Electron affinity refers to the condition in that the energy released when an electron is added to the outermost shell of a neutral gaseous atom is called ‘electron affinity’ (EA). In simple terms, electron affinity is the tendency of an atom or molecule to accept electrons. On moving from left to right in the periodic table, the value of electron affinity increases due to the decrease in the value of atomic radius. On moving from top to bottom in the periodic table, the value of electron affinity decreases due to increase in atomic radius. Electron affinity is a periodic property.
Following are the factors affecting electron affinity (EA):
- On increasing the value of atomic radius, the value of electron affinity decreases.
- As the value of atomic radius decreases, the value of electron affinity increases.
- As the value of effective nuclear charge increases, the value of electron affinity also increases.
- As the value of screening effect or shielding effect increases, the value of electron affinity decreases.
- The outermost electronic configuration of the stable electronic configuration is more stable because its electronic configuration is completely filled. For this reason, the value of their electron affinity will be either zero or positive. The electron affinity of chlorine is highest.
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