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(D) The first ionisation enthalpy $(IE_1)$ of lanthanoids generally increases with an increase in atomic number due to the lanthanoid contraction,whic

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$Yb$

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(D) The first ionisation enthalpy $(IE_1)$ of lanthanoids generally increases with an increase in atomic number due to the lanthanoid contraction,which leads to a decrease in atomic size and stronger attraction of the nucleus for the valence electrons. Among the given elements,$Ce$ $(Z=58)$,$La$ $(Z=57)$,$Gd$ $(Z=64)$,and $Yb$ $(Z=70)$,the element $Yb$ has the highest atomic number. $Yb$ has a stable electronic configuration of $[Xe] 4f^{14} 6s^2$. Due to the completely filled $4f$ subshell and the highest effective nuclear charge among the options,it requires the most energy to remove the first electron. Therefore,$Yb$ has the highest $IE_1$.

Identify the element having the highest first ionisation enthalpy $(IE_1)$ from the following.

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