Chemistry 1011
Slot 7 - Instructor: Dr. P. G. Mezey
Office: C4015 Phone: 864-8768
Detailed curriculum available from the website
Chemistry 1011 Curriculum Using the Textbook:
“Principles of Chemistry, A Molecular Approach” by Nivaldo J. TRO
( Prentice Hall, New Jersey 2010 )
Evaluation:
Tutorials - 15%
Class Tests (2) - 20%
Laboratory - 10%
Final Examination - 55%
Chemistry 1011 Curriculum Using "Principles of
Chemistry" by Tro
Curriculum in PDF format
Chemistry 1010 (a prerequisite for this course) covers chapters 1-9 in Tro. You should refresh
yourself on those chapters, particularly if you took Chem 1010 a while ago. Take a look at the
Review page for details.
18.2 Balancing Oxidation-Reduction Equations
(Note: This section is usually covered with a very brief review of oxidation numbers and
oxidizing/reducing agents, as covered in Chemistry 1010, which is found in section 4.9 of the
Tro text).
Chapter 10: Chemical Bonding II: Molecular Shapes, Valence Bond Theory
10.1 Artificial Sweeteners: Fooled by Molecular Shape (Suggested Reading)
10.2 VSEPR Theory: The Five Basic Shapes
10.3 VSEPR Theory: The Effect of Lone Pairs
10.4 VSEPR Theory: Predicting Molecular Geometries
10.5 Molecular Shape and Polarity
10.6 Valence Bond Theory: Orbital Overlap as a Chemical Bond
10.7 Valence Bond Theory: Hybridization of Atomic Orbitals (sp, sp2, sp3 hybridization only)
Chapter 11: Liquids, Solids, and Intermolecular Forces
11.1 Climbing Geckos and Intermolecular Forces (Suggested Reading)
11.2 Solids, Liquids and Gases: A Molecular Comparison
11.3 Intermolecular Forces: The Forces that Hold Condensed Phases Together
11.5 Vaporization and Vapor Pressure (Excluding the Clausius-Clapeyron Equation)
11.6 Sublimation and Fusion
11.7 Heating Curve for Water
11.11 Crystalline Solids: The Fundamental Types
Chapter 12: Solutions
12.1 Thirsty Solutions: Why You Should Not Drink Seawater
12.2 Types of Solutions and Solubility
12.5 Expressing Solution Concentration (Selected Topics)
12.6 Colligative Properties: Vapor Presssure Lowering, Freezing Point Depression, Boiling Point
Elevation and Osmotic Pressure (Selected Topics)
Chapter 13: Chemical Kinetics
13.1 Catching Lizards (Suggested Reading)
13.2 The Rate of a Chemical Reaction
13.3 The Rate Law: The Effect of Concentration on Reaction Rate
13.5 The Effect of Temperature on Reaction Rate
13.6 Reaction Mechanisms (Excluding Mechanisms with a Fast Initial Step)
13.7 Catalysis
Chapter 14: Chemical Equilibrium
14.1 Fetal Hemoglobin and Equilibrium (Suggested Reading)
14.2 The Concept of Dynamic Equilibrium
14.3 The Equilibrium Constant (K)
14.4 Expressing the Equilibrium Constant in Terms of Pressure
14.5 Heterogeneous Equilibria: Reactions Involving Solids and Liquids
14.6 Calculating the Equilibrium Constant from Measured Equilibrium Concentrations
14.7 The Reaction Quotient: Predicting the Direction of Change
14.8 Finding Equilibrium Concentrations
14.9 Le Chatelier’s Principle: How a System at Equilibrium Responds to Disturbances
Chapter 15: Acids and Bases
15.1 Heartburn (Suggested Reading)
15.2 The Nature of Acids and Bases
15.3 Definitions of Acids and Bases
15.4 Acid Strength an the Acid Ionization Constant (Ka)
15.5 Autoionization of Water and pH
15.6 Finding the [H3O+] and pH of Strong and Weak Acid Solutions (Excluding Polyprotic
Acids)
15.7 Base Solutions
15.8 The Acid-Base Properties of Ions and Salts (Excluding Metal Ion Acidity)
15.10 Lewis Acids and Bases
Chapter 16: Aqueous Ionic Equilibrium
16.1 The Danger of Antifreeze (Suggested Reading)
16.2 Buffers: Solutions that Resist pH Change
16.5 Solubility Equilibria and the Solubility Product Constant
16.6 Precipitation
Chapter 18: Electrochemistry
18.1 Pulling the Plug on the Power Grid (Suggested Reading)
18.3 Voltaic (or Galvanic) Cells: Generating Electricity from Spontaneous Chemical Reactions
18.4 Standard Electrode Potentials
18.7 Batteries: Using Chemistry to Generate Electricity
18.8 Electrolysis: Driving Nonspontaneous Chemical Reactions with Electricity
18.9 Corrosion: Undesirable Redox Reactions
Tutor
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