CHM 1045

Fall 2002

Dr. Light's Sections

General Chemistry I

Tentative Lecture Schedule

FLH 255

12:20-1:10 pm

Date

Chapter

Topic

Pages

Aug 26

M

1

Class Organization

1.2 Getting Started:  Some Key Terms

(1.3-1.6 To be covered in recitation)

3-9

9-28

Aug 28

W

2

2.1 Laws of Chemical Combination

2.2 John Dalton and the Atomic Theory of Matter

2.3 The Divisible Atom

2.4 Atomic Masses

36-38

38-40

40-42

42-45

Aug 30

F

2

2.5 The Periodic Table: Elements Organized

2.6 Molecules and Molecular Compounds

45-48

48-52

Sep 2

M

LABOR DAY (No Class)

Sep 4

W

2

2.7 Ions and Ionic Compounds

2.8 Acids, Bases, and Salts

52-58

58-61

Sep 6

F

2

2.9 Alkanes: Saturated Hydrocarbons

2.10 Types of Organic Compounds

61-67

67-71

Sep 9

M

3

3.1 Molecular Masses and Formula Masses

3.2 The Mole and Avogadro's Number

3.3 More on the Mole

82-84

84-86

86-90

Sep 11

W

3

3.4 Mass Percent Composition from Chemical Formulas

3.5 Chemical Formulas from Mass Percent Composition

3.6 Elemental Analysis: Experimental Determination of Mass Percent Composition

90-94

94-97

97-100

Sep 13

F

3

3.7 Writing and Balancing Chemical Equations

3.8 Stoichiometric Equivalence and Reaction

100-105

105-109

Sep 16

M

3

3.9 Limiting Reactants

3.10 Yields of Chemical Reactions

3.11 Solutions and Solution Stoichiometry

110-112

112-115

115-123

Sep 18

W

4

4.1 Some Electrical Properties of Aqueous Solutions

4.2 Reactions of Acids and Bases

133-137

137-148

Sep 20

F

1-3

Hour Test 1

Sep 23

M

4

4.2 Reactions of Acids and Bases (con't)

4.3 Reactions that Form Precipitates

137-148

148-153

Sep 25

W

4

4.4 Oxidation-Reduction

153-159

Sep 27

F

4

4.5 Oxidizing and Reducing Agents

4.6 Some Practical Applications of Oxidation-Reduction

160-163

163-169

Sep 30

M

5

5.1 Gases: What Are They Like?

5.2 The Kinetic-Molecular Theory: An Introduction

5.3 Gas Pressure

5.4 Boyle's Law: The Pressure-Volume Relationship

178

179

179-185

185-187

Oct 2

W

5

5.5 Charles's Law:  The Temperature-Volume Relationship

5.6 Avogadro's Law: The Mole-Volume Relationship

5.7 The Combined Gas Law

187-190

191-193

193-195

Oct 4

F

Fall Break (No Class)

Oct 7

M

5

5.8 The Ideal Gas Law

5.9 Gases in Reaction Stoichiometry

195-200

201-204

Oct 9

W

5

5.10 Mixtures of Gases: Dalton's Law of Partial Pressures

5.11 The Kinetic-Molecular Theory: Some Quantitative Aspects

5.12 Real Gases

204-209

210-216

216-217

Oct 11

F

4-5

Hour Test 2

Oct 14

M

6

6.1 Energy

6.2 Thermochemistry: Some Basic Terms

227-229

229-233

Oct 16

W

6

6.3 Internal Energy (U), State Functions, and the First Law of Thermodynamics

6.4 Heats of Reaction and Enthalpy Change (DH)

233-236

236-244

Oct 18

F

6

6.5 Calorimetry: Measuring Quantities of Heat

244-253

Oct 21

M

6

6.6 Hess's Law of Constant Heat Summation

6.7 Standard Enthalpies of Formation

6.8 Combustion and Respiration: Fuels and Foods

253-256

256-262

262-266

Oct 23

W

7

7.1 The Electron: Experiments of Thomson and Millikan

7.2 Atomic Models:  J.J. Thomson and Ernest Rutherford

7.3 Protons and Neutrons

276-279

279-281

281-283

Oct 25

F

7

7.4 Positive Ions and Mass Spectrometry

7.5 The Wave Nature of Light

283-284

284-290

Oct 28

M

7

7.6 Photons: Energy by the Quantum

7.7 Bohr's Hydrogen Atom: A Planetary Model

290-295

295-299

Oct 30

W

7

7.8 Wave Mechanics: Matter as Waves

7.9 Quantum Numbers and Atomic Orbitals

299-302

302-309

Nov 1

F

6-7

Hour Test 3

Nov 4

M

8

8.1 Multielectron Atoms

8.2 An Introduction to Electron Configurations

8.3 The Rules for Electron Configurations

317-318

318-319

319-321

Nov 6

W

8

8.4 Electron Configurations: The Aufbau Principle

8.5 Electron Configurations: Periodic Relationships

321-325

325-332

Nov 8

F

8

8.6 Magnetic Properties: Paired and Unpaired Electrons

8.7 Periodic Atomic Properties of the Elements

332-333

334-347

Nov 11

M

Veterans' Day (No Class)

Nov 13

W

8

8.8 Metals, Nonmetals, Metalloids, and Noble Gases

8.9 Explaining the Behavior of the Elements Through Atomic Properties and the Periodic Table

343-347

347-350

Nov 15

F

9

9.1 Chemical Bonds: A Preview

9.2 The Lewis Theory of Chemical Bonding: An Overview

9.3 Ionic Bonds and Ionic Crystals

359-360

360-362

362-363

Nov 18

M

9

9.4 Using Lewis Symbols to Represent Inoic Bonding

9.5 Energy Changes in Ionic Compound Formation

363-365

365-368

Nov 20

W

9

9.6 Lewis Structures of Some Simple Molecules

9.7 Polar Covalent Bonds and Electronegativity

368-372

372-375

Nov 22

F

8-9(part)

Hour Test 4

Nov 25

M

9

9.8 Strategies for Writing Lewis Structures

9.9 Molecules that Don't Follow the Octet Rule

375-384

385-389

Nov 27

W

9

9.10 Bond Lengths and Bond Energies

9.11 Alkenes and Alkynes

9.12 Polymers

390-395

395-397

397-401

Nov 29

F

8-9

Thanksgiving (No Class)

Dec 2

M

10

10.1 Valence-Shell Electron-Pair Repulsion (VSEPR Method)

409-419

Dec 4

W

10

10.2 Polar Molecules and Dipole Moments

10.3 Atomic Orbital Overlap

420-425

425-427

Dec 6

F

10

10.4 Hybridization of Atomic Orbitals

10.5 Hybrid Orbitals and Multiple Covalent Bonds

10.8 Bonding in Benzene

427-435

436-443

448-449

Dec 10

Tu

FINAL EXAM

Block Exam Time (7:30-9:30 a.m.)