Why are the E^{circ} values for Mn^{2+},Ni^{2 | vedclass

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(B) The $E^{\circ}$ value for $Mn^{2+}$ is more negative because of the extra stability of the half-filled $d^5$ configuration. For $Zn^{2+}$,the $E^{

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Due to stable electronic configurations and high hydration enthalpy

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(B) The $E^{\circ}$ value for $Mn^{2+}$ is more negative because of the extra stability of the half-filled $d^5$ configuration. For $Zn^{2+}$,the $E^{\circ}$ value is more negative due to the stability of the fully-filled $d^{10}$ configuration. For $Ni^{2+}$,the large negative $E^{\circ}$ value is attributed to its very high negative hydration enthalpy.

Why are the $E^{\circ}$ values for $Mn^{2+}$,$Ni^{2+}$,and $Zn^{2+}$ more negative than expected?

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