Question

Which of the following is a correct set of quantum numbers for an electron in a 3d orbital?

1) n = 3, l = 2, m = 0, s = +1/2
2) n = 2, l = 1, m = -1, s = -1/2
3) n = 4, l = 3, m = 2, s = -1/2
4) n = 3, l = 2, m = -1, s = -1/2

Answer 1

The correct set of quantum numbers for an electron in a 3d orbital is n = 3, l = 2, m1 = -1, ms = -1/2 (choice 4).

Step-by-step explanation:

The question asks which set of quantum numbers correctly describes an electron in a 3d orbital. Quantum numbers include the principal quantum number (n), angular momentum quantum number (l), magnetic quantum number (m1), and spin quantum number (ms).

For a 3d orbital, n would be 3 and l would be 2, since for d-type orbitals l = 2. The magnetic quantum number m1 for d orbitals can range from -2 to +2 (since it ranges from -l to +l), and the spin quantum number ms can be either +1/2 or -1/2.

Given the options, the correct set of quantum numbers for an electron in a 3d orbital is: n = 3, l = 2, m1 = -1, ms = -1/2, which corresponds to choice 4.