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 ***(m _{l})**: deals with the orientation of the atomic orbital in 3D space.

The possible values for m_{l} 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

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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: 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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