Which is a correct set of values of m for one of the subshells of n = 2? –1, 0, 1 –1, –2, 0, 1, 2 –1, –2, –3, 0, 1, 2, 3 –1, –2, –3, –4, 0, 1, 2, 3, 4

The correct answer is -1, 0, 1.

Explanation:

The Quantum numbers are:

1. Principle Quantum Number: This number describes the size of the orbital. It is represented by "n". The value of n = 1,2,3,4....

2. Azimuthal Quantum Number: This number describes the shape of the orbital. It is denoted as "l". The value of l ranges from 0 to (n-1).

3. Magnetic Quantum Number: This number describes the orientation of the orbitals in space. It is denoted as . The value of ranges from .

We are given:

n = 2 which means,

Value of l = 0 to (2 - 1) = 0, 1

Value of

Hence, the correct answer is -1, 0, 1.