Azimuthal quantum number (l) :
It describes the shape of electron cloud and the number of subshells in a shell. It can have value from 0 to (n-1)
`{:("Value of l",0,1,2,3),("subshell",s,p,d,r):}`
Number of orbitals in a subshell =2l+1
Orbital angular momentum L`=h/(2pi)sqrt(l(l+1)) =ħsqrt(l(l+1)) " " [ħ=h/(2pi)]`
Magnetic quantum number (m) :
It describes the orientations of the subshells . It can have values from -l to +l including zero, i.e. , total (2l+1) values . Each value corresponds to an orbital. s-subshell has one orbital , p-subshell three orbitals `(p_x ,p_y and p_z)` , d-subshell five orbitals `(d_"xy", d_"yz",d_(x^2-y^2), d_z^2)` and f-subshell has seven orbitals.
Spin quantum number (s) :
It describes the spin of the electron. It has values +1/2 and -1/2 . Signifies clockwise spinning and anticlockwise rotation of electron about its own axis.
Spin of the electron produces angular momentum equal to `S=sqrt(s(s+1)) h/(2pi)` where `s=+1/2`
Total spin of an atom `=+n/2` or `-n/2` (where n is the number of unpaired electron )
The magnetic moment of an atom
`mu_s=sqrt(n(n+2))` B.M. n=number of unpaired electrons
B.M. (Bohr magneton)
Orbital angular momentum of an electron is `sqrt3h/pi` then the number of orientations of this orbital in spaces are :

Options

A. 3
B. 5
C. 7
D. 9