Question

What is the maximum number of electrons that can occupy each of the following subshells?

Answer 1

s (l = 0) only two electrons

p (l = 1) sublevel six (6) electrons fit

d (l = 2) sub-level has 10 electrons

f (l = 3) has 7 has 14 electrons

Step-by-step explanation:

The electrons have an odd spin, so they must comply with the Pauli principle, therefore only two electrons fit in a given sublevel.

Sub level s (l = 0) only two electrons

Sub level p (l = 1) has three orbitals in which two electrons fit, therefore in the sublevel six (6) electrons fit

Sub-level d (l = 2) has 5 orbitals each with two electrons, the sub-level has 10 electors

Sub-level f (l = 3) has 7 orbitals and two electrons each, the sub-level has 14 electrons

Answer 2

Step-by-step explanation:

Using paulis exclusive principle which states that no two electrons can have the same four electronic quantum numbers,

A. 3 p

3p is in the 3rd shell (m), p orbital has 3 orbitals which contain only 2 electrons. Therefore, total electrons in the p orbital = 2 × 3

= 6 orbitals.

B. 5 d

5 d is in the 5th shell, d orbital has 5 orbitals which contain only 2 electrons. Therefore, total electrons in the p orbital = 2 × 5

= 10 orbitals.

C. 2 s

2 s is in the 2nd shell (l), s orbital has 1 orbitals which contain only 2 electrons. Therefore, total electrons in the p orbital = 2 × 1

= 2 orbitals.

D. 4 f

4 f is in the 4th shell (n), f orbital has 7 orbitals which contain only 2 electrons. Therefore, total electrons in the p orbital = 2 × 7

= 14 orbitals.