Main Textbook Table of Contents

• 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

• 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

• 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)

• 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

• 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

• 6.1 Electromagnetic Energy

  • Electromagnetic Energy
  • Waves
  • Standing Waves (Stationary Waves)
  • Blackbody Radiation and the Ultraviolet Catastrophe
  • The Photoelectric Effect
  • Line Spectra
  • Summary
• 6.2 The Bohr Model
• 6.3 Development of Quantum Theory

  • Development of Quantum Theory Intro
  • Behaviour in the Microscopic World
  • Quantum-Mechanical Model of an Atom
  • Understanding Quantum Theory of Electrons in Atoms
  • Pauli Exclusion Principle
• 6.4 Electronic Configurations

  • Intro
  • Orbital Energies and Atomic Structure
  • Electron configurations of Atoms
  • Electron Configurations of Ions
• 6.5 Periodic Properties

  • Introduction to Periodic Properties
  • Effective Nuclear Charge (Z_eff)
  • Variation in Covalent Radius
  • Variation in Ionic Radius
  • Variation in Ionization Energies
  • Successive Ionization Energies
  • Variations in Electron Affinities

• 7A.1 Ionic and Covalent bonding

  • Electronegativity
  • Electronegativity and bond type
  • Ionic Bonding
  • Covalent Bonding
  • Ionic and Covalent Bond Strength and Bond length
• 7A.2 Lewis Structures

  • Lewis Symbols and Structures
  • Exceptions to the Octet Rule
• 7A.3 “Curly Arrow” Notation

  • Curved/Curly Arrows introduction (arrow pushing)
• 7A.4 Resonance Structures

  • What is a Resonance Structure?
  • Equivalent and Non-Equivalent Resonance Structures
• 7A.5 Introduction to Reaction mechanisms

  • Introduction to Reaction mechanisms

• 7B.1 VSEPR

  • VSEPR Theory
  • Electron-Pair Geometry
  • Electron-Pair Geometry VS. Molecular Shape
  • Predicting Electron-Pair Geometry and Molecular Shape
  • Molecular Shape for Multicentered Molecules
• 7B.2 Isomers

  • Isomers
• 7B.3 Molecular Polarity

  • Electronegativity
  • Electronegativity and Bond Dipoles
  • Molecular Polarity and Dipole moments

• 8.1 Valence Bond Theory

  • Valence Bond Theory
• 8.2 Hybrid Atomic Orbitals

  • Hybrid Atomic Orbitals
  • sp Hybridization
  • sp² Hybridization
  • sp³ Hybridization
  • sp³d and sp³d² Hybridization
  • Assignment of Hybrid Orbitals to Central Atoms
  • Hybrid Atomic Orbitals Summary
• 8.3 Multiple Bonds

  • Multiple Bonds
  • Multiple Bonds Summary and Practice Questions

• 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

• 10.1 Intermolecular forces (IMFs)

  • Overview of Intermolecular forces (Van der Waals forces)
  • Induced dipole-induced dipole (London Dispersion forces)
  • Dipole-Dipole Interactions
  • Hydrogen bonding interactions
  • Summary of IMFs
• 10.2 Properties of Liquids (interactions of IMFs in the liquid state)

  • Overview

• 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

• 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

• 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

• 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

• 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

• 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

The following website is a great resource for learning the basics of naming organic molecules.