why is ionisation energy of oxygen less than that of nitrogen
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electronic configuration of oxygen
1s² 2s² 2p⁴
electronic configuration of nitrogen
1s² 2s² 2p³
due to the stability of halfly filled p orbital of oxygen more energy is required in order to remove the electron from its p orbital
the ionisation energy of nitrogen is high as compared to oxygen
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Answer:
Ionisation energy of oxygen is less than that of nitrogen because oxygen needs two electrons to complete its octet as it has 6 valence electrons in its last shell and nitrogen needs 3 electrons to complete its octet as it has 5 valence electrons in its last shell.
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