Correlations

Chemistry: The Central Science, 9th Edition ©2003

Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten, Julia R. Burdge

Correlated with AP* Chemistry, May 2002, May 2003

ST = Student textbook pages

1. Structure of Matter
   1. Atomic theory and atomic structure
      1. Evidence for the atomic theory
         ST: 36–41
      2. Atomic masses; determination by chemical and physical means
         ST: 44–45
      3. Atomic number and mass number; isotopes
         ST: 43
      4. Electron energy levels: atomic spectra, quantum numbers, atomic orbitals
         ST: 208, 213–215, 343–345
      5. Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation states
         ST: 128–132, 241–243, 246–252, 294
   2. Chemical bonding
      1. Binding forces
         1. Types: ionic, covalent, metallic hydrogen bonding, van der Waals (including London dispersion forces)
            ST: 275–284, 300–306, 411–417, 435, 930–933
         2. Relationships to states, structure, and properties of matter
            ST: 5–12
         3. Polarity of bonds, electronegativities
            ST: 285–289, 868
      2. Molecular models
         1. Lewis structures
            ST: 290–295, 316
         2. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds
            ST: 295–297, 330–343
         3. VSEPR
            ST: 318–328
      3. Geometry of molecules and ions, structural isomerism of simple organic molecules and coordination complexes; dipole moments of molecules; relation of properties to structure
         ST: 316–353, 962
   3. Nuclear chemistry: nuclear equations, half-lives and radioactivity; chemical applications
      ST: 541–542, 832–834, 840–846
   
   
2. States of Matter
   1. Gases
      1. Laws of ideal gases
         1. Equation of state for an ideal gas
            ST: 375–382
         2. Partial pressures
            ST: 383–386
      2. Kinetic-molecular theory
         1. Interpretation of ideal gas laws on the basis of this theory
            ST: 388
         2. Avogadro's hypothesis and the mole concept
            ST: 373–374
         3. Dependence of kinetic energy of molecules on temperature
            ST: 388
         4. Deviations from ideal gas laws
            ST: 388
   2. Liquids and solids
      1. Liquids and solids from the kinetic-molecular viewpoint
         ST: 408–409
      2. Phase diagrams of one-component systems
         ST: 427–430
      3. Changes of state, including critical points and triple points
         ST: 428
      4. Structure of solids; lattice energies
         ST: 278, 430–435
   3. Solutions
      1. Types of solutions and factors affecting solubility
         ST: 492–497
      2. Methods of expressing concentration (The use of normalities is not tested)
         ST: 497–502
      3. Raoult's law and colligative properties (nonvolatile solutes); osmosis
         ST: 502–511, 719–720
      4. Non-ideal behavior (qualitative aspects)
         ST: 515
   
   
3. Reactions
   1. Reaction types
      1. Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination complexes; amphoterism
         ST: 121–127, 614–616, 648–652
      2. Precipitation reactions
         ST: 117–121
      3. Oxidation-reduction reactions
         ST: 128–134, 777–784
         1. Oxidation number
            ST: 128–129, 294
         2. The role of the electron in oxidation-reduction
            ST: 128, 778–783
         3. Electrochemistry: electrolytic and galvanic cells; Faraday's laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions
            ST: 799–801, 803
   2. Stoichiometry
      1. Ionic and molecular species present in chemical systems: net ionic equations
         ST: 120–121
      2. Balancing of equations, including those for redox reactions
         ST: 76–79, 95–99, 779–784
      3. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants
         ST: 50–51, 87–89, 91–95, 99–103, 375–376
   3. Equilibrium
      1. Concept of dynamic equilibrium, physical and chemical; Le Chatelier's principle; equilibrium constants
         ST: 425–427, 578–586, 588–603, 627–628
      2. Quantitative treatment
         1. Equilibrium constants for gaseous reactions: Kp, Kc
            ST: 578–583, 586–594
         2. Equilibrium constants for reactions in solution
            1. Constants for acids and bases; pK; pH
               ST: 620
            2. Solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds
               ST: 678–681
            3. Common ion effect; buffers; hydrolysis
               ST: 662–671, 641, 650–652
   4. Kinetics
      1. Concept of rate of reaction
         ST: 527–532
      2. Use of differential rate laws to determine order of reaction and rate constant from experimental data
         ST: 532–542
      3. Effect of temperature change on rates
         ST: 543–549
      4. Energy of activation; the role of catalysts
         ST: 544–549, 555–561
      5. The relationship between the rate-determining step and a mechanism
         ST: 549–555
   5. Thermodynamics
      1. State functions
         ST: 161–162, 737–738
      2. First law: change in enthalpy; heat of formation; heat of reaction; Hess's law; heats of vaporization and fusion; calorimetry
         ST: 174–180, 735
      3. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes
         ST: 489, 740–748
      4. Relationship of change in free energy to equilibrium constants and electrode potentials
         ST: 261–266, 287–288
   
   
4. Descriptive Chemistry
   1. Chemical reactivity and products of chemical reactions
      ST: 80–83
   2. Relationships in the periodic table: horizontal, vertical, and diagonal with examples from alkali metals, alkaline earth metals, halogens, and the first series of transition elements
      ST: 46–48, 237–239, 252–265
   3. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties)
      ST: 62–65, 984–1011
   
   Chemical Calculations
   
   1. Percentage composition
      ST: 84–85
   2. Empirical and molecular formulas from experimental data
      ST: 50–51, 91–95
   3. Molar masses from gas density, freezing-point, and boiling-point measurements
      ST: 87–91, 379–381
   4. Gas laws, including the ideal gas law, Dalton's law, and Graham's law
      ST: 377–379
   5. Stoichiometric relations using the concept of the mole; titration calculations
      ST: 86–91, 140–144, 671–677
   6. Mole fractions; molar and molal solutions
      ST: 499–502, 679
   7. Faraday's law of electrolysis
      ST: 797–798
   8. Equilibrium constants and their applications, including their use for simultaneous equilibria
      ST: 578–586, 627–678
   9. Standard electrode potentials and their use; Nernst equation
      ST: 785, 799–801
   10. Thermodynamic and thermochemical calculations
       ST: 154–163, 737, 743
   11. Kinetics calculations
       ST: 524–573