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  Factors affecting electron affinity

Factors affecting electron affinity:

(1) Atomic size:

Electron affinity α (1/ Size of atom)

Lower the size of an atom, bigger is its electron affinity. Since the size of atom rises, the efficient nuclear charge reduces or the nuclear attraction for adding electron reduces. Consequently, atom will have fewer tendencies to attract additional electron towards it. Hence,

Electron affinity α Effective nuclear charge.

In common, electron affinity reduces in going down the group and raise in going from left to right across the period. On moving down the group atomic size rises and on going from left to right in a period atomic size reduces.

(2) Shielding or Screening Effect:

Electron affinity α (1/ effect Shielding)

Electronic energy state, lying among nucleus and outermost state hinder the nuclear attraction for incoming electron. Thus, greater the number of inner lying state low will be the electron affinity.

(3) Electronic Configuration:

The electronic configurations of elements persuade their electron affinities to a considerable amount.
Electron affinities of inert gases are zero. This is since their atoms have stable ns2 np6 configuration in their valence shell and there is no possibility for addition of an additional electron.

Electron affinity of magnesium, beryllium, and calcium is practically zero. This is accredited to extra stability of the fully completed s-orbitals in them. Therefore, if an atom has completely filled or half filled orbitals, its electron affinity will be less.

 

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