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(D) The electronic configuration of $Cr$ is $[Ar] 3d^5 4s^1$ and that of $Cu$ is $[Ar] 3d^{10} 4s^1$. Their second ionisation enthalpies are higher th

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$Cr, Cu$

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(D) The electronic configuration of $Cr$ is $[Ar] 3d^5 4s^1$ and that of $Cu$ is $[Ar] 3d^{10} 4s^1$. Their second ionisation enthalpies are higher than expected because after the removal of one electron,$Cr^+$ attains a stable half-filled $3d^5$ configuration,and $Cu^+$ attains a stable fully-filled $3d^{10}$ configuration. These configurations are significantly more stable than the configurations of their neighbors. Therefore,it requires much more energy to remove the second electron from these ions. Thus,option $(D)$ is correct.

Atom/Ion	Electronic Configuration
$(1) \ Cu$	$(A) 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^{10}$
$(2) \ Cu^{2+}$	$(B) 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^{10}, 4s^2$
$(3) \ Zn^{2+}$	$(C) 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^{10}, 4s^1$
$(4) \ Cr^{3+}$	$(D) 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^9$
	$(E) 1s^2, 2s^2, 2p^6, 3s^2, 3p^6, 3d^3$

Higher second ionisation enthalpies than expected are observed for

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