The quantum numbers of six electrons are given below. Arrange them in order of increasing energies. If any of these combination(s) has/have the same energy lists:
1. n = 4, l = 2, ml= –2 , ms = –1/2
2. n = 3, l = 2, ml= 1 , ms = +1/2
3. n = 4, l = 1, ml= 0 , ms = +1/2
4. n = 3, l = 2, ml= –2 , ms = –1/2
5. n = 3, l = 1, ml= –1 , ms = +1/2
6. n = 4, l = 1, ml= 0 , ms = +1/2
Quantum number refers to the set of four special numbers which provide the entire information about electrons of a particular atom.
‘n’ refers to the principle quantum number
‘l’ refers to the azimuthal quantum number
‘m’ refers to the magnetic quantum number
For n = 4 and L = 2, the orbital occupied is 4d.
For n = 3 and L = 2, the orbital occupied is 3d.
For n = 4 and L = 1, the orbital occupied is 4p.
Hence, the six electrons i.e., 1, 2,3,4,5, and 6 are present in the 4d, 3d, 4p, 3d, 3p, and 4p orbital respectively.
Therefore, the increasing order of energies of the electrons is 5[3p] < 2[3d] = 4[3d] <3[4p] = 6[4p] < 1[4d].