Four successive elements of the first transit | vedclass

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(D) The electronic configuration of $Mn^{2+}$ is $[Ar]3d^5$,which represents a stable half-filled $d$-orbital configuration.Removing the third electro

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Manganese $(Z = 25)$

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(D) The electronic configuration of $Mn^{2+}$ is $[Ar]3d^5$,which represents a stable half-filled $d$-orbital configuration.Removing the third electron from $Mn^{2+}$ requires a significantly higher amount of energy because it involves disrupting this stable half-filled configuration.Therefore,$Mn$ has the highest third ionization enthalpy among the given elements.

Four successive elements of the first transition series are given with their atomic numbers. Which one of them is expected to have the highest third ionization enthalpy?

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