List the possible combinations of all four quantum numbers when n=2, l=1, and ml=0?

I know when n=2 and l=1 that the subshell would be 2p. I also know that the electron spin quantum number is +1/2 or -1/2 . Would I just list them like this: (2,1,0, +1/2 ) and (2,1,0, -1/2 )? Is there something that I am missing or doing wrong?

1 Answer
Apr 5, 2018

Yes your answer is correct.

Explanation:

If the principle quantum number is n, the azimuthal quantum number or orbital angular momentum quantum number can take values ranging from a minimum of 0 to a maximum value of n-1 and is a representation of the shape of the said orbital.

The magnetic quantum number which describes the number of orbitals and their orientation in a certain subshell can take values ranging from a maximum value of +l to a minimum value of -l.

The electron spin quantum number, which describes the magnetic properties of does not depend upon any other quantum number, can only take two representative values of +1/2 and -1/2

Since your question freezes the value of all these quantum numbers except the electron spin quantum number, the only two possible combinations of all four quantum numbers will be,
( 2,1,0,+1/2) and (2,1,0,-1/2)