Question

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

n = 2, l = 0 2p = ____?

Answer 1

The set of quantum numbers n = 2, l = 0 corresponds to the 2s subshell, not the 2p subshell. In spectroscopic notation using quantum numbers, 2s is the correct description for these values, and the n = 2 shell can accommodate up to 8 electrons in total, considering both 2s and 2p subshells.

Step-by-step explanation:

To match the set of quantum numbers to the correct subshell description, we need to look at the values of the quantum numbers n and l. For the quantum numbers n = 2 and l = 0, they correspond to the 2s subshell, not the 2p subshell. The principal quantum number n indicates the shell level, which is the second shell in this case, and the angular momentum quantum number l defines the subshell. The value 0 for l designates the s subshell. Thereby, for the given quantum numbers, 2p would be incorrect. Instead, the correct subshell description would be 2s.

In quantum chemistry, subshells are denoted using the principal quantum number n followed by a letter corresponding to the angular momentum quantum number l, where l = 0 indicates an 's' subshell, l = 1 indicates a 'p' subshell, and so on. So, using this spectroscopic notation, the presented quantum numbers match the 2s subshell.

In total, for the n = 2 shell, there are two subshells: 2s and 2p. The 2s subshell can hold a maximum of 2 electrons, while the 2p subshell can hold up to 6 electrons, allowing for a total of 8 electrons within the n = 2 shell when considering all possible sets of quantum numbers, including magnetic (m) and spin (ms) quantum numbers.

Answer 2

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, the correct pairing would be:

2p: n=2. l=1