Chemistry Companion

Chemistry Thinkwell's Chemistry is a two-semester college-level course that's accessible enough for introductory college chemistry courses, but rigorous enough for science majors. It's taught by top professors from prestigious universities, so you'll have help from our nation's best chemistry teachers whenever you need it. When you use Thinkwell Chemistry as a study aid, you'll be completely prepared for class, which means better grades. Thinkwell Chemistry has similar content to all major chemistry textbooks, so stop depending on an old-fashioned textbook and start learning the way you want to. Thinkwell Chemistry is available 24/7 for one fixed price, instead of by the hour, so it's better than a tutor, too. If you're preparing for the Chemistry AP® test, check out Thinkwell's Chemistry compatible with AP®, which includes diagnostic assessments geared towards AP® exam preparation.   Our complete Chemistry package includes: 12-month Online Subscription to our complete Chemistry course with video lessons, automatically graded chemistry problems, and much more. Printed Notes (optional) are the Chemistry course notes from the Online Subscription printed in a color, on-the-go format.  Chemistry Materials Online Subscription, 12-month access Access to a complete online package that includes everything you need. Thinkwell's video lectures cover the comprehensive scope and sequence of topics covered in a college-level introductory course. Our automatically graded exercises with immediate feedback allow you to quickly determine which areas you'll need to spend extra time studying. Concise, illustrated review notes help you distill the fundamental ideas, concepts, and formulas you'll need to know. 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Chemistry Details Thinkwell's Chemistry includes all of these features to prepare you for the big exam: More than 260 video lessons 1000+ interactive chemistry problems with immediate feedback allow you to track your progress Practice tests and final tests for all 14 chapters, as well as a midterm and a final (only available in the homeschool version) Interactive animations with audio Printable illustrated notes for each topic Glossary of more than 850 chemistry terms Engaging content to help students advance their knowledge of chemistry: Atoms, molecules, and ions Stoichiometry and the mole Reactions in aqueous solutions Gases, liquids, and solids Modern atomic theory and quantum mechanics Electron configurations and periodicity Chemical bonding and reactions Properties of solutions Acids and bases Thermochemistry, electrochemistry, and biochemistry Table of Contents 1. An Introduction to Matter and Measurement 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. Atoms, Molecules, and Ions 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. Stoichiometry 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. Reactions in Aqueous Solutions 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. Gases 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. Thermochemistry 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. Modern Atomic Theory 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. Electron Configurations and Periodicity 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. Chemical Bonding: Fundamental Concepts 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. Molecular Geometry and Bonding Theory 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. Oxidation-Reduction Reactions 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. Condensed Phases: Liquids and Solids 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 12.4 Ceramics 12.4.1 Ceramics and Glass 12.4.2 CIA Demonstration: Superconductivity 13. Physical Properties of Solutions 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 13.4 Colloids 13.4.1 Colloid Formation and Flocculation 13.4.2 CIA Demonstration: The Tyndall Effect 14. Chemical Kinetics 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 Multi-step 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. Chemical Equilibrium 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 Effects 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. Acids and Bases 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 16.3 Polyprotic Acids 16.3.1 Examining Polyprotic Acids 16.4 Acid-Base Properties of Salts 16.4.1 Acid-Base Properties of Salt Solutions 17. Equilibrium in Aqueous Solution 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 17.4.5 The Effects of pH on Solubility 17.5 Complex Ion Equilibria 17.5.1 The Formation of Complex Ions 17.5.2 Amphoteric Metal Hydrox