 2 C l^{-}

C l

+ 1

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