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(C) The first ionization enthalpy $(IE_1)$ generally increases across a period due to an increase in effective nuclear charge and decreases down a gro

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$Ba < Ca < Se < S < Ar$

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(C) The first ionization enthalpy $(IE_1)$ generally increases across a period due to an increase in effective nuclear charge and decreases down a group due to an increase in atomic size and shielding effect.$1$. Comparing elements in the same period: $S$ (Group $16$,Period $3$) and $Ar$ (Group $18$,Period $3$). $Ar$ has a stable noble gas configuration,so it has the highest $IE_1$ among the given elements.$2$. Comparing elements in the same group: $Ca$ (Group $2$,Period $4$) and $Ba$ (Group $2$,Period $6$). Since $Ba$ is below $Ca$,$IE_1$ of $Ba $3$. Comparing $S$ and $Se$: $S$ (Period $3$) and $Se$ (Period $4$). Since $Se$ is below $S$,$IE_1$ of $Se $4$. Combining the trends: $Ba Therefore,the correct order is $Ba < Ca < Se < S < Ar$.

$B$	$801$
$Al$	$577$
$Ga$	$579$
$In$	$558$
$Tl$	$589$

Which of the following represents the correct order of increasing first ionization enthalpy for $Ca, Ba, S, Se$ and $Ar$?

Similar Questions

The first ionization enthalpy values (in $kJ\,mol^{-1}$) of group $13$ elements are :

$B$ $801$

$Al$ $577$

$Ga$ $579$

$In$ $558$

$Tl$ $589$

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