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I. Review

  Naming Compounds 41:24
   Intro 0:00 
   Periodic Table of Elements 0:15 
   Naming Compounds 3:13 
    Definition and Examples of Ions 3:14 
    Ionic (Symbol to Name): NaCl 5:23 
    Ionic (Name to Symbol): Calcium Oxide 7:58 
    Ionic - Polyatoms Anions: Examples 12:45 
    Ionic - Polyatoms Anions (Symbol to Name): KClO 14:50 
    Ionic - Polyatoms Anions (Name to Symbol): Potassium Phosphate 15:49 
    Ionic Compounds Involving Transition Metals (Symbol to Name): Co₂(CO₃)₃ 20:48 
    Ionic Compounds Involving Transition Metals (Name to Symbol): Palladium 2 Acetate 22:44 
    Naming Covalent Compounds (Symbol to Name): CO 26:21 
    Naming Covalent Compounds (Name to Symbol): Nitrogen Trifluoride 27:34 
    Naming Covalent Compounds (Name to Symbol): Dichlorine Monoxide 27:57 
    Naming Acids Introduction 28:11 
    Naming Acids (Name to Symbol): Chlorous Acid 35:08 
    % Composition by Mass Example 37:38 
  Stoichiometry 37:19
   Intro 0:00 
   Stoichiometry 0:25 
    Introduction to Stoichiometry 0:26 
    Example 1 5:03 
    Example 2 10:17 
    Example 3 15:09 
    Example 4 24:02 
    Example 5: Questions 28:11 
    Example 5: Part A - Limiting Reactant 30:30 
    Example 5: Part B 32:27 
    Example 5: Part C 35:00 

II. Aqueous Reactions & Stoichiometry

  Precipitation Reactions 31:14
   Intro 0:00 
   Precipitation Reactions 0:53 
    Dissociation of ionic Compounds 0:54 
    Solubility Guidelines for ionic Compounds: Soluble Ionic Compounds 8:15 
    Solubility Guidelines for ionic Compounds: Insoluble ionic Compounds 12:56 
    Precipitation Reactions 14:08 
    Example 1: Mixing a Solution of BaCl₂ & K₂SO₄ 21:21 
    Example 2: Mixing a Solution of Mg(NO₃)₂ & KI 26:10 
  Acid-Base Reactions 43:21
   Intro 0:00 
   Acid-Base Reactions 1:00 
    Introduction to Acid: Monoprotic Acid and Polyprotic Acid 1:01 
    Introduction to Base 8:28 
    Neutralization 11:45 
    Example 1 16:17 
    Example 2 21:55 
    Molarity 24:50 
    Example 3 26:50 
    Example 4 30:01 
    Example 4: Limiting Reactant 37:51 
    Example 4: Reaction Part 40:01 
  Oxidation Reduction Reactions 47:58
   Intro 0:00 
   Oxidation Reduction Reactions 0:26 
    Oxidation and Reduction Overview 0:27 
    How Can One Tell Whether Oxidation-Reduction has Taken Place? 7:13 
    Rules for Assigning Oxidation State: Number 1 11:22 
    Rules for Assigning Oxidation State: Number 2 12:46 
    Rules for Assigning Oxidation State: Number 3 13:25 
    Rules for Assigning Oxidation State: Number 4 14:50 
    Rules for Assigning Oxidation State: Number 5 15:41 
    Rules for Assigning Oxidation State: Number 6 17:00 
    Example 1: Determine the Oxidation State of Sulfur in the Following Compounds 18:20 
   Activity Series and Reduction Properties 25:32 
    Activity Series and Reduction Properties 25:33 
    Example 2: Write the Balance Molecular, Total Ionic, and Net Ionic Equations for Al + HCl 31:37 
    Example 3 34:25 
    Example 4 37:55 
  Stoichiometry Examples 31:50
   Intro 0:00 
   Stoichiometry Example 1 0:36 
    Example 1: Question and Answer 0:37 
   Stoichiometry Example 2 6:57 
    Example 2: Questions 6:58 
    Example 2: Part A Solution 12:16 
    Example 2: Part B Solution 13:05 
    Example 2: Part C Solution 14:00 
    Example 2: Part D Solution 14:38 
   Stoichiometry Example 3 17:56 
    Example 3: Questions 17:57 
    Example 3: Part A Solution 19:51 
    Example 3: Part B Solution 21:43 
    Example 3: Part C Solution 26:46 

III. Gases

  Pressure, Gas Laws, & The Ideal Gas Equation 49:40
   Intro 0:00 
   Pressure 0:22 
    Pressure Overview 0:23 
    Torricelli: Barometer 4:35 
    Measuring Gas Pressure in a Container 7:49 
    Boyle's Law 12:40 
    Example 1 16:56 
   Gas Laws 21:18 
    Gas Laws 21:19 
    Avogadro's Law 26:16 
    Example 2 31:47 
   Ideal Gas Equation 38:20 
    Standard Temperature and Pressure (STP) 38:21 
    Example 3 40:43 
  Partial Pressure, Mol Fraction, & Vapor Pressure 32:00
   Intro 0:00 
   Gases 0:27 
    Gases 0:28 
    Mole Fractions 5:52 
    Vapor Pressure 8:22 
    Example 1 13:25 
    Example 2 22:45 
  Kinetic Molecular Theory and Real Gases 31:58
   Intro 0:00 
   Kinetic Molecular Theory and Real Gases 0:45 
    Kinetic Molecular Theory 1 0:46 
    Kinetic Molecular Theory 2 4:23 
    Kinetic Molecular Theory 3 5:42 
    Kinetic Molecular Theory 4 6:27 
    Equations 7:52 
    Effusion 11:15 
    Diffusion 13:30 
    Example 1 19:54 
    Example 2 23:23 
    Example 3 26:45 
  AP Practice for Gases 25:34
   Intro 0:00 
   Example 1 0:34 
    Example 1 0:35 
   Example 2 6:15 
    Example 2: Part A 6:16 
    Example 2: Part B 8:46 
    Example 2: Part C 10:30 
    Example 2: Part D 11:15 
    Example 2: Part E 12:20 
    Example 2: Part F 13:22 
   Example 3 14:45 
    Example 3 14:46 
   Example 4 18:16 
    Example 4 18:17 
   Example 5 21:04 
    Example 5 21:05 

IV. Thermochemistry

  Energy, Heat, and Work 37:32
   Intro 0:00 
   Thermochemistry 0:25 
    Temperature and Heat 0:26 
    Work 3:07 
    System, Surroundings, Exothermic Process, and Endothermic Process 8:19 
    Work & Gas: Expansion and Compression 16:30 
    Example 1 24:41 
    Example 2 27:47 
    Example 3 31:58 
  Enthalpy & Hess's Law 32:34
   Intro 0:00 
   Thermochemistry 1:43 
    Defining Enthalpy & Hess's Law 1:44 
    Example 1 6:48 
    State Function 13:11 
    Example 2 17:15 
    Example 3 24:09 
  Standard Enthalpies of Formation 23:09
   Intro 0:00 
   Thermochemistry 1:04 
    Standard Enthalpy of Formation: Definition & Equation 1:05 
    ∆H of Formation 10:00 
    Example 1 11:22 
    Example 2 19:00 
  Calorimetry 39:28
   Intro 0:00 
   Thermochemistry 0:21 
    Heat Capacity 0:22 
    Molar Heat Capacity 4:44 
    Constant Pressure Calorimetry 5:50 
    Example 1 12:24 
    Constant Volume Calorimetry 21:54 
    Example 2 24:40 
    Example 3 31:03 

V. Kinetics

  Reaction Rates and Rate Laws 36:24
   Intro 0:00 
   Kinetics 2:18 
    Rate: 2 NO₂ (g) → 2NO (g) + O₂ (g) 2:19 
    Reaction Rates Graph 7:25 
    Time Interval & Average Rate 13:13 
    Instantaneous Rate 15:13 
    Rate of Reaction is Proportional to Some Power of the Reactant Concentrations 23:49 
    Example 1 27:19 
  Method of Initial Rates 30:48
   Intro 0:00 
   Kinetics 0:33 
    Rate 0:34 
    Idea 2:24 
    Example 1: NH₄⁺ + NO₂⁻ → NO₂ (g) + 2 H₂O 5:36 
    Example 2: BrO₃⁻ + 5 Br⁻ + 6 H⁺ → 3 Br₂ + 3 H₂O 19:29 
  Integrated Rate Law & Reaction Half-Life 32:17
   Intro 0:00 
   Kinetics 0:52 
    Integrated Rate Law 0:53 
    Example 1 6:26 
    Example 2 15:19 
    Half-life of a Reaction 20:40 
    Example 3: Part A 25:41 
    Example 3: Part B 28:01 
  Second Order & Zero-Order Rate Laws 26:40
   Intro 0:00 
   Kinetics 0:22 
    Second Order 0:23 
    Example 1 6:08 
    Zero-Order 16:36 
    Summary for the Kinetics Associated with the Reaction 21:27 
  Activation Energy & Arrhenius Equation 40:59
   Intro 0:00 
   Kinetics 0:53 
    Rate Constant 0:54 
    Collision Model 2:45 
    Activation Energy 5:11 
    Arrhenius Proposed 9:54 
    2 Requirements for a Successful Reaction 15:39 
    Rate Constant 17:53 
    Arrhenius Equation 19:51 
    Example 1 25:00 
    Activation Energy & the Values of K 32:12 
    Example 2 36:46 
  AP Practice for Kinetics 29:08
   Intro 0:00 
   Kinetics 0:43 
    Example 1 0:44 
    Example 2 6:53 
    Example 3 8:58 
    Example 4 11:36 
    Example 5 16:36 
    Example 6: Part A 21:00 
    Example 6: Part B 25:09 

VI. Equilibrium

  Equilibrium, Part 1 46:00
   Intro 0:00 
   Equilibrium 1:32 
    Introduction to Equilibrium 1:33 
    Equilibrium Rules 14:00 
    Example 1: Part A 16:46 
    Example 1: Part B 18:48 
    Example 1: Part C 22:13 
    Example 1: Part D 24:55 
    Example 2: Part A 27:46 
    Example 2: Part B 31:22 
    Example 2: Part C 33:00 
    Reverse a Reaction 36:04 
    Example 3 37:24 
  Equilibrium, Part 2 40:53
   Intro 0:00 
   Equilibrium 1:31 
    Equilibriums Involving Gases 1:32 
    General Equation 10:11 
    Example 1: Question 11:55 
    Example 1: Answer 13:43 
    Example 2: Question 19:08 
    Example 2: Answer 21:37 
    Example 3: Question 33:40 
    Example 3: Answer 35:24 
  Equilibrium: Reaction Quotient 45:53
   Intro 0:00 
   Equilibrium 0:57 
    Reaction Quotient 0:58 
    If Q > K 5:37 
    If Q < K 6:52 
    If Q = K 7:45 
    Example 1: Part A 8:24 
    Example 1: Part B 13:11 
    Example 2: Question 20:04 
    Example 2: Answer 22:15 
    Example 3: Question 30:54 
    Example 3: Answer 32:52 
    Steps in Solving Equilibrium Problems 42:40 
  Equilibrium: Examples 31:51
   Intro 0:00 
   Equilibrium 1:09 
    Example 1: Question 1:10 
    Example 1: Answer 4:15 
    Example 2: Question 13:04 
    Example 2: Answer 15:20 
    Example 3: Question 25:03 
    Example 3: Answer 26:32 
  Le Chatelier's principle & Equilibrium 40:52
   Intro 0:00 
   Le Chatelier 1:05 
    Le Chatelier Principle 1:06 
    Concentration: Add 'x' 5:25 
    Concentration: Subtract 'x' 7:50 
    Example 1 9:44 
    Change in Pressure 12:53 
    Example 2 20:40 
    Temperature: Exothermic and Endothermic 24:33 
    Example 3 29:55 
    Example 4 35:30 

VII. Acids & Bases

  Acids and Bases 50:11
   Intro 0:00 
   Acids and Bases 1:14 
    Bronsted-Lowry Acid-Base Model 1:28 
    Reaction of an Acid with Water 4:36 
    Acid Dissociation 10:51 
    Acid Strength 13:48 
    Example 1 21:22 
    Water as an Acid & a Base 25:25 
    Example 2: Part A 32:30 
    Example 2: Part B 34:47 
    Example 3: Part A 35:58 
    Example 3: Part B 39:33 
    pH Scale 41:12 
    Example 4 43:56 
  pH of Weak Acid Solutions 43:52
   Intro 0:00 
   pH of Weak Acid Solutions 1:12 
    pH of Weak Acid Solutions 1:13 
    Example 1 6:26 
    Example 2 14:25 
    Example 3 24:23 
    Example 4 30:38 
  Percent Dissociation: Strong & Weak Bases 43:04
   Intro 0:00 
   Bases 0:33 
    Percent Dissociation: Strong & Weak Bases 0:45 
    Example 1 6:23 
    Strong Base Dissociation 11:24 
    Example 2 13:02 
    Weak Acid and General Reaction 17:38 
    Example: NaOH → Na⁺ + OH⁻ 20:30 
    Strong Base and Weak Base 23:49 
    Example 4 24:54 
    Example 5 33:51 
  Polyprotic Acids 35:34
   Intro 0:00 
   Polyprotic Acids 1:04 
    Acids Dissociation 1:05 
    Example 1 4:51 
    Example 2 17:30 
    Example 3 31:11 
  Salts and Their Acid-Base Properties 41:14
   Intro 0:00 
   Salts and Their Acid-Base Properties 0:11 
    Salts and Their Acid-Base Properties 0:15 
    Example 1 7:58 
    Example 2 14:00 
    Metal Ion and Acidic Solution 22:00 
    Example 3 28:35 
    NH₄F → NH₄⁺ + F⁻ 34:05 
    Example 4 38:03 
  Common Ion Effect & Buffers 41:58
   Intro 0:00 
   Common Ion Effect & Buffers 1:16 
    Covalent Oxides Produce Acidic Solutions in Water 1:36 
    Ionic Oxides Produce Basic Solutions in Water 4:15 
    Practice Example 1 6:10 
    Practice Example 2 9:00 
    Definition 12:27 
    Example 1: Part A 16:49 
    Example 1: Part B 19:54 
    Buffer Solution 25:10 
    Example of Some Buffers: HF and NaF 30:02 
    Example of Some Buffers: Acetic Acid & Potassium Acetate 31:34 
    Example of Some Buffers: CH₃NH₂ & CH₃NH₃Cl 33:54 
    Example 2: Buffer Solution 36:36 
  Buffer 32:24
   Intro 0:00 
   Buffers 1:20 
    Buffer Solution 1:21 
    Adding Base 5:03 
    Adding Acid 7:14 
    Example 1: Question 9:48 
    Example 1: Recall 12:08 
    Example 1: Major Species Upon Addition of NaOH 16:10 
    Example 1: Equilibrium, ICE Chart, and Final Calculation 24:33 
    Example 1: Comparison 29:19 
  Buffers, Part II 40:06
   Intro 0:00 
   Buffers 1:27 
    Example 1: Question 1:32 
    Example 1: ICE Chart 3:15 
    Example 1: Major Species Upon Addition of OH⁻, But Before Rxn 7:23 
    Example 1: Equilibrium, ICE Chart, and Final Calculation 12:51 
    Summary 17:21 
    Another Look at Buffering & the Henderson-Hasselbalch equation 19:00 
    Example 2 27:08 
    Example 3 32:01 
  Buffers, Part III 38:43
   Intro 0:00 
   Buffers 0:25 
    Buffer Capacity Part 1 0:26 
    Example 1 4:10 
    Buffer Capacity Part 2 19:29 
    Example 2 25:12 
    Example 3 32:02 
  Titrations: Strong Acid and Strong Base 42:42
   Intro 0:00 
   Titrations: Strong Acid and Strong Base 1:11 
    Definition of Titration 1:12 
    Sample Problem 3:33 
    Definition of Titration Curve or pH Curve 9:46 
   Scenario 1: Strong Acid- Strong Base Titration 11:00 
    Question 11:01 
    Part 1: No NaOH is Added 14:00 
    Part 2: 10.0 mL of NaOH is Added 15:50 
    Part 3: Another 10.0 mL of NaOH & 20.0 mL of NaOH are Added 22:19 
    Part 4: 50.0 mL of NaOH is Added 26:46 
    Part 5: 100.0 mL (Total) of NaOH is Added 27:26 
    Part 6: 150.0 mL (Total) of NaOH is Added 32:06 
    Part 7: 200.0 mL of NaOH is Added 35:07 
    Titrations Curve for Strong Acid and Strong Base 35:43 
  Titrations: Weak Acid and Strong Base 42:03
   Intro 0:00 
   Titrations: Weak Acid and Strong Base 0:43 
    Question 0:44 
    Part 1: No NaOH is Added 1:54 
    Part 2: 10.0 mL of NaOH is Added 5:17 
    Part 3: 25.0 mL of NaOH is Added 14:01 
    Part 4: 40.0 mL of NaOH is Added 21:55 
    Part 5: 50.0 mL (Total) of NaOH is Added 22:25 
    Part 6: 60.0 mL (Total) of NaOH is Added 31:36 
    Part 7: 75.0 mL (Total) of NaOH is Added 35:44 
    Titration Curve 36:09 
  Titration Examples & Acid-Base Indicators 52:03
   Intro 0:00 
   Examples and Indicators 0:25 
    Example 1: Question 0:26 
    Example 1: Solution 2:03 
    Example 2: Question 12:33 
    Example 2: Solution 14:52 
    Example 3: Question 23:45 
    Example 3: Solution 25:09 
    Acid/Base Indicator Overview 34:45 
    Acid/Base Indicator Example 37:40 
    Acid/Base Indicator General Result 47:11 
    Choosing Acid/Base Indicator 49:12 

VIII. Solubility

  Solubility Equilibria 36:25
   Intro 0:00 
   Solubility Equilibria 0:48 
    Solubility Equilibria Overview 0:49 
    Solubility Product Constant 4:24 
    Definition of Solubility 9:10 
    Definition of Solubility Product 11:28 
    Example 1 14:09 
    Example 2 20:19 
    Example 3 27:30 
    Relative Solubilities 31:04 
  Solubility Equilibria, Part II 42:06
   Intro 0:00 
   Solubility Equilibria 0:46 
    Common Ion Effect 0:47 
    Example 1 3:14 
    pH & Solubility 13:00 
    Example of pH & Solubility 15:25 
    Example 2 23:06 
    Precipitation & Definition of the Ion Product 26:48 
    If Q > Ksp 29:31 
    If Q < Ksp 30:27 
    Example 3 32:58 
  Solubility Equilibria, Part III 43:09
   Intro 0:00 
   Solubility Equilibria 0:55 
    Example 1: Question 0:56 
    Example 1: Step 1 - Check to See if Anything Precipitates 2:52 
    Example 1: Step 2 - Stoichiometry 10:47 
    Example 1: Step 3 - Equilibrium 16:34 
    Example 2: Selective Precipitation (Question) 21:02 
    Example 2: Solution 23:41 
    Classical Qualitative Analysis 29:44 
    Groups: 1-5 38:44 

IX. Complex Ions

  Complex Ion Equilibria 43:38
   Intro 0:00 
   Complex Ion Equilibria 0:32 
    Complex Ion 0:34 
    Ligan Examples 1:51 
    Ligand Definition 3:12 
    Coordination 6:28 
    Example 1 8:08 
    Example 2 19:13 
  Complex Ions & Solubility 31:30
   Intro 0:00 
   Complex Ions and Solubility 0:23 
    Recall: Classical Qualitative Analysis 0:24 
    Example 1 6:10 
    Example 2 16:16 
    Dissolving a Water-Insoluble Ionic Compound: Method 1 23:38 
    Dissolving a Water-Insoluble Ionic Compound: Method 2 28:13 

X. Chemical Thermodynamics

  Spontaneity, Entropy, & Free Energy, Part I 56:28
   Intro 0:00 
   Spontaneity, Entropy, Free Energy 2:25 
    Energy Overview 2:26 
    Equation: ∆E = q + w 4:30 
    State Function/ State Property 8:35 
    Equation: w = -P∆V 12:00 
    Enthalpy: H = E + PV 14:50 
    Enthalpy is a State Property 17:33 
    Exothermic and Endothermic Reactions 19:20 
    First Law of Thermodynamic 22:28 
    Entropy 25:48 
    Spontaneous Process 33:53 
    Second Law of Thermodynamic 36:51 
    More on Entropy 42:23 
    Example 43:55 
  Spontaneity, Entropy, & Free Energy, Part II 39:55
   Intro 0:00 
   Spontaneity, Entropy, Free Energy 1:30 
    ∆S of Universe = ∆S of System + ∆S of Surrounding 1:31 
    Convention 3:32 
    Examining a System 5:36 
    Thermodynamic Property: Sign of ∆S 16:52 
    Thermodynamic Property: Magnitude of ∆S 18:45 
    Deriving Equation: ∆S of Surrounding = -∆H / T 20:25 
    Example 1 25:51 
    Free Energy Equations 29:22 
  Spontaneity, Entropy, & Free Energy, Part III 30:10
   Intro 0:00 
   Spontaneity, Entropy, Free Energy 0:11 
    Example 1 2:38 
    Key Concept of Example 1 14:06 
    Example 2 15:56 
    Units for ∆H, ∆G, and S 20:56 
    ∆S of Surrounding & ∆S of System 22:00 
    Reaction Example 24:17 
    Example 3 26:52 
  Spontaneity, Entropy, & Free Energy, Part IV 30:07
   Intro 0:00 
   Spontaneity, Entropy, Free Energy 0:29 
    Standard Free Energy of Formation 0:58 
    Example 1 4:34 
    Reaction Under Non-standard Conditions 13:23 
    Example 2 16:26 
    ∆G = Negative 22:12 
    ∆G = 0 24:38 
    Diagram Example of ∆G 26:43 
  Spontaneity, Entropy, & Free Energy, Part V 44:56
   Intro 0:00 
   Spontaneity, Entropy, Free Energy 0:56 
    Equations: ∆G of Reaction, ∆G°, and K 0:57 
    Example 1: Question 6:50 
    Example 1: Part A 9:49 
    Example 1: Part B 15:28 
    Example 2 17:33 
    Example 3 23:31 
    lnK = (- ∆H° ÷ R) ( 1 ÷ T) + ( ∆S° ÷ R) 31:36 
    Maximum Work 35:57 

XI. Electrochemistry

  Oxidation-Reduction & Balancing 39:23
   Intro 0:00 
   Oxidation-Reduction and Balancing 2:06 
    Definition of Electrochemistry 2:07 
    Oxidation and Reduction Review 3:05 
    Example 1: Assigning Oxidation State 10:15 
    Example 2: Is the Following a Redox Reaction? 18:06 
    Example 3: Step 1 - Write the Oxidation & Reduction Half Reactions 22:46 
    Example 3: Step 2 - Balance the Reaction 26:44 
    Example 3: Step 3 - Multiply 30:11 
    Example 3: Step 4 - Add 32:07 
    Example 3: Step 5 - Check 33:29 
  Galvanic Cells 43:09
   Intro 0:00 
   Galvanic Cells 0:39 
    Example 1: Balance the Following Under Basic Conditions 0:40 
    Example 1: Steps to Balance Reaction Under Basic Conditions 3:25 
    Example 1: Solution 5:23 
    Example 2: Balance the Following Reaction 13:56 
    Galvanic Cells 18:15 
    Example 3: Galvanic Cells 28:19 
    Example 4: Galvanic Cells 35:12 
  Cell Potential 48:41
   Intro 0:00 
   Cell Potential 2:08 
    Definition of Cell Potential 2:17 
    Symbol and Unit 5:50 
    Standard Reduction Potential 10:16 
    Example Figure 1 13:08 
    Example Figure 2 19:00 
    All Reduction Potentials are Written as Reduction 23:10 
    Cell Potential: Important Fact 1 26:49 
    Cell Potential: Important Fact 2 27:32 
    Cell Potential: Important Fact 3 28:54 
    Cell Potential: Important Fact 4 30:05 
    Example Problem 1 32:29 
    Example Problem 2 38:38 
  Potential, Work, & Free Energy 41:23
   Intro 0:00 
   Potential, Work, Free Energy 0:42 
    Descriptions of Galvanic Cell 0:43 
    Line Notation 5:33 
    Example 1 6:26 
    Example 2 11:15 
    Example 3 15:18 
    Equation: Volt 22:20 
    Equations: Cell Potential, Work, and Charge 28:30 
    Maximum Cell Potential is Related to the Free Energy of the Cell Reaction 35:09 
    Example 4 37:42 
  Cell Potential & Concentration 34:19
   Intro 0:00 
   Cell Potential & Concentration 0:29 
    Example 1: Question 0:30 
    Example 1: Nernst Equation 4:43 
    Example 1: Solution 7:01 
    Cell Potential & Concentration 11:27 
    Example 2 16:38 
    Manipulating the Nernst Equation 25:15 
    Example 3 28:43 
  Electrolysis 33:21
   Intro 0:00 
   Electrolysis 3:16 
    Electrolysis: Part 1 3:17 
    Electrolysis: Part 2 5:25 
    Galvanic Cell Example 7:13 
    Nickel Cadmium Battery 12:18 
    Ampere 16:00 
    Example 1 20:47 
    Example 2 25:47 

XII. Light

  Light 44:45
   Intro 0:00 
   Light 2:14 
    Introduction to Light 2:15 
    Frequency, Speed, and Wavelength of Waves 3:58 
    Units and Equations 7:37 
    Electromagnetic Spectrum 12:13 
    Example 1: Calculate the Frequency 17:41 
    E = hν 21:30 
    Example 2: Increment of Energy 25:12 
    Photon Energy of Light 28:56 
    Wave and Particle 31:46 
    Example 3: Wavelength of an Electron 34:46 

XIII. Quantum Mechanics

  Quantum Mechanics & Electron Orbitals 54:00
   Intro 0:00 
   Quantum Mechanics & Electron Orbitals 0:51 
    Quantum Mechanics & Electron Orbitals Overview 0:52 
    Electron Orbital and Energy Levels for the Hydrogen Atom 8:47 
    Example 1 13:41 
    Quantum Mechanics: Schrodinger Equation 19:19 
    Quantum Numbers Overview 31:10 
    Principal Quantum Numbers 33:28 
    Angular Momentum Numbers 34:55 
    Magnetic Quantum Numbers 36:35 
    Spin Quantum Numbers 37:46 
    Primary Level, Sublevels, and Sub-Sub-Levels 39:42 
    Example 42:17 
    Orbital & Quantum Numbers 49:32 
  Electron Configurations & Diagrams 34:04
   Intro 0:00 
   Electron Configurations & Diagrams 1:08 
    Electronic Structure of Ground State Atom 1:09 
    Order of Electron Filling 3:50 
    Electron Configurations & Diagrams: H 8:41 
    Electron Configurations & Diagrams: He 9:12 
    Electron Configurations & Diagrams: Li 9:47 
    Electron Configurations & Diagrams: Be 11:17 
    Electron Configurations & Diagrams: B 12:05 
    Electron Configurations & Diagrams: C 13:03 
    Electron Configurations & Diagrams: N 14:55 
    Electron Configurations & Diagrams: O 15:24 
    Electron Configurations & Diagrams: F 16:25 
    Electron Configurations & Diagrams: Ne 17:00 
    Electron Configurations & Diagrams: S 18:08 
    Electron Configurations & Diagrams: Fe 20:08 
    Introduction to Valence Electrons 23:04 
    Valence Electrons of Oxygen 23:44 
    Valence Electrons of Iron 24:02 
    Valence Electrons of Arsenic 24:30 
    Valence Electrons: Exceptions 25:36 
    The Periodic Table 27:52 

XIV. Intermolecular Forces

  Vapor Pressure & Changes of State 52:43
   Intro 0:00 
   Vapor Pressure and Changes of State 2:26 
    Intermolecular Forces Overview 2:27 
    Hydrogen Bonding 5:23 
    Heat of Vaporization 9:58 
    Vapor Pressure: Definition and Example 11:04 
    Vapor Pressures is Mostly a Function of Intermolecular Forces 17:41 
    Vapor Pressure Increases with Temperature 20:52 
    Vapor Pressure vs. Temperature: Graph and Equation 22:55 
    Clausius-Clapeyron Equation 31:55 
    Example 1 32:13 
    Heating Curve 35:40 
    Heat of Fusion 41:31 
    Example 2 43:45 
  Phase Diagrams & Solutions 31:17
   Intro 0:00 
   Phase Diagrams and Solutions 0:22 
    Definition of a Phase Diagram 0:50 
    Phase Diagram Part 1: H₂O 1:54 
    Phase Diagram Part 2: CO₂ 9:59 
    Solutions: Solute & Solvent 16:12 
    Ways of Discussing Solution Composition: Mass Percent or Weight Percent 18:46 
    Ways of Discussing Solution Composition: Molarity 20:07 
    Ways of Discussing Solution Composition: Mole Fraction 20:48 
    Ways of Discussing Solution Composition: Molality 21:41 
    Example 1: Question 22:06 
    Example 1: Mass Percent 24:32 
    Example 1: Molarity 25:53 
    Example 1: Mole Fraction 28:09 
    Example 1: Molality 29:36 
  Vapor Pressure of Solutions 37:23
   Intro 0:00 
   Vapor Pressure of Solutions 2:07 
    Vapor Pressure & Raoult's Law 2:08 
    Example 1 5:21 
    When Ionic Compounds Dissolve 10:51 
    Example 2 12:38 
    Non-Ideal Solutions 17:42 
    Negative Deviation 24:23 
    Positive Deviation 29:19 
    Example 3 31:40 
  Colligatives Properties 34:11
   Intro 0:00 
   Colligative Properties 1:07 
    Boiling Point Elevation 1:08 
    Example 1: Question 5:19 
    Example 1: Solution 6:52 
    Freezing Point Depression 12:01 
    Example 2: Question 14:46 
    Example 2: Solution 16:34 
    Osmotic Pressure 20:20 
    Example 3: Question 28:00 
    Example 3: Solution 30:16 

XV. Bonding

  Bonding & Lewis Structure 48:39
   Intro 0:00 
   Bonding & Lewis Structure 2:23 
    Covalent Bond 2:24 
    Single Bond, Double Bond, and Triple Bond 4:11 
    Bond Length & Intermolecular Distance 5:51 
    Definition of Electronegativity 8:42 
    Bond Polarity 11:48 
    Bond Energy 20:04 
    Example 1 24:31 
    Definition of Lewis Structure 31:54 
    Steps in Forming a Lewis Structure 33:26 
    Lewis Structure Example: H₂ 36:53 
    Lewis Structure Example: CH₄ 37:33 
    Lewis Structure Example: NO⁺ 38:43 
    Lewis Structure Example: PCl₅ 41:12 
    Lewis Structure Example: ICl₄⁻ 43:05 
    Lewis Structure Example: BeCl₂ 45:07 
  Resonance & Formal Charge 36:59
   Intro 0:00 
   Resonance and Formal Charge 0:09 
    Resonance Structures of NO₃⁻ 0:25 
    Resonance Structures of NO₂⁻ 12:28 
    Resonance Structures of HCO₂⁻ 16:28 
    Formal Charge 19:40 
    Formal Charge Example: SO₄²⁻ 21:32 
    Formal Charge Example: CO₂ 31:33 
    Formal Charge Example: HCN 32:44 
    Formal Charge Example: CN⁻ 33:34 
    Formal Charge Example: 0₃ 34:43 
  Shapes of Molecules 41:21
   Intro 0:00 
   Shapes of Molecules 0:35 
    VSEPR 0:36 
    Steps in Determining Shapes of Molecules 6:18 
    Linear 11:38 
    Trigonal Planar 11:55 
    Tetrahedral 12:45 
    Trigonal Bipyramidal 13:23 
    Octahedral 14:29 
    Table: Shapes of Molecules 15:40 
    Example: CO₂ 21:11 
    Example: NO₃⁻ 24:01 
    Example: H₂O 27:00 
    Example: NH₃ 29:48 
    Example: PCl₃⁻ 32:18 
    Example: IF₄⁺ 34:38 
    Example: KrF₄ 37:57 
  Hybrid Orbitals 40:17
   Intro 0:00 
   Hybrid Orbitals 0:13 
    Introduction to Hybrid Orbitals 0:14 
    Electron Orbitals for CH₄ 5:02 
    sp³ Hybridization 10:52 
    Example: sp³ Hybridization 12:06 
    sp² Hybridization 14:21 
    Example: sp² Hybridization 16:11 
    σ Bond 19:10 
    π Bond 20:07 
    sp Hybridization & Example 22:00 
    dsp³ Hybridization & Example 27:36 
    d²sp³ Hybridization & Example 30:36 
    Example: Predict the Hybridization and Describe the Molecular Geometry of CO 32:31 
    Example: Predict the Hybridization and Describe the Molecular Geometry of BF₄⁻ 35:17 
    Example: Predict the Hybridization and Describe the Molecular Geometry of XeF₂ 37:09 

XVI. AP Practice Exam

  AP Practice Exam: Multiple Choice, Part I 52:34
   Intro 0:00 
   Multiple Choice 1:21 
    Multiple Choice 1 1:22 
    Multiple Choice 2 2:23 
    Multiple Choice 3 3:38 
    Multiple Choice 4 4:34 
    Multiple Choice 5 5:16 
    Multiple Choice 6 5:41 
    Multiple Choice 7 6:20 
    Multiple Choice 8 7:03 
    Multiple Choice 9 7:31 
    Multiple Choice 10 9:03 
    Multiple Choice 11 11:52 
    Multiple Choice 12 13:16 
    Multiple Choice 13 13:56 
    Multiple Choice 14 14:52 
    Multiple Choice 15 15:43 
    Multiple Choice 16 16:20 
    Multiple Choice 17 16:55 
    Multiple Choice 18 17:22 
    Multiple Choice 19 18:59 
    Multiple Choice 20 20:24 
    Multiple Choice 21 22:20 
    Multiple Choice 22 23:29 
    Multiple Choice 23 24:30 
    Multiple Choice 24 25:24 
    Multiple Choice 25 26:21 
    Multiple Choice 26 29:06 
    Multiple Choice 27 30:42 
    Multiple Choice 28 33:28 
    Multiple Choice 29 34:38 
    Multiple Choice 30 35:37 
    Multiple Choice 31 37:31 
    Multiple Choice 32 38:28 
    Multiple Choice 33 39:50 
    Multiple Choice 34 42:57 
    Multiple Choice 35 44:18 
    Multiple Choice 36 45:52 
    Multiple Choice 37 48:02 
    Multiple Choice 38 49:25 
    Multiple Choice 39 49:43 
    Multiple Choice 40 50:16 
    Multiple Choice 41 50:49 
  AP Practice Exam: Multiple Choice, Part II 32:15
   Intro 0:00 
   Multiple Choice 0:12 
    Multiple Choice 42 0:13 
    Multiple Choice 43 0:33 
    Multiple Choice 44 1:16 
    Multiple Choice 45 2:36 
    Multiple Choice 46 5:22 
    Multiple Choice 47 6:35 
    Multiple Choice 48 8:02 
    Multiple Choice 49 10:05 
    Multiple Choice 50 10:26 
    Multiple Choice 51 11:07 
    Multiple Choice 52 12:01 
    Multiple Choice 53 12:55 
    Multiple Choice 54 16:12 
    Multiple Choice 55 18:11 
    Multiple Choice 56 19:45 
    Multiple Choice 57 20:15 
    Multiple Choice 58 23:28 
    Multiple Choice 59 24:27 
    Multiple Choice 60 26:45 
    Multiple Choice 61 29:15 
  AP Practice Exam: Multiple Choice, Part III 32:50
   Intro 0:00 
   Multiple Choice 0:16 
    Multiple Choice 62 0:17 
    Multiple Choice 63 1:57 
    Multiple Choice 64 6:16 
    Multiple Choice 65 8:05 
    Multiple Choice 66 9:18 
    Multiple Choice 67 10:38 
    Multiple Choice 68 12:51 
    Multiple Choice 69 14:32 
    Multiple Choice 70 17:35 
    Multiple Choice 71 22:44 
    Multiple Choice 72 24:27 
    Multiple Choice 73 27:46 
    Multiple Choice 74 29:39 
    Multiple Choice 75 30:23 
  AP Practice Exam: Free response Part I 47:22
   Intro 0:00 
   Free Response 0:15 
    Free Response 1: Part A 0:16 
    Free Response 1: Part B 4:15 
    Free Response 1: Part C 5:47 
    Free Response 1: Part D 9:20 
    Free Response 1: Part E. i 10:58 
    Free Response 1: Part E. ii 16:45 
    Free Response 1: Part E. iii 26:03 
    Free Response 2: Part A. i 31:01 
    Free Response 2: Part A. ii 33:38 
    Free Response 2: Part A. iii 35:20 
    Free Response 2: Part B. i 37:38 
    Free Response 2: Part B. ii 39:30 
    Free Response 2: Part B. iii 44:44 
  AP Practice Exam: Free Response Part II 43:05
   Intro 0:00 
   Free Response 0:12 
    Free Response 3: Part A 0:13 
    Free Response 3: Part B 6:25 
    Free Response 3: Part C. i 11:33 
    Free Response 3: Part C. ii 12:02 
    Free Response 3: Part D 14:30 
    Free Response 4: Part A 21:03 
    Free Response 4: Part B 22:59 
    Free Response 4: Part C 24:33 
    Free Response 4: Part D 27:22 
    Free Response 4: Part E 28:43 
    Free Response 4: Part F 29:35 
    Free Response 4: Part G 30:15 
    Free Response 4: Part H 30:48 
    Free Response 5: Diagram 32:00 
    Free Response 5: Part A 34:14 
    Free Response 5: Part B 36:07 
    Free Response 5: Part C 37:45 
    Free Response 5: Part D 39:00 
    Free Response 5: Part E 40:26 
  AP Practice Exam: Free Response Part III 28:36
   Intro 0:00 
   Free Response 0:43 
    Free Response 6: Part A. i 0:44 
    Free Response 6: Part A. ii 3:08 
    Free Response 6: Part A. iii 5:02 
    Free Response 6: Part B. i 7:11 
    Free Response 6: Part B. ii 9:40 
    Free Response 7: Part A 11:14 
    Free Response 7: Part B 13:45 
    Free Response 7: Part C 15:43 
    Free Response 7: Part D 16:54 
    Free Response 8: Part A. i 19:15 
    Free Response 8: Part A. ii 21:16 
    Free Response 8: Part B. i 23:51 
    Free Response 8: Part B. ii 25:07 

Duration: 60 hours, 26 minutes

Number of Lessons: 70

This online course is geared towards high school students taking the AP Chemistry exam, but is also suitable for college students taking introductory chemistry. Lessons go in-depth with real world examples to help you understand what is occurring at the molecular level. In addition to covering all AP and first-year college chemistry topics, Professor Hovasapian also dispenses useful tips and strategies while working out a previous AP exam.

Additional Features:

  • Free Sample Lessons
  • Closed Captioning (CC)
  • Downloadable Lecture Slides
  • Instructor Comments

Topics Include:

  • Stoichiometry
  • Oxidation Reduction Reactions
  • Gases
  • Enthalpy & Hess’s Law
  • Initial Rates
  • Equilibrium
  • Acids & Bases
  • Solubility
  • Complex Ions
  • Thermodynamics
  • Cell Potential
  • Light
  • Quantum Mechanics
  • Phase Diagrams
  • Shapes of Molecules
  • Sample AP Exam

With his 15+ years teaching and tutoring experience coupled with triple majors in Chemistry, Mathematics, and Classics, Raffi explains difficult chemistry concepts through essential theory followed by plenty of worked out examples. Be sure to check out his other math & science courses on Educator!

Student Testimonials:

“I am writing this comment to thank you for this AP Chemistry lecture series. I was going  to merely learn some basic chemical principles when I started this series last summer, but I ended up changing my mind about my future majors because of these lectures. I checked my AP scores for chemistry today and I got a 5 on it. Now I am planning to get a degree in chemistry (or some related field such as engineering), and I thank you for your effort to teach chemistry as clearly as possible so that people can appreciate this subject.” — Jinbin C.

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