Answer:
(a) n = 2, l = 0 ⇒ sublevel s, ⇒ ml = 0, number of orbitals = 1
(b) n = 3, l = 2 ⇒ sublevel d, ⇒ ml = 0, ±1, ±2, number of orbitals = 5
(c) n = 5, l = 1 ⇒ sublevel p, ⇒ ml = 0, ±1, number of orbitals = 3
Explanation:
The rules for electron quantum numbers are:
1. Shell number, 1 ≤ n,
2. Subshell number, 0 ≤ l ≤ n − 1, from s, p, d, f, g, h...
3. Orbital energy shift, -l ≤ ml ≤ l
4. Spin, either -1/2 or +1/2
In our case
(a) n = 2, l = 0 ⇒ sublevel s
-l ≤ ml ≤ l ⇒ ml = 0, number of orbitals = 1
(b) n = 3, l = 2 ⇒ sublevel d
-l ≤ ml ≤ l ⇒ ml = 0, ±1, ±2, number of orbitals = 5
(c) n = 5, l = 1 ⇒ sublevel p
-l ≤ ml ≤ l ⇒ ml = 0, ±1, number of orbitals = 3
