\[Mn{{O}_{4}}^{2-}\] undergoes disproportionation reaction in acidic medium but \[Mn{{O}_{4}}^{-}\] does not because

In \[Mn{{O}_{4}}^{2-},Mn\] is in lowest oxidation state

In \[Mn{{O}_{4}}^{2-}Mn\] is in intermediate oxidation state

In \[Mn{{O}_{4}}^{2-},Mn\] is in intermediate oxidation state

\[Mn{{O}_{4}}^{2-}\] undergoes disproportionation reaction in acidic m

1.	\[Mn{{O}_{4}}^{2-}\] undergoes disproportionation reaction in acidic medium but \[Mn{{O}_{4}}^{-}\] does not because
A.	In \[Mn{{O}_{4}}^{2-}Mn\] is in intermediate oxidation state
B.	In \[Mn{{O}_{4}}^{2-},Mn\] is in lowest oxidation state
C.	In \[Mn{{O}_{4}}^{2-},Mn\] is in intermediate oxidation state
D.	None of the above
Answer» B. In \[Mn{{O}_{4}}^{2-},Mn\] is in lowest oxidation state

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\[Mn{{O}_{4}}^{2-}\] undergoes disproportionation reaction in acidic medium but \[Mn{{O}_{4}}^{-}\] does not because

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