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(A) The first ionization enthalpy $(IE_1)$ of the $3d$ transition series elements generally increases from left to right across the period due to the

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$Zn > Fe > Cr > Sc$

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(A) The first ionization enthalpy $(IE_1)$ of the $3d$ transition series elements generally increases from left to right across the period due to the increase in effective nuclear charge.However,there are irregularities due to stable electronic configurations (like half-filled or fully-filled $d$-orbitals).The electronic configurations are: $Sc ([Ar] 3d^1 4s^2)$,$Cr ([Ar] 3d^5 4s^1)$,$Fe ([Ar] 3d^6 4s^2)$,and $Zn ([Ar] 3d^{10} 4s^2)$.Comparing their $(IE_1)$ values,the order is $Zn > Fe > Cr > Sc$.

Which from the following series of elements is $CORRECTLY$ arranged according to their decreasing order of ionization enthalpy $(IE_1)$?

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