Ch.8 - Periodic Properties of the ElementsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Part A. What is the only possible value of mℓ for an electron in an s orbital? Express your answer numerically.Part B. What are the possible values of mℓ for an electron in a d orbital? Express your a

Solution: Part A. What is the only possible value of mℓ for an electron in an s orbital? Express your answer numerically.Part B. What are the possible values of mℓ for an electron in a d orbital? Express your a

Problem

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

Part B. What are the possible values of mℓ 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, mℓ, ms) 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

Solution

We're asked to answer 3 parts of the problem. Part A asks the only possible values of ml for an electron in an s orbital, part B asks the possible values of m for an electron in a d orbital, and part C asks to check all applying sets of quantum numbers that apply for an electron in an atom.


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 are the range of –l to +l.

• Spin Quantum Number (ms): deals with the spin of the electron. The possible values for ms are either –1/2 (spin down) or +1/2 (spin up).


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