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Asked by Abhishek Last Modified
Answer 
Ionization enthalpy is the energy required to remove an electron from the outermost shell. Here the first case is of Boron and Beryllium where B has 1s2 2s2 electronic configuration and Be has 1s2 2s2 2p1. Now energy required to remove an electron from 2p1 is obviously less than that required to remove an electron from 2s2 (that is fully filled 2s orbital). Similar is the case of nitrogen and oxygen where nitrogen has full half filled 2p orbital and oxygen has more electron after having fully half filled 2p orbital.
read lessIonisation enthalpy increases in a period with increase in atomic number. The graph shows few exceptions and not the linear relationship. Ionisation enthalpy of Be is greater than that of B due to filled s-orbital in Be (Be – l.s2 1s2, B – 1s2 2s2 2pl).
Ionisation enthalpy of N is greater than that of O due to half-filled/?-orbitals in nitrogen.
(N – Is2 2s22p3 O – ls 2 2s2 2p4).
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