General Chemistry Resources

The following resources have been reviewed by the general chemistry instructors and believe they are useful resources to students.  These are external links and therefore we (instructors, Department of Chemistry, or University of Kentucky) cannot be held responsible for additional content which may appear on those sites.  All correlations are to "Chemistry: A Molecular Approach" by Nivaldo Tro, 3rd edition.  If you would like to suggest additional resources, please send to soult@uky.edu.

  • Chapter 1: Matter, Measurement, and Problem Solving

    • 1.1: Atoms and Molecules
    • 1.2: Scientific Approach to Knowledge
    • 1.3: Classification of Matter
    • 1.4: Physical and Chemical Changes and Physical and Chemical Properties
    • 1.5: Energy: A fundamental Part of Physical and Chemical Change
    • 1.6: The Units of Measurement
    • 1.7 The Reliability of Measurement
    • 1.8: Solving Chemical Problems
  • Chapter 2: Atoms and Elements
    • 2.1: Imaging and Moving Individual Atoms
    • 2.2: Early Ideas about the Building Blocks of Matter
    • 2.3: Modern Atomic Thery and the Lwas That Led to It
    • 2.4: The Discovery of the Electron
    • 2.5: The Structure of the Atom
    • 2.6: Subatomic Particles: Protons, Neutrons, and Electrons in Atoms
    • 2.7: Finding Patterns: The Periodic La and the Periodic Table
    • 2.8: Atomic Mass: The Average Mass of an Element's Atoms
    • 2.9: Molar Mass
  • Chapter 3: Molecules, Compounds, and Chemical Equations
    • 3.1: Hydrogen, Oxygen, and Water
    • 3.2: Chemical Bonds
    • 3.3: Representing Compounds: Chemical Formulas and MOlecular MOdels
    • 3.4: An ATomic-Level View of Elements and Compounds
    • 3.5: Ionic Compounds: Formulas and Names
    • 3.6: Molecular Compounds: Formulas and Names
    • 3.7: Summary of Inorganic Nomenclature
    • 3.8: Formula Mass and the Mole Concept for Compounds
    • 3.9: Composition of Compounds
    • 3.10: Determining a Chemical Formula From Experimental Data
    • 3.11: Writing and Balancing Chemical Equations
    • 3.12: Organic Compounds
  • Chapter 4: Chemical Quantities and Aqueous Reactions
    • 4.1: Climate Change and the Combustion of Fossil Fuels
    • 4.2: Reaction Stoichiometry: How Much Carbon Dioxide?
    • 4.3: Limiting Reactant, Theoretical Yield, and Percent Yield
    • 4.4: Solution Concentration and Solution Stoichiometry
    • 4.5: Types of Aqueous Solutions and Solubility
    • 4.6: Precipitation Reactions
    • 4.7: Representing Aqueous Reactions
    • 4.8: Acid-Base and Gas-Evolution Reactions
    • 4.9: Oxidation-Reduction Reactions
  • Chapter 5: Gases
    • 5.1: Breathing: Putting Pressure to Work
    • 5.2: Pressure: The Result of Molecular Collisions
    • 5.3: The Simple Gas Laws: Boyle's Law, Charles's Law, and Avogadro's Law
    • 5.4: The Ideal Gas Law
    • 5.5: Applications of the Ideal Gas Law
    • 5.6: Mixtures of Gases and Partial Pressures
    • 5.7: Gases in Chemical Reactions: Stoichiometry Revisited
    • 5.8: Kinetic Molecular Theory: A Model for Gases
    • 5.9: Mean Free Path, Diffusion, and Effusion of Gases
    • 5.10: Real Gases: The Effects of Size and Intermolecular Forces
  • Chapter 6: Thermochemistry
    • 6.1: Chemical Hand Warmers
    • 6.2: The Nature of Energy
    • 6.3: The First Law of Thermodynamics
    • 6.4: Quantifying Heat and Work
    • 6.5: Measuring ΔE for Chemical Reactions
    • 6.6: Enthalpy
    • 6.7: Constant-Pressure Calorimetry
    • 6.8: Relationships Involving ΔH<sub>rxn</sub>
    • 6.9: Determining Enthalpies of Reaction from Standard Enthalpies of Formation
    • 6.10: Energy Use and the Environment
  • Chapter 7: The Quantum-Mechanical Model of the Atom
    • 7.1: Schrodinger's Cat
    • 7.2 The Nature ofLight
    • 7.3: Atomic Spectroscopy and the Bohr Model
    • 7.4: The Wave Nature of Matter
    • 7.5: Quantum Mechanics and the Atom
    • 7.6: The Shapes of Atomic Orbitals
  • Chapter 8: Periodic Properties of the Elements
    • 8.1: Nerve Signal Transmission
    • 8.2: The Development of the Perioidic Table
    • 8.3: Electron Configurations
    • 8.4: Electron Configurations, Valence Electrons, and the Periodic Table
    • 8.5: The Explanatory Power of the Quantum-Mechanical Model
    • 8.6: Periodic Trends in the Size of Atoms and Effective Nuclear Charge
    • 8.7: Ions
    • 8.8: Electron Affinities and Metallic Character
    • 8.9: Some Examples of Periodic Chemical Behavior
  • Chapter 9: Chemical Bonding I: The Lewis Model
    • 9.1: Bonding Models and AIDS Drugs
    • 9.2: Types of Chemical Bonds
    • 9.3: Representing Valence Electrons with Dots
    • 9.4: Ionic Bonding
    • 9.5: Covalent Bonding
    • 9.6: Electronegativity and Bond Polarity
    • 9.7: Lewis Structures of Molecular Compounds and Polyatomic Ions
    • 9.8: Resonance and Formal Charge
    • 9.9: Exceptions to the Octet Rule
    • 9.10: Bond Energies and Bond Lengths
    • 9.11 : Bonding in Metals
  • Chapter 10: Chemical Bonding II
    • 10.1: Artificial Sweeteners
    • 10.2: VSEPR Theory: The Five Basic Shapes
    • 10.3: VSEPR Theory: The Effect of Lone Pairs
    • 10.4: VSEPR: 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
    • 10.8 Molecular Orbital Theory: Electron Delcocalization
  • Chapter 11: Liquids, Solids, and Intermolecular Forces
    • 11.1: Climbing Geckos and Intermolecular Forces
    • 11.2: Solids, Liquids, and Gases
    • 11.3: Intermolecular Forces
    • 11.4: Intermolecular Forces in Action
    • 11.5: Vaporization and Vapor Pressure
    • 11.6: Sublimation and Fusion
    • 11.7: Heating Curve for Water
    • 11.8: Phase Diagrams
    • 11.9 Water
    • 11.10: Crystalline Solids: Unit Cells and Basic Structures
    • 11.11: Crystalline Solids: Unit Cells and Basic Structures
    • 11.12: Crystalline Solids: The Fundamental Types
    • 11.13: Crystalline Solids: Band Theory
  • Chapter 12: Solutions
    • 12.1 Thirsty Solutions
    • 12.2: Types of Solutions and Solubility
    • 12.3: Energetics of Solution Formation
    • 12.4: Solution Equilibrium and Factors Affecting Solubility
    • 12.5: Expressing Solution Concentration
    • 12.6: Colligative Properites
    • 12.7: Colligative Properties of Strong Electrolyte Solutions
    • 12.8: Colloids
  • Chapter 13: Chemical Kinetics
    • 13.1: Catching Lizards
    • 13.2 The Rate of a Chemical Reaction
    • 13.3: The Rate Law
    • 13.4: The Integrated Rate Law
    • 13.5: The Effect of Temperature on Reaction Rate
    • 13.6: Reaction Mechanisms
    • 13.7: Catalsyis
  • Chapter 14: Chemical Equilibrium
    • 14.1: Fetal Hemoglobin and Equilibrium
    • 14.2: The Concept of Dynamic Equilibrium
    • 14.3: The Equilbrium Constant (K)
    • 14.4: Expressing te Equilbrium Constant in Terms of Pressure
    • 14.5: Heterogeneous Equilibra
    • 14.6: Calculating the Equilbrium Constant from Measured Equilibrium Concentrations
    • 14.7: The Reaction Quotient
    • 14.8: Finding Equilibrium Concentrations
    • 14.9: Le Chatelier's Principle
  • Chapter 15: Acids and Bases
    • 15.1: Heartburn
    • 15.2: The Nature of Acids and Bases
    • 15.3: Definitions of Acids and Bases
    • 15.4: Acid Strength and the Acid Ionization Constant
    • 15.5: Autoionization of Water and pH
    • 15.6: Finding the [H3O+] and pH of Strong and Weak Acid Solutions
    • 15.7: Base Solutions
    • 15.8: The Acid-Base Properties of Ions and Salts
    • 15.9: Polyprotic Acids
    • 15.10: Acid Strength and Molecular Structure
    • 15.11: Lewis Acids and Bases
    • 15.12: Acid Rain