Quantum Numbers: Angular Momentum Quantum Number Video Lessons

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Problem: What is the subshell corresponding to the following sets of quantum numbers? an example of a subshell is 2s?a. n=3, l=2b. n=3, l=1

FREE Expert Solution

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.


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Problem Details

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

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

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Based on our data, we think this problem is relevant for Professor Donnelly's class at UCF.