Rules Governing the Allowed Combinations of Quantum Numbers
• The three quantum numbers (n, I, and m) that describe an orbital are integers: 0, 1, 2, 3, and so on.
• The principal quantum number (n) cannot be zero. The allowed values of n are therefore 1, 2, 3, 4, and so on.
• The angular quantum number (1) can be any integer between 0 and n - 1. If n = 3 for example, I can be either 0, 1, or 2.
• The magnetic quantum number (m) can be any integer between -I and +1. If I = 2 m can be either -2, -1, 0, +1, or +2.
Hence,
n = 3 = 3, m_{1} = - 2 m_{s} = 1/2
here n = 3 and I = 3 which is not possible (it can only 0,1,2). There this set is not possible.
