We're asked to answer 3 parts of the problem. **Part A** asks the **only possible values of m _{l}** for an electron in an

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

• *Spin Quantum Number ***(m _{s})**: deals with the spin of the electron. The possible values for m

**Part A. **What is the only possible value of *m*ℓ for an electron in an *s* orbital? Express your answer numerically.

**Part B. **What are the possible values of *m*ℓ for an electron in a *d* orbital? Express your answer numerically with sequential values separated by commas.

**Part C. **Which of the following set of quantum numbers (ordered *n*, ℓ, *m*ℓ, *m*s) are possible for an electron in an atom? Check all that apply.

a. 3, 2, 0, -1/2

b. -4, 3, 1, 1/2

c. 3, 2, 2, -1/2

d. 5, 3, -3, 1/2

e. 3, 1, -2, -1/2

f. 3, 3, 1, -1/2

g. 2, 1, 0, -1

h. 4, 2, 3, -1/2

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