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(B) Electron gain enthalpy generally increases in a period from left to right and decreases in a group on moving downwards.However,members of the $3^{

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$O < S < F < Cl$

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(B) Electron gain enthalpy generally increases in a period from left to right and decreases in a group on moving downwards.However,members of the $3^{rd}$ period have higher electron gain enthalpy compared to the corresponding members of the $2^{nd}$ period due to their larger size,which reduces inter-electronic repulsion.$O$ and $S$ belong to group $16$,while $F$ and $Cl$ belong to group $17$.Thus,the electron gain enthalpy of $F$ and $Cl$ is higher than that of $O$ and $S$.Comparing within groups,$Cl > F$ and $S > O$ because the smaller size of $F$ and $O$ atoms leads to greater inter-electronic repulsion for the incoming electron.Therefore,the correct order of increasing electron gain enthalpy is $O < S < F < Cl$.

List-$I$ (Element)	List-$II$ ($\Delta_{eg}H$ in $kJ \ mol^{-1}$)
$A$. $O$	$I$. $-200$
$B$. $F$	$II$. $-349$
$C$. $Cl$	$III$. $-141$
$D$. $S$	$IV$. $-328$
	$V$. $+48$

Which of the following represents the correct order of increasing electron gain enthalpy with negative sign for the elements $O$,$S$,$F$ and $Cl$?

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Match the following:
List-$I$ (Element) List-$II$ ($\Delta_{eg}H$ in $kJ \ mol^{-1}$)
$A$. $O$ $I$. $-200$
$B$. $F$ $II$. $-349$
$C$. $Cl$ $III$. $-141$
$D$. $S$ $IV$. $-328$
$V$. $+48$

The correct answer is:

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