Explain why ionisation enthalpy of nitrogen is more than oxygen
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Nitrogen has half filled stable configuration. To remove it's outer electron we have to give more energy than oxygen as it is stable and half filled that is why it has more ionisation enthalpy.
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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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