A) \[Cl\]
B) Br
C) I
D) F
Correct Answer: A
Solution :
The electron affinity decreases from \[Cl\to Br+I\] i.e., on moving down the group. However, electron affinity of fluorine is unexpected low. It cannot be explained by any simple mechanism. It is probably due to small size of the atom. The addition of an extra electron produces high electron charge density in a relatively compact 2p sub-shell resulting in strong electron-electron repulsion. The repulsive forces between electrons imply low electron affinity. So, the correct order of electron affinity for halogens is: \[I<Br<F<Cl\]
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