Which of the following is not a disproportion | vedclass

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(B) disproportionation reaction is a redox reaction in which the same element is simultaneously oxidized and reduced, resulting in products with highe

Vedclass · Accepted Answer

$F_{2(g)} + 2 OH^{-}_{(aq)} \longrightarrow OF_{2(g)} + 2 F^{-}_{(aq)} + H_2O_{(l)}$

Vedclass · Answer

(B) disproportionation reaction is a redox reaction in which the same element is simultaneously oxidized and reduced, resulting in products with higher and lower oxidation states than the reactant.
In option $A$, $Cl_2$ $(0)$ goes to $ClO^-$ $(+1)$ and $Cl^-$ $(-1)$, which is a disproportionation reaction.
In option $B$, $F_2$ $(0)$ reacts with $OH^-$ to form $OF_2$ and $F^-$. In $OF_2$, the oxidation state of $F$ is $-1$ and in $F^-$, it is also $-1$. The oxidation state of $O$ changes from $-2$ in $OH^-$ to $+2$ in $OF_2$ and remains $-2$ in $H_2O$. Since the oxidation state of fluorine only decreases, this is not a disproportionation reaction.
In option $C$, $ClO_3^-$ $(+5)$ goes to $Cl^-$ $(-1)$ and $ClO_4^-$ $(+7)$, which is a disproportionation reaction.
In option $D$, $ClO^-$ $(+1)$ goes to $Cl^-$ $(-1)$ and $ClO_3^-$ $(+5)$, which is a disproportionation reaction.

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

Which of the following is not a disproportionation reaction?

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Refer to the periodic table and answer the following questions:
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Which of the following species can undergo disproportionation?

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