Question

type in the maximum number of electrons that can be present in each shell or subshell below.
m = 5 shell:
m = 2 shell:
m = 2, l = 0 subshell:
m = 2, l = 1 subshell:
3d subshell:
2s subshell:
5f subshell:

Explanation:

Step1: Use formula for number of electrons in a shell

The formula for the maximum number of electrons in a shell with principal quantum number \(n\) is \(2n^{2}\).
For \(n = 5\):

$$2\times5^{2}=2\times25 = 50$$

For \(n = 2\):

$$2\times2^{2}=2\times4=8$$

Step2: Use formula for number of electrons in a sub - shell

The formula for the maximum number of electrons in a sub - shell with azimuthal quantum number \(l\) is \(2(2l + 1)\)
For \(n = 2,l = 0\) (s - subshell):

$$2(2\times0 + 1)=2\times1 = 2$$

For \(n = 2,l = 1\) (p - subshell):

$$2(2\times1+ 1)=2\times3 = 6$$

For \(3d\) (\(l = 2\)):

$$2(2\times2 + 1)=2\times5 = 10$$

For \(2s\) (\(l = 0\)):

$$2(2\times0 + 1)=2\times1 = 2$$

For \(5f\) (\(l = 3\)):

$$2(2\times3+ 1)=2\times7 = 14$$

Answer:

\(n = 5\) shell: \(50\)
\(n = 2\) shell: \(8\)
\(n = 2,l = 0\) subshell: \(2\)
\(n = 2,l = 1\) subshell: \(6\)
\(3d\) subshell: \(10\)
\(2s\) subshell: \(2\)
\(5f\) subshell: \(14\)