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,You need to login to perform this action.
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