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  Change of Electron Affinity along a Group

Change of Electron Affinity along a Group:

On moving down a group, the size of atom raises appreciably and therefore, the effective nuclear attraction for the electron reduces. Accordingly the atom will possess fewer tendencies to attract additional electrons towards it. This means that electron affinity would reduce as we move down a group. In case of halogens the reduction in electron affinity from chlorine to iodine is due to the steady raise in atomic radii from chlorine to iodine.

On moving down a group the electron affinity reduces. Therefore, the electron affinity of Cl must be less than F. However actually the electron affinity of F (320 kJ mol-1) is less than Cl (348 kJ mol-1). The reason for this is perhaps due to small size of fluorine atom. The addition of an extra electron generates high electron density that raises strong electron-electron repulsion. The repulsive forces among electrons outcomes in low electron affinity.

The electron affinities of noble gases are zero. Since these atoms possess ns2 np6 configuration in their valence shells, these are most stable atoms and there are no chances for the addition of an extra electron. Therefore, the electron affinities of noble gases are zero.

Electron affinities of beryllium and nitrogen are approximately zero. This might be due to the extra stability of the complete 2s-orbital in beryllium and of the precisely half-filled p-orbital in nitrogen. Since these are stable electronic configurations, they do not have the tendency to accept electrons and thus, the electron affinities for beryllium and nitrogen are zero.

 

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