In which one of the following sets all species show...

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

Options

A ${ClO}_{4}^{-}, {MnO}_{4}^{-}, {ClO}_{2}^{-}$ and ${F}_{2}$
B ${MnO}_{4}^{2 -}, {ClO}_{2}^{-}, {Cl}_{2}$ and ${Mn}^{3 +}$
C ${Cr}_{2}{O}_{7}^{2 -}, {MnO}_{4}^{-}, {ClO}_{2}^{-}$ and ${Cl}_{2}$
D ${ClO}_{2}^{-}, {F}_{2}, {MnO}_{4}^{-}$ and ${Cr}_{2}{O}_{7}^{2 -}$

Correct answer

B. ${MnO}_{4}^{2 -}, {ClO}_{2}^{-}, {Cl}_{2}$ and ${Mn}^{3 +}$

Step-by-step solution

Disproportionation reactions are a special type of redox reactions. One of the reactants in a disproportionation reaction always contains an element that can exist in at least three oxidation states. The element of reacting species is in intermediate oxidation state and simultaneously gets oxidised and reduced. ${MnO}_{4}^{2 -}, {ClO}_{2}^{-}, {Cl}_{2}$ and ${Mn}^{3 +}$ are having intermediate oxidation states.

Note: No option is correct in the actual question. One option is modified for its correctness.

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