question_answer

If the nitrogen atom had electronic configuration \[1{{s}^{7}}\] it would have energy lower than that of the normal ground state configuration \[1{{s}^{2}}2{{s}^{2}}2{{p}^{3}}\] because the electrons would be closer to the nucleus. Yet \[1{{s}^{7}}\] is not observed. It violates

A) Heisenberg's uncertainty principle

B) Hund's rule

C) Pauli exclusion principle

D) Bohr postulate of stationary orbits