Ch.7 - Quantum MechanicsWorksheetSee 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
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Ch.10 - Molecular Shapes & Valence Bond Theory
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Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
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Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: 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

Problem

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

Solution

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 (ml): deals with the orientation of the atomic orbital in 3D space. The possible values for ml are the range of –l to +l.

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