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(B) The first ionization energy $(IE_1)$ generally decreases down a group due to the increase in atomic size and shielding effect.For group $14$ eleme

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$Sn$

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(B) The first ionization energy $(IE_1)$ generally decreases down a group due to the increase in atomic size and shielding effect.For group $14$ elements $(C, Si, Ge, Sn, Pb)$,the ionization energy decreases from $C$ to $Sn$.However,$Pb$ shows a higher $IE_1$ than $Sn$ due to the poor shielding effect of $d-$ and $f-$electrons,which leads to a higher effective nuclear charge $(Z_{eff})$ experienced by the valence electrons.Therefore,among the given options,$Sn$ has the lowest $IE_1$ value.

Element	Ionization energy $1^{st}$ $(kJ/mol)$	Ionization energy $2^{nd}$ $(kJ/mol)$
$X$	$495$	$4563$
$Y$	$731$	$1450$

Which among the following elements has the lowest value of $IE_1$?

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$Y$ $731$ $1450$

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