In which one of the following sets do all spe | vedclass

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(NONE) disproportionation reaction occurs when a species in an intermediate oxidation state is simultaneously oxidized and reduced. $MnO_{4}^{-}$ cont

Vedclass · Accepted Answer

$MnO_{4}^{-}, ClO_{2}^{-}, Cl_{2}$ and $Mn^{3+}$

Vedclass · Answer

(NONE) disproportionation reaction occurs when a species in an intermediate oxidation state is simultaneously oxidized and reduced. $MnO_{4}^{-}$ contains $Mn$ in the $+7$ oxidation state,which is its maximum oxidation state; therefore,it cannot be further oxidized. $Cr_{2}O_{7}^{2-}$ contains $Cr$ in the $+6$ oxidation state,which is its maximum oxidation state; therefore,it cannot be further oxidized. $ClO_{4}^{-}$ contains $Cl$ in the $+7$ oxidation state,which is its maximum oxidation state; therefore,it cannot be further oxidized. $F_{2}$ is the strongest oxidizing agent and can only be reduced to $F^{-}$,so it cannot undergo disproportionation. Since all provided options contain at least one species that cannot undergo disproportionation,none of the sets are correct.

In which one of the following sets do all species show a disproportionation reaction?

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Total number of species from the following which can undergo disproportionation reaction . . . . . . .
$H_2O_2$,$ClO_3^{-}$,$P_4$,$Cl_2$,$Ag$,$Cu^{+}$,$F_2$,$NO_2$,$K^{+}$

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