2.29 (6th Edition)

[Claudia Luong 4K]

I am confused on parts b and d on this problem. How does specifying the magnetic quantum number change the number of orbitals and/or the number of electrons that the orbitals can hold?

QUESTION
2.29 How many electrons can have the following quantum numbers in an atom: (b) n =4, l= 2,
ml= 2; (d) n =3, l=2, ml =1

[Chem_Mod]

Recall that the magnetic quantum number specifies which orbital we're looking at in a given subshell.
For example, in a p subshell (l=1), we have ml values (-1,0,1), and each of these correspond with a different p orbital orientation (px, py, pz). In each orbital, we can have 2 electrons maximum.