Variation of ionisation energy in periodic table

(i) Ionisation energy decreases in a group as the atomic number increases. This is based on the fact that as we go down the group, the size of atom increases, and the outer electrons become farther away from the nucleus hence reducing the force of attraction and hence ionisation energy decreases.

(ii) Ionisation energy increases along a period with increase in atomic number. This is because of the size of atom since it decreases along a period and outer electrons are most strongly attracted by the nucleus and hence more energy is required to remove the electron.

(iii) The ionisation energies of inert gases are greater than that of their immediate neighbour. It is due to their complete octet ns²p⁶ configuration which is highly stable. Hence, it is very difficult to remove an electron from the outermost orbit of an inert gas.

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