Question

Which is a correct set of values of m for one of the subshells of n = 2?

Answer 1

n=3 this is the answer

Answer 2

Answer: Thus correct set of values of m for of n = 2 is +1, 0 and -1.

Explanation:

1. Principle Quantum Number: This quantum number describes the size of the orbital. It is represented by n. here n=2, i.e L shell

2. Azimuthal Quantum Number: This quantum number describes the shape of the orbital. It is represented as 'l'. The value of l ranges from 0 to (n-1). For l=2= 0,1,.. the orbitals are s, p.

3. Magnetic Quantum Number: This quantum number describes the orientation of the orbitals. It is represented as m. The value of this quantum number ranges from $(-l\text{ to }+l)$. When l = 0, the value of m will be  0, if l = 1, m = +1, 0 and -1.