The species which does not undergo disproport | vedclass

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(B) disproportionation reaction is one in which the same element in a given oxidation state is simultaneously oxidized and reduced. For an element to

Vedclass · Accepted Answer

$ClO_4^{-}$

Vedclass · Answer

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

The species which does not undergo disproportionation reaction is:

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