Feel free to look at the syllabus or to scroll through the list of readings.

Feel free to examine the syllabus for the class.

Sample tests from previous semesters can be found here.

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Class 1: Introductions and the Nature of Science

Chapter 1 Sections 1.1-1.4, 1.13

Review Questions: 1, 3, 4

Class 2: Measurement.
If you have ever doubted the importance of keeping track of your units, this news story might set you straight. Here is an exmple of the group activity that we did to accompany our look at the topics in Chapter 1.

Chapter 1 Sections 1.10 and 1.11.

Review Questions: 9, 10
Problems: 19-22, 23-26, 45-52, 53-64
Additional Problems: 69-80

Class 3: 2.1 through 2.4 (pp. 40-50). The early laws of chemical composition and how atomic theory can acount for these laws. This activity helps to demonstrate how mass ratios arise from atom (or object) ratios.
Review Questions 1-3, 6-13
Problems 15-18, 21, 22, 25, 26, 35-38, 44, 45, 47

Class 4: Another activity that we did in class. This one examines some basics of nuclear structure, and helps accustom us to the symbols we use when describing atoms. The activity was designed to accompany Chap 3 sections 3.1,3.4-3.5.
Review Questions 2, 5, 7-10, 13-18, 27, 28 (p. 77)
Problems 31-36 (p. 78)

Class 5: After finishing our look at atomic symbols, we moved on to describing the electronic structure of an atom. That is, where do we expect to find an atom's electrons. Chap 3 sections 3.6-3.8
Review Questions: 11, 19-26, 34

Class 6: Building Bricks and Lewis Structures/Balls, Sticks, and Lewis Structures

4.1 The Art of Deduction: Stable Electron Configurations
Review Questions: 1-6
4.2 Lewis (Electron-Dot) Symbols
Problems: 7-8
4.10 Rules for Writing Lewis Formulas
Problems: 25-30
4.6 Covalent Bonds: Shared Electron Pairs
Skipping Nomenclature
Problems: 35 a, b, c, d (central atom = C), e (central atom = N); 36 a (central atom = N), b, d, e (central atom = C), f (central atom = S); 37 a, c (central atom = Br); 38 a, b (central atom = Cl)

Class 7: Ionic vs Covalent Bonding, Polar Covalent Bonds, Shape

4.3 Sodium Reacts with Chlorine: Facts
4.4 Using Lewis Symbols: More Ionic Compounds
Problems: 9-10
4.5 Formulas and Names of Binary Ionic Compound (skipping nomenclature)
Problems: 19

Class 8: Ionic vs Covalent Bonding, Polar Covalent Bonds, Shape

4.3 Sodium Reacts with Chlorine: Facts
4.4 Using Lewis Symbols: More Ionic Compounds
Problems: 9-10
4.5 Formulas and Names of Binary Ionic Compound (skipping nomenclature)
Problems: 19
4.7 Unequal Sharing: Polar Covalent Bonds
Problems 39-44
Problems 45-48
4.12 Molecular Shapes: The VSEPR Theory
Problems: 49, 50

Class 9: Polar Covalent Bonds, and Shape and Polar Molecules

4.7 Unequal Sharing: Polar Covalent Bonds
Problems 39-44
Problems 45-48
4.12 Molecular Shapes: The VSEPR Theory
Problems: 49, 50
4.13 Shapes and Properties: Polar and Nonpolar Molecules
Problems: 51-54
Additional Problems
59, 62-71

Class 10: Test on all topics up to this point

Shape and Polarity
Activity 8, Intermolecular Forces

Polar Covalent Bonds, and Shape and Polar Molecules

4.7 Unequal Sharing: Polar Covalent Bonds
Problems 39-44
Problems 45-48
4.12 Molecular Shapes: The VSEPR Theory
Problems: 49, 50
4.13 Shapes and Properties: Polar and Nonpolar Molecules
Problems: 51-54
Additional Problems
59, 62-71

Quiz 3

Solubility and Intermolecular Forces
Activity 9

6.2 Comparing Ionic and Molecular Compounds
6.4 Forces in Solution

Review Solubility and Intermolecular Forces

6.2 Comparing Ionic and Molecular Compounds
6.4 Forces in Solution

Predicting Precipitation Reactions
Activity 10

Molar Mass and Avogadro's Hypothesis

Chap 5, 5.3 Avagadro's Number and the Mole
Exercise 5.3a and 5.3b
5.4 Molar Mass: Mole-to-Mass and Mass-to-Mole Conversions (through p 132)

Away at Conference

Using Chemical Reactions to Determine the Amount of "Stuff" Present: Precipitation Reactions
Activity 11, determining the amount of NaCl present by precipitating AgCl from solution.

Chap 5.4 Molar Mass: Mole-to-Mass and Mass-to-Mole Conversions (p 133-136 and alternate method for determining mass relationships), Chap 5.5
Problems 33-38

Introduce Acid-Base Chemistry: Chap 7

7.1 Acids and Bases: Experimental Definitions
7.2 Acids, Bases, and Salts
7.5 Neutralization
7.9 Antacids: A Basic Remedy
7.10 Acids and Bases in Industry and in Us

Test 2: Test on material since last test

Using Chemical Reactions to Determine the Amount of "Stuff" Present: Acid digestion and spectrophotometric determination of Pb²⁺ concentration, Chap 7.5, 7.9, 7.10, Chap 5.4, Chap 5.5
Discuss upcoming laboratory and do sample calculations in Activity 14.

Identifying Bases: Chap 7.1, 7.2, 7.3
Activity 12

Identifying Acids: Chap 7.1, 7.2, 7.3
Activity 13

Using Chemical Reactions to Determine the Amount of "Stuff" Present: Acid-Base Titrations, Chap 7.5, 7.9, 7.10, Chap 5.5, Chap 5.4
Finish calculations for laboratory activity where the amount of antacid in a tablet is determined by reacting the tablet with excess hydrochloric acid.

Begin energy: Chap 15
Discuss energy, work. Define First and Second Laws. Define and dicsuss PE and KE, and their interconversion.
Establish chemical bonds as a source of potential energy.

Continue with eneregy, Chap 15
Examine sources of energy on earth. Consider the role of CO₂ in the environment, and how different fuels produce varying amounts of CO₂.

Continue with eneregy, Chap 15
Do activity that calculates CO₂ production from two different fuels.

Friday: Test on material since last test