Answer:
The correct electron configuration for a ground-state nitrogen atom is 1s2 2s2 2p3.
Step-by-step explanation:
In this electron configuration, the nitrogen atom has a total of seven electrons, which are arranged in the various energy levels or shells around the nucleus. The first two electrons are in the first energy level or shell, which is represented by the 1s orbital. The next two electrons are in the second energy level or shell, which is represented by the 2s and 2p orbitals. The final three electrons are in the third energy level or shell, which is represented by the 2p orbital.
This electron configuration corresponds to the ground state of the nitrogen atom, which is the lowest energy state that the atom can occupy. The electron configuration can be written in a shorter form using the noble gas shorthand notation, in which the electron configuration of the preceding noble gas is used as a starting point and the remaining electrons are added. Using this notation, the electron configuration of nitrogen can be written as [He] 2s2 2p3.