There are four quantum numbers for an orbital:
1. Principal quantum number n: It tells about the position of orbital that is shell number. The values are 1, 2, 3,....
2. Azimuthal quantum number l: It describes the shape of orbital, for s, p, d, f,... orbitals, the value is 0, 1, 2, 3,... so on.
3. Magnetic quantum number [tex]m_{l}[/tex] : The value of magnetic quantum number varies from -l to +l (including zero), it defines the sub shell of an orbital.
4. Spin quantum number s: Spin of the electron defines its movement, clockwise or anticlockwise thus, there are only two possible values for spin quantum number that is +1/2 or -1/2.
No two orbitals can have same value for all the four quantum numbers.
[tex]2p_{z}[/tex] orbital is suborbital of 2p orbital, the 2p orbital is drawn in the attachment.
The first three quantum numbers for [tex]2p_{z}[/tex] orbitals are n=2, l=1 and [tex]m_{l}[/tex] =-1. This set of quantum number is possible for only 1 orbital therefore, there is only 1 orbital with designation [tex]2p_{z}[/tex].
