This is a quick review of the quantum number notation we have used so far.
n = principle quantum number Describes the number of nodes in the wave function and its energy n = 1, 2, 3, ...
l = angular quantum number Describes the symmetry of the wave function and amount of angular momentum stored in the wave function l = 0, 1, ... n-1
m= magnetic quantum number Direction of angular momentum m = -l...0...l
This collection of numbers describe the energy and the wave function of an electron in an atom
In the early days of spectroscopy a different notation for describing electron energy states developed. This notation is still used widely in chemistry.
They use number and letters in this notation (you may find this familiar from chemistry class). s represents angular momentum = 0 or l = 0. p: l = 1; d: l=2 and so on.
Examples: 1s state is n=1, l=0
2s: n=1, l=0
2p: n=1, l=1, any value of m.
Hydrogen example:
-3.4 eV
-13.6 eV
Hydrogen also has energy levels at -1.51 eV (n = 3) and -0.85 eV (n = 4).
Use the n, l and m notation to write down all the possible energy states for these two values.