why is the 1st ionisation enthalpy of oxygen is smaller as compared to nitrogen ?

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Solution

Electronic configuration of nitrogen(N) -1s²2s²2p³.
Electronic configuration of oxygen (O) -1s²2s²2p².
Thus, outer p orbital of nitrogen is half filled whereas outer orbital p of oxygen contain two electron. Hence nitrogen consist of more stable electronic configuration than oxygen and its require higher ionization energy to remove outer electron from nitrogen outer p orbital.

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