Ch.8 - Periodic Properties of the ElementsWorksheetSee all chapters
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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: Which of the following set of quantum numbers is not allowed?a. n = 1, l = 0, m l = 0, ms = −1/2b. n = 3, l = 2, m l = −1, ms = 1/2c. n = 5, l = 2, m l = −3, ms = −1/2d. n = 4, l = 3, m l = −2, ms = 1

Problem

Which of the following set of quantum numbers is not allowed?

a. n = 1, l = 0, m l = 0, ms = −1/2

b. n = 3, l = 2, m = −1, ms = 1/2

c. n = 5, l = 2, m = −3, ms = −1/2

d. n = 4, l = 3, m l = −2, ms = 1/2

Solution

We’re being asked to find which set of quantum numbers is possible


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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