Correlations

General Chemistry: An Integrated Approach, 3rd Edition ©2002

John W. Hill and Ralph H. Petrucci

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: 38–40
      2. Atomic masses; determination by chemical and physical means
         ST: 43, 43–45, 87
      3. Atomic number and mass number; isotopes
         ST: 41, 46, 283, 330
      4. Electron energy levels: atomic spectra, quantum numbers atomic orbitals
         ST: 304, 306–308, 426–427, 428–436
      5. Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation states
         ST: 336–339, 340, 339–341, 341–343, 344–345
   2. Chemical bonding
      1. Binding forces
         1. Types: ionic, covalent, metallic hydrogen bonding, van der Waals (including London dispersion forces)
            ST: 52–57, 362, 365–367, 371, 374–375, 376, 433–436, 492–493, 1000
         2. Relationships to states, structure, and properties of matter
            ST: 370–373, 377–386, 401, 841–844, 998–999
         3. Polarity of bonds, electronegativities
            ST: 373–377, 422–423
      2. Molecular models
         1. Lewis structures
            ST: 370–373, 377–378, 381–384, 412
         2. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds
            ST: 426–427, 434, 436–443
         3. VSEPR
            ST: 410–421, 434
      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: 421, 423–425, 476
   3. Nuclear chemistry: nuclear equations, half-lives and radioactivity; chemical applications
      ST: 825, 827–831, 831–833, 844–846
   
   
2. States of Matter
   1. Gases
      1. Laws of ideal gases
         1. Equation of state for an ideal gas
            ST: 198, 199, 201
         2. Partial pressures
            ST: 206, 607–608, 610–611, 616–618
      2. Kinetic-molecular theory
         1. Interpretation of ideal gas laws on the basis of this theory
            ST: 182, 211–217
         2. Avogadro's hypothesis and the mole concept
            ST: 194–197
         3. Dependence of kinetic energy of molecules on temperature
            ST: 182, 211–217
         4. Deviations from ideal gas laws
            ST: 201–202
   2. Liquids and solids
      1. Liquids and solids from the kinetic-molecular viewpoint
         ST: 459–465, 466
      2. Phase diagrams of one-component systems
         ST: 465–466
      3. Changes of state, including critical points and triple points
         ST: 466
      4. Structure of solids; lattice energies
         ST: 369, 492
   3. Solutions
      1. Types of solutions and factors affecting solubility
         ST: 524–526
      2. Methods of expressing concentration (The use of normalities is not tested)
         ST: 116, 510–518
      3. Raoult's law and colligative properties (nonvolatile solutes); osmosis
         ST: 529–533, 542, 749
      4. Non-ideal behavior (qualitative aspects)
         ST: 520
   
   
3. Reactions
   1. Reaction types
      1. Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination complexes; amphoterism
         ST: 142, 675–680, 677
      2. Precipitation reactions
         ST: 153–155, 706, 710–711
      3. Oxidation-reduction reactions
         ST: 155, 159–161, 165–166, 168–169, 770–776
         1. Oxidation number
            ST: 154, 155, 162–163
         2. The role of the electron in oxidation-reduction
            ST: 166–168, 788–789
         3. Electrochemistry: electrolytic and galvanic cells; Faraday's laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions
            ST: 135, 276, 447, 840
   2. Stoichiometry
      1. Ionic and molecular species present in chemical systems: net ionic equations
         ST: 143, 148, 151
      2. Balancing of equations, including those for redox reactions
         ST: 100–105
      3. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants
         ST: 48, 93–97, 109–112
   3. Equilibrium
      1. Concept of dynamic equilibrium, physical and chemical; Le Chatelier's principle; equilibrium constants
         ST: 461, 600–601, 613–620, 667–669
      2. Quantitative treatment
         1. Equilibrium constants for gaseous reactions: Kp, Kc
            ST: 601–605, 606–607, 608–613, 754–762, 790, 792
         2. Equilibrium constants for reactions in solution
            1. Constants for acids and bases; pK; pH
               ST: 613–618, 652–659
            2. Solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds
               ST: 609–610, 611
            3. Common ion effect; buffers; hydrolysis
               ST: 140, 615–616
   4. Kinetics
      1. Concept of rate of reaction
         ST: 554, 556–558, 560
      2. Use of differential rate laws to determine order of reaction and rate constant from experimental data
         ST: 555, 558–561, 577–580
      3. Effect of temperature change on rates
         ST: 577–580
      4. Energy of activation; the role of catalysts
         ST: 586–590, 584–585
      5. The relationship between the rate-determining step and a mechanism
         ST: 584–586
   5. Thermodynamics
      1. State functions
         ST: 235, 750–751
      2. First law: change in enthalpy; heat of formation; heat of reaction; Hess's law; heats of vaporization and fusion; calorimetry
         ST: 235, 244–266
      3. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes
         ST: 237–244, 734, 738–746
      4. Relationship of change in free energy to equilibrium constants and electrode potentials
         ST: 231–232, 750–751
   
   
4. Descriptive Chemistry
   1. Chemical reactivity and products of chemical reactions
      ST: 5, 99–124, 149, 558, 565, 568, 570, 571, 757–758, 761
   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: 61–64, 64–65, 265, 398, 653, 679, 798, 859–866, 866–874, 967–969, 1014
   3. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties)
      ST: 58–60, 69–70, 142, 639, 645–646, 667–669, 675–680, 687–688, 980
   
   Chemical Calculations
   
   1. Percentage composition
      ST: 112, 511
   2. Empirical and molecular formulas from experimental data
      ST: 48, 93–95, 96, 96–97
   3. Molar masses from gas density, freezing-point, and boiling-point measurements
      ST: 86–90
   4. Gas laws, including the ideal gas law, Dalton's law, and Graham's law
      ST: 197, 202, 205, 206
   5. Stoichiometric relations using the concept of the mole; titration calculations
      ST: 84–90, 105, 106–124, 208, 243–244, 516
   6. Mole fractions; molar and molal solutions
      ST: 86–90, 514–516
   7. Faraday's law of electrolysis
      ST: 135, 276, 447, 804
   8. Equilibrium constants and their applications, including their use for simultaneous equilibria
      ST: 602, 607–613
   9. Standard electrode potentials and their use; Nernst equation
      ST: 777, 779, 806–807
   10. Thermodynamic and thermochemical calculations
       ST: 244–253, 262–266
   11. Kinetics calculations
       ST: 182, 211–217, 228, 575