Raffi Hovasapian
Naming Compounds
Slide Duration:Table of Contents
41m 24s
- Intro0:00
- Periodic Table of Elements0:15
- Naming Compounds3:13
- Definition and Examples of Ions3:14
- Ionic (Symbol to Name): NaCl5:23
- Ionic (Name to Symbol): Calcium Oxide7:58
- Ionic - Polyatoms Anions: Examples12:45
- Ionic - Polyatoms Anions (Symbol to Name): KClO14:50
- Ionic - Polyatoms Anions (Name to Symbol): Potassium Phosphate15:49
- Ionic Compounds Involving Transition Metals (Symbol to Name): Co₂(CO₃)₃20:48
- Ionic Compounds Involving Transition Metals (Name to Symbol): Palladium 2 Acetate22:44
- Naming Covalent Compounds (Symbol to Name): CO26:21
- Naming Covalent Compounds (Name to Symbol): Nitrogen Trifluoride27:34
- Naming Covalent Compounds (Name to Symbol): Dichlorine Monoxide27:57
- Naming Acids Introduction28:11
- Naming Acids (Name to Symbol): Chlorous Acid35:08
- % Composition by Mass Example37:38
37m 19s
- Intro0:00
- Stoichiometry0:25
- Introduction to Stoichiometry0:26
- Example 15:03
- Example 210:17
- Example 315:09
- Example 424:02
- Example 5: Questions28:11
- Example 5: Part A - Limiting Reactant30:30
- Example 5: Part B32:27
- Example 5: Part C35:00
31m 14s
- Intro0:00
- Precipitation Reactions0:53
- Dissociation of ionic Compounds0:54
- Solubility Guidelines for ionic Compounds: Soluble Ionic Compounds8:15
- Solubility Guidelines for ionic Compounds: Insoluble ionic Compounds12:56
- Precipitation Reactions14:08
- Example 1: Mixing a Solution of BaCl₂ & K₂SO₄21:21
- Example 2: Mixing a Solution of Mg(NO₃)₂ & KI26:10
43m 21s
- Intro0:00
- Acid-Base Reactions1:00
- Introduction to Acid: Monoprotic Acid and Polyprotic Acid1:01
- Introduction to Base8:28
- Neutralization11:45
- Example 116:17
- Example 221:55
- Molarity24:50
- Example 326:50
- Example 430:01
- Example 4: Limiting Reactant37:51
- Example 4: Reaction Part40:01
47m 58s
- Intro0:00
- Oxidation Reduction Reactions0:26
- Oxidation and Reduction Overview0:27
- How Can One Tell Whether Oxidation-Reduction has Taken Place?7:13
- Rules for Assigning Oxidation State: Number 111:22
- Rules for Assigning Oxidation State: Number 212:46
- Rules for Assigning Oxidation State: Number 313:25
- Rules for Assigning Oxidation State: Number 414:50
- Rules for Assigning Oxidation State: Number 515:41
- Rules for Assigning Oxidation State: Number 617:00
- Example 1: Determine the Oxidation State of Sulfur in the Following Compounds18:20
- Activity Series and Reduction Properties25:32
- Activity Series and Reduction Properties25:33
- Example 2: Write the Balance Molecular, Total Ionic, and Net Ionic Equations for Al + HCl31:37
- Example 334:25
- Example 437:55
31m 50s
- Intro0:00
- Stoichiometry Example 10:36
- Example 1: Question and Answer0:37
- Stoichiometry Example 26:57
- Example 2: Questions6:58
- Example 2: Part A Solution12:16
- Example 2: Part B Solution13:05
- Example 2: Part C Solution14:00
- Example 2: Part D Solution14:38
- Stoichiometry Example 317:56
- Example 3: Questions17:57
- Example 3: Part A Solution19:51
- Example 3: Part B Solution21:43
- Example 3: Part C Solution26:46
49m 40s
- Intro0:00
- Pressure0:22
- Pressure Overview0:23
- Torricelli: Barometer4:35
- Measuring Gas Pressure in a Container7:49
- Boyle's Law12:40
- Example 116:56
- Gas Laws21:18
- Gas Laws21:19
- Avogadro's Law26:16
- Example 231:47
- Ideal Gas Equation38:20
- Standard Temperature and Pressure (STP)38:21
- Example 340:43
32m
- Intro0:00
- Gases0:27
- Gases0:28
- Mole Fractions5:52
- Vapor Pressure8:22
- Example 113:25
- Example 222:45
31m 58s
- Intro0:00
- Kinetic Molecular Theory and Real Gases0:45
- Kinetic Molecular Theory 10:46
- Kinetic Molecular Theory 24:23
- Kinetic Molecular Theory 35:42
- Kinetic Molecular Theory 46:27
- Equations7:52
- Effusion11:15
- Diffusion13:30
- Example 119:54
- Example 223:23
- Example 326:45
25m 34s
- Intro0:00
- Example 10:34
- Example 10:35
- Example 26:15
- Example 2: Part A6:16
- Example 2: Part B8:46
- Example 2: Part C10:30
- Example 2: Part D11:15
- Example 2: Part E12:20
- Example 2: Part F13:22
- Example 314:45
- Example 314:46
- Example 418:16
- Example 418:17
- Example 521:04
- Example 521:05
37m 32s
- Intro0:00
- Thermochemistry0:25
- Temperature and Heat0:26
- Work3:07
- System, Surroundings, Exothermic Process, and Endothermic Process8:19
- Work & Gas: Expansion and Compression16:30
- Example 124:41
- Example 227:47
- Example 331:58
32m 34s
- Intro0:00
- Thermochemistry1:43
- Defining Enthalpy & Hess's Law1:44
- Example 16:48
- State Function13:11
- Example 217:15
- Example 324:09
23m 9s
- Intro0:00
- Thermochemistry1:04
- Standard Enthalpy of Formation: Definition & Equation1:05
- ∆H of Formation10:00
- Example 111:22
- Example 219:00
39m 28s
- Intro0:00
- Thermochemistry0:21
- Heat Capacity0:22
- Molar Heat Capacity4:44
- Constant Pressure Calorimetry5:50
- Example 112:24
- Constant Volume Calorimetry21:54
- Example 224:40
- Example 331:03
36m 24s
- Intro0:00
- Kinetics2:18
- Rate: 2 NO₂ (g) → 2NO (g) + O₂ (g)2:19
- Reaction Rates Graph7:25
- Time Interval & Average Rate13:13
- Instantaneous Rate15:13
- Rate of Reaction is Proportional to Some Power of the Reactant Concentrations23:49
- Example 127:19
30m 48s
- Intro0:00
- Kinetics0:33
- Rate0:34
- Idea2:24
- Example 1: NH₄⁺ + NO₂⁻ → NO₂ (g) + 2 H₂O5:36
- Example 2: BrO₃⁻ + 5 Br⁻ + 6 H⁺ → 3 Br₂ + 3 H₂O19:29
32m 17s
- Intro0:00
- Kinetics0:52
- Integrated Rate Law0:53
- Example 16:26
- Example 215:19
- Half-life of a Reaction20:40
- Example 3: Part A25:41
- Example 3: Part B28:01
26m 40s
- Intro0:00
- Kinetics0:22
- Second Order0:23
- Example 16:08
- Zero-Order16:36
- Summary for the Kinetics Associated with the Reaction21:27
40m 59s
- Intro0:00
- Kinetics0:53
- Rate Constant0:54
- Collision Model2:45
- Activation Energy5:11
- Arrhenius Proposed9:54
- 2 Requirements for a Successful Reaction15:39
- Rate Constant17:53
- Arrhenius Equation19:51
- Example 125:00
- Activation Energy & the Values of K32:12
- Example 236:46
29m 8s
- Intro0:00
- Kinetics0:43
- Example 10:44
- Example 26:53
- Example 38:58
- Example 411:36
- Example 516:36
- Example 6: Part A21:00
- Example 6: Part B25:09
46m
- Intro0:00
- Equilibrium1:32
- Introduction to Equilibrium1:33
- Equilibrium Rules14:00
- Example 1: Part A16:46
- Example 1: Part B18:48
- Example 1: Part C22:13
- Example 1: Part D24:55
- Example 2: Part A27:46
- Example 2: Part B31:22
- Example 2: Part C33:00
- Reverse a Reaction36:04
- Example 337:24
40m 53s
- Intro0:00
- Equilibrium1:31
- Equilibriums Involving Gases1:32
- General Equation10:11
- Example 1: Question11:55
- Example 1: Answer13:43
- Example 2: Question19:08
- Example 2: Answer21:37
- Example 3: Question33:40
- Example 3: Answer35:24
45m 53s
- Intro0:00
- Equilibrium0:57
- Reaction Quotient0:58
- If Q > K5:37
- If Q < K6:52
- If Q = K7:45
- Example 1: Part A8:24
- Example 1: Part B13:11
- Example 2: Question20:04
- Example 2: Answer22:15
- Example 3: Question30:54
- Example 3: Answer32:52
- Steps in Solving Equilibrium Problems42:40
31m 51s
- Intro0:00
- Equilibrium1:09
- Example 1: Question1:10
- Example 1: Answer4:15
- Example 2: Question13:04
- Example 2: Answer15:20
- Example 3: Question25:03
- Example 3: Answer26:32
40m 52s
- Intro0:00
- Le Chatelier1:05
- Le Chatelier Principle1:06
- Concentration: Add 'x'5:25
- Concentration: Subtract 'x'7:50
- Example 19:44
- Change in Pressure12:53
- Example 220:40
- Temperature: Exothermic and Endothermic24:33
- Example 329:55
- Example 435:30
50m 11s
- Intro0:00
- Acids and Bases1:14
- Bronsted-Lowry Acid-Base Model1:28
- Reaction of an Acid with Water4:36
- Acid Dissociation10:51
- Acid Strength13:48
- Example 121:22
- Water as an Acid & a Base25:25
- Example 2: Part A32:30
- Example 2: Part B34:47
- Example 3: Part A35:58
- Example 3: Part B39:33
- pH Scale41:12
- Example 443:56
43m 52s
- Intro0:00
- pH of Weak Acid Solutions1:12
- pH of Weak Acid Solutions1:13
- Example 16:26
- Example 214:25
- Example 324:23
- Example 430:38
43m 4s
- Intro0:00
- Bases0:33
- Percent Dissociation: Strong & Weak Bases0:45
- Example 16:23
- Strong Base Dissociation11:24
- Example 213:02
- Weak Acid and General Reaction17:38
- Example: NaOH → Na⁺ + OH⁻20:30
- Strong Base and Weak Base23:49
- Example 424:54
- Example 533:51
35m 34s
- Intro0:00
- Polyprotic Acids1:04
- Acids Dissociation1:05
- Example 14:51
- Example 217:30
- Example 331:11
41m 14s
- Intro0:00
- Salts and Their Acid-Base Properties0:11
- Salts and Their Acid-Base Properties0:15
- Example 17:58
- Example 214:00
- Metal Ion and Acidic Solution22:00
- Example 328:35
- NH₄F → NH₄⁺ + F⁻34:05
- Example 438:03
41m 58s
- Intro0:00
- Common Ion Effect & Buffers1:16
- Covalent Oxides Produce Acidic Solutions in Water1:36
- Ionic Oxides Produce Basic Solutions in Water4:15
- Practice Example 16:10
- Practice Example 29:00
- Definition12:27
- Example 1: Part A16:49
- Example 1: Part B19:54
- Buffer Solution25:10
- Example of Some Buffers: HF and NaF30:02
- Example of Some Buffers: Acetic Acid & Potassium Acetate31:34
- Example of Some Buffers: CH₃NH₂ & CH₃NH₃Cl33:54
- Example 2: Buffer Solution36:36
32m 24s
- Intro0:00
- Buffers1:20
- Buffer Solution1:21
- Adding Base5:03
- Adding Acid7:14
- Example 1: Question9:48
- Example 1: Recall12:08
- Example 1: Major Species Upon Addition of NaOH16:10
- Example 1: Equilibrium, ICE Chart, and Final Calculation24:33
- Example 1: Comparison29:19
40m 6s
- Intro0:00
- Buffers1:27
- Example 1: Question1:32
- Example 1: ICE Chart3:15
- Example 1: Major Species Upon Addition of OH⁻, But Before Rxn7:23
- Example 1: Equilibrium, ICE Chart, and Final Calculation12:51
- Summary17:21
- Another Look at Buffering & the Henderson-Hasselbalch equation19:00
- Example 227:08
- Example 332:01
38m 43s
- Intro0:00
- Buffers0:25
- Buffer Capacity Part 10:26
- Example 14:10
- Buffer Capacity Part 219:29
- Example 225:12
- Example 332:02
42m 42s
- Intro0:00
- Titrations: Strong Acid and Strong Base1:11
- Definition of Titration1:12
- Sample Problem3:33
- Definition of Titration Curve or pH Curve9:46
- Scenario 1: Strong Acid- Strong Base Titration11:00
- Question11:01
- Part 1: No NaOH is Added14:00
- Part 2: 10.0 mL of NaOH is Added15:50
- Part 3: Another 10.0 mL of NaOH & 20.0 mL of NaOH are Added22:19
- Part 4: 50.0 mL of NaOH is Added26:46
- Part 5: 100.0 mL (Total) of NaOH is Added27:26
- Part 6: 150.0 mL (Total) of NaOH is Added32:06
- Part 7: 200.0 mL of NaOH is Added35:07
- Titrations Curve for Strong Acid and Strong Base35:43
42m 3s
- Intro0:00
- Titrations: Weak Acid and Strong Base0:43
- Question0:44
- Part 1: No NaOH is Added1:54
- Part 2: 10.0 mL of NaOH is Added5:17
- Part 3: 25.0 mL of NaOH is Added14:01
- Part 4: 40.0 mL of NaOH is Added21:55
- Part 5: 50.0 mL (Total) of NaOH is Added22:25
- Part 6: 60.0 mL (Total) of NaOH is Added31:36
- Part 7: 75.0 mL (Total) of NaOH is Added35:44
- Titration Curve36:09
52m 3s
- Intro0:00
- Examples and Indicators0:25
- Example 1: Question0:26
- Example 1: Solution2:03
- Example 2: Question12:33
- Example 2: Solution14:52
- Example 3: Question23:45
- Example 3: Solution25:09
- Acid/Base Indicator Overview34:45
- Acid/Base Indicator Example37:40
- Acid/Base Indicator General Result47:11
- Choosing Acid/Base Indicator49:12
36m 25s
- Intro0:00
- Solubility Equilibria0:48
- Solubility Equilibria Overview0:49
- Solubility Product Constant4:24
- Definition of Solubility9:10
- Definition of Solubility Product11:28
- Example 114:09
- Example 220:19
- Example 327:30
- Relative Solubilities31:04
42m 6s
- Intro0:00
- Solubility Equilibria0:46
- Common Ion Effect0:47
- Example 13:14
- pH & Solubility13:00
- Example of pH & Solubility15:25
- Example 223:06
- Precipitation & Definition of the Ion Product26:48
- If Q > Ksp29:31
- If Q < Ksp30:27
- Example 332:58
43m 9s
- Intro0:00
- Solubility Equilibria0:55
- Example 1: Question0:56
- Example 1: Step 1 - Check to See if Anything Precipitates2:52
- Example 1: Step 2 - Stoichiometry10:47
- Example 1: Step 3 - Equilibrium16:34
- Example 2: Selective Precipitation (Question)21:02
- Example 2: Solution23:41
- Classical Qualitative Analysis29:44
- Groups: 1-538:44
43m 38s
- Intro0:00
- Complex Ion Equilibria0:32
- Complex Ion0:34
- Ligan Examples1:51
- Ligand Definition3:12
- Coordination6:28
- Example 18:08
- Example 219:13
31m 30s
- Intro0:00
- Complex Ions and Solubility0:23
- Recall: Classical Qualitative Analysis0:24
- Example 16:10
- Example 216:16
- Dissolving a Water-Insoluble Ionic Compound: Method 123:38
- Dissolving a Water-Insoluble Ionic Compound: Method 228:13
56m 28s
- Intro0:00
- Spontaneity, Entropy, Free Energy2:25
- Energy Overview2:26
- Equation: ∆E = q + w4:30
- State Function/ State Property8:35
- Equation: w = -P∆V12:00
- Enthalpy: H = E + PV14:50
- Enthalpy is a State Property17:33
- Exothermic and Endothermic Reactions19:20
- First Law of Thermodynamic22:28
- Entropy25:48
- Spontaneous Process33:53
- Second Law of Thermodynamic36:51
- More on Entropy42:23
- Example43:55
39m 55s
- Intro0:00
- Spontaneity, Entropy, Free Energy1:30
- ∆S of Universe = ∆S of System + ∆S of Surrounding1:31
- Convention3:32
- Examining a System5:36
- Thermodynamic Property: Sign of ∆S16:52
- Thermodynamic Property: Magnitude of ∆S18:45
- Deriving Equation: ∆S of Surrounding = -∆H / T20:25
- Example 125:51
- Free Energy Equations29:22
30m 10s
- Intro0:00
- Spontaneity, Entropy, Free Energy0:11
- Example 12:38
- Key Concept of Example 114:06
- Example 215:56
- Units for ∆H, ∆G, and S20:56
- ∆S of Surrounding & ∆S of System22:00
- Reaction Example24:17
- Example 326:52
30m 7s
- Intro0:00
- Spontaneity, Entropy, Free Energy0:29
- Standard Free Energy of Formation0:58
- Example 14:34
- Reaction Under Non-standard Conditions13:23
- Example 216:26
- ∆G = Negative22:12
- ∆G = 024:38
- Diagram Example of ∆G26:43
44m 56s
- Intro0:00
- Spontaneity, Entropy, Free Energy0:56
- Equations: ∆G of Reaction, ∆G°, and K0:57
- Example 1: Question6:50
- Example 1: Part A9:49
- Example 1: Part B15:28
- Example 217:33
- Example 323:31
- lnK = (- ∆H° ÷ R) ( 1 ÷ T) + ( ∆S° ÷ R)31:36
- Maximum Work35:57
39m 23s
- Intro0:00
- Oxidation-Reduction and Balancing2:06
- Definition of Electrochemistry2:07
- Oxidation and Reduction Review3:05
- Example 1: Assigning Oxidation State10:15
- Example 2: Is the Following a Redox Reaction?18:06
- Example 3: Step 1 - Write the Oxidation & Reduction Half Reactions22:46
- Example 3: Step 2 - Balance the Reaction26:44
- Example 3: Step 3 - Multiply30:11
- Example 3: Step 4 - Add32:07
- Example 3: Step 5 - Check33:29
43m 9s
- Intro0:00
- Galvanic Cells0:39
- Example 1: Balance the Following Under Basic Conditions0:40
- Example 1: Steps to Balance Reaction Under Basic Conditions3:25
- Example 1: Solution5:23
- Example 2: Balance the Following Reaction13:56
- Galvanic Cells18:15
- Example 3: Galvanic Cells28:19
- Example 4: Galvanic Cells35:12
48m 41s
- Intro0:00
- Cell Potential2:08
- Definition of Cell Potential2:17
- Symbol and Unit5:50
- Standard Reduction Potential10:16
- Example Figure 113:08
- Example Figure 219:00
- All Reduction Potentials are Written as Reduction23:10
- Cell Potential: Important Fact 126:49
- Cell Potential: Important Fact 227:32
- Cell Potential: Important Fact 328:54
- Cell Potential: Important Fact 430:05
- Example Problem 132:29
- Example Problem 238:38
41m 23s
- Intro0:00
- Potential, Work, Free Energy0:42
- Descriptions of Galvanic Cell0:43
- Line Notation5:33
- Example 16:26
- Example 211:15
- Example 315:18
- Equation: Volt22:20
- Equations: Cell Potential, Work, and Charge28:30
- Maximum Cell Potential is Related to the Free Energy of the Cell Reaction35:09
- Example 437:42
34m 19s
- Intro0:00
- Cell Potential & Concentration0:29
- Example 1: Question0:30
- Example 1: Nernst Equation4:43
- Example 1: Solution7:01
- Cell Potential & Concentration11:27
- Example 216:38
- Manipulating the Nernst Equation25:15
- Example 328:43
33m 21s
- Intro0:00
- Electrolysis3:16
- Electrolysis: Part 13:17
- Electrolysis: Part 25:25
- Galvanic Cell Example7:13
- Nickel Cadmium Battery12:18
- Ampere16:00
- Example 120:47
- Example 225:47
44m 45s
- Intro0:00
- Light2:14
- Introduction to Light2:15
- Frequency, Speed, and Wavelength of Waves3:58
- Units and Equations7:37
- Electromagnetic Spectrum12:13
- Example 1: Calculate the Frequency17:41
- E = hν21:30
- Example 2: Increment of Energy25:12
- Photon Energy of Light28:56
- Wave and Particle31:46
- Example 3: Wavelength of an Electron34:46
54m
- Intro0:00
- Quantum Mechanics & Electron Orbitals0:51
- Quantum Mechanics & Electron Orbitals Overview0:52
- Electron Orbital and Energy Levels for the Hydrogen Atom8:47
- Example 113:41
- Quantum Mechanics: Schrodinger Equation19:19
- Quantum Numbers Overview31:10
- Principal Quantum Numbers33:28
- Angular Momentum Numbers34:55
- Magnetic Quantum Numbers36:35
- Spin Quantum Numbers37:46
- Primary Level, Sublevels, and Sub-Sub-Levels39:42
- Example42:17
- Orbital & Quantum Numbers49:32
34m 4s
- Intro0:00
- Electron Configurations & Diagrams1:08
- Electronic Structure of Ground State Atom1:09
- Order of Electron Filling3:50
- Electron Configurations & Diagrams: H8:41
- Electron Configurations & Diagrams: He9:12
- Electron Configurations & Diagrams: Li9:47
- Electron Configurations & Diagrams: Be11:17
- Electron Configurations & Diagrams: B12:05
- Electron Configurations & Diagrams: C13:03
- Electron Configurations & Diagrams: N14:55
- Electron Configurations & Diagrams: O15:24
- Electron Configurations & Diagrams: F16:25
- Electron Configurations & Diagrams: Ne17:00
- Electron Configurations & Diagrams: S18:08
- Electron Configurations & Diagrams: Fe20:08
- Introduction to Valence Electrons23:04
- Valence Electrons of Oxygen23:44
- Valence Electrons of Iron24:02
- Valence Electrons of Arsenic24:30
- Valence Electrons: Exceptions25:36
- The Periodic Table27:52
52m 43s
- Intro0:00
- Vapor Pressure and Changes of State2:26
- Intermolecular Forces Overview2:27
- Hydrogen Bonding5:23
- Heat of Vaporization9:58
- Vapor Pressure: Definition and Example11:04
- Vapor Pressures is Mostly a Function of Intermolecular Forces17:41
- Vapor Pressure Increases with Temperature20:52
- Vapor Pressure vs. Temperature: Graph and Equation22:55
- Clausius-Clapeyron Equation31:55
- Example 132:13
- Heating Curve35:40
- Heat of Fusion41:31
- Example 243:45
31m 17s
- Intro0:00
- Phase Diagrams and Solutions0:22
- Definition of a Phase Diagram0:50
- Phase Diagram Part 1: H₂O1:54
- Phase Diagram Part 2: CO₂9:59
- Solutions: Solute & Solvent16:12
- Ways of Discussing Solution Composition: Mass Percent or Weight Percent18:46
- Ways of Discussing Solution Composition: Molarity20:07
- Ways of Discussing Solution Composition: Mole Fraction20:48
- Ways of Discussing Solution Composition: Molality21:41
- Example 1: Question22:06
- Example 1: Mass Percent24:32
- Example 1: Molarity25:53
- Example 1: Mole Fraction28:09
- Example 1: Molality29:36
37m 23s
- Intro0:00
- Vapor Pressure of Solutions2:07
- Vapor Pressure & Raoult's Law2:08
- Example 15:21
- When Ionic Compounds Dissolve10:51
- Example 212:38
- Non-Ideal Solutions17:42
- Negative Deviation24:23
- Positive Deviation29:19
- Example 331:40
34m 11s
- Intro0:00
- Colligative Properties1:07
- Boiling Point Elevation1:08
- Example 1: Question5:19
- Example 1: Solution6:52
- Freezing Point Depression12:01
- Example 2: Question14:46
- Example 2: Solution16:34
- Osmotic Pressure20:20
- Example 3: Question28:00
- Example 3: Solution30:16
48m 39s
- Intro0:00
- Bonding & Lewis Structure2:23
- Covalent Bond2:24
- Single Bond, Double Bond, and Triple Bond4:11
- Bond Length & Intermolecular Distance5:51
- Definition of Electronegativity8:42
- Bond Polarity11:48
- Bond Energy20:04
- Example 124:31
- Definition of Lewis Structure31:54
- Steps in Forming a Lewis Structure33:26
- Lewis Structure Example: H₂36:53
- Lewis Structure Example: CH₄37:33
- Lewis Structure Example: NO⁺38:43
- Lewis Structure Example: PCl₅41:12
- Lewis Structure Example: ICl₄⁻43:05
- Lewis Structure Example: BeCl₂45:07
36m 59s
- Intro0:00
- Resonance and Formal Charge0:09
- Resonance Structures of NO₃⁻0:25
- Resonance Structures of NO₂⁻12:28
- Resonance Structures of HCO₂⁻16:28
- Formal Charge19:40
- Formal Charge Example: SO₄²⁻21:32
- Formal Charge Example: CO₂31:33
- Formal Charge Example: HCN32:44
- Formal Charge Example: CN⁻33:34
- Formal Charge Example: 0₃34:43
41m 21s
- Intro0:00
- Shapes of Molecules0:35
- VSEPR0:36
- Steps in Determining Shapes of Molecules6:18
- Linear11:38
- Trigonal Planar11:55
- Tetrahedral12:45
- Trigonal Bipyramidal13:23
- Octahedral14:29
- Table: Shapes of Molecules15:40
- Example: CO₂21:11
- Example: NO₃⁻24:01
- Example: H₂O27:00
- Example: NH₃29:48
- Example: PCl₃⁻32:18
- Example: IF₄⁺34:38
- Example: KrF₄37:57
40m 17s
- Intro0:00
- Hybrid Orbitals0:13
- Introduction to Hybrid Orbitals0:14
- Electron Orbitals for CH₄5:02
- sp³ Hybridization10:52
- Example: sp³ Hybridization12:06
- sp² Hybridization14:21
- Example: sp² Hybridization16:11
- σ Bond19:10
- π Bond20:07
- sp Hybridization & Example22:00
- dsp³ Hybridization & Example27:36
- d²sp³ Hybridization & Example30:36
- Example: Predict the Hybridization and Describe the Molecular Geometry of CO32:31
- Example: Predict the Hybridization and Describe the Molecular Geometry of BF₄⁻35:17
- Example: Predict the Hybridization and Describe the Molecular Geometry of XeF₂37:09
52m 34s
- Intro0:00
- Multiple Choice1:21
- Multiple Choice 11:22
- Multiple Choice 22:23
- Multiple Choice 33:38
- Multiple Choice 44:34
- Multiple Choice 55:16
- Multiple Choice 65:41
- Multiple Choice 76:20
- Multiple Choice 87:03
- Multiple Choice 97:31
- Multiple Choice 109:03
- Multiple Choice 1111:52
- Multiple Choice 1213:16
- Multiple Choice 1313:56
- Multiple Choice 1414:52
- Multiple Choice 1515:43
- Multiple Choice 1616:20
- Multiple Choice 1716:55
- Multiple Choice 1817:22
- Multiple Choice 1918:59
- Multiple Choice 2020:24
- Multiple Choice 2122:20
- Multiple Choice 2223:29
- Multiple Choice 2324:30
- Multiple Choice 2425:24
- Multiple Choice 2526:21
- Multiple Choice 2629:06
- Multiple Choice 2730:42
- Multiple Choice 2833:28
- Multiple Choice 2934:38
- Multiple Choice 3035:37
- Multiple Choice 3137:31
- Multiple Choice 3238:28
- Multiple Choice 3339:50
- Multiple Choice 3442:57
- Multiple Choice 3544:18
- Multiple Choice 3645:52
- Multiple Choice 3748:02
- Multiple Choice 3849:25
- Multiple Choice 3949:43
- Multiple Choice 4050:16
- Multiple Choice 4150:49
32m 15s
- Intro0:00
- Multiple Choice0:12
- Multiple Choice 420:13
- Multiple Choice 430:33
- Multiple Choice 441:16
- Multiple Choice 452:36
- Multiple Choice 465:22
- Multiple Choice 476:35
- Multiple Choice 488:02
- Multiple Choice 4910:05
- Multiple Choice 5010:26
- Multiple Choice 5111:07
- Multiple Choice 5212:01
- Multiple Choice 5312:55
- Multiple Choice 5416:12
- Multiple Choice 5518:11
- Multiple Choice 5619:45
- Multiple Choice 5720:15
- Multiple Choice 5823:28
- Multiple Choice 5924:27
- Multiple Choice 6026:45
- Multiple Choice 6129:15
32m 50s
- Intro0:00
- Multiple Choice0:16
- Multiple Choice 620:17
- Multiple Choice 631:57
- Multiple Choice 646:16
- Multiple Choice 658:05
- Multiple Choice 669:18
- Multiple Choice 6710:38
- Multiple Choice 6812:51
- Multiple Choice 6914:32
- Multiple Choice 7017:35
- Multiple Choice 7122:44
- Multiple Choice 7224:27
- Multiple Choice 7327:46
- Multiple Choice 7429:39
- Multiple Choice 7530:23
47m 22s
- Intro0:00
- Free Response0:15
- Free Response 1: Part A0:16
- Free Response 1: Part B4:15
- Free Response 1: Part C5:47
- Free Response 1: Part D9:20
- Free Response 1: Part E. i10:58
- Free Response 1: Part E. ii16:45
- Free Response 1: Part E. iii26:03
- Free Response 2: Part A. i31:01
- Free Response 2: Part A. ii33:38
- Free Response 2: Part A. iii35:20
- Free Response 2: Part B. i37:38
- Free Response 2: Part B. ii39:30
- Free Response 2: Part B. iii44:44
43m 5s
- Intro0:00
- Free Response0:12
- Free Response 3: Part A0:13
- Free Response 3: Part B6:25
- Free Response 3: Part C. i11:33
- Free Response 3: Part C. ii12:02
- Free Response 3: Part D14:30
- Free Response 4: Part A21:03
- Free Response 4: Part B22:59
- Free Response 4: Part C24:33
- Free Response 4: Part D27:22
- Free Response 4: Part E28:43
- Free Response 4: Part F29:35
- Free Response 4: Part G30:15
- Free Response 4: Part H30:48
- Free Response 5: Diagram32:00
- Free Response 5: Part A34:14
- Free Response 5: Part B36:07
- Free Response 5: Part C37:45
- Free Response 5: Part D39:00
- Free Response 5: Part E40:26
28m 36s
- Intro0:00
- Free Response0:43
- Free Response 6: Part A. i0:44
- Free Response 6: Part A. ii3:08
- Free Response 6: Part A. iii5:02
- Free Response 6: Part B. i7:11
- Free Response 6: Part B. ii9:40
- Free Response 7: Part A11:14
- Free Response 7: Part B13:45
- Free Response 7: Part C15:43
- Free Response 7: Part D16:54
- Free Response 8: Part A. i19:15
- Free Response 8: Part A. ii21:16
- Free Response 8: Part B. i23:51
- Free Response 8: Part B. ii25:07
For more information, please see full course syllabus of AP Chemistry
AP Chemistry Naming Compounds
This lecture reviews the parts of the periodic table (nonmetals and metals, as well as alkali metals, alkaline earth metals, transition metals, halogens, and noble gases). Some elements naturally occur as diatomic molecules, like nitrogen and oxygen. The periodic table also lists the atomic number (average of isotopes), and the chemical symbols. Ionic compounds are neutral molecules formed from charged ions (one metal, one non-metal). Positive ions (cations) are listed first in the compound and negative ions (anions) second with an “-ide” suffix (oxide, chloride, etc.). Polyatomic ions contain more than one atom and can have a variety of prefixes and suffixes. Covalent compounds (nonmetals only) follow similar principles, but the number of atoms is described using prefixes like mono-, di-, tri-, etc. Acids follow special naming conventions and always list hydrogen first. The lecture concludes with a review of how to determine the percent composition of an element in a compound by mass.
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1 answer
Last reply by: Professor Hovasapian
Wed Aug 24, 2022 6:25 PM
Post by Mithil Krishnan on August 24, 2022
I wanted to know if you could provide me some worksheets.
1 answer
Last reply by: Professor Hovasapian
Wed Jul 1, 2020 12:54 PM
Post by Claire Zhang on July 1, 2020
Hello professor, I wonder if there's a way to identify wether a random polyatomic ion name ends in "ate" or "ite"
Thank you!
3 answers
Last reply by: Professor Hovasapian
Wed Aug 15, 2018 6:42 AM
Post by Nick Jiang on August 14, 2018
Hi Professor,
I have a few questions:
1. Is every compound that has hydrogen an acid? If so, why?
2. Kind of relating to my last question, I don't understand why we can't name H2SO4 as hydrogen sulfate. But there's also HSO4- for hydrogen sulfate.
Thanks,
Nick
1 answer
Last reply by: Professor Hovasapian
Tue Jun 19, 2018 5:55 AM
Post by Neeraj Lalwani on June 17, 2018
Hello Mr. Hovasapian,
Just a quick question: Why did you choose to write acetate as (AcO)- rather than (C2H3O2)-?
1 answer
Last reply by: Professor Hovasapian
Mon Jan 8, 2018 4:22 AM
Post by Amy Zhang on January 6, 2018
In the Sixth Editio Zumdahl Chemistry textbook you recommended to me, it says that the periodic table groups can be written as either 1-18, or with letters like 3A, 4A, etc. However, besides in the textbook, I've only ever seen the 1-18 and not the letter names. Is that like a new thing now, as the textbook was printed in 2003?
1 answer
Last reply by: Professor Hovasapian
Wed Jan 3, 2018 3:54 AM
Post by Qiaoxiang Dong on December 26, 2017
Hi Prof Hovasapian!
How would you name a covalent compound with a subscript that is greater than 10? Would you use other prefixes?
Thanks
Calvin Huang
1 answer
Last reply by: Professor Hovasapian
Thu Aug 31, 2017 5:40 AM
Post by Yosef Charkatli on August 30, 2017
Greetings professor Hovasapian!
I just wanted to thank you for your great lessons and let you know that I was able to score a 4 on the AP chemistry test by relying solely on your lessons, and I am sure that if I payed a little more attention to your lessons I would have scored a 5. You made this course a lot easier for me and you truely are the best chemistry teacher I have learned from. I simply can't thank you enough.
Best regards.
1 answer
Last reply by: Professor Hovasapian
Fri Aug 18, 2017 3:12 AM
Post by Carlins Almonor on August 16, 2017
My teacher includes the naming of hydrates in our assessments. How would one go about naming hydrates?
3 answers
Last reply by: Professor Hovasapian
Fri Jul 21, 2017 8:15 PM
Post by Amy Zhang on July 20, 2017
Hi Professor! I was wondering if you could give me the names and links for instructional textbooks and practice workbooks that follow your AP Chemistry course. Thanks!
2 answers
Last reply by: Kenneth Dietz
Mon Jul 17, 2017 1:22 PM
Post by Kenneth Dietz on July 10, 2017
so whats the story with compounds like monosodium glutamate? Is it just not following the rules. Not following these rules seems common on labels of ingredients. ( trisodium phosphate?) Is it just a different system?
1 answer
Last reply by: Professor Hovasapian
Tue Oct 25, 2016 10:56 PM
Post by Anu Yelisetti on October 25, 2016
Hi Prof. Hovasapian!
I just wanted to let you know that so far your lectures have helped me so much in school and I really enjoy them!
I don't have any specific questions pertaining to this video, but I had one about the overall course. I take Honors Chemistry in school right now, which does cover some of the basic concepts covered in AP chemistry, and I wanted to take the AP test for Chemistry this year, so would completing the course on this website be enough preparation, or would I have to take another "self-study" class outside of school? Currently, I've been using this site and reading the Chemistry textbook by Zumdahl. I'd really appreciate your feedback!
Thanks,
Anu Yelisetti
2 answers
Last reply by: Professor Hovasapian
Mon Jun 27, 2016 7:07 PM
Post by Mohamed E Sowaileh on June 19, 2016
Hello Dr. Hovasapian,
Is 2 months period enough to finish the whole course, or you don't recommend that? and is it sufficient to study from your lectures only without textbooks to gain full understanding?
1 answer
Last reply by: Professor Hovasapian
Wed May 11, 2016 2:33 AM
Post by Mohamed E Sowaileh on May 9, 2016
is this course suitable for a collage level? I mean the details.
1 answer
Last reply by: Professor Hovasapian
Sat Oct 24, 2015 7:02 PM
Post by Karthik Gnanakumar on October 24, 2015
Hello Prof. Hovasapian!
This a question not pertaining lesson specifically, but the whole AP Chemistry course you are teaching as a whole. All I wanted to ask is that if the AP Chemistry Lectures you teach are up-to-date. CollegeBoard is changing things up and the AP courses have new set of foundations being built upon. So do these lectures you teach pertain to the newer version of the AP Test or the old AP Test?
Thank You,
Karthik Gnanakumar
P.S: I love your lectures! Keep up the good work. The way you teach really helps me understand the subject.
1 answer
Last reply by: Professor Hovasapian
Mon Oct 19, 2015 12:04 AM
Post by Xinyuan Xing on October 17, 2015
Hi Professor Hovasapian,
I'm Alina from China. Just want to go back here to say Thank You. I've got a 5 on my AP chemistry, and your lectures are basically all my preparation materials. Thank you so much for your dedicated lectures! They are great lectures for students (including me) who desperately want to learn under a situation that no one around them is familiar with the subject.
Wish you all the best,
Alina
1 answer
Last reply by: Jim Tang
Sat Jul 18, 2015 9:59 PM
Post by Jim Tang on July 18, 2015
Wait, isn't acetate C2H3O2-? Where did you get AcO?
2 answers
Last reply by: Professor Hovasapian
Fri Jul 10, 2015 4:12 PM
Post by Jinbin Chen on July 7, 2015
Hi, Mr. Raffi.
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.
I do have a few questions though. Is the analytical chemistry lab a good substitute for general chemistry lab? I self-studied the entire AP curriculum, so I do want some exposure to the lab techniques without having to do general chem lecture again (since they tied the lecture and lab together). Also, are topics such as transitional metals and nuclear chemistry important later on for chem majors (these topics are left out completely in AP)?
Thanks
Jinbin
1 answer
Last reply by: Professor Hovasapian
Sat Jun 20, 2015 4:51 PM
Post by Katie Early on June 19, 2015
Professor Hovasapian- I just wanted to let you know that I took Biochemistry last year and it was your lessons that got me through it. I currently teach high school Chemistry, but I do not enjoy biochem and organic as much as straight inorganic. I am preparing to teach AP Chemistry and these lessons help better than anything I can find for those little "reminders." You are so awesome!
Thank You,
Katie Early
1 answer
Last reply by: Professor Hovasapian
Thu Mar 12, 2015 3:30 AM
Post by Richard Meador on March 5, 2015
The periodic table shows that the number of protons per element increases from 1 (Hydrogen) to 111 (Rg). Why are there no gaps? In other words, what in the formation process caused there to be no gaps in the rising number of protons per atom?
1 answer
Last reply by: Professor Hovasapian
Mon Mar 2, 2015 11:16 PM
Post by aimun amatul-hayee on March 2, 2015
do the transition metals have a charge
1 answer
Last reply by: Professor Hovasapian
Mon Mar 2, 2015 11:12 PM
Post by aimun amatul-hayee on March 2, 2015
how does calcium phosphides charge equal 0 if the formula is Ca3P2
2 answers
Last reply by: Andrew Lewis
Wed Mar 11, 2015 10:01 PM
Post by Hayley Gao on December 23, 2014
I can't watch any videos on this web. it's just show network error, but i can use any other webs and i still have the membership. Could you help me about that? Thanks!
1 answer
Last reply by: Professor Hovasapian
Thu Nov 6, 2014 1:34 AM
Post by Shih-Kuan Chen on November 5, 2014
Dear Dr. Hovasapian,
Do you think you could provide a list of signs and names of polyatomic anions that will possibly appear on the AP exam?
1 answer
Last reply by: Professor Hovasapian
Fri Aug 22, 2014 8:43 PM
Post by Okwudili Ezeh on August 22, 2014
Please could you tell me the difference between your own course and the other 2 general chemistry courses that are being offered on this website?
Are you covering more material?
1 answer
Last reply by: Professor Hovasapian
Tue Jul 1, 2014 6:56 PM
Post by Jerry Liu on June 30, 2014
Is this course still relevant to the new and updated AP test?
Thanks!
Jerry
2 answers
Last reply by: Datevig Daghlian
Fri Jun 27, 2014 11:33 AM
Post by Datevig Daghlian on June 12, 2014
Dear Dr. Hovasapian,
Thank you for responding to my previous question--your guidance and passion for chemistry is greatly seen in your lectures and your effort in teaching chemistry. I would ask you one more thing--I am currently home schooled and am in my Junior year. I have been looking around for an online, interactive AP Chemistry course and wanted to ask you if you had any particular recommendations? Please if you can let me know, I will be very thankful! Thanks again for your giving of your valuable time to assist me!
Thank You,
George Daghlian
2 answers
Last reply by: Datevig Daghlian
Wed Jun 11, 2014 9:47 AM
Post by Datevig Daghlian on June 10, 2014
Dear Dr. Hovasapian,
I would like to thank you for your passion in teaching and explaining the concepts of Chemistry. This coming year I will be taking AP Chemistry. Not having any chemistry background, how do you recommend I should prepare over the summer? Any insight you can give is greatly appreciated! God Bless!
Thank You,
George Daghlian
1 answer
Last reply by: Professor Hovasapian
Sun Jun 8, 2014 3:43 AM
Post by Jinbin Chen on June 6, 2014
Hi, professorï¼
I am very interested in starting this chemistry course, but the last time I took a chemistry class was two years ago (and it was very basic). Should I watch some other chemistry videos in this site before starting AP Chemistry?
By the way, the new AP Chem test is being administered starting from this year. Are you planning to post some new videos regarding the change in this exam?
Thanks and take care!
Jinbin
1 answer
Last reply by: Nada A.
Tue Nov 5, 2013 5:51 AM
Post by Nada A. on November 5, 2013
PCl5 ---> PhosphourPetaCloride ? it is ending with ide... doesnt that mean its an Ion? and its not... shouldn't it be PhosphoursPetaChlorine?
3 answers
Last reply by: Professor Hovasapian
Fri Nov 1, 2013 12:30 AM
Post by robina saeed on October 31, 2013
Hi Professor,
Is this a good course to prepare for the MCAT chemistry section or would I need to stick with a textbook? thanks and take care
0 answers
Post by yannick Haberkorn on October 9, 2013
at 17:08 i thought nitrogen carried a -3 charge and not a - 1 charge .. could someone please clarify
1 answer
Last reply by: Professor Hovasapian
Wed Oct 9, 2013 4:52 PM
Post by yannick Haberkorn on October 9, 2013
at 17:08 i thought nitrogen caries a -3 charge and not a -1 charge ? its not really clear
1 answer
Last reply by: robina saeed
Fri Aug 2, 2013 2:10 PM
Post by robina saeed on August 2, 2013
Hi Professor
Thanks for the earlier response. I have one more question. I have had a full year of general chemistry. Do I need organic chemistry to begin this course?
Thanks,
Robina
1 answer
Last reply by: Professor Hovasapian
Thu Feb 28, 2013 4:39 PM
Post by Youssef Sadki on February 28, 2013
I wpould like to thank you so much ...you make really like how easy to drink water...
0 answers
Post by Professor Hovasapian on February 18, 2013
Hi Raj,
I hope you're doing well. Thank you for your kind words, and I'm happy to hear you are enjoying AP Chem.
Regarding the OH, I'm wondering if you meant the OH- polyatomic Ion. If so, then, because it is an Ion that has a charge of -1, it is named as a single entity, and does not fall under the systematic procedures for naming compounds -- we simply rfer to it s Hydroxide.
Hydrogen Peroxide is actually H2O2. Now, O2- (an Oxygen atom with a 2- charge) binds to to H+ ions to create this molecule.
If the molecule were HO, without a charge, then you would be correct: it would be called Hydrogen Monoxide. In fact, water, which is the common name, and which you know as H2O -- it's systematic name is exactly Dihydrogen Monoxide.
If I have misinterpreted you question, Raj, please let me know, and I will remedy the issue.
Best wishes for a happy and productive year.
Raffi
0 answers
Post by rajendra irani on February 18, 2013
HO -Hydrogen peroxide. why not it is named as hydrogen monoxide?
0 answers
Post by rajendra irani on February 18, 2013
Dear Sir,
Great Teaching and I am really enjoying AP Chemistry.
Kind Regards
Raj
1 answer
Last reply by: Professor Hovasapian
Tue Jan 29, 2013 3:37 PM
Post by Antoni Szeglowski on January 27, 2013
Best teacher on Educator!
0 answers
Post by Riley Argue on June 14, 2012
I sat in first year chem in high school for a complete year, but my teacher could not explain this material to save her life.
But somehow you explained it so simply. Thank you!
0 answers
Post by Yaron Zaret on June 10, 2012
awesome teacher
0 answers
Post by Abdihakim Mohamed on May 7, 2012
Where where you professor for the past two years of my life, I wish I came across this website way earlier.
0 answers
Post by mateusz marciniak on May 5, 2012
great video but i was wondering, isn't Acetate C2H3O2 -1?
0 answers
Post by Miguel Suarez on April 6, 2012
Nice video really good work professor, wish all professor would explain like you