Answer
See the explanation
Work Step by Step
𝑛 = principal quantum number (1, 2, 3, …)
𝑙 = subshell type:
s → l = 0
p → l = 1
d → l = 2
f → l = 3
For a given 𝑛, 𝑙 can only be
0, 1, ..., 𝑛−1
→ So 𝑙 must be less than n.
Each orbital (defined by a unique
$𝑛, 𝑙, m_l$ holds 2 electrons (one ↑ and one ↓).
The maximum number of electrons that can have each of the following designations are:
\( 2 f \)
$n=2,l=3\Rightarrow l>n$ not allowed
0 electrons
\( 2 d_{x y} \)
$n=2,l=2\Rightarrow l=n$ not allowed
0 electrons
\( 3 p \):
$n=3,l=1\Rightarrow l
