Question

type in the maximum number of electrons that can be present in each shell or subshell below.

n = 5 shell:

n = 2 shell:

n = 2, l = 0 subshell:

n = 2, l = 1 subshell:

3d subshell:

2s subshell:

5f subshell:

done

Explanation:

Step1: 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: 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 \(3d\) subshell (\(l = 2\)):
\(2(2\times2 + 1)=2\times5=10\)
For \(2s\) subshell (\(l = 0\)):
\(2(2\times0 + 1)=2\)
For \(5f\) subshell (\(l = 3\)):
\(2(2\times3+1)=2\times7 = 14\)

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: \(14\)