The species given below that does NOT show di | 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.In $BrO_{4}^{-}$,th

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$BrO_{4}^{-}$

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(B) disproportionation reaction is one in which the same element in a given oxidation state is simultaneously oxidized and reduced.In $BrO_{4}^{-}$,the oxidation state of $Br$ is $+7$,which is its maximum possible oxidation state (group $17$ valence electrons).Since it cannot be oxidized further,it can only undergo reduction.Therefore,$BrO_{4}^{-}$ cannot show a disproportionation reaction.

The species given below that does $NOT$ show disproportionation reaction is :

Similar Questions

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