Andover's Chem 550/580:

Advanced Chemistry

(AP+)

Table of Contents

(Note: You should have a periodic table with element symbols and names, atomic numbers, and average atomic masses as well as a scientific calculator as you use this textbook.)

Chapter 1: Converting Units and Rounding Answers

Section 1-1: Converting Units Using Dimensional Analysis

Section 1-2: Significant Figures

Section 1-3: Rounding Answers

Section 1-4: Density

Section 1-5: Experiment – Determining the Density of a Solid by Water Displacement

Chapter 2: The Mole

Section 2-1: Introduction to Avogadro's Number and the Mole

Section 2-2: Molar Mass

Section 2-3: Converting Between Mass and Number of Atoms or Molecules

Chapter 3: Composition of Compounds and Experimental Determination of Chemical Formulas

Section 3-1: Percent Composition by Mass

Section 3-2: Determination of Empirical and Molecular Formulas

Section 3-3: Experiment – Determining the Formula of a Hydrate

Section 3-4: Experiment – Combustion Analysis

Chapter 4: Balancing Chemical Equations and Stoichiometry

Section 4-1: Balancing Chemical Equations and States of Matter

Section 4-2: Mole Ratios and Stoichiometry

Section 4-3: Limiting Reagents

Section 4-4: Percent Yield

Chapter 5: Gases

Section 5-1: The Ideal Gas Law

Section 5-2: Gas Stoichiometry

Section 5-3: Determining Molar Mass of a Gas and Gas Density

Section 5-4: Other Gas Laws

Section 5-5: Measuring Pressure With Barometers and Manometers

Section 5-6: Collecting Gases Over Water

Section 5-7: Experiment - Determining the Gas Constant R

Section 5-8: Root-Mean-Square Speed and Graham's Law

Chapter 6: Solutions

Section 6-1: Molarity

Section 6-2: Solution Stoichiometry

Section 6-3: Dilution

Chapter 7: Atomic Structure

Section 7-1: Protons, Neutrons, and Electrons

Section 7-2: Average Atomic Mass

Section 7-3: Atomic Orbitals and Electron Configurations

Section 7-4: Orbital Diagrams

Section 7-5: Quantum Numbers

Chapter 8: Trends in the Periodic Table

Section 8-1: Group Names

Section 8-2: Atomic and Ionic Radius

Section 8-3: Ionization Energy and Electron Affinity

Chapter 9: Chemical Bonding and Nomenclature

Section 9-1: Relationship Between Groups and Number of Valence Electrons

Section 9-2: Electronegativity

Section 9-3: Ionic Bonding and Ionic Nomenclature

Section 9-4: Molecular Compounds, Covalent Bonding, and Lewis Structures

Section 9-5: Bond Length, Resonance, and Formal Charge

Section 9-6: Nomenclature of Binary Molecular Compounds

Section 9-7: Introduction to Organic Nomenclature

Section 9-8: Names of Common Acids

Chapter 10: Chemical Tests and Chemical Reaction Types

Section 10-1: Laboratory Tests to Identify Chemicals

Section 10-2: Diatomic Nonmetals

Section 10-3: Combustion of Organic Compounds

Section 10-4: Reactions Involving Metals or Metal Compounds

Section 10-5: Aqueous Ionic Compounds and Molarity of Ions

Section 10-6: Solubility Rules, Precipitation Reactions, and Net Ionic Equations

Section 10-7: Acid + Base Neutralization Reactions and Molecular Equations

Section 10-8: Experiment – Acid + Base Titration

Chapter 11: Molecular Geometry, Polarity of Molecules, and Advanced Bonding Theory

Section 11-1: Molecular Geometry: Using VSEPR Theory to Determine Three-Dimensional Shapes and Bond Angles

Section 11-2: Polarity of Molecules

Section 11-3: Hybridization

Section 11-4: Sigma and Pi Bonds

Section 11-5: Molecular Orbital (MO) Theory

Chapter 12: Crystal Types and Intermolecular Forces

Section 12-1: Crystal Types

Section 12-2: Intermolecular Forces

Section 12-3: "Like Dissolves Like" and Solubility

Chapter 13: Thermochemistry

Section 13-1: Enthalpy of Reaction, ΔH

Section 13-2: Estimating ΔH Using Bond Energies

Section 13-3: Calculating ΔH Using Hess's Law

Section 13-4: Calculating ΔH° Using Standard Enthalpies of Formation, ΔH_f°

Section 13-5: Heat Transfer and the First Law of Thermodynamics

Section 13-6: Experiment - Determining the Specific Heat of a Metal Using Calorimetry

Section 13-7: Experiment – Determining ΔH Using Calorimetry

Section 13-8: ΔH for Changes of Physical State and Heating/Cooling Curves

Section 13-9: Experiment – Determining ΔH_fusion of Ice

Section 13-10: Lattice Energy and the Born-Haber Method

Chapter 14: Thermodynamics

Section 14-1: Predicting the Sign of the Entropy Change, ΔS

Section 14-2: Calculating ΔS° Using Standard Entropies, S°

Section 14-3: The Second Law of Thermodynamics and Gibbs Free Energy Change, ΔG

Section 14-4: The Effect of Temperature on ΔG and the Spontaneity of Reactions

Section 14-5: Calculating ΔG° from Standard Gibbs Free Energies of Formation, ΔG_f°

Chapter 15: Equilibrium

Section 15-1: Equilibrium Constant, K_c and K_p, Expressions

Section 15-2: Equilibrium Calculations and RICE Charts

Section 15-3: Reaction Quotients, Q_c and Q_p

Section 15-4: Heterogeneous Equilibria

Section 15-5: Le Châtelier’s Principle

Section 15-6: Converting Between K_c and K_p

Section 15-7: Relationship Between ΔG° and Equilibrium Constants

Section 15-8: The van't Hoff Equation - Effect of Temperature on Equilibrium Constants

Section 15-9: The Clausius-Clapeyron Equation - Effect of Temperature on Vapor Pressure

Chapter 16: Oxidation-Reduction (Redox) Reactions and Electrochemistry

Section 16-1: Oxidation and Reduction Half-Reactions

Section 16-2: Using Oxidation Numbers to Identify Oxidizing and Reducing Agents

Section 16-3: Balancing Redox Reactions in Aqueous Acidic and Basic Solutions

Section 16-4: Using a Standard Reduction Potentials Table to Compare Strengths of Oxidizing and Reducing Agents

Section 16-5: Calculating E°_cell and ΔG° to Determine Spontaneity of Redox Reactions

Section 16-6: Redox Reactions of Metals, Acids, and Halogens

Section 16-7: Experiment – Constructing a Galvanic Cell

Section 16-8: Nonspontaneous Redox Reactions and Electrolysis

Section 16-9: Calculating the Equilibrium Constant from E°_cell

Section 16-10: The Nernst Equation - Effect of Concentration

Chapter 17: Acids and Bases

Section 17-1: Arrhenius Theory, pH, and pOH

Section 17-2: Monoprotic Strong Acids and Strong Bases

Section 17-3: Monoprotic Weak Acids

Section 17-4: Polyprotic Weak Acids and Sulfuric Acid

Section 17-5: Bronsted Theory

Section 17-6: Weak Bases

Section 17-7: Lewis Structures and Acid Strength

Section 17-8: Hydrolysis – Aqueous Ions as Acids and Bases

Section 17-9: Reactions of Nonmetal Oxides with Water to Create Oxoacids

Section 17-10: Experiment – Determining the Molar Mass of an Unknown Monoprotic Weak Acid by Titration

Section 17-11: pH of Buffer Solutions

Section 17-12: pH and Titration Curves

Section 17-13: Acid-Base Indicators

Chapter 18: Solubility Equilibrium

Section 18-1: Solubility Equilibrium reactions and K_sp Expressions

Section 18-2: Molar Solubility and K_sp Calculations

Section 18-3: Predicting Precipitation Using Q_sp

Section 18-4: Experiment - Determining K_sp Using pH

Section 18-5: The Common-Ion Effect on Solubility

Section 18-6: Fractional Precipitation

Chapter 19: Chemical Kinetics

Section 19-1: Collision Theory and Factors That Increase Chemical Reaction Rates

Section 19-2: Reaction Energy Profiles (Reaction Progress Diagrams)

Section 19-3: Reaction Mechanisms

Section 19-4: Catalysis

Section 19-5: Determining Reaction Order and Rate Law Using Method of Initial Rates

Section 19-6: Determining Reaction Order and Rate Law Using Concentration Versus Time Data

Section 19-7: Relationship Between Rate Law and Reaction Mechanism

Section 19-8: The Arrhenius Equation - Effect of Temperature on Rate Constants

Chapter 20: Nuclear Chemistry

Section 20-1: Balancing Nuclear Equations

Section 20-2: Nuclear Kinetics and Half-Life

Chapter 21: Colligative Properties

Section 21-1: Molality

Section 21-2: Freezing Point Depression, Boiling Point Elevation, and the van't Hoff Factor

Section 21-3: Experiment - Determining Molar Mass Using Freezing Point Depression

Section 21-4: Raoult's Law and Vapor Pressure