Match each set of quantum numbers to the correct subshell description by typing in the correct number.

1: n = 2, l = 0 2p:
2: n = 3, l = 2 3d:
3: n = 1, l = 0 2s:
4: n = 2, l = 1 4f:
5: n = 4, l = 3 1s:

The location of the valence electron or the outermost electron is expressed in quantum numbers. There are five quantum numbers: prinicipal (n), angular momentum (l), magnetic (ms) and magnetic spin (ms) quantum numbers. This is based on Bohr's atomic model where electrons orbit around the nucleus. These electrons are in the orbitals with specific energy levels. Starting from energy level 1 that is closest to the nucleus, the energy level decreases to 2, 3, 4, 5, 6, and 7. These energy level numbers represent the principal quantum number. Within each orbital also contains subshell. From increasing to decreasing order, these subshells are the s, p, d and f subshells. These subshells represent the angular momentum quantum numer. Specifically, s=0, p=1, d=2 and f=3. Therefore, if the electron is in the orbital 5p, the quantum number would be: 5, 1. Applying these to the choices, the correct pairing would be:

2p: n=2. l=1
3d: n=3, l=2
2s: n=2. l=0
4f:  n=4. l=3
1s: n=1, l=0