**Possible values of l, m, and s when n=2**

When the principal quantum number (n) is given as 2, we need to determine the possible values of the azimuthal quantum number (l), the magnetic quantum number (m), and the spin quantum number (s).

The principal quantum number (n) defines the energy level or shell of an electron in an atom. In the case of n=2, it corresponds to the second energy level.

To determine the possible values of l, we use the rule that states l can have values ranging from 0 to (n-1). Therefore, for n=2, l can have values 0 and 1.

The azimuthal quantum number (l) determines the shape of the electron's orbital. When l=0, it represents an s orbital, and when l=1, it represents a p orbital.

Next, we need to determine the possible values of m. The magnetic quantum number (m) represents the orientation of the orbital in three-dimensional space. It can have values ranging from -l to +l.

For l=0, m can only be 0, as there is only one orientation for an s orbital.

For l=1, m can have values -1, 0, and 1, representing the three different orientations of a p orbital.

Finally, we need to determine the possible values of s. The spin quantum number (s) represents the direction of the electron's spin. It can have two possible values: +1/2 (spin up) and -1/2 (spin down).

Therefore, the possible values of l, m, and s when n=2 are as follows:

- l can have values 0 and 1.
- For l=0, m=0.
- For l=1, m can have values -1, 0, and 1.
- The spin quantum number (s) can have values +1/2 and -1/2.

In summary, when n=2:
- l can be 0 or 1
- m can be 0, -1, or 1 (depending on the value of l)
- s can be +1/2 or -1/2