The species which does not undergo disproport | vedclass

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Question

(B) Step $1$: $A$ disproportionation reaction is one in which the same element in a given oxidation state is simultaneously oxidized and reduced.Step

Vedclass · Accepted Answer

$ClO_4^{-}$

Vedclass · Answer

(B) Step $1$: $A$ disproportionation reaction is one in which the same element in a given oxidation state is simultaneously oxidized and reduced.Step $2$: For an element to undergo disproportionation, it must be in an intermediate oxidation state.Step $3$: In $ClO_4^{-}$, the oxidation state of $Cl$ is calculated as: $x + (-2 	imes 4) = -1$, which gives $x = +7$.Step $4$: Since $+7$ is the maximum possible oxidation state for Chlorine (as its valence shell configuration is $3s^2 3p^5$), it cannot be further oxidized.Step $5$: Therefore, $ClO_4^{-}$ cannot undergo disproportionation.

The species which does not undergo disproportionation reaction is:

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