Answer:
Nitrogen has extra stability due
to half filled p-orbitals :
\[1{{s}^{2}},2{{s}^{2}}2p_{x}^{1}2p_{y}^{1}2p_{z}^{1}\]
The stable atom resists the
addition of extra electron, i.e., external energy is required. On account of
this nitrogen has positive electron gain enthalpy.
Oxygen has unsymmetrical
configuration:
\[1{{s}^{2}},2{{s}^{2}}2p_{x}^{2}2p_{y}^{1}2p_{z}^{1}\]
The extra electron can be added
and the added electron comes under the influence of nuclear attraction. So, in
this process, energy is released and thus, electron gain enthalpy of oxygen is
negative.
The ionisation enthalpy of
nitrogen is higher on account of the stability of atom while in oxygen, the
electron is lost easily as the atom tries to acquire stable configuration of \[2{{p}^{3}}\]
from \[2{{p}^{4}}\] and hence, its ionisation enthalpy is lower than nitrogen.
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