I'm reviewing quantum numbers, and have a question about the 3rd quantum number, m_{l}. If m_{l} represents the specific orbital of an electron, why isn't the sum of the number of integers from -l to l equal to n^{2}, where n^{2} is the number of orbitals.

For instance: let's describe an electron in a p orbital. n=2, l=1, m_{l}= ^{-}1, 0, or 1, and m_{s} = -0.5 or 0.5.

My question is, why isn't the sum of the number of possible integers for the value of m_{l} (in this case 3) not equal to the total number of orbitals (which is n^{2}, which in this case is 4)

Is there an orbital which an electron cannot occupy?

Ah- I just answered my own question. The second quantum number specifies the subshell, hence the orbitals from s subshell are ignored in the 3rd quantum number. Posting this anyway, perhaps it will help someone else.