A) B < Be < N < C
B) Be > B > C > N
C) B < Be < C < N
D) Be < B < C < N
Correct Answer: C
Solution :
lionization 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 ionization 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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