An acidified manganate solution undergoes dis | vedclass

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(D) The disproportionation reaction of manganate $(MnO_{4}^{2-})$ in acidic medium is given by: $3 MnO_{4}^{2-} + 4 H^{+} \longrightarrow 2 MnO_{4}^{-

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(D) The disproportionation reaction of manganate $(MnO_{4}^{2-})$ in acidic medium is given by: $3 MnO_{4}^{2-} + 4 H^{+} \longrightarrow 2 MnO_{4}^{-} + MnO_{2} + 2 H_{2}O$ In this reaction,manganese is oxidized to $Mn^{+7}$ (in $MnO_{4}^{-}$) and reduced to $Mn^{+4}$ (in $MnO_{2}$). The product with the higher oxidation state is $MnO_{4}^{-}$,where the oxidation state of $Mn$ is $+7$. The electronic configuration of $Mn^{+7}$ is $[Ar] 3d^{0}$. Since there are no unpaired electrons $(n = 0)$,the spin-only magnetic moment is $\mu = \sqrt{n(n+2)} = \sqrt{0(0+2)} = 0 \, B.M.$

An acidified manganate solution undergoes disproportionation reaction. The spin-only magnetic moment value of the product having manganese in higher oxidation state is $....\, B.M.$ (Nearest integer)

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