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(B) The standard electrode potential $E^o_{M^{3+}/M^{2+}}$ depends on the stability of the $M^{2+}$ and $M^{3+}$ oxidation states.For $Mn \ (Z = 25)$,

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$Mn \ (Z = 25)$

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(B) The standard electrode potential $E^o_{M^{3+}/M^{2+}}$ depends on the stability of the $M^{2+}$ and $M^{3+}$ oxidation states.For $Mn \ (Z = 25)$,the electronic configuration is $[Ar] \ 3d^5 \ 4s^2$.The $Mn^{2+}$ ion has a stable $d^5$ configuration (half-filled),which is very stable.However,the $Mn^{3+}$ ion has a $d^4$ configuration.Because $Mn^{2+}$ is exceptionally stable,it is very difficult to oxidize $Mn^{2+}$ to $Mn^{3+}$,which makes the reduction potential $E^o_{Mn^{3+}/Mn^{2+}}$ very high (positive).Therefore,$Mn$ has the maximum $E^o_{M^{3+}/M^{2+}}$ value among the given elements.

Four successive members of the first row transition elements are listed below with their atomic numbers. Which of these elements has the maximum $E^o_{M^{3+}/M^{2+}}$ value?

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