Question

If an electron has the quantum numbers n = 2, l = 1, ml = -1, ms = + ½, which type of atomic orbital is it occupying?

a. 2s
b. 2p
c. 2d
d. 2

Answer 1

The electron with quantum numbers n = 2, l = 1, ml = -1, ms = + ½ is occupying a 2p atomic orbital.

Step-by-step explanation:

The electron with quantum numbers n = 2, l = 1, ml = -1, ms = + ½ is occupying a 2p atomic orbital.

The quantum numbers n, l, ml, and ms represent different properties of an electron in an atom. The value of n represents the principal quantum number, which determines the energy level or shell of the electron. The value of l represents the azimuthal quantum number, which determines the subshell or orbital type. The value of ml represents the magnetic quantum number, which determines the orientation of the orbital in space. The value of ms represents the spin quantum number, which represents the spin state of the electron, either +1/2 (spin up) or -1/2 (spin down).

In this case, the electron is in the n = 2 energy level, the l = 1 subshell (p orbital), the ml = -1 orientation, and the ms = + ½ spin state. Therefore, the electron is occupying the 2p atomic orbital.