CHEMISTRY 115 INTRODUCTORY CHEMISTRY FOR WATER QUALITY TECHNOLOGY I Prerequisites: Format: Chemistry 11 and Principles of Mathematics 12 is strongly recommended. 4 hours lecture + 3 hours lab per week Required Texts: 1. Chemistry, 9 th ed., Whitten, Davis, Peck and Stanley (2010) 3. Chemistry Lab Manual, CHEM 115 (2010) Evaluation: Term Tests (5) 40% Laboratory Work 20% Final Examination 40% Final Grade 100% It is the Department's policy that a student must obtain a passing grade (at least 50%) in both the lecture and the laboratory component of the course considered separately. Course Outline: 1. The Foundations of Chemistry (Chapter 1) 1-1 Matter and Energy 1-2 Chemistry a Molecular View of Matter 1-3 States of Matter 1-4 Chemical and Physical Properties 1-5 Chemical and Physical Changes 1-6 Mixtures, Substances, Compounds, and Elements 1-7 Measurements in Chemistry 1-8 Units of Measurement 1-9 Use of Numbers 1-10 The Unit Factor Method (Dimensional Analysis) 1-11 Percentage 1-12 Density and Specific Gravity 1-13 Heat and Temperature 1-14 Heat Transfer and the Measurement of Heat
2. Chemical Formulas and Composition Stoichiometry (Chapter 2) 2-1 Chemical Formulas 2-2 Ions and Ionic Compounds 2-3 Names and Formulas of Some Ionic Compounds 2-4 Atomic Weights 2-5 The Mole 2-6 Formula Weights, Molecular Weights, and Moles 2-7 Percent Composition and Formulas of Compounds 2-8 Derivation of Formulas from Elemental Composition 2-9 Determination of Molecular Formulas 2-10 Some Other Interpretations of Chemical Formulas 2-11 Purity of Samples 3. Chemical Equations and Reaction Stoichiometry (Chapter 3) 3-1 Chemical Equations 3-2 Calculations Based on Chemical Equations 3-3 The Limiting Reactant Concept 3-4 Percent Yields from Chemical Reactions 3-5 Sequential Reactions 3-6 Concentrations of Solutions 3-7 Dilution of Solutions 3-8 Using Solutions in Chemical Reactions 4. The Structure of Atoms (Chapter 4) 4-1 Fundamental Particles 4-2 The Discovery of Electrons 4-3 Canal Rays and Protons 4-4 Rutherford and the Nuclear Atom 4-5 Atomic Number 4-6 Neutrons 4-7 Mass Number and Isotopes 4-8 Mass Spectrometry and Isotopic Abundance 4-9 The Atomic Weight Scale and Atomic Weights 4-10 Electromagnetic Radiation 4-11 The Photoelectric Effect 4-12 Atomic Spectra and the Bohr Atom 4-13 The Wave Nature of the Electron 4-14 The Quantum Mechanical Picture of the Atom 4-15 Quantum Numbers 4-16 Atomic Orbitals 4-17 Electron Configurations 4-18 Paramagnetism and Diamagnetism 4-19 The Periodic Table and Electron Configurations
5. Chemical Periodictity (Chapter 5) 5-1 More About the Periodic Table 5-2 Atomic Radii 5-3 Ionization Energy 5-4 Electron Affinity 5-5 Ionic Radii 5-6 Electronegativity 6. Some Types of Chemical Reactions (Chapter 6) 6-1 Aqueous Solutions An Introduction 6-2 Reactions in Aqueous Solutions 6-3 Naming Some Binary Compounds 6-4 Naming Ternary Acids and Their Salts 7. Chemical Bonding (Chapter 7) 7-1 Lewis Dot Formulas of Atoms 7-2 Formation of Ionic Compounds 7-3 Formation of Covalent Bonds 7-4 Bond Lengths and Bond Energies 7-5 Lewis Formulas for Molecules and Polyatomic Ions 7-6 Writing Lewis Formulas: The Octet Rule 7-7 Formal Charges 7-8 Writing Lewis Formulas: Limitations of the Octet Rule 7-9 Resonance 7-10 Polar and Nonpolar Covalent Bonds 7-11 Dipole Moments 7-12 The Continuous Range of Bonding Types 8. Molecular Structure and Covalent Bonding Theories (Chapter 8) 8-1 A Preview of the Chapter 8-2 Valence Shell Electron Pair Repulsion Theory 8-3 Polar Molecules: The Influence of Molecular Geometry 8-4 Valence Bond (VB)Theory 8-5 Linear Electronic Geometry: AB 2 Species (No Lone Pairs of Electrons on A) 8-6 Trigonal Planar Electronic Geometry: AB 3 Species (No Lone Pairs of Electrons on A) 8-7 Tetrahedral Electronic Geometry: AB 4 Species (No Lone Pairs of Electrons on A) 8-8 Tetrahedral Electronic Geometry: AB 3 U Species (One Lone Pair of Electrons on A) 8-9 Tetrahedral Electronic Geometry: AB 2 U 2 Species (Two Lone Pairs of Electrons on A) 8-10 Tetrahedral Electronic Geometry: ABU 3 Species (Three Lone Pairs of Electrons on A) 8-11 Trigonal Bipyramidal Electronic Geometry: AB 5, AB 4 U, AB 3 U 2, and AB 2 U 3 8-12 Octahedral Electronic Geometry: AB 6,AB 5 U, and AB 4 U 2 8-13 Compounds Containing Double Bonds 8-14 Compounds Containing Triple Bonds 8-15 A Summary of Electronic and Molecular Geometries
12. Gases and the Kinetic-Molecular Theory (Chapter 12) 12-1 Comparison of Solids, Liquids, and Gases 12-2 Composition of the Atmosphere and Some Common Properties of Gases 12-3 Pressure 12-4 Boyle s Law: The Pressure-Volume Relationship 12-5 Charle slaw: The Volume-Temperature Relationship; The Absolute Temperature Scale 12-6 Standard Temperature and Pressure 12-7 The Combined Gas Law Equation 12-8 Avogadro s Law and the Standard Molar Volume 12-9 Summary of the Gas Laws: The Ideal Gas Equation 12-10 Determination of Molecular Weights and Molecular Formulas of Gaseous Substances 12-11 Dalton s Law of Partial Pressures 12-12 Mass-Volume Relationships in Reactions Involving Gases 12-13 The Kinetic-Molecular Theory 12-14 Diffusion and Effusion of Gases 12-15 Deviations from Ideal Gas Behaviour 13. Liquids and Solids (Chapter 13) 13-1 Kinetic Molecular Description of Liquids and Solids 13-2 Intermolecular Attractions and Phase Changes 13-3 Viscosity 13-4 Surface Tension 13-5 Capillary Action 13-6 Evaporation 13-7 Vapor Pressure 13-8 Boiling Points and Distillation 13-9 Heat Transfer Involving Liquids 13-10 Melting Point 13-11 Heat Transfer Involving Solids 13-12 Sublimation and the Vapor Pressure of Solids 13-13 Phase Diagrams 13-14 Amorphous Solids and Crystalline Solids 13-15 Structures of Crystals 13-16 Bonding in Solids 13-17 Band Theory of Metals
14. Solutions (Chapter 14) 14-1 Spontaneity of the Dissolution Process 14-2 Dissolution of Solids in Solution 14-3 Dissolution of Liquids in Liquids (Miscibility) 14-4 Dissolution of Gases in Liquids 14-5 Rates of Dissolution and Saturation 14-6 Effect of Temperature on Solubility 14-7 Effect of Pressure on Solubility 14-8 Molality and Mole Fraction 14-9 Lowering of Vapor Pressure and Raoult s Law 14-10 Fractional Distillation 14-11 Boiling Point Elevation 14-12 Freezing Point Depression 14-13 Determination of Molecular Weights by Freezing Point Depression or Boiling Point Elevation 14-14 Colligative Properties and Dissociation of Electrolytes 14-15 Osmotic Pressure 14-16 The Tyndall Effect 14-17 The Adsorption Phenomenon 14-18 Hydrophilic and Hydrophobic Colloids