INTRODUCTORY CHEMISTRY FOR WATER QUALITY TECHNOLOGY I. Chemistry 11 and Principles of Mathematics 12 is strongly recommended.

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1 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 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

3 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 Octahedral Electronic Geometry: AB 6,AB 5 U, and AB 4 U Compounds Containing Double Bonds 8-14 Compounds Containing Triple Bonds 8-15 A Summary of Electronic and Molecular Geometries

4 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 Determination of Molecular Weights and Molecular Formulas of Gaseous Substances Dalton s Law of Partial Pressures Mass-Volume Relationships in Reactions Involving Gases The Kinetic-Molecular Theory Diffusion and Effusion of Gases 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 Melting Point Heat Transfer Involving Solids Sublimation and the Vapor Pressure of Solids Phase Diagrams Amorphous Solids and Crystalline Solids Structures of Crystals Bonding in Solids Band Theory of Metals

5 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 Fractional Distillation Boiling Point Elevation Freezing Point Depression Determination of Molecular Weights by Freezing Point Depression or Boiling Point Elevation Colligative Properties and Dissociation of Electrolytes Osmotic Pressure The Tyndall Effect The Adsorption Phenomenon Hydrophilic and Hydrophobic Colloids