Which of the following is a possible set of quantum numbers for an electron (n, l, m0, ms) ?

(1, 1, 0, + )

(2, 1, 2, + )

(3, 2, 0, - )

(3, - 2, 1, - )

Answer is: (3, 2, 0, - 1/2).

The principal quantum number (n) is one of four quantum numbers which are assigned to each electron in an atom to describe that electron's state.

For principal quantum number n=3:

1) azimuthal quantum number (l) can be l = 0 ... n-1:

l = 0, 1, 2.

The azimuthal quantum number determines its orbital angular momentum and describes the shape of the orbital.

2) magnetic quantum number (ml) can be ml = - l ... + l.

ml = - 2, - 1, 0, + 1, + 2.

Magnetic quantum number specify orientation of electrons in magnetic field and number of electron states (orbitals) in subshells.

3) the spin quantum number (ms), is the spin of the electron.

ms = + 1/2, - 1/2.

(1, 1, 0, + 1/2) is not correct because orbital quantum number cannot be l = 1 for n = 1.

(2, 1, 2, + 1/2) is not correct because magnetic quantum number cannot be ml = 2 for orbital quantum number l = 1.

(3, - 2, 1, - 1/2) is not correct because orbital quantum number cannot be l = - 2 for principal quantum number n = 3.