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Arrange the elements N, P, O and S in the order of (i) increasing first ionisation enthalpy. (ii) increasing non-metallic character. Give reason for the arrangement assigned.

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Nitrogen will have maximum ionisation enthalpy as half filled stability in 2p3, then phosphorus as electron had to be removed from farther orbital 3p3, in 16 group,oxyg oxygen followed by sulphur. So S<O<P<N ii) P<N<S<O,as oxygen electronegativity is more than Sulphur, similarly, nitrogen...
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Nitrogen will have maximum ionisation enthalpy as half filled stability in 2p3, then phosphorus as electron had to be removed from farther orbital 3p3, in 16 group,oxyg oxygen followed by sulphur. So S<O<P<N ii) P<N<S<O,as oxygen electronegativity is more than Sulphur, similarly, nitrogen more electronegative than phosphorus read less
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