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).
Which of the following sets of quantum numbers are not allowed? For each incorrect set, state why it is incorrect.
a. n = 3, ℓ = 3, mℓ = 0, ms = -1/2
b. n = 4, ℓ = 3, mℓ = 2, ms = -1/2
c. n = 4, ℓ = 1, mℓ = 1, ms = +1/2
d. n = 2, ℓ = 1, mℓ = -1, ms = -1
e. n = 5, ℓ = -4, mℓ = 2, ms = +1/2
f. n = 3, ℓ = 1, mℓ = 2, ms = -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 Quantum Numbers: Spin Quantum Number concept. You can view video lessons to learn Quantum Numbers: Spin Quantum Number. Or if you need more Quantum Numbers: Spin Quantum Number practice, you can also practice Quantum Numbers: Spin Quantum Number practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Onwuachi's class at HCC.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.