Question 2.62: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 = –1/22. n = 3, l = 2, ml= 1 , ms = 1/23. n = 4, l = 1, ml = 0 , ms = 1/24. n = 3, l =...
Question 2.62:
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
1 answers
Answer:
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 orbitals respectively.
Therefore, the increasing order of energies is 5(3p)
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