If nitrogen atom had an electronic configuration of $1s^7$, it would have energy lower than it’s normal ground state configuration of $1s^{2}2s^{2}2p^3.Yet,1s^7$ is not observed as it violates:

Q. If the nitrogen atom had an electronic configuration of $1s^7$ it would have lower energy than that of the normal ground state configuration $1s^2,2s^2,2p^3$ because the electrons would be closer to the nucleus. $1s^7$ is not observed because it violates:

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

Q.

If carbon atom has electronic configuration 1$s^6$, it would have energy lower than that of the normal ground state configuration 1$s^2$ 2$s^2$ 2$p^2$. Yet 1$s^6$ is not observed because it violates

Q. If the nitrogen atom had electronic configuration $1S^7$, it would have enrgy lower than that of the normal ground state configuration $1s^2,2s^2,2p^3$, because the electrons would be closer to the nucleus. Yet $1s^7$ is not observed because it violates.

Q. If carbon has electronic configuration $1s^6$, it would have lower energy than that of the normal ground state configuration $1s^{2}2s^{2}2p^2$, because the electrons would be closer to the nucleus. Yet $1s^6$ is not observed, since it violates