Which of the following is a correct set of quantum numbers for an electron in a 3d orbital?

a. n = 3, l = 0, m _{l} = -1

b. n = 3, l = 1, m _{l} = +3

c. n = 3, l = 2, m _{l} = 3

d. n = 3, l = 3, m _{l} = + 2

e. n = 3, l = 2, m _{l} = -2

We’re being asked to find **which set of quantum numbers** is **possible** for a **3d electron**.

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

Introduction to Quantum Mechanics

Introduction to Quantum Mechanics

Introduction to Quantum Mechanics

Introduction to Quantum Mechanics