We’re being asked to determine the number of orbitals for n=3, l=2 and n=3, l = 1
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 is the range of l: –l to +l.
What is the subshell corresponding to the following sets of quantum numbers? an example of a subshell is 2s?
a. n=3, l=2
b. n=3, l=1
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 Introduction to Quantum Mechanics concept. You can view video lessons to learn Introduction to Quantum Mechanics. Or if you need more Introduction to Quantum Mechanics practice, you can also practice Introduction to Quantum Mechanics practice problems.