D and P orbital question

[Kai Johnson 3B]

Quick question,

If the D orbital is always one lower than the S orbital therfore coming first when writing out electron configuration, why isn't p orbital lower as well. Why do we start at 2p rather than 1p?

[Autumn Kasl-Godley 3J]

I'm still not entirely sure why d can be lower energy than s, but there is no 1p subshell. Not every subshell (n) has every type of subshell (l), and we can figure this out using the quantum numbers. If acceptable values of l are everything up until n-1, then the n=1 subshell can only have l values of 0, which corresponds to only the s subshell. N=2 has l=0 or l=1, so the second shell has both s and p subshells. N=3 has s, n, and d, and n=4 has f as well. Therefore, you cannot put electrons in the 1p subshell, since it doesn't exist.

[405996618]

The configuration has the ordered list that we follow, there are however certain tricky parts. We start with 1s, 1p, 2p, 1d, 2d, 3d.... however, we use 4s before going to 3d because 4s is lower in energy.

[Averie Moore 2F]

We start at 2p because there is no 1p orbital. The d orbital comes before because of the arrangements of energy in these orbitals. The orbitals fill from lowest to highest energy levels.

[105561735]

For the 1p orbital question, in the first shell there can only exist a maximum of 2 electrons therefore the most suitable orbital would be 1s