Which one of the following represents an acceptable set of quantum numbers for an electron in an atom? (arranged as n, 1, m, and ms) A) 3, 2, - 2, - 1/2 B) 3, 3,-4, 1/2 C) 3,2,0,0 D) 3,3,3, - 1/2 E) 3, 4, 6, - 1/2 A-2

The correct option is A) 3, 2, - 2, - 1/2.

Explanation:

Quantum numbers represent different properties regarding the level, sublevel and orbital in which an electron is. There are 4 quantum numbers:

Principal quantum number (n) : indicates the level of energy and gives information about the size of an orbital. It can only take positive and integer values, e. g., 1, 2, 3 ... Angular quantum number (l) : indicates the sublevel of energy and provides information about the shape of the orbital. Some common shapes are spherical (l=0) and polar (l=1). Shapes for bigger l are more complicated. l values depend on n values. l values can be integers up to (n-1). For example. if n = 2, l can take the values 0 and 1. Magnetic quantum number (m) : it gives information about the orientation in space of an orbital. It may take any integer value between - l and + l. For example, if l = 1, m can take values - 1, 0 and 1, each one referring to an orbital p along a different axis in the space (x, y and z axes). Spin quantum number (ms) : it refers to the spin angular momentum of an electron and it can take 2 values: - 1/2 or + 1/2.

A) 3, 2, - 2, - 1/2 is correct because it follows every rule.

B) 3, 3,-4, 1/2 is wrong because if n=3, l can only be up to 2, and l from - 3 to + 3.

C) 3,2,0,0 is wrong because ms cannot take the value 0.

D) 3,3,3, - 1/2 is wrong because if n=3, l can only be up to 2.

E) 3, 4, 6, - 1/2 is wrong because if n=3, l can only be up to 2, and l from - 3 to + 3.