Which of the following set of quantum numbers is not allowed?
a. n = 1, l = 0, m l = 0, ms = −1/2
b. n = 3, l = 2, m l = −1, ms = 1/2
c. n = 5, l = 2, m l = −3, ms = −1/2
d. n = 4, l = 3, m l = −2, ms = 1/2
We’re being asked to find which set of quantum numbers is possible.
Recall that the quantum numbers that define an electron are:
• Principal Quantum Number(n): deals with the size and energy of the atomic orbital. The possible values for n are 1 to ∞.
• Angular Momentum Quantum Number (l): deals with the shape of the atomic orbital. The possible values for l are 0 to n – 1.
• Magnetic Quantum Number (ml): deals with the orientation of the atomic orbital in 3D space. The possible values for ml are the range of –l to +l.
• Spin Quantum Number (ms): deals with the spin of the electron. The possible values for ms are either –1/2 (spin down) or +1/2 (spin up).