Which of the following do not show disproportionation reaction? $\mathrm{ClO}_{4}^{-}, \mathrm{F}_{2},…
Which of the following do not show disproportionation reaction? $\mathrm{ClO}_{4}^{-}, \mathrm{F}_{2}, \mathrm{Cl}_{2}, \mathrm{ClO}_{2}^{-}, \mathrm{ClO}_{2}^{-}, \mathrm{P}_{4}, \mathrm{~S}_{8}$, and $\mathrm{ClO}^{-}$
$\mathrm{ClO}_{2}^{-}, \mathrm{ClO}_{4}^{-}$, and $\mathrm{ClO}^{-}$
$\mathrm{F}_{2}$ only
$\mathrm{F}_{2}$ and $\mathrm{ClO}_{4}^{-}$
$\mathrm{ClO}_{4}^{-}$ only
Solution
$\mathrm{F}_{2}$ being most electronegative element cannot exhibit any positive oxidation state. In $\mathrm{ClO}_{4}^{-}$ chlorine is present in its highest oxidation state i.e $+7$. Therefore it does not show disproportionation reaction.