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 ***(m**_{l}**)**: deals with the orientation of the atomic orbital in 3D space. The possible values for m_{l} are the range of **–l to +l**.

• *Spin Quantum Number ***(m**_{s}**)**: deals with the spin of the electron. The possible values for m_{s} are either **–1/2 (spin down) or +1/2 (spin up)**.

Which of the following set of quantum numbers is not allowed?

a. n = 1, l = 0, m _{l} = 0, m_{s} = −1/2

b. n = 3, l = 2, m _{l }= −1, m_{s} = 1/2

c. n = 5, l = 2, m _{l }= −3, m_{s} = −1/2

d. n = 4, l = 3, m _{l} = −2, m_{s} = 1/2

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Spin Quantum Number concept. You can view video lessons to learn The Spin Quantum Number. Or if you need more The Spin Quantum Number practice, you can also practice The Spin Quantum Number practice problems.