Provide the complete set of quantum numbers for all the electrons that could populate the 3d subshell of an atom.

My answer: n = 5, l = 4, ml = -4, -3, -2, -1, 0, 1, 2, 3, 4, ms = -1/2 or 1/2

Am I correct or did I make a mistake?

I believe you need to regroup. If it's the 3d orbital then n = 3. Isn't that right?

1s2 2s2 2p6 3s2 3p6 3d10 4s2 etc.

Your answer is incorrect. Let me explain how to determine the quantum numbers for electrons in the 3d subshell.

The quantum numbers for an electron consist of four values: the principal quantum number (n), the azimuthal quantum number (l), the magnetic quantum number (ml), and the spin quantum number (ms).

1. Principal quantum number (n): This quantum number represents the energy level or shell in which the electron resides. In this case, since we are considering the 3d subshell, the principal quantum number would be 3.

2. Azimuthal quantum number (l): This quantum number determines the shape of the orbital. It is related to the subshell type. For d subshell, the value of l is 2.

3. Magnetic quantum number (ml): This quantum number describes the orientation of the orbital within a particular subshell. The possible values of ml range from -l to +l, including 0. For the d subshell, with l = 2, the values of ml would be -2, -1, 0, 1, and 2.

4. Spin quantum number (ms): This quantum number represents the spin state of the electron, either +1/2 (spin-up) or -1/2 (spin-down).

So, the correct set of quantum numbers for all the electrons in the 3d subshell would be:
n = 3, l = 2, ml = -2, -1, 0, 1, 2, ms = -1/2 or 1/2.

Therefore, the complete set of quantum numbers for the electrons that could populate the 3d subshell would be n = 3, l = 2, ml = -2, -1, 0, 1, 2, ms = -1/2 or 1/2.