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

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.

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

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