first ionization enthalpy of nitrogen is higher than that of oxygen
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This causes free movement of electrons form 1st position to 2 or 3 (electrons keep interchanging their position). ... So oxygen would readily loose an electron to attain a stable configuration that is half filled configuration. So first Ionization energy of nitrogen is more than first ionization energy of oxygen
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(1) The electronic configuration of nitrogen (N, Z = 7) is 1s², 2s², 2p³ and that of oxygen (O, Z=8) is 1s², 2s² 2p^4.
(2) Nitrogen atom acquires extra stability due to half- filled 2p-orbitals while oxygen can acquire half-filled orbital and extra stability by losing one electron. Thus, oxygen can easily lose one electron.
(3) Nitrogen requires more energy to remove an electron due to extra stability. Therefore, first ionisation enthalpy of oxygen is less than that of nitrogen.
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