Explain why oxygen has lower ionisation enthalpy than nitrogen and fluorine.
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Oxygen has low ionisation energy (than that of nitrogen). It is due to an electron being added to an already half full orbital in oxygen, which results in electron electron repulsion, which will lower the ionisation energy. ... As Nitrogen is more stable, therefore it is much difficult to remove the valence electron.
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To become stable, both fluorine and oxygen must achieve a full octet, or set of 8 electrons in their outer shells. Therefore, it is more difficult to remove an electron from fluorine than from oxygen, giving it the higher ionization energy (highest one on the periodic table).
Explanation:
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