Thinkwell.Chemistry.Course

Thinkwell.Chemistry.Course




- An Introduction to Matter and Measurement

* 1.1 An Introduction to Chemistry and the Scientific Method
o 1.1.1 An Introduction to Chemistry
o 1.1.2 The Scientific Method

* 1.2 Properties of Matter
o 1.2.1 States of Matter
o 1.2.2 A Word About Laboratory Safety
o 1.2.3 CIA Demonstration: Differences in Density Due to Temperature
o 1.2.4 Properties of Matter

* 1.3 Scientific Measurement
o 1.3.1 The Measurement of Matter
o 1.3.2 Precision and Accuracy
o 1.3.3 CIA Demonstration: Precision and Accuracy with Glassware
o 1.3.4 Significant Figures
o 1.3.5 Dimensional Analysis

* 1.4 Mathematics of Chemistry
o 1.4.1 Scientific (Exponential) Notation
o 1.4.2 Common Mathematical Functions

- Atoms, Molecules, and Ions

* 2.1 Early Atomic Theory
o 2.1.1 Early Discoveries and the Atom
o 2.1.2 Understanding Electrons
o 2.1.3 Understanding the Nucleus

* 2.2 Atomic Structure
o 2.2.1 Mass Spectrometry: Determining Atomic Masses
o 2.2.2 Examining Atomic Structure
o 2.2.3 CIA Demonstration: Flame Colors

* 2.3 The Periodic Table
o 2.3.1 Creating the Periodic Table

* 2.4 Chemical Nomenclature
o 2.4.1 Describing Chemical Formulas
o 2.4.2 Naming Chemical Compounds
o 2.4.3 Organic Nomenclature

- Stoichiometry

* 3.1 Chemical Equations
o 3.1.1 An Introduction to Chemical Reactions and Equations
o 3.1.2 CIA Demonstration: Magnesium and Dry Ice
o 3.1.3 Balancing Chemical Equations

* 3.2 The Mole
o 3.2.1 The Mole and Avogadro's Number
o 3.2.2 Introducing Conversions of Masses, Moles, and Number of Particles

* 3.3 Solving Problems Involving Mass/Mole Relationships
o 3.3.1 Finding Empirical and Molecular Formulas
o 3.3.2 Stoichiometry and Chemical Equations
o 3.3.3 Finding Limiting Reagents
o 3.3.4 CIA Demonstration: Self-Inflating Hydrogen Balloons
o 3.3.5 Theoretical Yield and Percent Yield
o 3.3.6 A Problem Using the Combined Concepts of Stoichiometry

- Reactions in Aqueous Solutions

* 4.1 An Introduction to Solutions
o 4.1.1 Properties of Solutions
o 4.1.2 CIA Demonstration: The Electric Pickle
o 4.1.3 Concentrations of Solutions
o 4.1.4 Factors Determining Solubility

* 4.2 Reactions Involving Solutions
o 4.2.1 Precipitation Reactions
o 4.2.2 Acid-Base Reactions
o 4.2.3 Oxidation-Reduction Reactions

* 4.3 Stoichiometry Problems in Solutions
o 4.3.1 Acid-Base Titrations
o 4.3.2 Solving Titration Problems
o 4.3.3 Gravimetric Analysis

- Gases

* 5.1 Gases and Gas Laws
o 5.1.1 Properties of Gases
o 5.1.2 Boyle's Law
o 5.1.3 Charles's Law
o 5.1.4 The Combined Gas Law
o 5.1.5 Avogadro's Law
o 5.1.6 CIA Demonstration: The Potato Cannon

* 5.2 The Ideal Gas Law and Kinetic-Molecular Theory of Gases
o 5.2.1 The Ideal Gas Law
o 5.2.2 Partial Pressure and Dalton's Law
o 5.2.3 Applications of the Gas Laws
o 5.2.4 The Kinetic-Molecular Theory of Gases
o 5.2.5 CIA Demonstration: The Ammonia Fountain

* 5.3 Molecular Motion of Gases
o 5.3.1 Molecular Speeds
o 5.3.2 Effusion and Diffusion

* 5.4 Behavior of Real Gases
o 5.4.1 Comparing Real and Ideal Gases

- Thermochemistry

* 6.1 An Introduction to Energy
o 6.1.1 The Nature of Energy
o 6.1.2 Energy, Calories, and Nutrition
o 6.1.3 The First Law of Thermodynamics
o 6.1.4 Work
o 6.1.5 Heat
o 6.1.6 CIA Demonstration: Cool Fire

* 6.2 Enthalpy
o 6.2.1 Heats of Reaction: Enthalpy
o 6.2.2 CIA Demonstration: The Thermite Reaction

* 6.3 Calorimetry
o 6.3.1 Constant Pressure Calorimetry
o 6.3.2 Bomb Calorimetry (Constant Volume)

* 6.4 Hess's Law and Enthalpies of Formation
o 6.4.1 Hess's Law
o 6.4.2 Enthalpies of Formation

- Modern Atomic Theory

* 7.1 Electromagnetic Radiation and the Idea of Quantum
o 7.1.1 The Wave Nature of Light
o 7.1.2 Absorption and Emission
o 7.1.3 CIA Demonstration: Luminol
o 7.1.4 The Ultraviolet Catastrophe
o 7.1.5 The Photoelectric Effect
o 7.1.6 The Bohr Model
o 7.1.7 The Heisenberg Uncertainty Principle

* 7.2 Quantum Mechanics
o 7.2.1 The Wave Nature of Matter
o 7.2.2 Radial Solutions to the Schr?dinger Equation
o 7.2.3 Angular Solutions to the Schr?dinger Equation

* 7.3 Atomic Orbitals
o 7.3.1 Atomic Orbital Size
o 7.3.2 Atomic Orbital Shapes and Quantum Numbers
o 7.3.3 Atomic Orbital Energy

- Electron Configurations and Periodicity

* 8.1 Electron Spin and the Pauli Exclusion Principle
o 8.1.1 Understanding Electron Spin
o 8.1.2 Electron Shielding
o 8.1.3 Electron Configurations through Neon
o 8.1.4 Electron Configurations beyond Neon
o 8.1.5 Periodic Relationships

* 8.2 Periodicity
o 8.2.1 Periods and Atomic Size
o 8.2.2 Ionization Energy
o 8.2.3 Electron Affinity
o 8.2.4 An Introduction to Electronegativity

* 8.3 Group Trends
o 8.3.1 Hydrogen, Alkali Metals and Alkaline Earth Metals
o 8.3.2 Transition Metals and Nonmetals

- Chemical Bonding: Fundamental Concepts

* 9.1 Valence Electrons and Chemical Bonding
o 9.1.1 Valence Electrons and Chemical Bonding
o 9.1.2 Ionic Bonds
o 9.1.3 CIA Demonstration: Conductivity Apparatus-Ionic versus Covalent Bonds

* 9.2 Lewis Dot Structures
o 9.2.1 Lewis Dot Structures for Covalent Bonds
o 9.2.2 Predicting Lewis Dot Structures

* 9.3 Resonance Structures and Formal Charge
o 9.3.1 Resonance Structures
o 9.3.2 Formal Charge
o 9.3.3 Electronegativity, Formal Charge, and Resonance

* 9.4 Bond Properties
o 9.4.1 Bond Properties
o 9.4.2 Using Bond Dissociation Energies

- Molecular Geometry and Bonding Theory

* 10.1 Molecular Geometry and the VSEPR Theory
o 10.1.1 Valence-Shell Electron-Pair Repulsion Theory
o 10.1.2 Molecular Shapes for Steric Numbers 2-4
o 10.1.3 Molecular Shapes for Steric Numbers 5 & 6
o 10.1.4 Predicting Molecular Characteristics Using VSEPR Theory

* 10.2 Valence Bond Theory and Molecular Orbital Theory
o 10.2.1 Valence Bond Theory
o 10.2.2 An Introduction to Hybrid Orbitals
o 10.2.3 Pi Bonds
o 10.2.4 Molecular Orbital Theory
o 10.2.5 Applications of the Molecular Orbital Theory
o 10.2.6 Beyond Homonuclear Diatomics
o 10.2.7 CIA Demonstration: The Paramagnetism of Oxygen

- Oxidation-Reduction Reactions

* 11.1 Looking In-Depth at Redox Reactions
o 11.1.1 Oxidation Numbers
o 11.1.2 Balancing Redox Reactions by the Oxidation Number Method
o 11.1.3 Balancing Redox Reactions Using the Half-Reaction Method
o 11.1.4 The Activity Series of the Elements
o 11.1.5 CIA Demonstration: The Reaction between Al and Br2

- Condensed Phases: Liquids and Solids

* 12.1 Intermolecular Forces
o 12.1.1 An Introduction to Intermolecular Forces and States of Matter
o 12.1.2 Intermolecular Forces

* 12.2 Physical Properties of Liquids
o 12.2.1 Properties of Liquids
o 12.2.2 CIA Demonstration: Boiling Water at Reduced Pressure
o 12.2.3 Vapor Pressure and Boiling Point
o 12.2.4 Molecular Structure and Boiling Point
o 12.2.5 Phase Diagrams
o 12.2.6 CIA Demonstration: Boiling Water in a Paper Cup

* 12.3 Solid State: Structure and Bonding
o 12.3.1 Types of Solids
o 12.3.2 CIA Demonstration: The Conductivity of Molten Salts
o 12.3.3 Crystal Structure
o 12.3.4 Calculating Atomic Mass and Radius from a Unit Cell
o 12.3.5 Crystal Packing

* 12.4 Ceramics
o 12.4.1 Ceramics and Glass
o 12.4.2 CIA Demonstration: Superconductivity

- Physical Properties of Solutions

* 13.1 Characterizing Solutions
o 13.1.1 Types of Solutions
o 13.1.2 Molarity and the Mole Fraction
o 13.1.3 Molality
o 13.1.4 Energy and the Solution Process

* 13.2 Effects of Temperature and Pressure on Solubility
o 13.2.1 Temperature Change and Solubility
o 13.2.2 Extractions
o 13.2.3 Pressure Change and Solubility

* 13.3 Colligative Properties
o 13.3.1 Vapor Pressure Lowering
o 13.3.2 Boiling Point Elevation and Freezing Point Depression
o 13.3.3 Boiling Point Elevation Problem
o 13.3.4 Osmosis
o 13.3.5 Colligative Properties of Ionic Solutions

* 13.4 Colloids
o 13.4.1 Colloid Formation and Flocculation
o 13.4.2 CIA Demonstration: The Tyndall Effect

- Chemical Kinetics

* 14.1 Reaction Rates
o 14.1.1 An Introduction to Reaction Rates
o 14.1.2 Rate Laws: How the Reaction Rate Depends on Concentration
o 14.1.3 Determining the Form of a Rate Law

* 14.2 Orders of Reaction
o 14.2.1 First-Order Reactions
o 14.2.2 Second-Order Reactions
o 14.2.3 A Kinetics Problem

* 14.3 Temperature and Rates
o 14.3.1 The Collision Model
o 14.3.2 The Arrhenius Equation
o 14.3.3 Using the Arrhenius Equation

* 14.4 Reaction Mechanisms
o 14.4.1 Defining the Molecularity of a Reaction
o 14.4.2 Determining the Rate Laws of Elementary Reactions
o 14.4.3 Calculating the Rate Laws of Multistep Reactions
o 14.4.4 Steady State Kinetics

* 14.5 Catalysts
o 14.5.1 Catalysts and Types of Catalysts
o 14.5.2 A Word About Laboratory Safety
o 14.5.3 CIA Demonstration: Elephant Snot
o 14.5.4 CIA Demonstration: The Cobalt(II)-Catalyzed Reaction of Potassium Sodium Tartrate
o 14.5.5 CIA Demonstration: The Copper-Catalyzed Decomposition of Acetone

- Chemical Equilibrium

* 15.1 Principles of Chemical Equilibrium
o 15.1.1 The Concept of Equilibrium
o 15.1.2 The Law of Mass Action and Types of Equilibrium
o 15.1.3 Converting Between Kc and Kp

* 15.2 Using Equilibrium Constants
o 15.2.1 Approaching Chemical Equilibrium
o 15.2.2 Predicting the Direction of a Reaction
o 15.2.3 Strategies for Solving Equilibrium Problems
o 15.2.4 Solving Problems Far from Equilibrium
o 15.2.5 An Equilibrium Problem Using the Quadratic Equation

* 15.3 Shifting Chemical Equilibrium
o 15.3.1 Le Châtelier's Principle
o 15.3.2 The Effect of Changing Amounts on Equilibrium
o 15.3.3 The Effect of Pressure and Volume on Equilibrium
o 15.3.4 The Effects of Temperature and Catalysts on Equilibrium
o 15.3.5 CIA Demonstration: NO2/N2O4
o 15.3.6 CIA Demonstration: Shifting the Equilibrium of FeSCN2+

- Acids and Bases

* 16.1 Acid-Base Concepts
o 16.1.1 Arrhenius/Br?nsted-Lowry Definitions of Acids and Bases
o 16.1.2 Hydronium, Hydroxide, and the pH Scale

* 16.2 Acid and Base Strengths
o 16.2.1 Strong Acids and Bases
o 16.2.2 CIA Demonstration: Natural Acid-Base Indicators
o 16.2.3 Weak Acids
o 16.2.4 Weak Bases
o 16.2.5 Lewis Acids and Bases
o 16.2.6 Trends in Acid and Base Strengths

* 16.3 Polyprotic Acids
o 16.3.1 Examining Polyprotic Acids

* 16.4 Acid-Base Properties of Salts
o 16.4.1 Acid-Base Properties of Salt Solutions

- Equilibrium in Aqueous Solution

* 17.1 Reactions of Acids and Bases
o 17.1.1 Strong Acid-Strong Base and Weak Acid-Strong Base Reactions
o 17.1.2 Strong Acid-Weak Base and Weak Acid-Weak Base Reactions
o 17.1.3 The Common Ion Effect

* 17.2 Buffers
o 17.2.1 An Introduction to Buffers
o 17.2.2 CIA Demonstration: Buffers in Action
o 17.2.3 Acidic Buffers
o 17.2.4 Basic Buffers
o 17.2.5 The Henderson-Hasselbalch Equation

* 17.3 Acid-Base Titration
o 17.3.1 Strong Acid-Strong Base Titration
o 17.3.2 CIA Demonstration: Barium Hydroxide-Sulfuric Acid Titration
o 17.3.3 Weak Acid-Strong Base Titration
o 17.3.4 Polyprotic Acid-Strong Base Titration
o 17.3.5 Weak Base-Strong Acid Titration
o 17.3.6 Acid-Base Indicators

* 17.4 Solubility Equilibria
o 17.4.1 The Solubility Product Constant
o 17.4.2 CIA Demonstration: Silver Chloride and Ammonia
o 17.4.3 Solubility and the Common Ion Effect
o 17.4.4 Fractional Precipitation
o 17.4.5 The Effects of pH on Solubility

* 17.5 Complex Ion Equilibria
o 17.5.1 The Formation of Complex Ions
o 17.5.2 Amphoteric Metal Hydroxides

- Introduction to Organic Reactions

* 18.1 Acid Strength in Organic Molecules
o 18.1.1 An Introduction to Reactivity
o 18.1.2 Bond Strengths
o 18.1.3 Inductive Effects
o 18.1.4 Hybridization Effects
o 18.1.5 Resonance Effects
o 18.1.6 Solvent Effects: Acid Dissociation versus Proton Affinity

* 18.2 Base Strength in Organic Molecules
o 18.2.1 A Review of Relationship between Acids and Conjugate Bases
o 18.2.2 Strengths of Organic Bases
o 18.2.3 Solvent Effects on Organic Base Strength

* 18.3 Lewis Acid and Base Reactions
o 18.3.1 Lewis Acids and the Formation of Acid-Base Adducts
o 18.3.2 Oxides as Lewis Acids

* 18.4 Introduction to Electrophiles and Nucleophiles
o 18.4.1 Nucleophilic Substitution at sp3 Carbon
o 18.4.2 Nucleophilic Substitution at sp2 Carbon
o 18.4.3 Elimination Reactions
o 18.4.4 CIA Demonstration: Slime

- Thermodynamics

* 19.1 An Introduction to Thermodynamics
o 19.1.1 Spontaneous Processes

* 19.2 Entropy
o 19.2.1 Entropy and the Second Law of Thermodynamics
o 19.2.2 Entropy and Temperature

* 19.3 Gibbs Free Energy and Free Energy Change
o 19.3.1 Gibbs Free Energy
o 19.3.2 Standard Free Energy Changes of Formation

* 19.4 Using Free Energy
o 19.4.1 Enthalpy and Entropy Contributions to K
o 19.4.2 The Temperature Dependence of K
o 19.4.3 Free Energy Away from Equilibrium

- Electrochemistry

* 20.1 Principles of Electrochemistry
o 20.1.1 Reviewing Oxidation-Reduction Reactions

* 20.2 Galvanic Cells
o 20.2.1 Electrochemical Cells
o 20.2.2 Electromotive Force
o 20.2.3 Standard Reduction Potentials
o 20.2.4 Using Standard Reduction Potentials
o 20.2.5 The Nernst Equation
o 20.2.6 Electrochemical Determinants of Equilibria

* 20.3 Batteries
o 20.3.1 Batteries
o 20.3.2 CIA Demonstration: The Fruit-Powered Clock

* 20.4 Corrosion
o 20.4.1 Corrosion and the Prevention of Corrosion

* 20.5 Electrolysis and Electrolytic Cells
o 20.5.1 Electrolytic Cells
o 20.5.2 The Stoichiometry of Electrolysis

- Nuclear Chemistry

* 21.1 Radioactivity
o 21.1.1 The Nature of Radioactivity
o 21.1.2 The Stability of Atomic Nuclei
o 21.1.3 Binding Energy

* 21.2 Rates of Disintegration
o 21.2.1 Rates of Disintegration Reactions
o 21.2.2 Radiochemical Dating

* 21.3 Nuclear Fission and Fusion
o 21.3.1 Nuclear Fission
o 21.3.2 Nuclear Fusion
o 21.3.3 Applications of Nuclear Chemistry

- Chemistry of Metals

* 22.1 An Introduction to Metals
o 22.1.1 Metallurgical Processes
o 22.1.2 Band Theory of Conductivity
o 22.1.3 Intrinsic Semiconductors
o 22.1.4 Doped Semiconductors

* 22.2 Physical and Chemical Processes of Metals
o 22.2.1 The Alkali Metals
o 22.2.2 The Alkaline Earth Metals
o 22.2.3 Aluminum
o 22.2.4 CIA Demonstration: The Reaction between Al and Br2

- Transition Metals

* 23.1 Examining Transition Metals
o 23.1.1 Properties of Transition Metals
o 23.1.2 CIA Demonstration: Copper One-Pot Reactions

* 23.2 Coordination Compounds
o 23.2.1 Complexes and Ligands
o 23.2.2 Naming Coordination Compounds
o 23.2.3 Structures of Coordination Compounds and Isomers

* 23.3 Bonding in Coordination Compounds
o 23.3.1 Color and Transition Metals
o 23.3.2 Crystal Field Theory
o 23.3.3 Ligand Field Theory
o 23.3.4 Magnetic Properties and Spin

- Nonmetals

* 24.1 An Introduction to Nonmetals and Hydrogen
o 24.1.1 General Properties of Nonmetals
o 24.1.2 Hydrogen

* 24.2 Group 14: Carbon and Silicon
o 24.2.1 General Properties of Carbon
o 24.2.2 Silicon

* 24.3 Group 15: Nitrogen and Phosphorus
o 24.3.1 Nitrogen
o 24.3.2 Phosphorus

* 24.4 Group 16: Oxygen and Sulfur
o 24.4.1 Oxygen
o 24.4.2 CIA Demonstration: Creating Acid Rain
o 24.4.3 Sulfur

* 24.5 Group 17: The Halogens
o 24.5.1 Halogens
o 24.5.2 Aqueous Halogen Compounds

* 24.6 Group 18: The Noble Gases
o 24.6.1 Properties of Noble Gases

- Organic Chemistry

* 25.1 Hydrocarbons
o 25.1.1 Alkanes
o 25.1.2 Alkenes and Alkynes
o 25.1.3 Isomers
o 25.1.4 Aromatic Hydrocarbons

* 25.2 The Functional Groups
o 25.2.1 Alcohols, Ethers, and Amines
o 25.2.2 Carbonyl-Containing Functional Groups

* 25.3 Organic Polymers
o 25.3.1 Organic Polymers
o 25.3.2 CIA Demonstration: The Synthesis of Nylon

- Biochemistry

* 26.1 Biological Molecules
o 26.1.1 Proteins
o 26.1.2 Nucleic Acids
o 26.1.3 Carbohydrates
o 26.1.4 Lipids

- Instructional Laboratory Demonstrations

* 27.1 Laboratory Techniques
o 27.1.1 CIA Demonstration: Laboratory Safety
o 27.1.2 CIA Demonstration: Chromatography
o 27.1.3 CIA Demonstration: Distillation
o 27.1.4 CIA Demonstration: Pipetting
o 27.1.5 CIA Demonstration: Dilutions
o 27.1.6 CIA Demonstration: Titrations
o 27.1.7 CIA Demonstration: Extractions
o 27.1.8 CIA Demonstration: Filtrations
o 27.1.9 CIA Demonstration: Weighing on an Analytical Balance
o 27.1.10 CIA Demonstration: Recrystallization