A) \[[Ne],\text{ }2{{s}^{2}},\text{ }3{{p}^{2}}\]
B) \[[Ne],\text{ }3{{s}^{2}},\text{ }3{{p}^{3}}\]
C) \[[Ne],\text{ 3}{{s}^{2}},\text{ 2}{{p}^{4}}\]
D) \[[He],\text{ }2{{s}^{2}},\text{ }2{{p}^{3}}\]
Correct Answer: D
Solution :
: Nitrogen\[([He]\text{ }2{{s}^{2}}\text{ }2{{p}^{3}})\]has a stable electronic configuration due to extra-stability of the half filled orbitals. Hence, more energy is required to remove an electron from nitrogen. Also, ionization energy decreases as we move down the group,
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