Why electron gain enthalpy of nitrogen is more than oxygen?
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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 configuration of N, it cannot readily lose electron and therefore, its ionization enthalpy is higher than that of O.
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Due to this extra stable electronic configuration, it is difficult to remove an electron from the valence shell of nitrogen (or any other Group 15 element) and thus more energy is required. Thus ionization enthalpy of nitrogen is higher than oxygen.
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