Considering the elements $F, C l, O and S$ , the correct order of their electron affinity values is:

F > C l > O > S

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F > O > C l > S

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C l > F > S > O

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O > F > S > C l

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Solution

The correct option is C $C l > F > S > O$
Electron gain enthalpy increases as we move from left to right in a periodic table because effective nuclear charge increases, so $F, C l$ have more electron gain enthalpy than $O$ and $S$ .
Fluorine and oxygen have the smallest size in their respective groups. In case of fluorine, valence shell electronic configuration is $2 s^{2} 2 p^{5}$ . On adding another electron to the valence shell, it causes severe electron-electron repulsion due to which system becomes comparatively unstable. The same happens in case of oxygen. So, electron gain enthalpy of $C l > F$ and $S > O$ .
Therefore, correct order is: $C l > F > S > O$

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Considering the elements F,Cl,O and S, the correct order of their electron affinity values is:

Considering the elements $F, C l, O and S$ , the correct order of their electron affinity values is: