A) \[B<Be<C<\text{O}<N\]
B) \[B<Be<C<N<O\]
C) \[Be<B<C<N<O\]
D) \[Be<B<C<O<N\]
Correct Answer: A
Solution :
The ionisation potential increases from left to right in a period but the first ionization potential of nitrogen is greater than oxygen due to half-filled stable configuration and ionisation potential of Be is greater than B due to completely filled 5-orbital. Hence, the order of ionisation potential is as: Element: \[B\,\,\,<\,\,\,Be\,\,\,<\,\,\,C\,\,\,<\,\,O\,\,<\,\,N\] IP(eV) : 8.3 9.3 11.2 13.6 14.5
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