Chem 120 Topics / ChemWiki Links
Chapter: 1) Chemical Foundations; 2) Atoms, Compounds, and Ions; 3) Stoichiometry; 4) Types of Chemical Reactions and Solution Stoichiometry; 5) Gases; 6) Thermochemistry; 7) Atomic Structure and Periodicity; 8) Bonding: General Concepts; 10) Liquids and Solids; 11) Properties of Solutions; 13) Chemical Equilibrium; 14) Acis and Base Equilibria
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1.2: The Scientific Method 1.3: Units of Measurement 1.4: Uncertainty in Measurement 1.5: Significant Figures and Calculations 1.6: Systematically Solving Problems
1.7: Dimensional Analysis: Unit Conversions 1.8: Temperature 1.9: Density 1.10: Classification of Matter |
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Timeline of Chemistry 2.2: The Fundamentals of Chemistry 2.3: Dalton's Atomic Theory 2.4: Early Atomic Experiments 2.5: Modern Atomic Theory 2.6: Molecules and Ions 2.7: The Periodic Table 2.8: Chemical Nomenclature |
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3.2: Average Atomic Masses 3.3: Avogadro's Number 3.4: Molar Mass 3.5: Problem Solving 3.6: Percent Composition 3.7: Empirical and Molecular Formulas 3.8: Writing Chemical Equations 3.9: Balancing Chemical Equations 3.10: Determining the Amount of Reactant and Product 3.11: Limiting and Excess Reagents |
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4.2: Strong and Weak Electrolytes 4.3: Molarity and Dilution 4.4: Chemical Reactions 4.5: Precipitation Reactions 4.6: Types of Equations that Represent Reactions in Solution 4.7: Stoichiometry for Reactions in Solution 4.8: Acid-Base Reactions 4.9: Redox Reactions 4.10: Balancing Redox Reactions |
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5.2: The Empirical Gas Laws 5.3: Ideal Gases 5.4: Stoichiometry and Gases 5.5: Mixtures of Gases
5.6: The Kinetic Molecular Theory 5.7: Molecular Effusion and Diffusion 5.8: Non-ideal Gases 5.9: Properties of Some Non-ideal Gases 5.10: Chemistry in Earth's Atmosphere |
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6.2: Enthalpy and Calorimetry 6.3: Hess's Law 6.4: Standard Enthalpies of Formation and Reaction 6.5: Current Sources of Energy 6.6: Potential Sources of Energy |
7.1: Electromagnetic Radiation 7.2: Matter 7.3: Hydrogen Emission Spectrum 7.4: Bohr's Model of the Hydrogen Atom 7.5: Quantum Theory 7.6: Quantum Numbers 7.7: Shapes and Energies of Hydrogen Orbitals 7.8: The Pauli Exclusion Principle 7.9: Polyelectronic Atoms 7.10: Development of the Periodic Table 7.11: The Aufbau Principle 7.12: Periodic Trends 7.13: The Alkali Metals in Group 1 |
8.1: Classification of Chemical Bonds 8.2: Electronegativity 8.3: Polarity 8.4: Electron Configurations of Ions 8.5: Lattice Energy 8.6: Percent Ionic Character of a Bond 8.7: Bonding in Covalent Molecules 8.8: Bond Energies and Enthalpies 8.9: The Localized Electron Model 8.10: Drawing Lewis Structures 8.11: Octet Rule Exceptions 8.12: Resonance Structures 8.13: VSEPR Theory |
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10.2: Liquids 10.3: Types of Solids 10.4: Metallic Solids 10.5: Covalent-Network Solids 10.6: Molecular Solids 10.7: Ionic Solids 10.8: Vapor Pressure and Phase Changes 10.9: Phase Diagrams |
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11.1: Molality, Mass Percent, and Mole Fraction 11.2: Thermodynamics of Solubility 11.3: Effects of Structure, Temperature, and Pressure on Solubility 11.4: The Vapor Pressures of Solutions 11.5: Boiling-Point Elevation and Freezing-Point Depression 11.6: Osmotic Pressure 11.7: Colligative Properties of Electrolyte Solutions 11.8: Colloids |
13.1: Introduction to Equilibrium 13.2: The Equilibrium Constant and Expression 13.3: Pressure Equilibrium Expressions 13.4: Heterogeneous Equilibria 13.5: Utilizing the Equilibrium Constant 13.6: Solving Equilibrium Expressions
13.7: Effect of Concentration, Temperature, and Pressure Changes on Equilibrium |
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14.1: Models for Acids and Bases 14.2: Effect of Molecular Structure on Acid Strength 14.3: pH and pOH 14.4: Strong Acids 14.5: Weak Acids 14.6: Bases 14.7: Diprotic and Polyprotic Acids 14.8: Acidic and Basic Salt Solutions 14.9: Relationship Between Structure and Acid-Base Properties 14.10: Acidic and Basic Oxides 14.11: Lewis Acids and Bases 14.12: Solving Acid-Base Problems |