Answer:
(a) n = 2; l = 0; ml = -1 ⇒ WRONG
change ml = 0, or l = 1 to correct.
(b) n = 4, l = 3; ml = -1 ⇒ CORRECT
(c) n = 3, l = 1; ml = 0 ⇒ CORRECT
(d) n = 5, l = 2; ml = +3 ⇒ WRONG
change ml = 0, ±1 or ±2, or l = 3 or l = 4 to correct.
Explanation:
The rules for electron quantum numbers are:
1. Shell number, 1 ≤ n
2. Subshell number, 0 ≤ l ≤ n − 1
3. Orbital energy shift, -l ≤ ml ≤ l
4. Spin, either -1/2 or +1/2
Now, apply in our case
(a) n = 2; l = 0; ml = -1 ⇒ WRONG
-l ≤ ml ≤ l, so either change ml = 0 or l = 1 to correct.
(b) n = 4, l = 3; ml = -1 ⇒ CORRECT
(c) n = 3, l = 1; ml = 0 ⇒ CORRECT
(d) n = 5, l = 2; ml = +3 ⇒ WRONG
-l ≤ ml ≤ l, so either change ml = 0, ±1 or ±2, or l = 3 or l = 4 to correct.
