The second ionisation energy of the following | vedclass

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(A) Key Point: For elements with similar electronic configuration of the outermost shell, atomic size determines the value of ionisation energy. Large

Vedclass · Accepted Answer

$Zn > Cd < Hg$

Vedclass · Answer

(A) Key Point: For elements with similar electronic configuration of the outermost shell, atomic size determines the value of ionisation energy. Larger size leads to lower ionisation energy.Electronic configuration for $II^{nd}$ $I.E$:$Zn^{+}$ ion $(Z=30) = [Ar] 3d^{10} 4s^{1} - (1734 \ kJ/mol)$$Cd^{+}$ ion $(Z=48) = [Kr] 4d^{10} 5s^{1} - (1631 \ kJ/mol)$$Hg^{+}$ ion $(Z=80) = [Xe] 4f^{14} 5d^{10} 6s^{1} - (1809 \ kJ/mol)$Since the size of $Cd^{+} > Zn^{+}$, it has lower $II^{nd}$ ionisation energy. Due to the lanthanoid contraction (i.e.,poor screening by $4f$ and $5d$ electrons), $Hg^{+}$ has a higher $II^{nd}$ ionisation energy.Hence, the correct order is $Zn > Cd < Hg$, and option $(A)$ is the correct answer.

The second ionisation energy of the following elements follows the order

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