Nitrogen has positive electron gain enthalpy whereas oxygen has negative. However, oxygen has lower ionisation enthalpy than nitrogen. Explain.

Explanation

The outermost electronic configuration of nitrogen is `2s ^(2)2p_(x) ""^(1)2p_(z) ""^(1).` It is stable because it has exactly half filled 2p-subshell. Therefore, it has no tendency to accept extra electron and energy has to b e supplied to add additional electron. Thus, electron gain enthalpy of nitrogen is slightly positive. On the other hand, the outermost electronic configuration of O is `2s ^(2), 2p _(x) ""^(2) 2p _(y) ""^(1) 2p _(z) ""^(1).` It has higer positive change (+8) than nitrogen (+7) and lower atomic size than N. Therefore, it has a tendency to accept an extra electron. Thus, electron gain enthalpy of O is negative. However, oxygen has four electrons in the 2p subshell and can lose one electron to acquire stable half filled configuration and therefore, it has low ionization enthalpy. Because of stable configurition of N, it cannot readily lose electron and therefore, its ionization enthalpy is higher than that of O.