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Can anyone explain the first ionisation energy order of NO, O AND N ?
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Can anyone explain the first ionisation energy order of NO, O AND N ?
Among N and O , N has the higher ionisation energy because of half filled configuration. Since in NO the last e goes to the antibonding orbital so it's easier to remove it. So trend follows N>O>NO
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Can anyone explain the first ionisation energy order of NO, O AND N ?
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