🤓 Based on our data, we think this question is relevant for Professor Giles' class at VCU.

What is the total number of orbitals having *n* = 4 and *l* = 2?

- 2

- 5

- 16

- 4

- 6

We’re being asked to **determine the number of orbitals** for **n = 4 and l = 2**.

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**.