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account the following:

a)ionization enthalpy of nitrogen is greater than that of oxygen

b)atomic radius decreses from left to right in a period

c)electron gain enthalpy of fluorine is less negative than that of chlorine

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a)The configuration of Nitrogen is-1s22s22p3 which is half filled and half filled and full filled electronic configuration is a stable configuration. So Nitrogen will not like to lose one electron as after losing it will not have full filled configuration and will become unstable. So more amount of energy is required to remove the electron. Whereas the electronic congfiguration for Oxygen is-1s22s22p4which is not half filled and after losing one electron it will gain half filled configuration which is stable. So energy required for removal of electron is less and oxygen has less I.P. than nitrogen.

b)In a period as we move from left to right the electrons are added to same valence shel and so nuclear charge over the valence electron increases and atomic size decreases.

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