Description of Lecture
Chemistry Lecture 2 hours per week, and recitation
Focus of
Lecture Introduction to Chemistry - Chemical symbols, formulas, and
equations; the states of matter; electronic structure and bonding
Text: Chemistry
McMurry and Fay, Prentice Hall Publisher; Chemical
Principles
Zumdahl, third edition, Houghton Mifflin Co.; General Chemistry - An Integrated
Approach.
Hill and Petrucci. Second Edition. Prentice Hall Publishers or to be decided.
Topics of Lecture
· Basic Chemical Concepts
· Atoms, Molecules and Ions
· Stoichiometry: Chemical Formulas and Equations
· Aqueous Reactions and Solution Stoichiometry
· Energy Relations in Chemistry: Thermochemistry
· Electronic Structure of Atoms
· Periodic Properties of the Elements
· Basic Concepts of Chemical Bonding
· Molecular Geometry and Bonding Theories
· Gases
· Intermolecular Forces
· State of matter
· Physical properties of solutions
· Kinetics
· Equilibria
· Thermodynamics
· Electrochemistry
· Organic chemistry
Contents of Lecture
Hypotheses, Theories and Facts
Dimensional Analysis
Introduction to Matter
Elements and Compounds
The Atomic Theory of Matter
The Discovery of Atomic Structure
Modern View of Atomic Structure
The Periodic Table
Molecules and Ions
Naming of Inorganic Compounds
Chemical Equations
Patterns of Chemical Reactivity
Atomic and Molecular Weights
The Mole
Empirical Formulas from Analyses
Quantitative Information from Balanced Equations
Limiting Reactants
Solution Composition
Solution Stoichiometry
The Nature of Energy
Heat and Enthalpy Changes
Calorimetry
Hess's Law
Enthalpies of Formation
Foods and Fuels
The Wave Nature of Light
Quantum Effects and Photons
Bohr's Model of the Hydrogen Atom
The Dual Nature of the Electron
Quantum Mechanics and Atomic Orbitals
Representations of Orbitals
Orbitals in Many-electron Atoms
Electron Configurations
Electron Configurations and the Periodic Table
Development of the Periodic Table
Electron Shells in Atoms
Sizes of Atoms
Ionization Energy
Electronic Affinities
Metals, Nonmetals and Metalloids
Group Trends: the Active Metals
Group Trends: Selected Nonmetals
Lewis Symbols and the Octet Rule
Ionic Bonding
Sizes of Ions
Covalent Bonding
Bond Polarity
Drawing Lewis Structures
Resonance Structures
Exceptions to the Octet Rule
Strengths of Covalent Bonds
Oxidation Numbers
Molecular Geometries
The VSEPR Model
Polarity of Molecules
Covalent Bonding and Orbital Overlap
Hybrid Orbitals
Multiple Bonds
Characteristics of Gases
Pressure
The Gas Law
The Ideal Gas Equation
Molar Mass and Gas Densities
Gas Mixtures and Partial Pressures
Volumes of Gases in Chemical Reactions
Kinetic-Molecular Theory
Molecular Effusion and Diffusion
Deviation from Ideal Behavior
The Kinetic-molecular Description of Liquids and Solids
Intermolecular Forces
Properties of Liquids: Viscosity and Surface Tension
Changes of State
Vapor Pressure
Phase Diagrams
Bonding in Solids
Phase changes involving solids
van der Waals Forces
Hydrogen bonds
Network covalent solids
Ionic bonds
Structures of Solids
Energetics of solution formation
Equilibrium in solution formation
Solubility of gases
Vapor pressure of solutions
Freezing point depression and boiling
point elevation
Osmotic pressure
Solutions of electrolytes
Colloids
Measuring reaction rates
The rate law of a reaction
First-order reactions
Reactions of other orders
Theories of chemical kinetics
Effect of temperature on rate
Reaction mechanisms
Catalysis
Enzyme catalysis
Modifying equilibrium constant expressions
Le Chatelier's Principle
Equilibrium calculations
The pH scale
Equilibrium solutions of weak acids and
bases
Polyprotic acids
Ions as acids and bases
The common-ion effect
Buffer solutions
Acid-base indicators
Neutralization reactions and titration curves
Lewis acids and bases
Common-ion effect in equilibria
Occurance of precipitation
Effect of pH on solubility
Equilibria of complex ions
Qualitative inorganic analysis
Entropy: disorder and spontaneity
Free energy and free energy change
Standard free energy change DG0
Free energy change and equilibrium
Dependence of DG0 and
Keq on temperature
Voltaic cells
Standard electrode potentials
Electrode potentials
Effect of concentrations on cell voltage
Batteries
Corrosion
Predicting electrolysis reactions
Quantitative electrolysis
Applications of electrolysis
Organic
chemistry
The nature of organic molecules
Writing organic structures
Naming molecules
The shapes of organic molecules
Functional groups
Saturated and unsaturated hydrocarbons
The reactions of organic molecules
Polymers
Biochemistry
Proteins
Amino Acids and peptides
Nucleic acids
Lipids
Sample Lecture Calendar
|
Date |
Text Chapter |
Topic |
Text pp |
|
|
1. Chemistry: Matter and Measurement 2. Atoms, Molecules and Ions |
1.2 Getting Started: Some Key Terms 2.1 Laws of Chemical Combination |
3-9 36-38 |
|
|
|
2.2 John Dalton and the Atomic Theory of Matter 2.3 The Divisible Atom 2.4 Atomic Masses |
38-40 40-42 42-44 |
|
|
|
2.5 The Periodic Table Elements Organized 2.6 Molecules and Molecular Compounds |
45-48 48-52 |
|
|
|
2.7 Ions and Ionic Compounds 2.8 Acids, Bases, and Salts |
52-58 58-61 |
|
|
|
2.9 Alkanes: Saturated Hydrocarbons 2.10 Types of Organic Compounds |
61-66 67-71 |
|
|
3. Stoichiometry: Chemical Calculations |
3.1 Molecular Masses and Formula Masses 3.2 The Mole and Avocadro's Number 3.3 More on the Mole |
82-84 84-86 86-90 |
|
|
|
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 |
90-93 94-97 97-100 |
|
|
|
3.7 Writing and Balancing Chemical Equations 3.8 Stoichiometric Equivalence and Reaction Stoichiometry |
100-105 105-109 |
|
|
|
3.9 Limiting Reactants 3.10 Yields of Chemical Reactions 3.11 Solutions and Solution Stoichiometry |
110-112 112-115 115-123 |
|
|
4. Chemical Reactions in Aqueous Solutions |
4.1 Some Electrical Properties of Aqueous Solutions 4.2 Reactions of Acids and Bases |
133-137 137-147 |
|
|
|
4.3 Reactions that Form Precipitates 4.4 Oxidation-Reduction |
148-152 153-159 |
|
|
|
4.5 Oxidizing and Reducing Agents 4.6 Some Practical Applications of Oxidation and Reduction |
160-163 163-169 |
|
|
5. Gases |
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 |
178 179 179-184 185-187 |
|
|
|
5.5 Charles' Law: The Temperature-Volume Relationship 5.6 Avogadro's Law: The Mole-Volume Relationship 5.7 The Combined Gas Law |
187-191 191-192 193-194 |
|
|
|
5.8 The Ideal Gas Law 5.9 Gases in Reaction Stoichiometry |
195-200 201-204 |
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5.10 Mixtures of Gases: Dalton's Law of Partial Pressures 5.11 The Kinetic-Molecular Theory: Some Quantitative Aspects 5.12 Real Gases |
204-209 210-215 216-217 |
|
|
6. Thermochemistry |
6.1 Energy 6.2 Thermochemistry: Some Basic Terms |
227-229 229-233 |
|
|
|
6.3 Internal Energy (U), State Functions, and the First Law of
Thermodynamics HD6.4 Heats of Reaction
and Enthalpy Change, |
233-236 236-244 |
|
|
|
6.5 Calorimetry: Measuring Quantities of Heat |
244-253 |
|
|
|
6.6 Hess' 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 |
|
|
7. Atomic Structure |
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 |
|
|
|
7.4 Positive Ions and Mass Spectrometry 7.5 The Wave Nature of Light |
283-284 284-290 |
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|
7.6 Photons: Energy by the Quantum 7.7 Bohr's Hydrogen Atom: A Planetary Model |
290-295 295-299 |
|
|
|
7.8 Wave Mechanics: Matter as Waves 7.9 Quantum Numbers and Atomic Orbitals |
299-302 302-309 |
|
|
8. Electron Configurations, Atomic Properties and the
Periodic Table |
8.1 Multielectron Atoms 8.2 An Introduction to Electron Configurations 8.3 The Rules for Electron Configurations |
317-318 318-319 319-321 |
|
|
|
8.4 Electron Configurations: The Aufbau Principle 8.5 Electron Configurations: Periodic Relationships |
321-325 325-331 |
|
|
|
8.6 Magnetic Properties: Paired and Unpaired Electrons 8.7 Periodic Atomic Properties of the Elements |
332-333 334-343 |
|
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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 |
|
|
9. Chemical Bonds |
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 |
|
|
|
9.4 Using Lewis Symbols to Represent Ionic Bonding 9.5 Energy Changes in Ionic Compound Formation |
363-365 365-368 |
|
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9.6 Lewis Structures of Some Simple Molecules 9.7 Polar Covalent Bonds and Electronegativity |
368-372 372-375 |
|
|
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9.8 Strategies for Writing Lewis Structures |
375-385 |
|
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9.9 Molecules that Don't Follow the Octet Rule 9.10 Bond Lengths and Bond Energies |
385-390 390-395 |
|
|
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9.11 Alkenes and Alkynes 9.12 Polymers |
395-397 397-401 |
|
|
10. Bonding Theory and Molecular Structure |
10.1 Valence-Shell Electron-Pair Repulsion (VSEPR) Method |
409-419 |
|
|
|
10.2 Polar Molecules and Dipole Moments 10.3 Atomic Orbital Overlap |
420-425 425-427 |
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10.4 Hybridization of Atomic Orbitals |
427-436 |
|
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10.5 Hybrid Orbitals and Multiple Covalent Bonds |
436-443 |
|
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10.6 Characteristics of Molecular Orbitals 10.7 Homonuclear Diatomic Molecules of the Second-Period Elements 10.8 Bonding in Benzene 10.9 Aromatic Compounds |
444-445 445-448 448-449 450-451 |