The electron gain enthalpies of halogen are as given below: F=−332,Cl=−349,Br=−324,I=−295kJmol−1The less negative for F as compared to that of Cl is due to:

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The electron gain enthalpies of halogen are as given below: $F = - 332, Cl = - 349, Br = - 324, I = - 295 kJ {mol}^{- 1}$

The less negative for F as compared to that of $Cl$ is due to:

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strong electron-electron repulsions in the compact 2-p sub shell of F

strong electron-electron repulsions in the bigger 3-p sub shell of Cl

higher elec:tronegativity value of Cl

higher effective nuclear charge of F

answer is A.

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Detailed Solution

Due to the short size of the F atom, the tight 2p subshell's strong electron-electron repulsions prevent the incoming electron from being taken as readily as it is with Cl (less electron-electron repulsions).
Because of this, chlorine has a greater negative electron gain enthalpy than fluorine.

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