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Imagine having the world’s best Chemistry professors at your side to help you learn the fundamentals of AP Chemistry. Thinkwell gives you just that! Learn the basics of AP Chemistry from award-winning Chemistry professors Gordon Yee and Dean Harman. They’ll teach you the powerful ideas and intuitions behind Chemistry that will help you score a perfect 5 on the AP Chemistry exam. Thinkwell's online AP Chemistry subscription gives you access to a complete web-based solution that includes all of the content and tools you'll need to succeed in AP Chemistry.
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1.1 An Introduction to Chemistry and the Scientific Method
1.1.1 An Introduction to Chemistry
1.1.2 The Scientific Method
1.2 Properties of Matter
1.2.1 States of Matter
1.2.2 A Word About Laboratory Safety
1.2.3 CIA Demonstration: Differences in Density Due to Temperature
1.2.4 Properties of Matter
1.3 Scientific Measurement
1.3.1 The Measurement of Matter
1.3.2 Precision and Accuracy
1.3.3 CIA Demonstration: Precision and Accuracy with Glassware
1.3.4 Significant Figures
1.3.5 Dimensional Analysis
1.4 Mathematics of Chemistry
1.4.1 Scientific (Exponential) Notation
1.4.2 Common Mathematical Functions
2.1 Early Atomic Theory
2.1.1 Early Discoveries and the Atom
2.1.2 Understanding Electrons
2.1.3 Understanding the Nucleus
2.2 Atomic Structure
2.2.1 Mass Spectrometry: Determining Atomic Masses
2.2.2 Examining Atomic Structure
2.2.3 CIA Demonstration: Flame Colors
2.3 The Periodic Table
2.3.1 Creating the Periodic Table
2.4 Chemical Nomenclature
2.4.1 Describing Chemical Formulas
2.4.2 Naming Chemical Compounds
2.4.3 Organic Nomenclature
3.1 Chemical Equations
3.1.1 An Introduction to Chemical Reactions and Equations
3.1.2 CIA Demonstration: Magnesium and Dry Ice
3.1.3 Balancing Chemical Equations
3.2 The Mole
3.2.1 The Mole and Avogadro's Number
3.2.2 Introducing Conversions of Masses, Moles, and Number of Particles
3.3 Solving Problems Involving Mass/Mole Relationships
3.3.1 Finding Empirical and Molecular Formulas
3.3.2 Stoichiometry and Chemical Equations
3.3.3 Finding Limiting Reagents
3.3.4 CIA Demonstration: Self-Inflating Hydrogen Balloons
3.3.5 Theoretical Yield and Percent Yield
3.3.6 A Problem Using the Combined Concepts of Stoichiometry
4.1 An Introduction to Solutions
4.1.1 Properties of Solutions
4.1.2 CIA Demonstration: The Electric Pickle
4.1.3 Concentrations of Solutions
4.1.4 Factors Determining Solubility
4.2 Reactions Involving Solutions
4.2.1 Precipitation Reactions
4.2.2 Acid-Base Reactions
4.2.3 Oxidation-Reduction Reactions
4.3 Stoichiometry Problems in Solutions
4.3.1 Acid-Base Titrations
4.3.2 Solving Titration Problems
4.3.3 Gravimetric Analysis
5.1 Gases and Gas Laws
5.1.1 Properties of Gases
5.1.2 Boyle's Law
5.1.3 Charles's Law
5.1.4 The Combined Gas Law
5.1.5 Avogadro's Law
5.1.6 CIA Demonstration: The Potato Cannon
5.2 The Ideal Gas Law and Kinetic-Molecular Theory of Gases
5.2.1 The Ideal Gas Law
5.2.2 Partial Pressure and Dalton's Law
5.2.3 Applications of the Gas Laws
5.2.4 The Kinetic-Molecular Theory of Gases
5.2.5 CIA Demonstration: The Ammonia Fountain
5.3 Molecular Motion of Gases
5.3.1 Molecular Speeds
5.3.2 Effusion and Diffusion
5.4 Behavior of Real Gases
5.4.1 Comparing Real and Ideal Gases
6.1 An Introduction to Energy
6.1.1 The Nature of Energy
6.1.2 Energy, Calories, and Nutrition
6.1.3 The First Law of Thermodynamics
6.1.4 Work
6.1.5 Heat
6.1.6 CIA Demonstration: Cool Fire
6.2 Enthalpy
6.2.1 Heats of Reaction: Enthalpy
6.2.2 CIA Demonstration: The Thermite Reaction
6.3 Calorimetry
6.3.1 Constant Pressure Calorimetry
6.3.2 Bomb Calorimetry (Constant Volume)
6.4 Hess's Law and Enthalpies of Formation
6.4.1 Hess's Law
6.4.2 Enthalpies of Formation
7.1 Electromagnetic Radiation and the Idea of Quantum
7.1.1 The Wave Nature of Light
7.1.2 Absorption and Emission
7.1.3 CIA Demonstration: Luminol
7.1.4 The Ultraviolet Catastrophe
7.1.5 The Photoelectric Effect
7.1.6 The Bohr Model
7.1.7 The Heisenberg Uncertainty Principle
7.2 Quantum Mechanics
7.2.1 The Wave Nature of Matter
7.2.2 Radial Solutions to the Schrödinger Equation
7.2.3 Angular Solutions to the Schrödinger Equation
7.3 Atomic Orbitals
7.3.1 Atomic Orbital Size
7.3.2 Atomic Orbital Shapes and Quantum Numbers
7.3.3 Atomic Orbital Energy
8.1 Electron Spin and the Pauli Exclusion Principle
8.1.1 Understanding Electron Spin
8.1.2 Electron Shielding
8.1.3 Electron Configurations through Neon
8.1.4 Electron Configurations beyond Neon
8.1.5 Periodic Relationships
8.2 Periodicity
8.2.1 Periods and Atomic Size
8.2.2 Ionization Energy
8.2.3 Electron Affinity
8.2.4 An Introduction to Electronegativity
8.3 Group Trends
8.3.1 Hydrogen, Alkali Metals and Alkaline Earth Metals
8.3.2 Transition Metals and Nonmetals
9.1 Valence Electrons and Chemical Bonding
9.1.1 Valence Electrons and Chemical Bonding
9.1.2 Ionic Bonds
9.1.3 CIA Demonstration: Conductivity Apparatus-Ionic versus Covalent Bonds
9.2 Lewis Dot Structures
9.2.1 Lewis Dot Structures for Covalent Bonds
9.2.2 Predicting Lewis Dot Structures
9.3 Resonance Structures and Formal Charge
9.3.1 Resonance Structures
9.3.2 Formal Charge
9.3.3 Electronegativity, Formal Charge, and Resonance
9.4 Bond Properties
9.4.1 Bond Properties
9.4.2 Using Bond Dissociation Energies
10.1 Molecular Geometry and the VSEPR Theory
10.1.1 Valence-Shell Electron-Pair Repulsion Theory
10.1.2 Molecular Shapes for Steric Numbers 2-4
10.1.3 Molecular Shapes for Steric Numbers 5 & 6
10.1.4 Predicting Molecular Characteristics Using VSEPR Theory
10.2 Valence Bond Theory and Molecular Orbital Theory
10.2.1 Valence Bond Theory
10.2.2 An Introduction to Hybrid Orbitals
10.2.3 Pi Bonds
10.2.4 Molecular Orbital Theory
10.2.5 Applications of the Molecular Orbital Theory
10.2.6 Beyond Homonuclear Diatomics
10.2.7 CIA Demonstration: The Paramagnetism of Oxygen
11.1 Looking In-Depth at Redox Reactions
11.1.1 Oxidation Numbers
11.1.2 Balancing Redox Reactions by the Oxidation Number Method
11.1.3 Balancing Redox Reactions Using the Half-Reaction Method
11.1.4 The Activity Series of the Elements
11.1.5 CIA Demonstration: The Reaction between Al and Br2
12.1 Intermolecular Forces
12.1.1 An Introduction to Intermolecular Forces and States of Matter
12.1.2 Intermolecular Forces
12.2 Physical Properties of Liquids
12.2.1 Properties of Liquids
12.2.2 CIA Demonstration: Boiling Water at Reduced Pressure
12.2.3 Vapor Pressure and Boiling Point
12.2.4 Molecular Structure and Boiling Point
12.2.5 Phase Diagrams
12.2.6 CIA Demonstration: Boiling Water in a Paper Cup
12.3 Solid State: Structure and Bonding
12.3.1 Types of Solids
12.3.2 CIA Demonstration: The Conductivity of Molten Salts
12.3.3 Crystal Structure
12.3.4 Calculating Atomic Mass and Radius from a Unit Cell
12.3.5 Crystal Packing
13.1 Characterizing Solutions
13.1.1 Types of Solutions
13.1.2 Molarity and the Mole Fraction
13.1.3 Molality
13.1.4 Energy and the Solution Process
13.2 Effects of Temperature and Pressure on Solubility
13.2.1 Temperature Change and Solubility
13.2.2 Extractions
13.2.3 Pressure Change and Solubility
13.3 Colligative Properties
13.3.1 Vapor Pressure Lowering
13.3.2 Boiling Point Elevation and Freezing Point Depression
13.3.3 Boiling Point Elevation Problem
13.3.4 Osmosis
13.3.5 Colligative Properties of Ionic Solutions
14.1 Reaction Rates
14.1.1 An Introduction to Reaction Rates
14.1.2 Rate Laws: How the Reaction Rate Depends on Concentration
14.1.3 Determining the Form of a Rate Law
14.2 Orders of Reaction
14.2.1 First-Order Reactions
14.2.2 Second-Order Reactions
14.2.3 A Kinetics Problem
14.3 Temperature and Rates
14.3.1 The Collision Model
14.3.2 The Arrhenius Equation
14.3.3 Using the Arrhenius Equation
14.4 Reaction Mechanisms
14.4.1 Defining the Molecularity of a Reaction
14.4.2 Determining the Rate Laws of Elementary Reactions
14.4.3 Calculating the Rate Laws of Multistep Reactions
14.4.4 Steady State Kinetics
14.5 Catalysts
14.5.1 Catalysts and Types of Catalysts
14.5.2 A Word About Laboratory Safety
14.5.3 CIA Demonstration: Elephant Snot
14.5.4 CIA Demonstration: The Cobalt(II)-Catalyzed Reaction of Potassium Sodium Tartrate
14.5.5 CIA Demonstration: The Copper-Catalyzed Decomposition of Acetone
15.1 Principles of Chemical Equilibrium
15.1.1 The Concept of Equilibrium
15.1.2 The Law of Mass Action and Types of Equilibrium
15.1.3 Converting Between Kc and Kp
15.2 Using Equilibrium Constants
15.2.1 Approaching Chemical Equilibrium
15.2.2 Predicting the Direction of a Reaction
15.2.3 Strategies for Solving Equilibrium Problems
15.2.4 Solving Problems Far from Equilibrium
15.2.5 An Equilibrium Problem Using the Quadratic Equation
15.3 Shifting Chemical Equilibrium
15.3.1 Le Châtelier's Principle
15.3.2 The Effect of Changing Amounts on Equilibrium
15.3.3 The Effect of Pressure and Volume on Equilibrium
15.3.4 The Effects of Temperature and Catalysts on Equilibrium
15.3.5 CIA Demonstration: NO2/N2O4
15.3.6 CIA Demonstration: Shifting the Equilibrium of FeSCN2+
16.1 Acid-Base Concepts
16.1.1 Arrhenius/Brønsted-Lowry Definitions of Acids and Bases
16.1.2 Hydronium, Hydroxide, and the pH Scale
16.2 Acid and Base Strengths
16.2.1 Strong Acids and Bases
16.2.2 CIA Demonstration: Natural Acid-Base Indicators
16.2.3 Weak Acids
16.2.4 Weak Bases
16.2.5 Lewis Acids and Bases
16.2.6 Trends in Acid and Base Strengths
17.1 Reactions of Acids and Bases
17.1.1 Strong Acid-Strong Base and Weak Acid-Strong Base Reactions
17.1.2 Strong Acid-Weak Base and Weak Acid-Weak Base Reactions
17.1.3 The Common Ion Effect
17.2 Buffers
17.2.1 An Introduction to Buffers
17.2.2 CIA Demonstration: Buffers in Action
17.2.3 Acidic Buffers
17.2.4 Basic Buffers
17.2.5 The Henderson-Hasselbalch Equation
17.3 Acid-Base Titration
17.3.1 Strong Acid-Strong Base Titration
17.3.2 CIA Demonstration: Barium Hydroxide-Sulfuric Acid Titration
17.3.3 Weak Acid-Strong Base Titration
17.3.4 Polyprotic Acid-Strong Base Titration
17.3.5 Weak Base-Strong Acid Titration
17.3.6 Acid-Base Indicators
17.4 Solubility Equilibria
17.4.1 The Solubility Product Constant
17.4.2 CIA Demonstration: Silver Chloride and Ammonia
17.4.3 Solubility and the Common Ion Effect
17.4.4 Fractional Precipitation
18.1 An Introduction to Thermodynamics
18.1.1 Spontaneous Processes
18.2 Entropy
18.2.1 Entropy and the Second Law of Thermodynamics
18.2.2 Entropy and Temperature
18.3 Gibbs Free Energy and Free Energy Change
18.3.1 Gibbs Free Energy
18.3.2 Standard Free Energy Changes of Formation
18.4 Using Free Energy
18.4.1 Enthalpy and Entropy Contributions to K
18.4.2 The Temperature Dependence of K
18.4.3 Free Energy Away from Equilibrium
19.1 Principles of Electrochemistry
19.1.1 Reviewing Oxidation-Reduction Reactions
19.2 Galvanic Cells
19.2.1 Electrochemical Cells
19.2.2 Electromotive Force
19.2.3 Standard Reduction Potentials
19.2.4 Using Standard Reduction Potentials
19.2.5 The Nernst Equation
19.2.6 Electrochemical Determinants of Equilibria
19.3 Batteries
19.3.1 Batteries
19.3.2 CIA Demonstration: The Fruit-Powered Clock
19.4 Corrosion
19.4.1 Corrosion and the Prevention of Corrosion
19.5 Electrolysis and Electrolytic Cells
19.5.1 Electrolytic Cells
19.5.2 The Stoichiometry of Electrolysis
20.1 Radioactivity
20.1.1 The Nature of Radioactivity
20.1.2 The Stability of Atomic Nuclei
20.1.3 Binding Energy
20.2 Rates of Disintegration
20.2.1 Rates of Disintegration Reactions
20.2.2 Radiochemical Dating
20.3 Nuclear Fission and Fusion
20.3.1 Nuclear Fission
20.3.2 Nuclear Fusion
20.3.3 Applications of Nuclear Chemistry
21.1 An Introduction to Metals
21.1.1 Metallurgical Processes
21.1.2 Band Theory of Conductivity
21.1.3 Intrinsic Semiconductors
21.1.4 Doped Semiconductors
21.2 Physical and Chemical Processes of Metals
21.2.1 The Alkali Metals
21.2.2 The Alkaline Earth Metals
21.2.3 Aluminum
21.2.4 CIA Demonstration: The Reaction between Al and Br2
22.1 An Introduction to Nonmetals and Hydrogen
22.1.1 General Properties of Nonmetals
22.1.2 Hydrogen
22.2 Group 14: Carbon and Silicon
22.2.1 General Properties of Carbon
22.2.2 Silicon
22.3 Group 15: Nitrogen and Phosphorus
22.3.1 Nitrogen
22.3.2 Phosphorus
22.4 Group 16: Oxygen and Sulfur
22.4.1 Oxygen
22.4.2 CIA Demonstration: Creating Acid Rain
22.4.3 Sulfur
22.5 Group 17: The Halogens
22.5.1 Halogens
22.5.2 Aqueous Halogen Compounds
22.6 Group 18: The Noble Gases
22.6.1 Properties of Noble Gases
23.1 Laboratory Techniques
23.1.1 CIA Demonstration: Laboratory Safety
23.1.2 CIA Demonstration: Chromatography
23.1.3 CIA Demonstration: Distillation
23.1.4 CIA Demonstration: Pipetting
23.1.5 CIA Demonstration: Dilutions
23.1.6 CIA Demonstration: Titrations
23.1.7 CIA Demonstration: Extractions
23.1.8 CIA Demonstration: Filtrations
23.1.9 CIA Demonstration: Weighing on an Analytical Balance
23.1.10 CIA Demonstration: Recrystallization
Dean Harman
University of Virginia
Dean Harman is a professor of chemistry at the University of Virginia, where he has been honored with several teaching awards. He heads the Harman Research Group, which specializes in the novel organic transformations made possible by electron-rich metal centers such as Os(II), RE(I), and W(0). Prof. Harman holds a Ph.D. from Stanford University.
Gordon Yee
Virginia Tech
Gordon Yee is an associate professor of chemistry at Virginia Tech in Blacksburg, VA. He received his Ph.D. from Stanford University and completed postdoctoral work at DuPont. A widely published author, Professor Yee studies molecule-based magnetism.
Tarek Sammakia
University of Colorado at Boulder
Tarek Sammakia is a Professor of Chemistry at the University of Colorado at Boulder where he teaches organic chemistry to undergraduate and graduate students. He received his Ph.D. from Yale University and carried out postdoctoral research at Harvard University. He has received several national awards for his work in synthetic and mechanistic organic chemistry.
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