I^{-}ClO_{4}^{-}NO_{2}HNO_{2}Cu^{+2}Cu^{+}(A) | vedclass

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(A) Disproportionation is a redox reaction in which the same element in an intermediate oxidation state is simultaneously oxidized and reduced.Let us

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$C, D, F$

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(A) Disproportionation is a redox reaction in which the same element in an intermediate oxidation state is simultaneously oxidized and reduced.Let us analyze the oxidation states of the central atoms in each species:$(A) \ I^{-}$: Iodine is in its lowest oxidation state $(-1)$,so it can only be oxidized. It cannot disproportionate.$(B) \ ClO_{4}^{-}$: Chlorine is in its highest oxidation state $(+7)$,so it can only be reduced. It cannot disproportionate.$(C) \ NO_{2}$: Nitrogen is in the $+4$ oxidation state. It can be oxidized to $+5$ $(NO_{3}^{-})$ and reduced to $+3$ $(HNO_{2})$. It can disproportionate.$(D) \ HNO_{2}$: Nitrogen is in the $+3$ oxidation state. It can be oxidized to $+5$ $(NO_{3}^{-})$ and reduced to $+2$ $(NO)$. It can disproportionate.$(E) \ Cu^{+2}$: Copper is in its highest stable oxidation state $(+2)$,so it can only be reduced. It cannot disproportionate.$(F) \ Cu^{+}$: Copper is in the $+1$ oxidation state. It can be oxidized to $+2$ $(Cu^{+2})$ and reduced to $0$ $(Cu)$. It can disproportionate.Therefore,the species that can undergo disproportionation are $C, D,$ and $F$.

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

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

Which of the following species can undergo disproportionation?

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$I^{-}$$ClO_{4}^{-}$$NO_{2}$$HNO_{2}$$Cu^{+2}$$Cu^{+}$$(A)$$(B)$$(C)$$(D)$$(E)$$(F)$Which of the following species can undergo disproportionation?