Textbook: Zumdahl, Steven and Susan, and DeCoste, Don. World of Chemisty Boston: Houghton Mifflin, 2002

Unit A: Matter (Chapter 1 & 2)
  • What is chemistry
  • Matter as particles
  • Elements, compounds, atoms, and molecules
  • Physical properties – physical changes
  • Chemical properties – chemical changes
  • Mixtures and pure substances
  • Separation of mixtures
Unit B: Measurement (Chapter 5)
  • Scientific notation
  • Units
  • Length, volume, and mass
  • Uncertainty and significant figures
  • Dimensional analysis
  • Density
Unit C: The Atom (Chapter 3)
  • Representing the elements
  • Lavoisier – Law of conservationof mass
  • Proust and Gay-Lussac – Law of constant composition
  • Dalton and atomic theory
  • Using formulas to represent compounds
  • Thomson – electrons
  • Rutherford - nucleus
  • Isotopes
  • The periodic table
  • Ions
Init D: Modern atomic theory (Chapter 11)
  • Energy and light
  • Atomic emission spectra
  • The Bohr atom
  • Schrodinger – the wave model of the atom
  • Electron configuration
  • Periodicity
Unit E: Nomenclature (Chapter 4)
  • Ionic compounds
  • Molecular compounds
  • Acids
Unit F: Chemical composition (Chapter 6)
  • Counting by weighing
  • Atomic masses
  • The mole
  • Molar mass
  • Percent composition
  • Empirical and molecular formulas
Unit G: Chemical Reactions (Chapter 7 & 8)
  • Evidence
  • Equations
  • Balancing
  • Precipitate reactions
  • Acid/base reactions
  • Oxidation/reduction reactions
  • Synthesis
  • Decomposition
  • Combustion
Uni H: Chemical quantities (Chapter 9)
  • Mole more relationships
  • Mass calculations
  • Limiting reactants
  • Percent yield
Unit I: Chemical bonding (Chapter 12)
  • Types of chemical bonds – ionic vs molecular
  • Electronegativity
  • Polarity
  • Lewis structures
  • VSEPR - molecular structure and geometry

Generally, this is as far as we get in the course... in an ideal world, we would like to cover another unit or two as listed below.

Unit J: Energy (Chapter 10)

  • The nature of energy
  • Temperature vs heat
  • Exothermic and endothermic reactions
  • Thermodynamics
  • Calorimetry
  • Hess’s law
  • Energy as a driving force
Unit K: Gases (Chapter 13)
  • Pressure
  • Boyle’s law - P * V
  • Charles Law - V / T
  • Gay-Lussac’s Law – P / T
  • Ideal gas law
  • Dalton’s law of partial pressures
  • Kinetic molecular theory
  • Real gases
  • Gas stoichiometry