To determine the electron configuration of nitrogen (N), we first consider its atomic number, which is 7. This means a neutral nitrogen atom has 7 electrons. These electrons will occupy the available orbitals in a specific sequence according to the principles of quantum mechanics, which dictate the order of filling based on increasing energy levels.
The sequence in which atomic orbitals are filled is guided by the Aufbau principle, Hund's rule, and the Pauli exclusion principle. Here’s the filling order:
1. The 1s orbital is filled first since it is the lowest in energy. It can hold up to 2 electrons.
2. Next, the 2s orbital is filled. It can also hold up to 2 electrons.
3. Finally, the 2p orbitals are filled. These orbitals can collectively hold up to 6 electrons, but since we only have 3 remaining electrons to place, they will partially fill the 2p orbitals.
Step by step, we fill the orbitals as follows:
1. 1s orbital: Takes the first 2 electrons
- Configuration so far: [tex]\(1s^2\)[/tex]
2. 2s orbital: Takes the next 2 electrons
- Configuration so far: [tex]\(1s^2 2s^2\)[/tex]
3. 2p orbitals: The remaining 3 electrons go into the 2p orbitals
- Configuration so far: [tex]\(1s^2 2s^2 2p^3\)[/tex]
Thus, the electron configuration of nitrogen (N) is as follows:
[tex]\( 1s^2 2s^2 2p^3 \)[/tex].
So, the correct option is:
[tex]\[ \boxed{1s^2 2s^2 2p^3} \][/tex]
