Which of the following does not show a dispro | vedclass

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Question

(C) disproportionation reaction is a type of redox reaction in which the same element is simultaneously oxidized and reduced.For an element to undergo

Vedclass · Accepted Answer

$ClO_4^{-}$

Vedclass · Answer

(C) disproportionation reaction is a type of redox reaction in which the same element 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: $x + 4(-2) = -1$,which gives $x = +7$.Since $+7$ is the maximum possible oxidation state for chlorine (as it has $7$ valence electrons),it cannot be further oxidized.Therefore,$ClO_4^{-}$ cannot undergo a disproportionation reaction.

$I^{-}$	$ClO_{4}^{-}$	$NO_{2}$	$HNO_{2}$	$Cu^{+2}$	$Cu^{+}$
$(A)$	$(B)$	$(C)$	$(D)$	$(E)$	$(F)$

Which of the following does not show a disproportionation reaction?

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$I^{-}$ $ClO_{4}^{-}$ $NO_{2}$ $HNO_{2}$ $Cu^{+2}$ $Cu^{+}$
$(A)$ $(B)$ $(C)$ $(D)$ $(E)$ $(F)$

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