Honors Chemistry (College Level)


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Thinkwell's Honors Chemistry

Thinkwell's Honors Chemistry is adapted from a two-semester college-level course.  It's intended for successful college-bound students, especially ones interested in pursuing science.  The course is taught by top professors from prestigious universities. Thinkwell's Chemistry has similar content to leading chemistry textbooks and the instructional videos are ideal for households where parents are not scientists! 

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. What's the difference between Honors and AP Chem? Check out a comparison of the courses here.

The Printed Notes (optional) are the Honors Chemistry course notes from the Online Subscription printed in color, on-the-go format. 

Prerequisites: High School Chemistry and Algebra 2

Course Features

Video Lessons

313 engaging 5-15 minute lesson videos
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Lesson Plan

Detailed, 37-week lesson plan and schedule
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Automatically graded exercises and tests with step-by-step feedback
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Concise, illustrated course notes for every topic
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Course Overview

What You Get

  • 12-month, online subscription to our complete Honors Chemistry course
  • 37-week, day-by-day course lesson plan
  • 310+ course lessons with streaming videos
  • Illustrated course notes with key terms and definitions
  • Automatically graded drill-and-practice exercises with step-by-step answer feedback
  • Chapter & Practice tests, a Midterm & Final Exam....and more!

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  • Grade reports and certificates of completion are available at request
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Thinkwell's Honors Chemistry Authors
Gordon Yee, Dean Harman, and Tarek Sammakia

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.

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.

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.

Thinkwell's Honors Chemistry Table of Contents
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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

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

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

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   

18. Introduction to Organic Reactions

18.1 Acid Strength in Organic Molecules  
18.1.1  An Introduction to Reactivity  
18.1.2  Bond Strengths  
18.1.3  Inductive Effects  
18.1.4  Hybridization Effects  
18.1.5  Resonance Effects  
18.1.6  Solvent Effects: Acid Dissociation versus Proton Affinity    
18.2  Base Strength in Organic Molecules  
18.2.1  A Review of Relationship Between Acids and Conjugate Bases  
18.2.2  Strengths of Organic Bases  
18.2.3  Solvent Effects on Organic Base Strength    
18.3  Lewis Acid and Base Reactions  
18.3.1  Lewis Acids and the Formation of Acid-Base Adducts    
18.3.2  Oxides as Lewis Acids    
18.4  Introduction to Electrophiles and Nucleophiles  
18.4.1  Nucleophilic Substitution at sp3 Carbon  
18.4.2  Nucleophilic Substitution at sp2 Carbon  
18.4.3  Elimination Reactions  
18.4.4  CIA Demonstration: Slime

19. Thermodynamics

19.1 An Introduction to Thermodynamics
19.1.1 Spontaneous Processes
19.2 Entropy
19.2.1 Entropy and the Second Law of Thermodynamics
19.2.2 Entropy and Temperature
19.3 Gibbs Free Energy and Free Energy Change
19.3.1 Gibbs Free Energy
19.3.2 Standard Free Energy Changes of Formation
19.4 Using Free Energy
19.4.1 Enthalpy and Entropy Contributions to K
19.4.2 The Temperature Dependence of K
19.4.3 Free Energy Away from Equilibrium

20. Electrochemistry

20.1 Principles of Electrochemistry
20.1.1 Reviewing Oxidation-Reduction Reactions
20.2 Galvanic Cells
20.2.1 Electrochemical Cells
20.2.2 Electromotive Force
20.2.3 Standard Reduction Potentials
20.2.4 Using Standard Reduction Potentials
20.2.5 The Nernst Equation
20.2.6 Electrochemical Determinants of Equilibria
20.3 Batteries
20.3.1 Batteries
20.3.2 CIA Demonstration: The Fruit-Powered Clock
20.4 Corrosion
20.4.1 Corrosion and the Prevention of Corrosion
20.5 Electrolysis and Electrolytic Cells
20.5.1 Electrolytic Cells
20.5.2 The Stoichiometry of Electrolysis

21. Nuclear Chemistry

21.1 Radioactivity
21.1.1 The Nature of Radioactivity
21.1.2 The Stability of Atomic Nuclei
21.1.3 Binding Energy
21.2 Rates of Disintegration
21.2.1 Rates of Disintegration Reactions
21.2.2 Radiochemical Dating
21.3 Nuclear Fission and Fusion
21.3.1 Nuclear Fission
21.3.2 Nuclear Fusion
21.3.3 Applications of Nuclear Chemistry

22. Chemistry of Metals

22.1 An Introduction to Metals
22.1.1 Metallurgical Processes
22.1.2 The Band Theory of Conductivity
22.1.3 Intrinsic Semiconductors
22.1.4 Doped Semiconductors
22.2 Physical and Chemical Processes of Metals
22.2.1 The Alkali Metals
22.2.2 The Alkaline Earth Metals
22.2.3 Aluminum
22.2.4 CIA Demonstration: The Reaction Between Al and Br2

23. Nonmetals

23.1 An Introduction to Nonmetals and Hydrogen
23.1.1 General Properties of Nonmetals
23.1.2 Hydrogen
23.2 Group 14: Carbon and Silicon
23.2.1 General Properties of Carbon
23.2.2 Silicon
23.3 Group 15: Nitrogen and Phosphorus
23.3.1 Nitrogen
23.3.2 Phosphorus
23.4 Group 16: Oxygen and Sulfur
23.4.1 Oxygen
23.4.2 CIA Demonstration: Creating Acid Rain
23.4.3 Sulfur
23.5 Group 17: The Halogens
23.5.1 Halogens
23.5.2 Aqueous Halogen Compounds
23.6 Group 18: The Noble Gases
23.6.1 Properties of Noble Gases

24. Instructional Laboratory Demonstrations

24.1 Laboratory Techniques
24.1.1 CIA Demonstration: Laboratory Safety
24.1.2 CIA Demonstration: Chromatography
24.1.3 CIA Demonstration: Distillation
24.1.4 CIA Demonstration: Pipetting
24.1.5 CIA Demonstration: Dilutions
24.1.6 CIA Demonstration: Titrations
24.1.7 CIA Demonstration: Extractions
24.1.8 CIA Demonstration: Filtrations
24.1.9 CIA Demonstration: Weighing on an Analytical Balance
24.1.10 CIA Demonstration: Recrystallization
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Yes, Thinkwell Honors Chemistry is a two-semester college course of Chemistry 1 and Chemistry 2. The main difference between college Chemistry and high school Chemistry is the depth of topic coverage and the pace.

Is Thinkwell Honors Chemistry appropriate for my accelerated student?

Yes, it is college-level content. This course is best suited to college-bound students, especially ones interested in pursuing degrees in math or science. If you are interested preparing for the Chemistry AP exam®, you’ll want to investigate Thinkwell’s Chemistry compatible with AP® course.

What is the math prerequisite for Honors Chemistry?

Precalculus is a suggested prerequisite or concurrent course.

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The course grade is calculated this way: Chapter Tests 33.3%, Midterm: 33.3%, Final: 33.3%.

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