A) \[B<Be<C<O<N\]
B) \[B<Be<C<N<O\]
C) \[~Be<B<C<N<\text{O}\]
D) \[~Be<B<C<O<N\]
Correct Answer: A
Solution :
The ionisation potential increases from left to right in a period but -the first ionisation 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 s-orbital. Hence, the order of ionisation potential is as: \[\begin{align} & \text{Element:}\,\,\,B\,\,\,<\,\,\,Be\,\,\,\,\,<\,\,\,\,C\,\,\,\,<\,\,\,\,O\,\,\,\,\,\,\,\,<\,\,\,\,N\, \\ & \text{IP(eV)}\,\,\,\,\,\,8.3\,\,\,\,\,\,\,\,\,9.3\,\,\,\,\,\,\,\,\,11.2\,\,\,\,\,\,\,13.6\,\,\,\,\,\,14.5\, \\ \end{align}\]
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