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
Mahibur R.
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#)

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