Question

Which of the following correctly lists all possible values of m l , the magnetic quantum number, for a subshell designation of 3d?

a. 0
b. 1, 0, −1
c. 3, 2, 1, 0, −1, −2, −3
d. 2, 1, 0, −1, −2

Answer 1

Option D: The correct values of the magnetic quantum number for a 3d subshell are –2, –1, 0, +1, and +2, which relate to the five different orientations of the d orbitals.

Step-by-step explanation:

The question regards the possible values of the magnetic quantum number (ml) for a 3d subshell. The magnetic quantum number describes the orientation of an electron's orbital within a magnetic field and can have values ranging from –l to +l, including zero. For a d subshell where l = 2, the values of ml can be –2, –1, 0, +1, and +2. Therefore, the correct listing of all possible values of ml for a 3d subshell are –2, –1, 0, +1, and +2, corresponding to the five different d orbitals present in the subshell.

The magnetic quantum number, m₁, specifies the relative spatial orientation of a particular orbital. Generally speaking, m₁ can be equal to -1, −(1 − 1), ..., 0, ..., (1 – 1), 1.

The subshell designation of 3d corresponds to n = 3 and l = 2. For l = 2, the possible values of m₁ are -2, -1, 0, 1, and 2. Therefore, the correct answer is d. 2, 1, 0, −1, −2.