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(D) Ionisation enthalpy $(IE)$ is the energy required to remove an electron from a gaseous atom or ion. $Mn^{2+}$ has a stable $d^5$ configuration $([

Vedclass · Accepted Answer

$Mn^{2+} < Fe^{2+}$

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(D) Ionisation enthalpy $(IE)$ is the energy required to remove an electron from a gaseous atom or ion. $Mn^{2+}$ has a stable $d^5$ configuration $([Ar] 3d^5)$,which makes it very difficult to remove another electron,resulting in a very high $IE$. $Fe^{2+}$ has a $d^6$ configuration $([Ar] 3d^6)$. Since $Mn^{2+}$ is more stable than $Fe^{2+}$,the energy required to remove an electron from $Mn^{2+}$ is higher than that for $Fe^{2+}$. Therefore,the relationship $Mn^{2+}  Fe^{2+}$.

The incorrect relationship in the following pairs in relation to ionisation enthalpies is $:$

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