A) \[B<Be<N<C\]
B) \[Be>B>C>N\]
C) \[B<Be<C<N\]
D) \[Be<B<C<N\]
Correct Answer: C
Solution :
Ionisation energy generally increase in a period from left to right. But due to comparatively stabler configuration of\[Be(1{{s}^{2}},\,\,2{{s}^{2}})\], it has more ionisation energy than Boron\[(1{{s}^{2}},\,\,2{{s}^{2}}2{{p}^{1}})\]. Hence, the correct order is: \[B<Be<C<N\]
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