Question

#35. What are the 3 rules that govern the filling of atomic orbitals by electrons? #36. Arrange the following sublevels in order of increasing energy: 3d, 2s, 4s, 3p #37. Which of these orbital designations is invalid? 4s 2d 3f 3p #38. What is the maximum number of electrons that can go in each of the following sublevels? 2s / 4s / 4p / 4f / 10 3p / 3d / 5s / 5p /

Answer 1

Explanation:

35.

The 3 rules are:-

Pauli Exclusion Principle:-

It states that no two electrons present in an atom or a molecule can have same set of the four quantum numbers.  

Even if the two electrons are present in same state which means that if it is present in the same orbital , n, l and m are same but still the forth quantum number which is spin quantum number is different for them. Both the two electrons have opposing spins having value either $\frac {1}{2}$ or $\frac {-1}{2}$.

Hund's rule of maximum multiplicity:-

Firstly, every orbital which is present in the sublevel is singly occupied and then the orbital is doubly occupied.

Aufbau principle:-

It states that the electrons fill the atomic orbitals from the lowest energy to the highest energy levels in ground state.

36.

Increasing Energy levels:-

2s < 3p < 4s < 3d

This is arranged according to the aufbau's principle and n+l rule.

37.

The designations which are invalid are:-

2d as n = 2 Acceptable l = 0 and 1 only

d belongs to l =2

3f as n = 3 Acceptable l = 0, 1 and 2 only

f belongs to l =3

38.

2s can accommodate 2 electrons.

4s can accommodate 2 electrons.

4p can accommodate 6 electrons.

4f can accommodate 14 electrons.

3p can accommodate 6 electrons.

3d can accommodate 10 electrons.

5s can accommodate 2 electrons.

5p can accommodate 6 electrons.