Which set of numbers gives the correct possible values of l for n = 2?
0
0, 1
0, 1, 2
0, 1, 2, 3

0, 1

Explanation:

1) n and ℓ are two quantum numbers.

The quantum numbers are:

Principal quantum number (n)

Azimuthal quantum number (ℓ)

Magnetic quantum number (m)

Spin quantum number (s)

2) Principal quantum number (n), tells the main energy level, which is related with the size of the orbitals. It is also refered as the shell of the electrons.

The principal quantum number (n) may be an integer number among 1, 2, 3, 4, 5, 6, and 7.

3) Azimuthal quantum number (ℓ) tells the shape of the orbital. It is seen as the sub-shell.

This quantum number may be identified either by a number of a letter. These are the correspondences between the letter and the numbers.

quantum number (ℓ) orbital or subshell

0 s

1 p

2 f

3 d

3) The main energy level, n = 1, can only have one subshell: the s subshell. So, when n = 1, ℓ can only be 0.

When n = 2, ℓ can only be 0 or 1

When n = 3, ℓ can only be 0, 1, or 2.

And so on.

This is summarized by the following rule: the values of ℓ are 0, 1, 2, ... n - 1. This is any whole number less than n.

So, since the question states n = 2, ℓ can be 0 or 1 (orbitals s or p).