I. Introduction to measurements, matter, and the atom
     A. Units and significant figures  (1.3)
     B. Accuracy and Precision (1.4)
     C. Classes, phases, and properties of matter (1.9)
     D. Atomic theory – history, atomic number, mass number (2.1-2.2, 3.1)
II. Formulas
     A. Calculations of atomic mass, mass spectrometer (3.1)
     B. Mole calculations, empirical formulas, and molecular formula (3.2-3.5)
     C. Nomenclature (2.8)
III. Reactions
    A. Chemical reactions (complete, molecular style) – balancing types, stoichiometry (3.6-3.9, 4.4-4.6, 4.8-4.9)
    B. Introductory aqueous chemistry — molarity, net ionic equations, solubility rules (4.1-4.3, 11.3, Table 4.13)
    C. Precipitation reactions—solubility, net ionic equations (4.5-4.7, Table 4.1)
    D. Oxidation-reduction reactions and electrochemistry
          1. Oxidation numbers (4.9)
          2. balancing equations by half-reactions (4.10)
          3. Standard electrode potentials, including reaction spontaneity (17.2)
          4. Voltaic/galvanic cells (17.1)
          5. Electrolytic cells (17.7)
          6. Faraday’s Law (17.3)
          7. Nernst equation (17.4)
     E. Acid –base reactions
          1.Theories—Arrhenius, Bronsted-Lowry, Lewis (14.1, 14.11)
          2.Ionization/dissociation equations for strong and weak acids and bases  (14.1-14.2)
          3. Kw and pH  (14.2-14.3)
          4. Introduction to equilibrium (Ka and Kb)  (14.4-14.7)
          5. Salts (14.8)
IV. Thermodynamics—Part I: Thermochemistry
     A. Introductory energy concepts – types of energy, units, system, and surroundings  (6.1)
     B. First Law of Thermodynamics – state functions, calculations of work and Heat (6.1)
     C. Calorimetry  (6.2)
     D. Hess’s Law  (6.3)
     E. Standard enthalpy of formation  (6.4)
V. Electronic structure and periodicity
     A. Electronic structure
          1. Nature of light – waves, quantized energy  (7.1-7.2)
          2. Bohr model of the atom – line spectra, classical physics approach, electron energy calculations  (7.3-7.4)
          3. Quantum mechanics – dual nature of matter, orbitals, quantum numbers  (7.5-7.8)
          4. Electron notations/configurations (7.11)
     B. Periodic table
          1. History  (7.10)
          2. Trends in radius, ionization energy, electron affinity energy, metal-nonmetal characteristics; irregularities in trends         

                 (7.12-7.13)
          3. Explanation of trends and irregularities: effective nucleus, radius (distance), shielding, charge density
IV. Bonding
     A. Ionic bonds
          1. Born-Haber cycle – energy diagrams, relater reactions, energy calculations  (8.1-8.2, 18.5)
          2. Coulomb’s Law relationships  (8.1)
     B. Covalent bonds
          1. Bond energy – energy minimum graph, calculations; number, length, and strength of bonds  (8.8)
          2. Bond polarity, electronegativity  (8.2)
          3. Molecular models – VSEPR theory, hybrid orbitals, resonance; dipole moment, geometries, Lewis structures, sigma and pi

                bonds  (8.10, 8.13)
     C. Organic chemistry
          1. Alkanes, alkenes, alkynes – structures, introductory nomenclature (22.1-22.2)
          2. functional groups  (22.5)
          3. Isomers (22.1)
VII. States of Matter
     A. Gases
          1. Gas laws – Boyle’s, Charles’s,  Avogadro’s, Gay-Lussac’s, Dalton’s (partial pressure)  (5.2)
          2. Ideal Gas Law – calculations and deviations (5.3)
          3. Kinetic molecular theory, energy distribution graphs (5.6)
     B. Liquids and Solids
          1. Kinetic molecular descriptions
          2. Phase changes – vapor pressure, heats of vaporization and fusion, heating curves, phase diagrams (boiling point, triple    

                point, critical temperature)  (10.8-10.9)
          3. Attractive forces/ intermolecular forces – types and associated properties  (10.3)
     C. Solutions
          1. Solution process (11.1)
          2. Concentration calculations  (11.1)
          3. Solubility – saturation, temperature effects, pressure effects, solute-solvent interactions  (11.3)
          4. Colligative properties  (11.7)
VIII. Kinetics
      A. Reaction rates – average rate expressions, units, graphs, stoichiometry (12.1-12.2)
      B. Differential rate law – orders, rate constants, concentrations, working with data (12.3)
      C. Integral rate law – graphs, lab applications (12.4)
      D. Collision theory – activation energy and orientation of particles;  effects of concentrations, temperature, catalysts  (12.7)
      E. Potential energy diagrams – construct, interpret; relate to energy distribution graphs (12.7)
      F. Arrhenius equation (12.7, pg. 590)
      G. Mechanisms (12.7)
IX. Equilibrium
      A. Gas equilibrium
          1. Equilibrium concepts – expressions, constants, graphs, calculations (13.3)
          2. Le Chatelier’s Principle; effects of temperature, pressure, volume (13.7)
      B. Acid-base equilibria
          1. Ka and Kb (previously introduced) (14.4, 14.7)
          2. Common ion effects (15.1)
          3. Buffers (15.2-15.3)
          4. Titration – curves, including shape, midpoint, and equivalence point determinations; calculations of concentration and

                pH; indicators (15.4)
      C. Solubility products
          1.Saturated solutions (15.6)
          2. writing reaction equations and Ksp expressions (15.6)
          3. Determining solubility and concentrations, common ion effects (15.6)
          4. Determining precipitation from calculations of Q versus Ksp (15.7)
      D. Complex ions
          1. Formulas and equation writing (15.8)
X. Part II Entropy and free energy
      A. Spontaneous reactions – thermodynamics versus kinetics, driving forces (16.1)
      B. Entropy – second and third laws of thermodynamics, sign conventions, calculations, molecular level interpretations (16.2)
      C. Free energy – calculations from tables, thermochemical data, equilibrium constants, and electrical potential; interpretation

            of reaction spontaneity (16.4)
XI. Nuclear chemistry
      A. Particles (21.1)
      B. Nuclear equations – writing and balancing reactions, predicting products (21.1)
      C. Half-life calculations (21.2)