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, $$m_l$$ = –2 , ms = $$-\dfrac{1}{2}$$

2. n = 3, l = 2, $$m_l$$= 1 , ms = $$+\dfrac{1}{2}$$

3. n = 4, l = 1, $$m_l$$ = 0 , ms = $$+\dfrac{1}{2}$$

4. n = 3, l = 2, $$m_l$$= –2 , ms = $$-\dfrac{1}{2}$$

5. n = 3, l = 1, $$m_l$$ = –1 , ms= $$+\dfrac{1}{2}$$

6. n = 4, l = 1, $$m_l$$ = 0 , ms = $$+\dfrac{1}{2}$$

Asked by Abhisek | 1 year ago |  161

##### Solution :-

Electrons  1, 2, 3, 4, 5, and 6 reside in the 4d, 3d, 4p, 3d, 3p, and 4p orbitals (respectively). Ranking these orbitals in the increasing order of energies: (3p) < (3d) < (4p)  < (4d).

Answered by Abhisek | 1 year ago

### Related Questions

#### How many sub-shells are associated with n = 4?

(a) How many sub-shells are associated with n = 4?

(b) How many electrons will be present in the sub-shells having ms value of $$- \dfrac{1}{2}$$ for n = 4?

#### Indicate the number of unpaired electrons in:

Indicate the number of unpaired electrons in:

(a) P

(b) Si

(c) Cr

(d) Fe

(e) Kr

#### The unpaired electrons in Al and Si are present in 3p orbital.

The unpaired electrons in Al and Si are present in 3p orbital. Which electrons will experience more effective nuclear charge from the nucleus?

#### Among the following pairs of orbitals which orbital will experience the larger effective nuclear charge?

Among the following pairs of orbitals which orbital will experience the larger effective nuclear charge?

(i) 2s and 3s,

(ii) 4d and 4f,

(iii) 3d and 3p