Factors affecting the value of electron affinity
(i) Atomic size : The value of electron affinity decreases with the increase in the size of atom since the nuclear attraction decreases down a group as the atomic number increases. The value of it increases as we move along a period since the size of atoms decreases along a period. Lower value of F than Cl is because of the very small size of F in which negative charge is highly concentrated and repels the incoming electron thereby reducing the force of attraction of the nucleus towards the adding electron and hence decreasing the electron affinity. Hence, chlorine has a highest value of electron affinity.
(ii) Nuclear charge : The value of electron affinity increases with increasing nuclear charge. Hence, its value increases with the increase in nuclear charge along a period.
(iii) Screening or shielding effect : The value of electron affinity increases with the decrease in shielding effect of inner electrons. Further, the value of electron affinity also depends to some extent upon the type of orbital in which electron is added. Value of it is greater when electron enters 's' orbital and decreases successively for p, d and f orbitals(2)
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