Answer
The four quantum numbers of interest are n (principal quantum number), l (angular momentum) m1 (magnetic , and ms (spin )
A generic 4d2z orbital has n=4 and l=2.n=4 specifies the energy level ,and l specifices the orbitl's shape . s→l=0,p→l=1 etc, .Thus , its m1 varies as 0,±1,±2 and the orbital has projection above the plane and below the plane .
Depending on how full the orbital is, ms varies. If it happens to be a 4d1 configuration, for example, then one of five orbitals are filled ( (dx2−y2,d2z,dx,dxz,dyz)) with one electron. In that case, the electron is, by default,
spin ±12 Thus, ms=±12
In this case, it would give a term symbol of 2D1/2,2D3/2 and 2D5/2 The notation is :
2S+1LJ
where J=L+S
(The most stable one would be the 2D1/2 state, according to Hund's rules for less-than-half-filled orbitals with the same S and the same L.)
Here, the spin multiplicity is 02S+1=2(1/2)+1=2 ,and the total angular momentum J=L+S=|ml|+|ms|
=0+1/2,1+1/2, and 2+1/2=1/2,3/2, and 5/5
(2−−1/2=1+1+1/2 , and 1−1/2=0+1/2 , which are duplicates , while by the selection rules , ΔL=0,±1,ΔS=0, and ΔJ=0,±1