Pressure, Gas Laws, & The Ideal Gas Equation, AP Chemistry

Pressure, Gas Laws, & The Ideal Gas Equation

III. Gases: Lecture 1 | 49:40 min

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Pressure, Gas Laws, & The Ideal Gas Equation

Pressure is defined as Force per Area, and its SI unit is the Pascal
Ideal Gas Law: PV = nRT. This equation expresses a relationship among the various measureable quantities of a given gas sample. It might better be written as PV/nT = R.
In other words, given a sample of gas, its Pressure times the volume it occupies divided by the number of mols of gas times its Kelvin temperature is equal to a Constant.
When some mathematical arrangement of parameters is equal to a constant, this is profoundly important.
R is the Gas Constant: 0.08306 Liter-Atmosphere/Mol-Kelvin
Units used must match the units of R.
Standard Temperature and Pressure (STP) is 0 K and 1 atm.

Pressure, Gas Laws, & The Ideal Gas Equation

Lecture Slides are screen-captured images of important points in the lecture. Students can download and print out these lecture slide images to do practice problems as well as take notes while watching the lecture.

Intro

Pressure

Gas Laws

Ideal Gas Equation

I. Review
	Naming Compounds	41:24
	Stoichiometry	37:19
II. Aqueous Reactions & Stoichiometry
	Precipitation Reactions	31:14
	Acid-Base Reactions	43:21
	Oxidation Reduction Reactions	47:58
	Stoichiometry Examples	31:50
III. Gases
	Pressure, Gas Laws, & The Ideal Gas Equation	49:40
	Partial Pressure, Mol Fraction, & Vapor Pressure	32:00
	Kinetic Molecular Theory and Real Gases	31:58
	AP Practice for Gases	25:34
IV. Thermochemistry
	Energy, Heat, and Work	37:32
	Enthalpy & Hess's Law	32:34
	Standard Enthalpies of Formation	23:09
	Calorimetry	39:28
V. Kinetics
	Reaction Rates and Rate Laws	36:24
	Method of Initial Rates	30:48
	Integrated Rate Law & Reaction Half-Life	32:17
	Second Order & Zero-Order Rate Laws	26:40
	Activation Energy & Arrhenius Equation	40:59
	AP Practice for Kinetics	29:08
VI. Equilibrium
	Equilibrium, Part 1	46:00
	Equilibrium, Part 2	40:53
	Equilibrium: Reaction Quotient	45:53
	Equilibrium: Examples	31:51
	Le Chatelier's principle & Equilibrium	40:52
VII. Acids & Bases
	Acids and Bases	50:11
	pH of Weak Acid Solutions	43:52
	Percent Dissociation: Strong & Weak Bases	43:04
	Polyprotic Acids	35:34
	Salts and Their Acid-Base Properties	41:14
	Common Ion Effect & Buffers	41:58
	Buffer	32:24
	Buffers, Part II	40:06
	Buffers, Part III	38:43
	Titrations: Strong Acid and Strong Base	42:42
	Titrations: Weak Acid and Strong Base	42:03
	Titration Examples & Acid-Base Indicators	52:03
VIII. Solubility
	Solubility Equilibria	36:25
	Solubility Equilibria, Part II	42:06
	Solubility Equilibria, Part III	43:09
IX. Complex Ions
	Complex Ion Equilibria	43:38
	Complex Ions & Solubility	31:30
X. Chemical Thermodynamics
	Spontaneity, Entropy, & Free Energy, Part I	56:28
	Spontaneity, Entropy, & Free Energy, Part II	39:55
	Spontaneity, Entropy, & Free Energy, Part III	30:10
	Spontaneity, Entropy, & Free Energy, Part IV	30:07
	Spontaneity, Entropy, & Free Energy, Part V	44:56
XI. Electrochemistry
	Oxidation-Reduction & Balancing	39:23
	Galvanic Cells	43:09
	Cell Potential	48:41
	Potential, Work, & Free Energy	41:23
	Cell Potential & Concentration	34:19
	Electrolysis	33:21
XII. Light
	Light	44:45
XIII. Quantum Mechanics
	Quantum Mechanics & Electron Orbitals	54:00
	Electron Configurations & Diagrams	34:04
XIV. Intermolecular Forces
	Vapor Pressure & Changes of State	52:43
	Phase Diagrams & Solutions	31:17
	Vapor Pressure of Solutions	37:23
	Colligatives Properties	34:11
XV. Bonding
	Bonding & Lewis Structure	48:39
	Resonance & Formal Charge	36:59
	Shapes of Molecules	41:21
	Hybrid Orbitals	40:17
XVI. AP Practice Exam
	AP Practice Exam: Multiple Choice, Part I	52:34
	AP Practice Exam: Multiple Choice, Part II	32:15
	AP Practice Exam: Multiple Choice, Part III	32:50
	AP Practice Exam: Free response Part I	47:22
	AP Practice Exam: Free Response Part II	43:05
	AP Practice Exam: Free Response Part III	28:36

Advanced Placement Chemistry

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

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Advanced Placement Chemistry

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