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
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 statement about quantum numbers is  incorrect?  Answer (e) if they are all correct or all incorrect.a. The principal quantum number cannot equal zero.b. When n = 3, the angular quantum number ca

Problem

Which statement about quantum numbers is  incorrect?  Answer (e) if they are all correct or all incorrect.

a. The principal quantum number cannot equal zero.

b. When n = 3, the angular quantum number can be equal to 0, 1, or 2.

c. For an angular quantum number equal to 1, the magnetic quantum number can be +1, 0, o-1.

d. For any value of the angular quantum number (l), there are 2(2l+1) values of the magnetic quantum number.

e. All the above statements are correct or all are incorrect.

Solution

We’re being asked to determine the incorrect statement among the choices


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 is the range of l: –l to +l.


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