The magnetic quantum number specifies the orientation in space of an orbital of given energy and shape. This number divides the subshell into individual orbitals which hold the electrons; there are (2L+1) orbitals in each subshell. Thus, the s subshell has only one orbital, the p subshell has three orbitals, and so on.
For n=4, we have s,p,d,f subshells.
For s subshell, we have 2×0+1=1.
For p subshell, we have 2×1+1=3.
For d subshell, we have 2×2+1=5.
For f subshell, we have 2×3+1=7.
The total value of m will be 1+3+5+7=16
The principal quantum number is given as n=4
Thus the azimuthal quantum number has values, l=0 to (n−1).
∴l=0,1,2 and 3
