Balancing an entire sheet of chemistry equations, memorizing the Periodic Table, and answering tough vocabulary questions is much easier when you have a strong foundation in General Chemistry. Whether you are taking your first college chemistry course or still in high school, knowledge of chemical processes provides insights into a variety of biological and physical phenomena. These phenomena and more are explored in Professor Franklin Ow’s General Chemistry course. In each of his lessons, Professor Ow explains concepts in easy to understand language and follows with plenty of examples you will likely see on homework and exams. Lesson topics include Stoichiometry, Gases, Acid Base Reactions, and Electrochemistry. Professor Ow obtained both his BS and PhD in chemistry from the University of California, Los Angeles. He currently teaches chemistry classes at three universities and has won multiple awards in his academic field.

Loading video...

Table of Contents
expand all collapse all

I. Basic Concepts & Measurement of Chemistry
	Basic Concepts of Chemistry			16:26
		Intro		0:00
		Lesson Overview		0:07
		Introduction		0:56
			What is Chemistry?	0:57
			What is Matter?	1:16
		Solids		1:43
			General Characteristics	1:44
			Particulate-level Drawing of Solids	2:34
		Liquids		3:39
			General Characteristics of Liquids	3:40
			Particulate-level Drawing of Liquids	3:55
		Gases		4:23
			General Characteristics of Gases	4:24
			Particulate-level Drawing Gases	5:05
		Classification of Matter		5:27
			Classification of Matter	5:26
		Pure Substances		5:54
			Pure Substances	5:55
		Mixtures		7:06
			Definition of Mixtures	7:07
			Homogeneous Mixtures	7:11
			Heterogeneous Mixtures	7:52
		Physical and Chemical Changes/Properties		8:18
			Physical Changes Retain Chemical Composition	8:19
			Chemical Changes Alter Chemical Composition	9:32
		Physical and Chemical Changes/Properties, cont'd		10:55
			Physical Properties	10:56
			Chemical Properties	11:42
		Sample Problem 1: Chemical & Physical Change		12:22
		Sample Problem 2: Element, Compound, or Mixture?		13:52
		Sample Problem 3: Classify Each of the Following Properties as chemical or Physical		15:03
	Tools in Quantitative Chemistry			29:22
		Intro		0:00
		Lesson Overview		0:07
		Units of Measurement		1:23
			The International System of Units (SI): Mass, Length, and Volume	1:39
		Percent Error		2:17
			Percent Error	2:18
			Example: Calculate the Percent Error	2:56
		Standard Deviation		3:48
			Standard Deviation Formula	3:49
		Standard Deviation cont'd		4:42
			Example: Calculate Your Standard Deviation	4:43
		Precisions vs. Accuracy		6:25
			Precision	6:26
			Accuracy	7:01
		Significant Figures and Uncertainty		7:50
			Consider the Following (2) Rulers	7:51
			Consider the Following Graduated Cylinder	11:30
		Identifying Significant Figures		12:43
			The Rules of Sig Figs Overview	12:44
			The Rules for Sig Figs: All Nonzero Digits Are Significant	13:21
			The Rules for Sig Figs: A Zero is Significant When It is In-Between Nonzero Digits	13:28
			The Rules for Sig Figs: A Zero is Significant When at the End of a Decimal Number	14:02
			The Rules for Sig Figs: A Zero is not significant When Starting a Decimal Number	14:27
		Using Sig Figs in Calculations		15:03
			Using Sig Figs for Multiplication and Division	15:04
			Using Sig Figs for Addition and Subtraction	15:48
			Using Sig Figs for Mixed Operations	16:11
		Dimensional Analysis		16:20
			Dimensional Analysis Overview	16:21
			General Format for Dimensional Analysis	16:39
			Example: How Many Miles are in 17 Laps?	17:17
			Example: How Many Grams are in 1.22 Pounds?	18:40
		Dimensional Analysis cont'd		19:43
			Example: How Much is Spent on Diapers in One Week?	19:44
		Dimensional Analysis cont'd		21:03
			SI Prefixes	21:04
		Dimensional Analysis cont'd		22:03
			500 mg → ? kg	22:04
			34.1 cm → ? um	24:03
		Summary		25:11
		Sample Problem 1: Dimensional Analysis		26:09
II. Atoms, Molecules, and Ions
	Atoms, Molecules, and Ions			52:18
		Intro		0:00
		Lesson Overview		0:08
		Introduction to Atomic Structure		1:03
			Introduction to Atomic Structure	1:04
			Plum Pudding Model	1:26
		Introduction to Atomic Structure Cont'd		2:07
			John Dalton's Atomic Theory: Number 1	2:22
			John Dalton's Atomic Theory: Number 2	2:50
			John Dalton's Atomic Theory: Number 3	3:07
			John Dalton's Atomic Theory: Number 4	3:30
			John Dalton's Atomic Theory: Number 5	3:58
		Introduction to Atomic Structure Cont'd		5:21
			Ernest Rutherford's Gold Foil Experiment	5:22
		Introduction to Atomic Structure Cont'd		7:42
			Implications of the Gold Foil Experiment	7:43
			Relative Masses and Charges	8:18
		Isotopes		9:02
			Isotopes	9:03
		Introduction to The Periodic Table		12:17
			The Periodic Table of the Elements	12:18
		Periodic Table, cont'd		13:56
			Metals	13:57
			Nonmetals	14:25
			Semimetals	14:51
		Periodic Table, cont'd		15:57
			Group I: The Alkali Metals	15:58
			Group II: The Alkali Earth Metals	16:25
			Group VII: The Halogens	16:40
			Group VIII: The Noble Gases	17:08
		Ionic Compounds: Formulas, Names, Props.		17:35
			Common Polyatomic Ions	17:36
			Predicting Ionic Charge for Main Group Elements	18:52
		Ionic Compounds: Formulas, Names, Props.		20:36
			Naming Ionic Compounds: Rule 1	20:51
			Naming Ionic Compounds: Rule 2	21:22
			Naming Ionic Compounds: Rule 3	21:50
			Naming Ionic Compounds: Rule 4	22:22
		Ionic Compounds: Formulas, Names, Props.		22:50
			Naming Ionic Compounds Example: Al₂O₃	22:51
			Naming Ionic Compounds Example: FeCl₃	23:21
			Naming Ionic Compounds Example: CuI₂ 3H₂O	24:00
			Naming Ionic Compounds Example: Barium Phosphide	24:40
			Naming Ionic Compounds Example: Ammonium Phosphate	25:55
		Molecular Compounds: Formulas and Names		26:42
			Molecular Compounds: Formulas and Names	26:43
		The Mole		28:10
			The Mole is 'A Chemist's Dozen'	28:11
			It is a Central Unit, Connecting the Following Quantities	30:01
		The Mole, cont'd		32:07
			Atomic Masses	32:08
			Example: How Many Moles are in 25.7 Grams of Sodium?	32:28
			Example: How Many Atoms are in 1.2 Moles of Carbon?	33:17
		The Mole, cont'd		34:25
			Example: What is the Molar Mass of Carbon Dioxide?	34:26
			Example: How Many Grams are in 1.2 Moles of Carbon Dioxide?	25:46
		Percentage Composition		36:43
			Example: How Many Grams of Carbon Contained in 65.1 Grams of Carbon Dioxide?	36:44
		Empirical and Molecular Formulas		39:19
			Empirical Formulas	39:20
			Empirical Formula & Elemental Analysis	40:21
		Empirical and Molecular Formulas, cont'd		41:24
			Example: Determine Both the Empirical and Molecular Formulas - Step 1	41:25
			Example: Determine Both the Empirical and Molecular Formulas - Step 2	43:18
		Summary		46:22
		Sample Problem 1: Determine the Empirical Formula of Lithium Fluoride		47:10
		Sample Problem 2: How Many Atoms of Carbon are Present in 2.67 kg of C₆H₆?		49:21
III. Chemical Reactions
	Chemical Reactions			43:24
		Intro		0:00
		Lesson Overview		0:06
		The Law of Conservation of Mass and Balancing Chemical Reactions		1:49
			The Law of Conservation of Mass	1:50
			Balancing Chemical Reactions	2:50
		Balancing Chemical Reactions Cont'd		3:40
			Balance: N₂ + H₂ → NH₃	3:41
			Balance: CH₄ + O₂ → CO₂ + H₂O	7:20
		Balancing Chemical Reactions Cont'd		9:49
			Balance: C₂H₆ + O₂ → CO₂ + H₂O	9:50
		Intro to Chemical Equilibrium		15:32
			When an Ionic Compound Full Dissociates	15:33
			When an Ionic Compound Incompletely Dissociates	16:14
			Dynamic Equilibrium	17:12
		Electrolytes and Nonelectrolytes		18:03
			Electrolytes	18:04
			Strong Electrolytes and Weak Electrolytes	18:55
			Nonelectrolytes	19:23
		Predicting the Product(s) of an Aqueous Reaction		20:02
			Single-replacement	20:03
			Example: Li (s) + CuCl₂ (aq) → 2 LiCl (aq) + Cu (s)	21:03
			Example: Cu (s) + LiCl (aq) → NR	21:23
			Example: Zn (s) + 2HCl (aq) → ZnCl₂ (aq) + H₂ (g)	22:32
		Predicting the Product(s) of an Aqueous Reaction		23:37
			Double-replacement	23:38
			Net-ionic Equation	25:29
		Predicting the Product(s) of an Aqueous Reaction		26:12
			Solubility Rules for Ionic Compounds	26:13
		Predicting the Product(s) of an Aqueous Reaction		28:10
			Neutralization Reactions	28:11
			Example: HCl (aq) + NaOH (aq) → ?	28:37
			Example: H₂SO₄ (aq) + KOH (aq) → ?	29:25
		Predicting the Product(s) of an Aqueous Reaction		30:20
			Certain Aqueous Reactions can Produce Unstable Compounds	30:21
			Example 1	30:52
			Example 2	32:16
			Example 3	32:54
		Summary		33:54
		Sample Problem 1		34:55
			ZnCO₃ (aq) + H₂SO₄ (aq) → ?	35:09
			NH₄Br (aq) + Pb(C₂H₃O₂)₂ (aq) → ?	36:02
			KNO₃ (aq) + CuCl₂ (aq) → ?	37:07
			Li₂SO₄ (aq) + AgNO₃ (aq) → ?	37:52
		Sample Problem 2		39:09
			Question 1	39:10
			Question 2	40:36
			Question 3	41:47
	Chemical Reactions II			55:40
		Intro		0:00
		Lesson Overview		0:10
		Arrhenius Definition		1:15
			Arrhenius Acids	1:16
			Arrhenius Bases	3:20
		The Bronsted-Lowry Definition		4:48
			Acids Dissolve In Water and Donate a Proton to Water: Example 1	4:49
			Acids Dissolve In Water and Donate a Proton to Water: Example 2	6:54
			Monoprotic Acids & Polyprotic Acids	7:58
			Strong Acids	11:30
			Bases Dissolve In Water and Accept a Proton From Water	12:41
			Strong Bases	16:36
		The Autoionization of Water		17:42
			Amphiprotic	17:43
			Water Reacts With Itself	18:24
		Oxides of Metals and Nonmetals		20:08
			Oxides of Metals and Nonmetals Overview	20:09
			Oxides of Nonmetals: Acidic Oxides	21:23
			Oxides of Metals: Basic Oxides	24:08
		Oxidation-Reduction (Redox) Reactions		25:34
			Redox Reaction Overview	25:35
			Oxidizing and Reducing Agents	27:02
			Redox Reaction: Transfer of Electrons	27:54
		Oxidation-Reduction Reactions Cont'd		29:55
			Oxidation Number Overview	29:56
			Oxidation Number of Homonuclear Species	31:17
			Oxidation Number of Monatomic Ions	32:58
			Oxidation Number of Fluorine	33:27
			Oxidation Number of Oxygen	34:00
			Oxidation Number of Chlorine, Bromine, and Iodine	35:07
			Oxidation Number of Hydrogen	35:30
			Net Sum of All Oxidation Numbers In a Compound	36:21
		Oxidation-Reduction Reactions Cont'd		38:19
			Let's Practice Assigning Oxidation Number	38:20
			Now Let's Apply This to a Chemical Reaction	41:07
		Summary		44:19
		Sample Problems		45:29
			Sample Problem 1	45:30
			Sample Problem 2: Determine the Oxidizing and Reducing Agents	48:48
			Sample Problem 3: Determine the Oxidizing and Reducing Agents	50:43
IV. Stoichiometry
	Stoichiometry I			42:10
		Intro		0:00
		Lesson Overview		0:23
		Mole to Mole Ratios		1:32
			Example 1: In 1 Mole of H₂O, How Many Moles Are There of Each Element?	1:53
			Example 2: In 2.6 Moles of Water, How Many Moles Are There of Each Element?	2:24
		Mole to Mole Ratios Cont'd		5:13
			Balanced Chemical Reaction	5:14
		Mole to Mole Ratios Cont'd		7:25
			Example 3: How Many Moles of Ammonia Can Form If you Have 3.1 Moles of H₂?	7:26
			Example 4: How Many Moles of Hydrogen Gas Are Required to React With 6.4 Moles of Nitrogen Gas?	9:08
		Mass to mass Conversion		11:06
			Mass to mass Conversion	11:07
			Example 5: How Many Grams of Ammonia Can Form If You Have 3.1 Grams of H₂?	12:37
			Example 6: How Many Grams of Hydrogen Gas Are Required to React With 6.4 Grams of Nitrogen Gas?	15:34
			Example 7: How Man Milligrams of Ammonia Can Form If You Have 1.2 kg of H₂?	17:29
		Limiting Reactants, Percent Yields		20:42
			Limiting Reactants, Percent Yields	20:43
			Example 8: How Many Grams of Ammonia Can Form If You Have 3.1 Grams of H₂ and 3.1 Grams of N₂	22:25
			Percent Yield	25:30
			Example 9: How Many Grams of The Excess Reactant Remains?	26:37
		Summary		29:34
		Sample Problem 1: How Many Grams of Carbon Are In 2.2 Kilograms of Carbon Dioxide?		30:47
		Sample Problem 2: How Many Milligrams of Carbon Dioxide Can Form From 23.1 Kg of CH₄(g)?		33:06
		Sample Problem 3: Part 1		36:10
		Sample Problem 3: Part 2 - What Amount Of The Excess Reactant Will Remain?		40:53
	Stoichiometry II			42:38
		Intro		0:00
		Lesson Overview		0:10
		Molarity		1:14
			Solute and Solvent	1:15
			Molarity	2:01
		Molarity Cont'd		2:59
			Example 1: How Many Grams of KBr are Needed to Make 350 mL of a 0.67 M KBr Solution?	3:00
			Example 2: How Many Moles of KBr are in 350 mL of a 0.67 M KBr Solution?	5:44
			Example 3: What Volume of a 0.67 M KBr Solution Contains 250 mg of KBr?	7:46
		Dilutions		10:01
			Dilution: M₁V₂=M₁V₂	10:02
			Example 5: Explain How to Make 250 mL of a 0.67 M KBr Solution Starting From a 1.2M Stock Solution	12:04
		Stoichiometry and Double-Displacement Precipitation Reactions		14:41
			Example 6: How Many grams of PbCl₂ Can Form From 250 mL of 0.32 M NaCl?	15:38
		Stoichiometry and Double-Displacement Precipitation Reactions		18:05
			Example 7: How Many grams of PbCl₂ Can Form When 250 mL of 0.32 M NaCl and 150 mL of 0.45 Pb(NO₃)₂ Mix?	18:06
		Stoichiometry and Neutralization Reactions		21:01
			Example 8: How Many Grams of NaOh are Required to Neutralize 4.5 Grams of HCl?	21:02
		Stoichiometry and Neutralization Reactions		23:03
			Example 9: How Many mL of 0.45 M NaOH are Required to Neutralize 250 mL of 0.89 M HCl?	23:04
		Stoichiometry and Acid-Base Standardization		25:28
			Introduction to Titration & Standardization	25:30
			Acid-Base Titration	26:12
			The Analyte & Titrant	26:24
		The Experimental Setup		26:49
			The Experimental Setup	26:50
		Stoichiometry and Acid-Base Standardization		28:38
			Example 9: Determine the Concentration of the Analyte	28:39
		Summary		32:46
		Sample Problem 1: Stoichiometry & Neutralization		35:24
		Sample Problem 2: Stoichiometry		37:50
V. Thermochemistry
	Energy & Chemical Reactions			55:28
		Intro		0:00
		Lesson Overview		0:14
		Introduction		1:22
			Recall: Chemistry	1:23
			Energy Can Be Expressed In Different Units	1:57
		The First Law of Thermodynamics		2:43
			Internal Energy	2:44
		The First Law of Thermodynamics Cont'd		6:14
			Ways to Transfer Internal Energy	6:15
			Work Energy	8:13
			Heat Energy	8:34
			∆U = q + w	8:44
		Calculating ∆U, Q, and W		8:58
			Changes In Both Volume and Temperature of a System	8:59
		Calculating ∆U, Q, and W Cont'd		11:01
			The Work Equation	11:02
			Example 1: Calculate ∆U For The Burning Fuel	11:45
		Calculating ∆U, Q, and W Cont'd		14:09
			The Heat Equation	14:10
		Calculating ∆U, Q, and W Cont'd		16:03
			Example 2: Calculate The Final Temperature	16:04
		Constant-Volume Calorimetry		18:05
			Bomb Calorimeter	18:06
			The Effect of Constant Volume On The Equation For Internal Energy	22:11
			Example 3: Calculate ∆U	23:12
		Constant-Pressure Conditions		26:05
			Constant-Pressure Conditions	26:06
		Calculating Enthalpy: Phase Changes		27:29
			Melting, Vaporization, and Sublimation	27:30
			Freezing, Condensation and Deposition	28:25
			Enthalpy Values For Phase Changes	28:40
			Example 4: How Much Energy In The Form of heat is Required to Melt 1.36 Grams of Ice?	29:40
		Calculating Enthalpy: Heats of Reaction		31:22
			Example 5: Calculate The Heat In kJ Associated With The Complete Reaction of 155 g NH₃	31:23
		Using Standard Enthalpies of Formation		33:53
			Standard Enthalpies of Formation	33:54
		Using Standard Enthalpies of Formation		36:12
			Example 6: Calculate The Standard Enthalpies of Formation For The Following Reaction	36:13
		Enthalpy From a Series of Reactions		39:58
			Hess's Law	39:59
		Coffee-Cup Calorimetry		42:43
			Coffee-Cup Calorimetry	42:44
			Example 7: Calculate ∆H° of Reaction	45:10
		Summary		47:12
		Sample Problem 1		48:58
		Sample Problem 2		51:24
VI. Quantum Theory of Atoms
	Structure of Atoms			42:33
		Intro		0:00
		Lesson Overview		0:07
		Introduction		1:01
			Rutherford's Gold Foil Experiment	1:02
		Electromagnetic Radiation		2:31
			Radiation	2:32
			Three Parameters: Energy, Frequency, and Wavelength	2:52
		Electromagnetic Radiation		5:18
			The Electromagnetic Spectrum	5:19
		Atomic Spectroscopy and The Bohr Model		7:46
			Wavelengths of Light	7:47
		Atomic Spectroscopy Cont'd		9:45
			The Bohr Model	9:46
		Atomic Spectroscopy Cont'd		12:21
			The Balmer Series	12:22
			Rydberg Equation For Predicting The Wavelengths of Light	13:04
		The Wave Nature of Matter		15:11
			The Wave Nature of Matter	15:12
		The Wave Nature of Matter		19:10
			New School of Thought	19:11
			Einstein: Energy	19:49
			Hertz and Planck: Photoelectric Effect	20:16
			de Broglie: Wavelength of a Moving Particle	21:14
		Quantum Mechanics and The Atom		22:15
			Heisenberg: Uncertainty Principle	22:16
			Schrodinger: Wavefunctions	23:08
		Quantum Mechanics and The Atom		24:02
			Principle Quantum Number	24:03
			Angular Momentum Quantum Number	25:06
			Magnetic Quantum Number	26:27
			Spin Quantum Number	28:42
		The Shapes of Atomic Orbitals		29:15
			Radial Wave Function	29:16
			Probability Distribution Function	32:08
		The Shapes of Atomic Orbitals		34:02
			3-Dimensional Space of Wavefunctions	34:03
		Summary		35:57
		Sample Problem 1		37:07
		Sample Problem 2		40:23
VII. Electron Configurations and Periodicity
	Periodic Trends			38:50
		Intro		0:00
		Lesson Overview		0:09
		Introduction		0:36
		Electron Configuration of Atoms		1:33
			Electron Configuration & Atom's Electrons	1:34
			Electron Configuration Format	1:56
		Electron Configuration of Atoms Cont'd		3:01
			Aufbau Principle	3:02
		Electron Configuration of Atoms Cont'd		6:53
			Electron Configuration Format 1: Li, O, and Cl	6:56
			Electron Configuration Format 2: Li, O, and Cl	9:11
		Electron Configuration of Atoms Cont'd		12:48
			Orbital Box Diagrams	12:49
			Pauli Exclusion Principle	13:11
			Hund's Rule	13:36
		Electron Configuration of Atoms Cont'd		17:35
			Exceptions to The Aufbau Principle: Cr	17:36
			Exceptions to The Aufbau Principle: Cu	18:15
		Electron Configuration of Atoms Cont'd		20:22
			Electron Configuration of Monatomic Ions: Al	20:23
			Electron Configuration of Monatomic Ions: Al³⁺	20:46
			Electron Configuration of Monatomic Ions: Cl	21:57
			Electron Configuration of Monatomic Ions: Cl¹⁻	22:09
		Electron Configuration Cont'd		24:31
			Paramagnetism	24:32
			Diamagnetism	25:00
		Atomic Radii		26:08
			Atomic Radii	26:09
			In a Column of the Periodic Table	26:25
			In a Row of the Periodic Table	26:46
		Ionic Radii		27:30
			Ionic Radii	27:31
			Anions	27:42
			Cations	27:57
			Isoelectronic Species	28:12
		Ionization Energy		29:00
			Ionization Energy	29:01
		Electron Affinity		31:37
			Electron Affinity	31:37
		Summary		33:43
		Sample Problem 1: Ground State Configuration and Orbital Box Diagram		34:21
			Fe	34:48
			P	35:32
		Sample Problem 2		36:38
			Which Has The Larger Ionization Energy: Na or Li?	36:39
			Which Has The Larger Atomic Size: O or N ?	37:23
			Which Has The Larger Atomic Size: O²⁻ or N³⁻ ?	38:00
VIIII. Molecular Geometry & Bonding Theory
	Bonding & Molecular Structure			52:39
		Intro		0:00
		Lesson Overview		0:08
		Introduction		1:10
		Types of Chemical Bonds		1:53
			Ionic Bond	1:54
			Molecular Bond	2:42
		Electronegativity and Bond Polarity		3:26
			Electronegativity (EN)	3:27
			Periodic Trend	4:36
		Electronegativity and Bond Polarity Cont'd		6:04
			Bond Polarity: Polar Covalent Bond	6:05
			Bond Polarity: Nonpolar Covalent Bond	8:53
		Lewis Electron Dot Structure of Atoms		9:48
			Lewis Electron Dot Structure of Atoms	9:49
		Lewis Structures of Polyatomic Species		12:51
			Single Bonds	12:52
			Double Bonds	13:28
			Nonbonding Electrons	13:59
		Lewis Structures of Polyatomic Species Cont'd		14:45
			Drawing Lewis Structures: Step 1	14:48
			Drawing Lewis Structures: Step 2	15:16
			Drawing Lewis Structures: Step 3	15:52
			Drawing Lewis Structures: Step 4	17:31
			Drawing Lewis Structures: Step 5	19:08
			Drawing Lewis Structure Example: Carbonate	19:33
		Resonance and Formal Charges (FC)		24:06
			Resonance Structures	24:07
			Formal Charge	25:20
		Resonance and Formal Charges Cont'd		27:46
			More On Formal Charge	27:47
		Resonance and Formal Charges Cont'd		28:21
			Good Resonance Structures	28:22
		VSEPR Theory		31:08
			VSEPR Theory Continue	31:09
		VSEPR Theory Cont'd		32:53
			VSEPR Geometries	32:54
			Steric Number	33:04
			Basic Geometry	33:50
			Molecular Geometry	35:50
		Molecular Polarity		37:51
			Steps In Determining Molecular Polarity	37:52
			Example 1: Polar	38:47
			Example 2: Nonpolar	39:10
			Example 3: Polar	39:36
			Example 4: Polar	40:08
		Bond Properties: Order, Length, and Energy		40:38
			Bond Order	40:39
			Bond Length	41:21
			Bond Energy	41:55
		Summary		43:09
		Sample Problem 1		43:42
			XeO₃	44:03
			I₃⁻	47:02
			SF₅	49:16
	Advanced Bonding Theories			71:41
		Intro		0:00
		Lesson Overview		0:09
		Introduction		0:38
		Valence Bond Theory		3:07
			Valence Bond Theory	3:08
			spᶟ Hybridized Carbon Atom	4:19
		Valence Bond Theory Cont'd		6:24
			spᶟ Hybridized	6:25
			Hybrid Orbitals For Water	7:26
		Valence Bond Theory Cont'd (spᶟ)		11:53
			Example 1: NH₃	11:54
		Valence Bond Theory Cont'd (sp²)		14:48
			sp² Hybridization	14:49
			Example 2: BF₃	16:44
		Valence Bond Theory Cont'd (sp)		22:44
			sp Hybridization	22:46
			Example 3: HCN	23:38
		Valence Bond Theory Cont'd (sp³d and sp³d²)		27:36
			Valence Bond Theory: sp³d and sp³d²	27:37
		Molecular Orbital Theory		29:10
			Valence Bond Theory Doesn't Always Account For a Molecule's Magnetic Behavior	29:11
		Molecular Orbital Theory Cont'd		30:37
			Molecular Orbital Theory	30:38
			Wavefunctions	31:04
			How s-orbitals Can Interact	32:23
			Bonding Nature of p-orbitals: Head-on	35:34
			Bonding Nature of p-orbitals: Parallel	39:04
			Interaction Between s and p-orbital	40:45
			Molecular Orbital Diagram For Homonuclear Diatomics: H₂	42:21
			Molecular Orbital Diagram For Homonuclear Diatomics: He₂	45:23
			Molecular Orbital Diagram For Homonuclear Diatomic: Li₂	46:39
			Molecular Orbital Diagram For Homonuclear Diatomic: Li₂⁺	47:42
			Molecular Orbital Diagram For Homonuclear Diatomic: B₂	48:57
			Molecular Orbital Diagram For Homonuclear Diatomic: N₂	54:04
			Molecular Orbital Diagram: Molecular Oxygen	55:57
			Molecular Orbital Diagram For Heteronuclear Diatomics: Hydrochloric Acid	62:16
		Sample Problem 1: Determine the Atomic Hybridization		67:20
			XeO₃	67:21
			SF₆	67:49
			I₃⁻	68:20
		Sample Problem 2		69:04
IX. Gases, Solids, & Liquids
	Gases			35:06
		Intro		0:00
		Lesson Overview		0:07
		The Kinetic Molecular Theory of Gases		1:23
			The Kinetic Molecular Theory of Gases	1:24
		Parameters To Characterize Gases		3:35
			Parameters To Characterize Gases: Pressure	3:37
			Interpreting Pressure On a Particulate Level	4:43
		Parameters Cont'd		6:08
			Units For Expressing Pressure: Psi, Pascal	6:19
			Units For Expressing Pressure: mm Hg	6:42
			Units For Expressing Pressure: atm	6:58
			Units For Expressing Pressure: torr	7:24
		Parameters Cont'd		8:09
			Parameters To Characterize Gases: Volume	8:10
			Common Units of Volume	9:00
		Parameters Cont'd		9:11
			Parameters To Characterize Gases: Temperature	9:12
			Particulate Level	9:36
			Parameters To Characterize Gases: Moles	10:24
		The Simple Gas Laws		10:43
			Gas Laws Are Only Valid For…	10:44
			Charles' Law	11:24
		The Simple Gas Laws		13:13
			Boyle's Law	13:14
		The Simple Gas Laws		15:28
			Gay-Lussac's Law	15:29
		The Simple Gas Laws		17:11
			Avogadro's Law	17:12
		The Ideal Gas Law		18:43
			The Ideal Gas Law: PV = nRT	18:44
		Applications of the Ideal Gas Law		20:12
			Standard Temperature and Pressure for Gases	20:13
		Applications of the Ideal Gas Law		21:43
			Ideal Gas Law & Gas Density	21:44
		Gas Pressures and Partial Pressures		23:18
			Dalton's Law of Partial Pressures	23:19
		Gas Stoichiometry		24:15
			Stoichiometry Problems Involving Gases	24:16
			Using The Ideal Gas Law to Get to Moles	25:16
			Using Molar Volume to Get to Moles	25:39
		Gas Stoichiometry Cont'd		26:03
			Example 1: How Many Liters of O₂ at STP are Needed to Form 10.5 g of Water Vapor?	26:04
		Summary		28:33
		Sample Problem 1: Calculate the Molar Mass of the Gas		29:28
		Sample Problem 2: What Mass of Ag₂O is Required to Form 3888 mL of O₂ Gas When Measured at 734 mm Hg and 25°C?		31:59
	Intermolecular Forces & Liquids			33:47
		Intro		0:00
		Lesson Overview		0:10
		Introduction		0:46
			Intermolecular Forces (IMF)	0:47
		Intermolecular Forces of Polar Molecules		1:32
			Ion-dipole Forces	1:33
			Example: Salt Dissolved in Water	1:50
			Coulomb's Law & the Force of Attraction Between Ions and/or Dipoles	3:06
		IMF of Polar Molecules cont'd		4:36
			Enthalpy of Solvation or Enthalpy of Hydration	4:37
		IMF of Polar Molecules cont'd		6:01
			Dipole-dipole Forces	6:02
		IMF of Polar Molecules cont'd		7:22
			Hydrogen Bonding	7:23
			Example: Hydrogen Bonding of Water	8:06
		IMF of Nonpolar Molecules		9:37
			Dipole-induced Dipole Attraction	9:38
		IMF of Nonpolar Molecules cont'd		11:34
			Induced Dipole Attraction, London Dispersion Forces, or Vand der Waals Forces	11:35
			Polarizability	13:46
		IMF of Nonpolar Molecules cont'd		14:26
			Intermolecular Forces (IMF) and Polarizability	14:31
		Properties of Liquids		16:48
			Standard Molar Enthalpy of Vaporization	16:49
			Trends in Boiling Points of Representative Liquids: H₂O vs. H₂S	17:43
		Properties of Liquids cont'd		18:36
			Aliphatic Hydrocarbons	18:37
			Branched Hydrocarbons	20:52
		Properties of Liquids cont'd		22:10
			Vapor Pressure	22:11
			The Clausius-Clapeyron Equation	24:30
		Properties of Liquids cont'd		25:52
			Boiling Point	25:53
		Properties of Liquids cont'd		27:07
			Surface Tension	27:08
			Viscosity	28:06
		Summary		29:04
		Sample Problem 1: Determine Which of the Following Liquids Will Have the Lower Vapor Pressure		30:21
		Sample Problem 2: Determine Which of the Following Liquids Will Have the Largest Standard Molar Enthalpy of Vaporization		31:37
	The Chemistry of Solids			25:13
		Intro		0:00
		Lesson Overview		0:07
		Introduction		0:46
			General Characteristics	0:47
			Particulate-level Drawing	1:09
		The Basic Structure of Solids: Crystal Lattices		1:37
			The Unit Cell Defined	1:38
			Primitive Cubic	2:50
		Crystal Lattices cont'd		3:58
			Body-centered Cubic	3:59
			Face-centered Cubic	5:02
		Lattice Enthalpy and Trends		6:27
			Introduction to Lattice Enthalpy	6:28
			Equation to Calculate Lattice Enthalpy	7:21
		Different Types of Crystalline Solids		9:35
			Molecular Solids	9:36
			Network Solids	10:25
		Phase Changes Involving Solids		11:03
			Melting & Thermodynamic Value	11:04
			Freezing & Thermodynamic Value	11:49
		Phase Changes cont'd		12:40
			Sublimation & Thermodynamic Value	12:41
			Depositions & Thermodynamic Value	13:13
		Phase Diagrams		13:40
			Introduction to Phase Diagrams	13:41
			Phase Diagram of H₂O: Melting Point	14:12
			Phase Diagram of H₂O: Normal Boiling Point	14:50
			Phase Diagram of H₂O: Sublimation Point	15:02
			Phase Diagram of H₂O: Point C ( Supercritical Point)	15:32
		Phase Diagrams cont'd		16:31
			Phase Diagram of Dry Ice	16:32
		Summary		18:15
		Sample Problem 1, Part A: Of the Group I Fluorides, Which Should Have the Highest Lattice Enthalpy?		19:01
		Sample Problem 1, Part B: Of the Lithium Halides, Which Should Have the Lowest Lattice Enthalpy?		19:54
		Sample Problem 2: How Many Joules of Energy is Required to Melt 546 mg of Ice at Standard Pressure?		20:55
		Sample Problem 3: Phase Diagram of Helium		22:42
X. Solutions, Rates of Reaction, & Equilibrium
	Solutions & Their Behavior			38:06
		Intro		0:00
		Lesson Overview		0:10
		Units of Concentration		1:40
			Molarity	1:41
			Molality	3:30
			Weight Percent	4:26
			ppm	5:16
		Like Dissolves Like		6:28
			Like Dissolves Like	6:29
		Factors Affecting Solubility		9:35
			The Effect of Pressure: Henry's Law	9:36
			The Effect of Temperature on Gas Solubility	12:16
			The Effect of Temperature on Solid Solubility	14:28
		Colligative Properties		16:48
			Colligative Properties	16:49
			Changes in Vapor Pressure: Raoult's Law	17:19
		Colligative Properties cont'd		19:53
			Boiling Point Elevation and Freezing Point Depression	19:54
		Colligative Properties cont'd		26:13
			Definition of Osmosis	26:14
			Osmotic Pressure Example	27:11
		Summary		31:11
		Sample Problem 1: Calculating Vapor Pressure		32:53
		Sample Problem 2: Calculating Molality		36:29
	Chemical Kinetics			37:45
		Intro		0:00
		Lesson Overview		0:06
		Introduction		1:09
			Chemical Kinetics and the Rate of a Reaction	1:10
			Factors Influencing Rate	1:19
		Introduction cont'd		2:27
			How a Reaction Progresses Through Time	2:28
			Rate of Change Equation	6:02
		Rate Laws		7:06
			Definition of Rate Laws	7:07
			General Form of Rate Laws	7:37
		Rate Laws cont'd		11:07
			Rate Orders With Respect to Reactant and Concentration	11:08
		Methods of Initial Rates		13:38
			Methods of Initial Rates	13:39
		Integrated Rate Laws		17:57
			Integrated Rate Laws	17:58
			Graphically Determine the Rate Constant k	18:52
		Reaction Mechanisms		21:05
			Step 1: Reversible	21:18
			Step 2: Rate-limiting Step	21:44
			Rate Law for the Reaction	23:28
		Reaction Rates and Temperatures		26:16
			Reaction Rates and Temperatures	26:17
			The Arrhenius Equation	29:06
		Catalysis		30:31
			Catalyst	30:32
		Summary		32:02
		Sample Problem 1: Calculate the Rate Constant and the Time Required for the Reaction to be Completed		32:54
		Sample Problem 2: Calculate the Energy of Activation and the Order of the Reaction		35:24
	Principles of Chemical Equilibrium			34:09
		Intro		0:00
		Lesson Overview		0:08
		Introduction		1:02
		The Equilibrium Constant		3:08
			The Equilibrium Constant	3:09
		The Equilibrium Constant cont'd		5:50
			The Equilibrium Concentration and Constant for Solutions	5:51
			The Equilibrium Partial Pressure and Constant for Gases	7:01
			Relationship of Kc and Kp	7:30
		Heterogeneous Equilibria		8:23
			Heterogeneous Equilibria	8:24
		Manipulating K		9:57
			First Way of Manipulating K	9:58
			Second Way of Manipulating K	11:48
		Manipulating K cont'd		12:31
			Third Way of Manipulating K	12:32
		The Reaction Quotient Q		14:42
			The Reaction Quotient Q	14:43
			Q > K	16:16
			Q < K	16:30
			Q = K	16:43
		Le Chatlier's Principle		17:32
			Restoring Equilibrium When It is Disturbed	17:33
			Disturbing a Chemical System at Equilibrium	18:35
		Problem-Solving with ICE Tables		19:05
			Determining a Reaction's Equilibrium Constant With ICE Table	19:06
		Problem-Solving with ICE Tables cont'd		21:03
			Example 1: Calculate O₂(g) at Equilibrium	21:04
		Problem-Solving with ICE Tables cont'd		22:53
			Example 2: Calculate the Equilibrium Constant	22:54
		Summary		25:24
		Sample Problem 1: Calculate the Equilibrium Constant		27:59
		Sample Problem 2: Calculate The Equilibrium Concentration		30:30
XI. Acids & Bases Chemistry
	Acid-Base Chemistry			43:44
		Intro		0:00
		Lesson Overview		0:06
		Introduction		0:55
			Bronsted-Lowry Acid & Bronsted -Lowry Base	0:56
			Water is an Amphiprotic Molecule	2:40
			Water Reacting With Itself	2:58
		Introduction cont'd		4:04
			Strong Acids	4:05
			Strong Bases	5:18
		Introduction cont'd		6:16
			Weak Acids and Bases	6:17
		Quantifying Acid-Base Strength		7:35
			The pH Scale	7:36
		Quantifying Acid-Base Strength cont'd		9:55
			The Acid-ionization Constant Ka and pKa	9:56
		Quantifying Acid-Base Strength cont'd		12:13
			Example: Calculate the pH of a 1.2M Solution of Acetic Acid	12:14
		Quantifying Acid-Base Strength		15:06
			Calculating the pH of Weak Base Solutions	15:07
		Writing Out Acid-Base Equilibria		17:45
			Writing Out Acid-Base Equilibria	17:46
		Writing Out Acid-Base Equilibria cont'd		19:47
			Consider the Following Equilibrium	19:48
			Conjugate Base and Conjugate Acid	21:18
		Salts Solutions		22:00
			Salts That Produce Acidic Aqueous Solutions	22:01
			Salts That Produce Basic Aqueous Solutions	23:15
			Neutral Salt Solutions	24:05
		Diprotic and Polyprotic Acids		24:44
			Example: Calculate the pH of a 1.2 M Solution of H₂SO₃	24:43
		Diprotic and Polyprotic Acids cont'd		27:18
			Calculate the pH of a 1.2 M Solution of Na₂SO₃	27:19
		Lewis Acids and Bases		29:13
			Lewis Acids	29:14
			Lewis Bases	30:10
			Example: Lewis Acids and Bases	31:04
		Molecular Structure and Acidity		32:03
			The Effect of Charge	32:04
			Within a Period/Row	33:07
		Molecular Structure and Acidity cont'd		34:17
			Within a Group/Column	34:18
			Oxoacids	35:58
		Molecular Structure and Acidity cont'd		37:54
			Carboxylic Acids	37:55
			Hydrated Metal Cations	39:23
		Summary		40:39
		Sample Problem 1: Calculate the pH of a 1.2 M Solution of NH₃		41:20
		Sample Problem 2: Predict If The Following Slat Solutions are Acidic, Basic, or Neutral		42:37
	Applications of Aqueous Equilibria			55:26
		Intro		0:00
		Lesson Overview		0:07
		Calculating pH of an Acid-Base Mixture		0:53
			Equilibria Involving Direct Reaction With Water	0:54
			When a Bronsted-Lowry Acid and Base React	1:12
			After Neutralization Occurs	2:05
		Calculating pH of an Acid-Base Mixture cont'd		2:51
			Example: Calculating pH of an Acid-Base Mixture, Step 1 - Neutralization	2:52
			Example: Calculating pH of an Acid-Base Mixture, Step 2 - React With H₂O	5:24
		Buffers		7:45
			Introduction to Buffers	7:46
			When Acid is Added to a Buffer	8:50
			When Base is Added to a Buffer	9:54
		Buffers cont'd		10:41
			Calculating the pH	10:42
			Calculating the pH When 0.010 mol NaOH is Added to 1.0 L of the Buffer	14:03
		Buffers cont'd		14:10
			Calculating the pH When 0.010 mol NaOH is Added to 1.0 L of the Buffer: Step 1 -Neutralization	14:11
			Calculating the pH When 0.010 mol NaOH is Added to 1.0 L of the Buffer: Step 2- ICE Table	15:22
		Buffer Preparation and Capacity		16:38
			Example: Calculating the pH of a Buffer Solution	16:42
			Effective Buffer	18:40
		Acid-Base Titrations		19:33
			Acid-Base Titrations: Basic Setup	19:34
		Acid-Base Titrations cont'd		22:12
			Example: Calculate the pH at the Equivalence Point When 0.250 L of 0.0350 M HClO is Titrated With 1.00 M KOH	22:13
		Acid-Base Titrations cont'd		25:38
			Titration Curve	25:39
		Solubility Equilibria		33:07
			Solubility of Salts	33:08
			Solubility Product Constant: Ksp	34:14
		Solubility Equilibria cont'd		34:58
			Q < Ksp	34:59
			Q > Ksp	35:34
		Solubility Equilibria cont'd		36:03
			Common-ion Effect	36:04
			Example: Calculate the Solubility of PbCl₂ in 0.55 M NaCl	36:30
		Solubility Equilibria cont'd		39:02
			When a Solid Salt Contains the Conjugate of a Weak Acid	39:03
			Temperature and Solubility	40:41
		Complexation Equilibria		41:10
			Complex Ion	41:11
			Complex Ion Formation Constant: Kf	42:26
		Summary		43:35
		Sample Problem 1: Question		44:23
		Sample Problem 1: Part a) Calculate the pH at the Beginning of the Titration		45:48
		Sample Problem 1: Part b) Calculate the pH at the Midpoint or Half-way Point		48:04
		Sample Problem 1: Part c) Calculate the pH at the Equivalence Point		48:32
		Sample Problem 1: Part d) Calculate the pH After 27.50 mL of the Acid was Added		53:00
XII. Thermodynamics & Electrochemistry
	Entropy & Free Energy			36:13
		Intro		0:00
		Lesson Overview		0:08
		Introduction		0:53
		Introduction to Entropy		1:37
			Introduction to Entropy	1:38
		Entropy and Heat Flow		6:31
			Recall Thermodynamics	6:32
			Entropy is a State Function	6:54
			∆S and Heat Flow	7:28
		Entropy and Heat Flow cont'd		8:18
			Entropy and Heat Flow: Equations	8:19
			Endothermic Processes: ∆S > 0	8:44
		The Second Law of Thermodynamics		10:04
			Total ∆S = ∆S of System + ∆S of Surrounding	10:05
			Nature Favors Processes Where The Amount of Entropy Increases	10:22
		The Third Law of Thermodynamics		11:55
			The Third Law of Thermodynamics & Zero Entropy	11:56
		Problem-Solving involving Entropy		12:36
			Endothermic Process and ∆S	12:37
			Exothermic Process and ∆S	13:19
		Problem-Solving cont'd		13:46
			Change in Physical States: From Solid to Liquid to Gas	13:47
			Change in Physical States: All Gases	15:02
		Problem-Solving cont'd		15:56
			Calculating the ∆S for the System, Surrounding, and Total	15:57
			Example: Calculating the Total ∆S	16:17
		Problem-Solving cont'd		18:36
			Problems Involving Standard Molar Entropies of Formation	18:37
		Introduction to Gibb's Free Energy		20:09
			Definition of Free Energy ∆G	20:10
			Spontaneous Process and ∆G	20:19
		Gibb's Free Energy cont'd		22:28
			Standard Molar Free Energies of Formation	22:29
			The Free Energies of Formation are Zero for All Compounds in the Standard State	22:42
		Gibb's Free Energy cont'd		23:31
			∆G° of the System = ∆H° of the System - T∆S° of the System	23:32
			Predicting Spontaneous Reaction Based on the Sign of ∆G° of the System	24:24
		Gibb's Free Energy cont'd		26:32
			Effect of reactant and Product Concentration on the Sign of Free Energy	26:33
			∆G° of Reaction = -RT ln K	27:18
		Summary		28:12
		Sample Problem 1: Calculate ∆S° of Reaction		28:48
		Sample Problem 2: Calculate the Temperature at Which the Reaction Becomes Spontaneous		31:18
		Sample Problem 3: Calculate Kp		33:47
	Electrochemistry			41:16
		Intro		0:00
		Lesson Overview		0:08
		Introduction		0:53
		Redox Reactions		1:42
			Oxidation-Reduction Reaction Overview	1:43
		Redox Reactions cont'd		2:37
			Which Reactant is Being Oxidized and Which is Being Reduced?	2:38
		Redox Reactions cont'd		6:34
			Balance Redox Reaction In Neutral Solutions	6:35
		Redox Reactions cont'd		10:37
			Balance Redox Reaction In Acidic and Basic Solutions: Step 1	10:38
			Balance Redox Reaction In Acidic and Basic Solutions: Step 2 - Balance Each Half-Reaction	11:22
		Redox Reactions cont'd		12:19
			Balance Redox Reaction In Acidic and Basic Solutions: Step 2 - Balance Hydrogen	12:20
		Redox Reactions cont'd		14:30
			Balance Redox Reaction In Acidic and Basic Solutions: Step 3	14:34
			Balance Redox Reaction In Acidic and Basic Solutions: Step 4	15:38
		Voltaic Cells		17:01
			Voltaic Cell or Galvanic Cell	17:02
			Cell Notation	22:03
		Electrochemical Potentials		25:22
			Electrochemical Potentials	25:23
		Electrochemical Potentials cont'd		26:07
			Table of Standard Reduction Potentials	26:08
		The Nernst Equation		30:41
			The Nernst Equation	30:42
			It Can Be Shown That At Equilibrium E =0.00	32:15
		Gibb's Free Energy and Electrochemistry		32:46
			Gibbs Free Energy is Relatively Small if the Potential is Relatively High	32:47
			When E° is Very Large	33:39
		Charge, Current and Time		33:56
			A Battery Has Three Main Parameters	33:57
			A Simple Equation Relates All of These Parameters	34:09
		Summary		34:50
		Sample Problem 1: Redox Reaction		35:26
		Sample Problem 2: Battery		38:00
XIII. Transition Elements & Coordination Compounds
	The Chemistry of The Transition Metals			39:03
		Intro		0:00
		Lesson Overview		0:11
		Coordination Compounds		1:20
			Coordination Compounds	1:21
		Nomenclature of Coordination Compounds		2:48
			Rule 1	3:01
			Rule 2	3:12
			Rule 3	4:07
		Nomenclature cont'd		4:58
			Rule 4	4:59
			Rule 5	5:13
			Rule 6	5:35
			Rule 7	6:19
			Rule 8	6:46
		Nomenclature cont'd		7:39
			Rule 9	7:40
			Rule 10	7:45
			Rule 11	8:00
			Nomenclature of Coordination Compounds: NH₄[PtCl₃NH₃]	8:11
			Nomenclature of Coordination Compounds: [Cr(NH₃)₄(OH)₂]Br	9:31
		Structures of Coordination Compounds		10:54
			Coordination Number or Steric Number	10:55
			Commonly Observed Coordination Numbers and Geometries: 4	11:14
			Commonly Observed Coordination Numbers and Geometries: 6	12:00
		Isomers of Coordination Compounds		13:13
			Isomers of Coordination Compounds	13:14
			Geometrical Isomers of CN = 6 Include: ML₄L₂'	13:30
			Geometrical Isomers of CN = 6 Include: ML₃L₃'	15:07
		Isomers cont'd		17:00
			Structural Isomers Overview	17:01
			Structural Isomers: Ionization	18:06
			Structural Isomers: Hydrate	19:25
			Structural Isomers: Linkage	20:11
			Structural Isomers: Coordination Isomers	21:05
		Electronic Structure		22:25
			Crystal Field Theory	22:26
			Octahedral and Tetrahedral Field	22:54
		Electronic Structure cont'd		25:43
			Vanadium (II) Ion in an Octahedral Field	25:44
			Chromium(III) Ion in an Octahedral Field	26:37
		Electronic Structure cont'd		28:47
			Strong-Field Ligands and Weak-Field Ligands	28:48
		Implications of Electronic Structure		30:08
			Compare the Magnetic Properties of: [Fe(OH₂)₆]²⁺ vs. [Fe(CN)₆]⁴⁻	30:09
			Discussion on Color	31:57
		Summary		34:41
		Sample Problem 1: Name the Following Compound [Fe(OH)(OH₂)₅]Cl₂		35:08
		Sample Problem 1: Name the Following Compound [Co(NH₃)₃(OH₂)₃]₂(SO₄)₃		36:24
		Sample Problem 2: Change in Magnetic Properties		37:30
XIV. Nuclear Chemistry
	Nuclear Chemistry			16:39
		Intro		0:00
		Lesson Overview		0:06
		Introduction		0:40
			Introduction to Nuclear Reactions	0:41
		Types of Radioactive Decay		2:10
			Alpha Decay	2:11
			Beta Decay	3:27
			Gamma Decay	4:40
			Other Types of Particles of Varying Energy	5:40
		Nuclear Equations		6:47
			Nuclear Equations	6:48
		Nuclear Decay		9:28
			Nuclear Decay and the First-Order Kinetics	9:29
		Summary		11:31
		Sample Problem 1: Complete the Following Nuclear Equations		12:13
		Sample Problem 2: How Old is the Rock?		14:21

Quick links

Ready to join?

Subscription benefits:

Most comprehensive scholastic content on the web!
Over 500 math science computer science software training and linguistic subjects
Innovative lecture presentation whiteboard
Self-paced learning
Ability to pinpoint exactly where your subject of interest is explained
Unlimited access to all courses for one price!
Unlimited personal support from the professor! All lesson questions and discussions are answered by the professor!

Choose a Subscription Plan:

Monthly	Annual
$35/mo.	$240/yr.

Or find out about our Multiuser plans: Corporate and Educational

Free Sample Lecture

Free Sample Lecture will get you started (Flash® 10 required).

Educator

the best free way to manage your classroom

Free Class Website!

Free Unlimited Hosting!

Free Educator.com Domain!

General Chemistry
with: Franklin Ow

Table of Contents
expand all collapse all

Quick links

Ready to join?

Subscription benefits:

Free Sample Lecture

Educator

the best free way to manage your classroom

Free Class Website!

Free Unlimited Hosting!

Free Educator.com Domain!

General Chemistrywith: Franklin Ow

Table of Contentsexpand all collapse all

Quick links

Ready to join?

Subscription benefits:

Free Sample Lecture

General Chemistry
with: Franklin Ow

Table of Contents
expand all collapse all