The CORRECT ionisation energy order is | vedclass

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(C) Ionisation energy depends on the electronic configuration and the stability of the resulting ion.For $Mn^{2+}$,$Ni^{2+}$,and $Ca^{2+}$:$Mn^{2+} =

Vedclass · Accepted Answer

$Mn^{2+} > Ni^{2+} > Ca^{2+}$

Vedclass · Answer

(C) Ionisation energy depends on the electronic configuration and the stability of the resulting ion.For $Mn^{2+}$,$Ni^{2+}$,and $Ca^{2+}$:$Mn^{2+} = [Ar] 3d^5$ (Half-filled stable configuration,high $IE$).$Ni^{2+} = [Ar] 3d^8$.$Ca^{2+} = [Ar]$ (Noble gas configuration,but removing an electron from a stable shell requires high energy,however,in the context of transition metals,$Mn^{2+}$ has a stable $d^5$ configuration,making its $IE$ higher than $Ni^{2+}$ and $Ca^{2+}$).Comparing the options:Option $C$ is correct because $Mn^{2+}$ has a stable $d^5$ configuration,leading to a higher ionisation energy compared to $Ni^{2+}$ and $Ca^{2+}$.

The $CORRECT$ ionisation energy order is

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