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what  is electron affinity ,ionization energy and intraelectronic repulsion

Dear Student,

It's interelectronic repulsion instead of intraelectronic repulsion 

  • Interelectronic repulsion is the opposing force or the force of repulsion that exists b/w the electrons revolving around an atom in their fixed orbits.
  • Electron affinity ia the amount of energy that is released when a neutral atom in its gaseous state accepts an electron to form an anion i.e. a negatively charged ion 

             X (atom)       +        e- (electron)                        >        X- (anion)        +      energy released (electron affinity)

  • Ionisation potential is the amount of energy that is needed to remove a loosely bound electron frm the valence shell of an isolated gaseous atom to form a cation i.e. a positively charged ion

            X (atom)        +       energy (ionisation energy)                      >         X+        +        e-

Hope it is clear to u !!!

Best Wishes!

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Ionisation energies are always concerned with the formation of positive ions. Electron affinities are the negative ion equivalent, and their use is almost always confined to elements in groups 6 and 7 of the Periodic Table.

Defining first electron affinity

The first electron affinity is the energy released when 1 mole of gaseous atoms each acquire an electron to form 1 mole of gaseous 1- ions.

This is more easily seen in symbol terms.

It is the energy released (per mole of X) when this change happens.

First electron affinities have negative values. For example, the first electron affinity of chlorine is -349 kJ mol-1. By convention, the negative sign shows a release of energy.

The first electron affinities of the group 7 elements
F-328 kJ mol-1
Cl-349 kJ mol-1
Br-324 kJ mol-1
I-295 kJ mol

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