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Question
Arrange the elements \[\ce{N, P, O}\] and \[\ce{S}\] in the order of increasing first ionisation enthalpy. Give reason for the arrangement assigned.
Solution
\[\ce{S < P < O < N}\]
Ionisation enthalpy increases from left to right in a period and decreases down the group. N has higher ionisation enthalpy than \[\ce{O}\] due to extra stability of half-filled orbitals. Similarly, \[\ce{P}\] has higher ionisation enthalpy than S due to half-filled orbitals.
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