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Chemistry, by Raymond Chang
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Week#
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Lecture#
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Topic
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Chapter
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Pages
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Examples
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Problems
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1
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1
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Introduction, SI-Units and their Prefix,
Temperature Scales
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1
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15-17
19-21
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1.3
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1.17, 1.18, 1.23, 1.25, 1.26
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2
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The Atomic Theory, The Structure of the Atom
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2
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42-49
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3
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Atomic Number, Mass Number, and Isotopes
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2
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49-50
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2.1
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2.10, 2.11, 2.12, 2.14, 2.16, 2.18
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2
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4
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The Periodic Table, Molecules and Ions, Chemical Formulas
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2
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50-58
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2.2, 2.3, 2.4
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2.26, 2.34, 2.36, 2.44, 2.46
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5
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Naming Compounds
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2
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59-64
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2.5, 2.6, 2.7, 2.8
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2.58, 2.60
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6
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Atomic Mass, problem 3.6 p107
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3
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78-79
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3.1
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3.5, 3.6, 3.7, 3.8
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3
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7
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Avogadro’s Number and the Molar Mass of an Element
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3
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79-82
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3.2, 3.3, 3.4
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3.14, 3.16, 3.18, 3.20, 3.22
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8
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Molecular Mass
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3
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83-85
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3.5, 3.6, 3.7
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3.24, 3.26, 3.28
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9
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Percent Composition of Compounds, Experimental Determination of Empirical and Molecular Formulas
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3
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86-92
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3.8, 3.9, 3.10, 3.11
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3.40, 3.42, 3.44, 3.46, 3.48, 3.50, 3.52
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4
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10
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Chemical Reactions and Chemical Equations - Amounts of Reactants and Products
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3
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92-101
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3.12, 3.13, 3.14
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3.60
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11
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Limiting Reagents, Reaction Yield
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3
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101-106
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3.15, 3.16
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3.84, 3.86
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12
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Concentration of Solutions (Molarity and Dilution)
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4
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142-148
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4.6, 4.7, 4.8
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4.60, 4.62, 4.64, 4.66, 4.70, 4.72, 4.74
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5
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13
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Substances That Exist as Gases, Pressure of a Gas, The Gas Laws
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5
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170-178
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5.1, 5.2
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5.1, 5.2, 5.3, 5.8, 5.14, 5.22
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14
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The Gas Laws, The Ideal Gas Equations
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5
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178 - 189
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5.3, 5.4, 5.5, 5.8, 5.9, 5.10
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5.24, 5.32, 5.36, 5.38, 5.40, 5.44, 5.48, 5.50, 5.94
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15
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Gas Stoichiometry, Dalton’s Law of Partial Pressures
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5
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190-196
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5.11, 5.12, 5.14, 5.15
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5.52, 5.54, 5.64, 5.66, 5.68, 5.70
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6
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16
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From Classical Physics to Quantum Theory
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7
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268-272
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7.2, 7.3
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7.3, 7.8, 7.16, 7.18,
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17
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Bohr’s Theory of the Hydrogen Atom, The Dual Nature of the Electron
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7
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274-282
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7.4, 7.5
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7.32, 7.34, 7.40, 7.42, 7.120
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18
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Quantum Mechanics, Quantum Numbers, Atomic Orbitals
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7
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283-292
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7.6, 7.7
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7.56, 7.58, 7.62, 7.66, 7.70
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7
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19
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Electron Configurations, The Building-Up Principle
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7
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292-302
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7.8, 7.9, 7.10, 7.11
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7.76, 7.78, 7.79, 7.84, 7.88, 7.90, 7.124
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20
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Periodic Classification of the Elements
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8
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318-322
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8.1
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8.5, 8.8, 8.12, 8.20, 8.24, 8.26, 8.28, 8.30, 8.32
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21
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Periodic Variation in Physical Properties
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8
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322-327
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8.2, 8.3
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8.36, 8.38, 8.40, 8.44, 8.46
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8
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22
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Ionization Energy, Electron Affinity
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8
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329-335
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8.4
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8.52, 8.54, 8.62, 8.64
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23
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Lewis Dot Symbols, The Ionic Bond, The Covalent Bond, Electronegativity
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9
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358-360 366-372
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9.1, 9.2
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9.16, 9.18, 9.30, 9.36, 9.74
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24
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Writing Lewis Structures, Formal Charge and Lewis Structures
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9
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372-377
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9.3, 9.4, 9.5, 9.6, 9.7
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9.44, 9.46, 9.48,
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9
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25
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The Concept of Resonance, Exceptions to the Octet Rule
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9
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377-385
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9.8, 9.9, 9.10, 9.11, 9.12
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9.52, 9.56, 9.64, 9.80
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26
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The Concept of Equilibrium and the Equilibrium Constant, Writing Equilibrium Constant Expressions
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14
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602-612
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14.1, 14.2, 14.3, 14.4, 14.5, 14.6
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14.3, 14.8, 14.16, 14.18, 14.20, 14.22
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27
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Multiple Equilibria, The Relationship Between Chemical Kinetics and Chemical Equilibrium, What Does the Equilibrium Constant Tell Us?
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14
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612-622
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14.7, 14.8, 14.9
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14.30, 14.32, 14.36, 14.42, 14.44, 14.48, 14.72, 14.82
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10
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28
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Factors That Affect Chemical Equilibrium
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14
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623-630
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14.11, 14.12, 14.13
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14.51, 14.54, 14.56, 14.58, 14.62
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29
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The Acid-Base Properties of Water, pH—A Measure of Acidity
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15
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647-652
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15.2, 15.3, 15.4, 15.5
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15.9, 15.13, 15.16, 15.18, 15.20, 15.22, 15.24, 15.26
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30
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The Common Ion Effect
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16
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698-701
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16.1
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16.4, 16.6
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11
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31
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Buffer Solutions
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16
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701-705
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16.2, 16.3, 16.4
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16.7, 16.10, 16.12, 16.14, 16.18, 16.20
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32
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Solubility Equilibria
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16
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718-725
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16.8, 16.9, 16.10
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16.41, 16.44, 16.46, 16.48, 16.50
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33
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Hybridization of Atomic Orbitals
(sp3, sp2, sp)
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10
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417-423
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10.3
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10.34, 10.38, 10.42, 10.44
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12
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34
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Classes of Organic Compounds, Aliphatic Hydrocarbons
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24
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1004-1008
1011-1115
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24.1, 24.2, 24.3
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24.2, 24.3, 24.7, 24.14, 24.26, 24.28
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35
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Aromatic Hydrocarbons,
Chemistry of the Functional Groups (Functional groups only)
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1017-1018
1020-1025
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24.32, 24.36, 24.38, 24.42, 24.50, 24.58, 24.60
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36
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Proteins, Nucleic Acids
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25
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1045-1056
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25.13, 25.20, 25,23, 25.25
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