Question

Which one of the following sets of quantum numbers can correctly represent a 3p orbital?

a) (n = 3 l = 1, ml = 2)

b)(n = 1, l = 3, ml = 3)

c) (n = 3, l = 2, ml = 1)

d) (n = 3, l = 1, ml = -1)

e) (n = 3, l = 0, ml = 1)

Answer 1

3p so

n = 3
l = 1 because it's a p
ml can be -1 or 0 or +1

You take it from here.
You can immediately rule out a because of mL, b because of n, c because l, etc.

Answer 2

The answer should be Option (d) (n = 3, l = 1, mₗ = -1).

This is because a 3p orbital must have n = 3.
*That eliminates Option (b), because it has n = 1*

A p orbital must have l = 1.
*That eliminates Options (c), and (e), because they have l = 2, and 0*

The mₗ is required to be an integer satisfying −l ≤ m ≤ l, so mₗ could be any of −1, 0, or +1.
*That eliminates Option (a), because they have mₗ = 2*

The only correct option is:
(d) n = 3, l = 1, mₗ = -1