This subset of the textbook is tailored for the content of CHEM 203. For the extended textbook content, see here.

Background: Chemistry Review (Chapters 1-4 & 9)

Chapter 1: Chemistry of the Lab

• Introduction: Chemistry of the lab

  • The Scientific Method
  • Domains of Chemistry
• Matter

  • Types of Matter
  • Mass versus Weight
  • Law of Conservation of Mass
  • Classifying Matter
• Properties of Matter

  • Physical Change
  • Chemical Change
  • Extensive & Intensive properties
• Measurements

  • Measurements Overview
  • SI Units
  • Derived SI Units
• Measurement Uncertainty and Significant Figures

  • Uncertainty in Measurements
  • Accuracy and Precision

    • Accuracy and Precision
    • Outliers in Data Sets
  • Significant Figures

    • Significant Figures
    • Significant Figures: Rules for Rounding
    • Significant Figures in Adding or Subtracting
    • Significant Figures in Multiplication and Division
    • Significant Figures in Logarithms
  • Sources of Error in the Lab
• Scientific Analysis in Lab Reports

  • Claim-Evidence-Reasoning Statements
• Safety in the Laboratory

  • Where to find safety information
  • WHMIS (Workplace Hazardous Materials Information System)
  • Best Practices in the Laboratory
  • Review Videos

Chapter 2: Periodic Table, Atoms & Molecules

• The Periodic Table
• Chemical Symbols
• Anatomy of an Atom

  • Atomic Structure
  • History of the atom
  • Isotopes
  • Atomic Mass (AMU)
• Atom versus Compound

  • Difference between an atom and a compound/molecule
  • Polyatomic ions
  • Naming inorganic compounds
  • Ionic compounds
  • Covalent compounds
  • Chemical formula
• The Mole

  • Formula Mass
  • The Mole

Chapter 3: Solutions

• Solutions and Dilutions (Interactive tutorial)
• Other units of concentration

  • Mass percent (%w/w)
  • Volume percent (%v/v)
  • Mass-Volume percent (%w/v)
  • PPM (parts per million) & PPB (parts per billion)

Chapter 4: Chemical Reactions

• Balancing Equations

  • How to Balance Chemical Equations
  • Additional Information about equations
  • Equations for Ionic Reactions
  • Balancing Redox Equations (coming soon)
  • Summary & more Practice
• Stoichiometric ratio / stoichiometric factor
• Reaction Yields

Chapter 9: Gases

• 9.1 Gas Pressure

  • Gas Pressure
• 9.2 The Ideal Gas Law

  • The Ideal Gas Law Intro
  • Pressure and Temperature: Amontons’s Law
  • Volume and Temperature: Charles’s Law
  • Volume and Pressure: Boyle’s Law
  • Moles of Gas and Volume: Avogadro’s Law
  • The Ideal Gas Law
  • Standard Conditions of Temperature and Pressure
  • The Ideal Gas Law Summary
• 9.3 Stoichiometry of Gaseous Substances, Mixtures, and Reactions

  • Stoichiometry of Gaseous Substances, Mixtures, and Reactions
  • Gas Density and Molar Mass
  • The Pressure of a Mixture of Gases: Dalton’s Law
  • Collection of Gases over Water
  • Chemical Stoichiometry and Gases
  • Avogadro’s Law Revisited
  • Summary of Stoichiometry of Gaseous Substances, Mixtures, and Reactions
• 9.4 Effusion and Diffusion of Gases

  • Effusion and Diffusion of Gases
  • Effusion and Diffusion of Gases Summary
• 9.5 The Kinetic-Molecular Theory

  • The Kinetic-Molecular Theory
  • The Kinetic-Molecular Theory Explains the Behaviour of Gases, Part I
  • Molecular Speeds and Kinetic Energy
  • The Kinetic-Molecular Theory Explains the Behaviour of Gases, Part II
  • Kinetic-Molecular Theory Summary
• 9.6 Non-Ideal Gas Behaviour

  • Non-Ideal Gas Behaviour

How Far (Equilibrium)?

Chapter 13: Chemical Equilibrium

• 13.1 Chemical Equilibria

  • Chemical Equilibria
• 13.2 Equilibrium Constants

  • Equilibrium Constants
  • Homogeneous Equilibria
  • Heterogeneous Equilibria
  • Coupled Equilibria
  • Summary
• 13.3 Shifting Equilibria: Le Chatelier’s Principle

  • Shifting Equilibria: Le Chatelier’s Principle
  • Effect of a change in Concentration
  • Effect of a Change in Temperature
  • Effect of a Catalyst
  • An Interesting Case Study
  • Summary
• 13.4 Equilibrium Calculations

  • Equilibrium Calculations
  • Calculation of an Equilibrium Constant
  • Calculation of a Missing Equilibrium Concentration
  • Calculation of Equilibrium Concentrations from Initial Concentrations
  • Calculation of equilibrium concentrations using an Algebra-Simplifying Assumption
  • Summary

How Fast (Kinetics)?

Chapter 12: Chemical Kinetics

• 12.1 Chemical Reaction Rates

  • Kinetics Introduction
  • Expressing Reaction Rates
  • Determining Rates of Reaction
  • Relative Rates of Reaction
  • Summary & Problems
• 12.2 Factors Affecting Reaction Rates

  • Chemical Nature of the Reactants
  • Physical States of the Reactants
  • Temperature of the Reactants
  • Concentrations of the Reactants
  • Presence of a Catalyst
  • Summary & Problems
• 12.3 Rate Laws

  • Rate Laws
  • Orders of Reaction
  • Method of Initial Rates
  • Reaction Order and Rate Constant Units
  • Summary & Problems
• 12.4 Integrated Rate Laws

  • Integrated Rate Laws
    • First Order Reactions
    • Second Order Reactions
    • Zero Order Reactions
  • Half-Life of a Reaction
    • First Order Reactions
    • Second Order Reactions
    • Zero Order Reactions
  • Summary and Problems
• 12.5 Collision Theory

  • Collision Theory
  • Activation Energy & Arrhenius Equation
• 12.6 Reaction Mechanisms

  • Reaction Mechanisms
  • Unimolecular Elementary Reactions
  • Bimolecular Elementary Reactions
  • Termolecular Elementary Reactions
  • Relating Reaction Mechanisms to Rate Laws
  • Summary and Practice Problems
• 12.7 Catalysis

  • Catalysis
  • Homogeneous Catalysts
  • Heterogeneous Catalysts
  • Summary and Practice Problems

How much Energy (Thermodynamics)?

Chapter 5: Thermochemistry

• 5.1 Energy Basics

  • Energy Basics
  • Energy
  • Thermal Energy Temperature and Heat
  • Energy Basics Summary
• 5.2 Calorimetry
• 5.3 Enthalpy

  • Enthalpy
  • Standard Enthalpy of Combustion
  • Standard Enthalpy of Formation
  • Hess’s Law
  • Summary of Enthalpy

Chapter 16: Thermodynamics

• 16.1 Spontaneity

  • Spontaneity
  • Dispersal of Matter and Energy
  • Summary
• 16.2 Entropy

  • Entropy
  • Entropy and Microstates
  • Predicting the Sign of ΔS
  • Summary
• 16.3 The Second and Third Laws of Thermodynamics

  • The Second and Third Laws of Thermodynamics
  • The Second Law of Thermodynamics
  • The Third Law of Thermodynamics
  • Summary
• 16.4 Free Energy

  • Free Energy
  • What’s “Free” about ΔG?
  • Calculating Free Energy Change
  • Free Energy Changes for Coupled Reactions
  • Temperature Dependence of Spontaneity
  • Free Energy and Equilibrium
  • Summary

Chemical Reactions

Chapter 14: Acid-Base Equilibria

• 14.1 Brønsted-Lowry Acids and Bases

  • Brønsted-Lowry Acids and Bases
  • Ion Concentrations in Pure Water
  • The Inverse Relationship between H₃O⁺ and OH^–
  • Representing the Acid-Base Behaviour of an Amphoteric Substance
  • Summary
• 14.2 pH and pOH

  • pH and pOH
  • Summary
• 14.3 Relative Strengths of Acids and Bases

  • Relative Strengths of Acids and Bases
  • Acid and Base Ionization Constants
  • Relative Strengths of Conjugate Acid-Base Pairs
  • Acid-Base Equilibrium Calculations
  • Effect of Molecular Structure on Acid-Base Strength:
    • Binary Acids and Bases
    • Ternary Acids and Bases
  • Summary
• 14.4 Hydrolysis of Salts

  • Hydrolysis of Salts
  • Salts with Acidic Ions
  • Salts with Basic Ions
  • Salts with Acidic and Basic Ions
  • The Ionization of Hydrated Metal Ions
  • Summary
• 14.5 Polyprotic Acids

  • Polyprotic Acids
• 14.6 Buffers

  • Buffers
  • How Buffers Work
  • Buffer Capacity
  • Selection of Suitable Buffer Mixtures
  • The Henderson-Hasselbalch Equation
  • Summary
• 14.7 Acid-Base Titrations

  • Acid-Base Titrations
  • Acid-Base Indicators

Chapter 15: Other Equilibria

• 15.1 Precipitation and Dissolution

  • Precipitation and Dissolution
  • The Solubility Product
  • K_sp and Solubility
  • Predicting Precipitation
  • Common Ion Effect
  • Summary
• 15.2 Lewis Acids and Bases

  • Lewis Acids and Bases
• 15.3 Coupled Equilibria

  • Coupled Equilibria
  • Increased Solubility in Acidic Solutions
  • Multiple Equilibria
  • Summary & Problems

Chapter 17: Electrochemistry

• 17.1 Review of Redox Chemistry

  • Review of Redox Chemistry
  • Oxidation Numbers
  • Balancing Redox Equations
  • Summary
• 17.2 Galvanic Cell

  • Galvanic Cell
  • Cell Notation
  • Summary
• 17.3 Electrode and Cell Potentials

  • Electrode and Cell Potentials
  • Interpreting Electrode and Cell Potentials
  • Summary
• 17.4 Potential, Free Energy, and Equilibrium

  • Potential, Free Energy, and Equilibrium
  • E° and ΔG°
  • E° and K
  • Potentials at Nonstandard Conditions: The Nernst Equation
  • Summary
• 17.5 Batteries and Fuel Cells

  • Batteries and Fuel Cells
  • Single-Use Batteries
  • Rechargeable (Secondary) Batteries
  • Fuel Cells
  • Summary
• 17.6 Corrosion

  • Corrosion
• 17.7 Electrolysis

  • Electrolysis
  • The Electrolysis of Molten Sodium Chloride
  • The Electrolysis of Water
  • The Electrolysis of Aqueous Sodium Chloride
  • Electroplating
  • Quantitative Aspects of Electrolysis
  • Summary

  

Appendices

1. The Periodic Table
2. Essential Mathematics
3. Units and Conversion Factors
4. Fundamental Physical Constants
5. Water Properties
6. Composition of Commercial Acids and Bases
7. Standard Thermodynamic Properties for Selected Substances
8. Ionization Constants of Weak Acids
9. Ionization Constants of Weak Bases
10. Solubility Products
11. Formation Constants for Complex Ions
12. Standard Electrode (Half-Cell) Potentials
13. Half-Lives for Several Radioactive Isotopes