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 higher

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.

Which of the following is not a disproportionation reaction?

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