States of Matter, Intermolecular Forces, Gases and Gas laws, Chemistry

States of Matter, Intermolecular Forces, Gases and Gas laws

VIII. States of Matter: Lecture 1 | 61:12 min

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States of Matter, Intermolecular Forces, Gases and Gas laws

States of matter are solid (s), liquid (l), and gas (g)
Phase changes have names: freezing/melting; boiling/condensing
Solid going directly to gas: subliming; example dry ice, CO₂(g)
Forces between particles in decreasing order of strength are: ionic; ion/dipole; hydrogen bonding; dipole/dipole; London (dispersion)
H-bonding only for O…H; N…H; F…H
H-bonding very important in proteins, nucleic acids
The atmosphere: nitrogen, oxygen and 1% argon
Pressure = F/A
Units of pressure can be Pascals (SI); atmospheres (1 atm. = 760 mm Hg = 760 torr)
Kinetic molecular theory models gases as rapidly randomly moving molecules
Ideal gas law (includes other gas laws) PV = nRT; watch for consistency of units.
Molar mass of gas from gas density measurements: PV = (m/M)RT

States of Matter, Intermolecular Forces, Gases and Gas laws

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

States of Matter: Solid, Liquid, Gas

Phase Transitions

Ionic Forces and Ion Dipole Forces

Dipole-Dipole Forces and Hydrogen Bonding

Dispersion or London Forces

Boiling Points of Noble Gases

Hydrogen Bonding in Water and Biological Systems

Gaseous State: Kinetic Molecular Model

Gases of the Atmosphere

Percentage by Volume

Pressure

Mercury Barometer

Units of Pressure

Gas Laws and the Ideal Gas Law

Example: Gas Law Calculations

Molar Mass from Gas Law Calculations

Example: Experimental Gas

Additional Example 1

Additional Example 2

I. Introduction
	Introduction to Chemistry	47:38
II. Atoms
	Atomic Theory and Measurement	62:38
	The Chemist's Atom	22:20
III. Significant Figures
	Significant Figures and the Mole	51:06
IV. Equations and Formulas
	Balancing Equations, Limiting Reagents, Percentage Yield	58:17
	Empirical and Molecular Formulas	61:11
V. Chemical Reactions
	Classifying Chemical Reactions	42:43
	Energy in Chemical Reactions	63:47
VI. Electromagnetic Radiation
	Electromagnetic Radiation Quantum Theory	63:35
VII. Periodic Table and Bonding
	Periodic Table, Electronic Configurations, Ionic Bond	73:12
	Covalent Bond, Lewis Structures, Molecular Orbitals	77:27
	Shapes of Molecules and Hybridization	71:19
VIII. States of Matter
	States of Matter, Intermolecular Forces, Gases and Gas laws	61:12
IX. Gases
	Partial Pressure, Real Gases, Atmospheric Pollution	61:12
X. Phases
	Vapor Pressure, Boiling Point, Phase Diagrams	56:58
XI. Solids
	Types of Solids, X-Ray Diffraction, Unit Cells	57:30
XII. Carbon
	Carbon Allotropes, Band Theory of Solids	52:34
XIII. Solutions
	Solutions, Henry's Law, Concentration Equations	65:40
XIV. Colligative Properties
	Colligative Properties, Colloids, Surfactants	70:42
XV. Kinetics
	Kinetics, Rate Laws, Reaction Mechanism	68:48
XVI. Temperature Effects
	Temperature Effects, Reaction Rate Theory, Catalysis	62:56
XVII. Equilibrium
	Physical and Chemical Equilibrium, Equilibrium Law, Le Chatelier's Principle	70:47
XVIII. Acids and Bases
	Acids and Bases: Strong and Weak, pH	60:41
	pH Calculations, Polyprotic Acids	60:09
	Titrations, Indicators, Buffers	66:19
XIX. Solubility
	Solubility Product Constant, Precipitation	59:36
XX. Enthalpy and Entropy
	Enthalpy, Entropy, Second Law of Thermodynamics	53:51
XXI. Gibbs' Function
	Gibbs' Function, Equilibrium	61:10
XXII. Redox Reactions
	Balancing Redox Reactions, Half Reactions	67:26
XXIII. Electrochemistry
	Electrochemical Cells, Half-Cell Potentials	67:52
	Practical Batteries, Electrolysis	62:06
XXIV. Radioactivity
	Radioactivity, Nuclear Equations, Mass Energy Equivalence	40:35
	Radioactive Decay, Half-Life, Nuclear Reactions	56:12
XXV. Miscellaneous
	Organic Structures, Isomers, Functional Groups	68:32
	Chemistry and the Environment	50:13

Advanced Placement Chemistry

I. Introduction
	Introduction to Chemistry			47:38
		Intro		0:00
		What is Chemistry?		0:07
			Experimental Science	0:48
			Changes in Matter	1:18
			Energy and its Redistribution	2:20
			Central Science	2:45
		Properties of Matter		7:10
			Physical	7:45
			Example: Physical Properties	7:58
			Chemical	9:02
			Example: Chemical Properties	9:18
		Physical Changes (Reversible)		11:19
			Melting	11:39
			Boiling (Evaporation and Condensation)	13:21
			Dissolving (Solution)	15:41
		Chemical Changes		18:04
			Example: Balanced Chemical Equation	18:37
		Compositions of Matter		23:15
			Heterogeneous Mixture	23:27
			Example: Milk	23:40
			Example: Dirt	25:07
			Homogenous Mixture	25:40
			Example: Air, Gas, Vinegar	26:20
			Solutions vs Pure Substances	27:06
			Compounds and Elements	29:13
		Additional Example 1		8:52
		Additional Example 2		7:32
II. Atoms
	Atomic Theory and Measurement			62:38
		Intro		0:00
		Dalton's Atomic Theory		0:05
			Law of Multiple Proportions	3:10
		Current Atomic Theory		5:59
			Components: Electrons, Protons, Neutrons	6:51
			Isotopes	8:04
			Complex Molecules	9:35
		Fundamental Definition of an Element		11:27
			Nuclear Charge (Z)	11:35
			Atomic Number	12:37
			Isotopes	13:37
		Atomic Masses		15:53
			Hydrogen, Carbon, Chlorine	16:33
		Measurement		22:35
			SI Units	23:50
		Basic Units		26:39
			Meter, Kilogram, Second, Kelvin, Liter	26:52
		Multiplier Prefixes		33:05
		Measure Quantity		40:50
			Number x Unit	41:05
			Example: Height, Volume	41:16
		Additional Example 1		8:23
		Additional Example 2		4:03
	The Chemist's Atom			22:20
		Intro		0:00
		JJ Thompson and the Electron		1:11
			Cathode Ray Tube	1:19
			Electron Prediction	3:31
			Millikan, Charge of Electron	3:57
			Proton	4:45
		Rutherford and the Nucleus		5:42
			Alpha Particles	6:06
			Nucleus	8:05
		Chadwick and the Neutron		12:35
			Neutron	13:27
		Constitutions of Atoms		17:05
			Example: Hydrogen Isotopes	17:09
			Example: Iodine 127	20:08
III. Significant Figures
	Significant Figures and the Mole			51:06
		Intro		0:00
		Significant Figures: Sphere		0:14
		Example: Cube		7:11
			Example: Weight	10:40
		The Mole		13:36
			Examples: Number of Entities	14:00
			Avogadro's Number	15:10
			Carbon 12	16:16
			Mass of 1 Mol	17:49
			Molar Mass of Oxygen	20:01
		Stoichiometry		25:15
			Example: Molar Masses	26:25
		Molar Mass		26:39
			Example: Cholesterol	27:08
			Example: Insulin	38:38
		Additional Example 1		4:46
		Additional Example 2		5:16
IV. Equations and Formulas
	Balancing Equations, Limiting Reagents, Percentage Yield			58:17
		Intro		0:00
		Balancing Chemical Equations		0:49
			Atoms and Charges	1:50
			Example: Mercury and Oxygen	2:45
			Example: Combustion of a Hydrocarbon	6:19
		Redox: Oxidation and Reduction		12:30
			Example: Sodium and Chlorine	23:55
			Electron Transfer	19:34
		Limiting Reagent		22:25
			Example: Nuts and Bolts	22:45
			Example: Mercury and Oxygen	27:24
		Reaction Formulas		32:03
			Example: Iron Oxide and Carbon	32:11
			Example: Benzene and Chlorine	38:28
		Theoretical Yields, Actual Yields		42:13
			Percentage Yield	42:53
			Example	43:08
			Theoretical Yield from Limiting Reagent	45:11
			Example: Benzene and Chlorine	45:35
		Additional Example 1		3:12
		Additional Example 2		6:02
	Empirical and Molecular Formulas			61:11
		Intro		0:00
			Empirical Formula	0:45
			Molecular Formula	1:22
		Percentage by Mass		1:40
			Elements in Compounds	1:48
			Example: Water	2:44
			Example: Copper Sulfate	7:29
		Empirical Formula		13:02
			Example: Hydrocarbons	13:37
		Calculating Empirical Formula		20:24
			Example: C, H, O	20:32
		Molar Mass and Molecular Formulas		27:54
		Determining Molar Mass		32:21
			Mass Spectrometry	32:38
			Gas Laws	36:28
			Colligative Properties	39:18
		Empirical and Molecular Formulas		39:30
			Example: Ethylene and Chlorine	39:32
		Additional Example 1		5:23
		Additional Example 2		6:45
V. Chemical Reactions
	Classifying Chemical Reactions			42:43
		Intro		0:00
		Combustion Reactions		0:39
			Example: Balancing	2:33
		Exchange Reactions		7:58
			Example: Silver Nitrate + Sodium Chloride	9:11
			Precipitate	10:56
			Example: Sulfuric Acid + Sodium Chloride	13:20
			Naming Ions With Oxygen	16:10
			Example: Benzene and Chlorine	17:26
		Acid Base Reactions		18:50
			Recognizing Acids	19:18
			Recognizing Bases	23:48
			Litmus Test	26:02
			Common Acids	26:31
			Common Bases	28:40
		Redox Reactions		34:13
			Example: Potassium + Fluorine	35:54
			Example: Sodium + Oxygen	39:11
	Energy in Chemical Reactions			63:47
		Intro		0:00
		Forms of Energy		1:30
			Potential Energy and Kinetic Energy	1:32
			Example: Potential	2:53
			Example: Kinetic	4:07
		Units of Energy		5:20
			Example: Kinetic Energy, Joules	6:40
			Calorie	8:02
		Conservation of Energy		11:41
			First Law of Thermodynamics	12:22
		Heat Capacity and Measurement		17:10
			Heat Capacity	17:38
			Calorimeter	19:04
			Examples: Elements and Compounds	20:37
		Enthalpy		25:40
		Enthalpy Changes in Physical/Chemical Processes		31:25
			Exothermic	32:09
			Endothermic	34:16
			Example: Water	36:09
			Reversing a Process	38:21
			Example: Hydrogen + Oxygen	39:06
		Hess's Law		42:38
			Example: Hydrogen + Oxygen	43:46
		Enthalpy of Formation		47:05
			Example: Hydrogen + Oxygen	49:53
		Enthalpy of Formation: Carbon Disulfide		51:13
		Additional Example 1		5:42
VI. Electromagnetic Radiation
	Electromagnetic Radiation Quantum Theory			63:35
		Intro		0:00
		Waves and Their Characteristics		0:32
			Amplitude, Trough, Crest	1:01
			Wavelength	1:40
			Frequency	2:11
			Velocity (Speed of Light)	2:58
		Electromagnetic Radiation		5:10
			Gamma Rays and X-Rays	5:43
			Visible Light	6:19
			Infrared	6:54
			Radio Waves	7:16
		Spectra and Spectroscopy		7:58
		Hydrogen Atom Spectrum		10:13
			Emission Spectrum vs Absorption Spectrum	14:13
			Rydberg Formula	14:51
		Planck's Quantum Theory		16:55
			Black Body Radiation and Quanta	17:30
		Photoelectric Effect		23:29
		Bohr's Theory of the Hydrogen Atom		28:20
			Ground State	29:17
			Excited State	29:26
		Heisenberg and the Uncertainty Principle		34:48
		De Broglie and the Wave Nature of Particles		40:07
		Principle Quantum Number		44:05
		First Quantum Number		45:46
		m1 Quantum Number		51:00
		Spin Quantum Number		54:28
		Pauli Principle		54:58
		Additional Example 1		5:30
VII. Periodic Table and Bonding
	Periodic Table, Electronic Configurations, Ionic Bond			73:12
		Intro		0:00
		Periodic Law of Mendeleev and Meyer		0:43
		Modern Periodic Table		5:09
			Atomic Number	5:51
			Noble Gases	6:46
			Halogens	7:06
			Group Number	7:16
			Metals	8:07
			Groups and Periods	8:30
			Transition Metals	9:18
			Lanthanides	10:23
			Actinides	11:26
		Quantum Numbers and the Shape of the Table		12:06
		Electron Configuration of Atoms		17:59
		Electron Configuration of Neutral Atoms		19:49
			Example: Elements	20:23
			Example: Noble Gases	25:26
		Electron Configuration of Monatomic Ions		28:40
			Example: Elements	29:42
		Atomic Size		37:59
			Larger as Down a Group	38:44
			Smaller as Across a Period	39:34
		Sizes of Monatomic Ions		42:05
			Example: Elements	43:15
		Noble Gas Electron Configurations		45:52
			Example: Elements	46:10
		Electron Affinity		50:20
		Ionization Energy		52:32
			Example: First Ionization Energy	52:43
			Periodic Table Trend	53:37
			Example: Boron	54:22
		Ionic Compounds (NaCl)		57:00
			Ionic Bond (Electrostatic)	57:57
		Additional Example 1		9:08
		Additional Example 2		5:59
	Covalent Bond, Lewis Structures, Molecular Orbitals			77:27
		Intro		0:00
		Covalent Bond		1:05
			Hydrogen Atom	1:38
			Lewis	2:41
			Sharing of Electrons	3:14
		Valence Electrons		4:13
			Example: Lewis Symbols	5:35
		Lewis Structures of Atoms and Ions		10:05
			Example: Ions	10:56
		Octet Rule		13:34
			Noble Gases	14:14
		How to Draw Lewis Structures		17:35
			Single Bond	21:39
			Double Bond	21:54
			Triple Bond	22:02
			Examples: Compounds	22:23
		Formal Charges		32:44
			Example: 3 Structures of FCN	34:01
		Exceptions to the Octet Rule		40:17
			Fewer Than 8 Electrons	41:07
			Example: Boron (Electron Deficiency)	41:53
			More Than 8 Electrons	44:22
			Example: Compounds	45:37
		Electronegativity		48:09
			Example: Values	49:24
			Ionic or Polar Covalent Bond	52:02
		Molecular Orbitals		54:16
		Sigma and Pi Bonding		55:56
		Additional Example 1		11:33
		Additional Example 2		7:14
	Shapes of Molecules and Hybridization			71:19
		Intro		0:00
		VSEPR: Valence Shell Electron Pair Repulsion		0:53
		Counting Electron Sets		4:20
			Example: Methane	4:48
			Example: Ammonia	5:48
			Example: Formaldehyde	7:06
			Example: Hydrogen Cyanide	8:48
		Geometry of 2 and 3 Sets		10:28
			Two Sets: Linear	11:30
			Examples	11:57
			Three Sets: Trigonal and Planar	14:29
			Examples	15:48
		Geometry of 4 Sets		19:46
			Four Sets: Tetrahedral	20:08
			Examples	22:03
		Geometry of 5 and 6 Sets		27:50
			Five Sets: Trigonal Bipyramid	28:12
			Six Sets: Octahedron	30:28
		Hybridization and Hybrid Orbitals		32:07
			Linus Pauling	33:27
			Example: Carbon	33:46
		Orbital Phases		40:14
			Wave Function Phases	40:20
			Example: 2p Orbital	41:09
		Sigma Bonds		42:51
			Example: Ethane	46:37
		Pi Bonds		49:04
			Example: Ethylene	50:15
		Additional Example 1		10:31
		Additional Example 2		5:45
VIII. States of Matter
	States of Matter, Intermolecular Forces, Gases and Gas laws			61:12
		Intro		0:00
		States of Matter: Solid, Liquid, Gas		0:43
			Solid	1:10
			Liquid	2:14
			Gas	3:10
		Phase Transitions		4:36
			Melting, Freezing, Boiling, Condensing	5:09
			Sublimation, Condensation	6:49
			Example: Dry Ice	7:25
		Ionic Forces and Ion Dipole Forces		8:42
			Example: Ionic Forces	11:04
			Example: Ion Dipole Forces (Polar)	12:44
		Dipole-Dipole Forces and Hydrogen Bonding		15:51
			Example: Water Molecules	16:06
			Example: Liquid Hydrogen Chloride	16:46
			Strong Dipole-Dipole, Hydrogen Bonds	17:43
			Boiling Points	19:30
		Dispersion or London Forces		22:36
			Boiling Points of Noble Gases	26:39
		Hydrogen Bonding in Water and Biological Systems		28:17
			Example: Crystalline Water (Open Structure)	28:28
			Example: Protein	29:34
			Example: DNA Double Helix	30:31
		Gaseous State: Kinetic Molecular Model		31:00
		Gases of the Atmosphere		33:31
			Percentage by Volume	33:59
		Pressure		33:15
			Mercury Barometer	36:14
		Units of Pressure		38:33
			Pascal	39:23
			Bar, Torr, Atm	39:49
		Gas Laws and the Ideal Gas Law		41:47
			Boyle's Law	42:01
			Charles' Law	42:45
			Ideal Gas Law (Combined Law)	43:25
			Gas Constant R	44:11
		Example: Gas Law Calculations		45:02
		Molar Mass from Gas Law Calculations		47:21
			Example: Experimental Gas	48:21
		Additional Example 1		5:29
		Additional Example 2		4:03
IX. Gases
	Partial Pressure, Real Gases, Atmospheric Pollution			61:12
		Intro		0:00
		Partial Pressure and Mole Fraction		1:08
			Example: Gases A, B, C	3:00
			Example: Mole Fraction of A, B, C	4:28
		Dalton's Law of Partial Pressures		6:29
			Example: Gases A, B, C	8:14
			Example: Air	11:27
		Applications of Dalton's Law		12:23
			Example: Potassium Chlorate	12:39
		Real Gases		20:16
			Example: Hydrogen and Nitrogen	21:05
			Departure from Ideal Gas Law	23:42
		Van der Waals' Equation		28:52
			Corrective Equation	31:18
		Ozone and the Ozone Hole		34:01
			How Ozone is Formed	35:56
		Effects of Chlorofluorocarbons (CFC)		40:49
			Example: Freon	52:59
		Oxides of Nitrogen		47:15
		Sulfur Dioxide		51:32
		Acid Rain		54:19
		Additional Example 1		3:11
X. Phases
	Vapor Pressure, Boiling Point, Phase Diagrams			56:58
		Intro		0:00
		Vapor Pressure: An Equilibrium Phenomenon		0:55
			Thought Experiment: Water Equilibrium	1:06
		Boiling Point and Normal Boiling Point		6:19
			Reducing Boiling Point	3:10
			Example: Water	9:51
		Surface Tension		14:12
			Example: Water	15:55
		Viscosity		19:53
			Intermolecular Forces	22:22
			Example: Ethanol, Antifreeze, Glycerol	22:52
		Enthalpies of Phase Changes		28:08
			Example: Water	28:22
		Phase Diagrams (Water)		32:22
			Vapor Pressure Curve	35:30
			Melting Point Line	35:54
			Triple Point	36:36
			Critical Point	37:50
		Phase Diagrams (Carbon Dioxide)		38:42
			Sublimation	40:11
			Critical Point	42:56
		Triple Point and Critical Point		44:54
			Example: Carbon Dioxide	46:11
XI. Solids
	Types of Solids, X-Ray Diffraction, Unit Cells			57:30
		Intro		0:00
		Solids: Crystalline and Amorphous		0:59
			X-Ray Diffraction	4:30
		Types of Crystalline Solids: Atomic		5:39
			Example: Metallic Copper	5:50
		Types of Crystalline Solids: Ionic Crystal		7:20
			Example: NaCl	7:37
		Types of Crystalline Solids: Molecular Crystal		11:30
			Example: Ice	11:42
		Types of Crystalline Solids: Network Solid		13:22
			Example: Carbon Allotropes (Diamond and Graphite)	13:36
		X-Ray Diffraction and Bragg's Law		18:26
			Bragg's Law Equation	23:53
		Unit Cell		26:55
			Simple Cubic Unit Cell	27:47
		Face-Centered and Body-Centered Unit Cells		31:06
			Body-Centered Cubic	31:22
			Face-Centered Cubic	32:53
		Unit Cell and Densities of Crystalline Solids		36:13
			Example: Platinum	36:39
		First Law of Thermodynamics and Lattice Energy		42:14
			Example: NaCl	42:33
		Lattice Energies and Constitutions of Ionic Solids		47:33
		Additional Example 1		7:09
XII. Carbon
	Carbon Allotropes, Band Theory of Solids			52:34
		Intro		0:00
		Diamond and Graphite		0:55
			Diamond	1:32
			Graphite	3:25
		C-60: An Unexpected Allotrope		6:59
			Buckyball (R. Buckminster Fuller)	9:30
		Carbon Nanotubes		11:42
			Possible Uses	13:51
		Metals, Semiconductors, and Insulators		15:34
			3 Classes of Conductors	15:41
		Conductivity and Band Theory		20:30
			Example: Valence Band	22:46
		P-Type and N-Type Semiconductors		27:21
			Phosphorus to Silicon	29:21
			Boron to Silicon	31:38
		P/N Junctions		33:48
			Integrated Circuit	38:49
		Glasses and Ceramics		40:26
			Glasses	41:02
			Example: Common Window Glass	44:49
			Ceramics	47:16
XIII. Solutions
	Solutions, Henry's Law, Concentration Equations			65:40
		Intro		0:00
		Types of Solutions		1:43
			Examples: Homogeneous Mixtures	2:37
			Examples: Solid Solutions	6:59
		Saturation Solubility		8:47
			Example: Solvent and Soluten (Salt and Water)	9:15
			Solubility Dependencies	14:54
		Henry's Law		15:36
			Values for Henry's Law Constant (Water)	18:01
			Example: Soda Can	19:27
			Example: SCUBA	21:10
		Solution Concentration Expressions		26:02
			Percentage by Mass	26:16
			Example: Salt and Water	26:52
			Molarity	28:18
			Molality	31:26
		Calculation of Solution Concentrations		32:42
			Example: Sodium Chloride Solution	32:49
		Dilution of Solutions		37:35
			Example: Hydrochloric Acid	38:54
		Effects of Temperature on Solubility (Gases in Liquids)		42:01
			Example: Water	42:40
		Effects of Temperature on Solubility (Solids in Liquids)		45:42
			Examples: Various Salts	46:47
		Entropy: Qualitative Introduction		52:25
		Temperature Effects: Enthalpy, Entropy		55:39
		Additional Example 1		7:20
XIV. Colligative Properties
	Colligative Properties, Colloids, Surfactants			70:42
		Intro		0:00
		Colligative Properties and Raoult's Law		0:43
			Colligative (Collective)	0:46
			Raoult's Law	1:55
			Uses of Raoult's Law (Mole Fraction and Molar Mass)	4:34
		Boiling Point Elevation, Freezing Point Depression		5:47
			Pure Water and Solution in Water	6:17
			Lower Vapor Pressure	6:53
			Higher Boiling Point (Elevation)	7:04
			Lower Freezing Point (Depression)	7:52
			Example: Antifreeze	8:37
			Change in Boiling Point (Molality)	10:55
		Molar Mass from Elevation and Depression		12:49
			Example: Water and Cystine	13:20
		Van der Waals' Alpha Factor		18:59
			Alpha Factor Equation	20:15
			Example: Salt Ions	21:11
		Osmosis		23:02
			Blood (Isotonic, Hypertonic, Hypotonic)	23:47
		Osmotic Pressure		27:40
			Osmotic Pressure Definition (Pi)	30:14
			Van der Waals'	30:57
		Molar Mass from Osmotic Pressure		33:29
			Example: Peptide in Water	34:20
		Colloids and the Tyndall Effect		38:33
			Light Beam (Solution and Colloidal Suspension)	41:05
		Surfactants		44:11
			Example: Sodium Stearate (Soap)	45:10
		Soaps and Detergents		49:24
			Ordinary Soaps Problem	52:36
			Synthetic Soaps	53:57
		Additional Example 1		5:57
		Additional Example 2		6:41
XV. Kinetics
	Kinetics, Rate Laws, Reaction Mechanism			68:48
		Intro		0:00
		Reaction Rate		1:30
			Chemical Reaction Rate	2:36
			Example: Methyl Bromide and Sodium Hydroxide	4:04
		Reaction Rates: Changing Concentrations		10:28
			Example: Double Initial Concentrations	11:33
		Order of Reaction		17:05
			Experimental Rate Law	17:47
			Overall Rate	21:27
		Initial Rate Measurement		23:24
			Example: Methyl Bromide and Sodium Hydroxide	23:44
		Integrated Rate Laws: First Order Reaction		29:54
			Integrated Rate Equation	31:12
			Example: Transitional Metal Complex	33:48
		Integrated Rate Laws: Second Order Reaction		38:12
			Integrated Rate Equation	38:37
		Experimental Rate Laws		39:41
			Example: Transitional Metal Complex	39:55
		Experimental Rate Laws, cont.		42:45
			Example: Nitramide	43:00
		Reaction Mechanism		46:12
			Hypothetical Aspect	47:38
			Predict Outcomes	48:02
		Elementary Reactions and Reaction Mechanisms		49:43
			Example: Methyl Bromide and Hydroxide Ion	51:02
		Rate Limiting Step		54:47
			Example: Rate Limiting Step	55:41
		Additional Example 1		3:00
		Additional Example 2		7:07
XVI. Temperature Effects
	Temperature Effects, Reaction Rate Theory, Catalysis			62:56
		Intro		0:00
		Effects of Temperature on Reaction Rates		1:05
			Common Examples	4:30
		Arrhenius' Equation		6:40
			Activation Energy	9:09
			Example: Nitrogen Pentoxide	11:52
		Reaction Rate Theory		15:20
			Activated Complex and Transition State	17:05
			Example: Methyl Bromide and Hydroxide Ion	19:58
		Calculating Activation Energy		22:32
			Plotting ln K and Inverse T	23:38
		Catalysis in Practice		25:33
			Example: Catalytic Converter	26:43
			Example: Oil Refinery	29:30
		Acid Catalysis of Ehtyl Acetate Hydrolysis		31:48
			Example	32:03
		Industrial Production of Ammonia		35:54
			Haber Bosch Process	36:06
		Industrial Production of Sulfuric Acid		41:02
			Series of Processes	41:38
		Enzymes as Catalysts		45:59
			Example: Amino Acid	47:04
			Example: Protein	47:18
		Additional Example 1		4:15
XVII. Equilibrium
	Physical and Chemical Equilibrium, Equilibrium Law, Le Chatelier's Principle			70:47
		Intro		0:00
		Equilibrium in Physical Processes		1:13
			Example: Water Equilibrium (Vapor Pressure)	1:30
			Example: Water Equilibrium (Melting )	1:58
		Equilibrium in Chemical Processes		3:37
			Example: Acetic Acid and Ethanol	3:51
		The Equilibrium Law and Equilibrium Constant		9:11
			Equilibrium Law	11:32
			Equilibrium Constant K	12:47
		Equilibrium Expressions and Constants		14:11
			Example: Acetic Acid and Ethanol	14:24
			Example: Calcium Carbonate (Lime Burning)	17:23
		Standard Concentration and Activities		21:13
		Kp and Kr		23:56
			Example: Nitric Oxide	24:26
		Calculations of Equilibria		29:06
			Example: Acetic Acid and Ethanol	29:17
		Le Chatelier's Principle		40:47
			Stressors	42:55
			Example: Haber Bosch	49:26
		Additional Example 1		6:48
		Additional Example 2		6:29
XVIII. Acids and Bases
	Acids and Bases: Strong and Weak, pH			60:41
		Intro		0:00
		Acids		0:36
			React with Some Metals	2:25
			Litmus Test (Red)	3:04
		Bases		4:33
			Litmus Test (Blue)	5:52
			Acids and Base Neutralize	6:43
		Classification: Arrhenius and Bronsted-Lowry		8:52
			Arrhenius Classification	9:11
			Example: HCl (Hydronium) and NaOH (Hydroxide)	11:08
			Bronsted-Lowry Classification	12:42
			Example: HCl	13:30
			Conjugate Acid, Conjugate Base	14:08
		Lewis Acids and Bases		16:23
			Lewis Base: Electron Pair Donor	17:24
			Lewis Acid: Electron Pair Acceptor	18:24
			Example: Lewis Acid Base Reaction	20:03
		Common Strong Acids		22:02
		Common Strong Bases		24:39
		Common Weak Acids		26:24
		Common Weak Bases		31:14
		Water as an Acid and Base: Kw		34:01
			K of Water	35:21
		Ionization Constants for Weak Acids		38:11
			Examples: Constants	38:20
		Ionization Constants for Weak Bases		40:30
			Examples: Constants	40:44
		pH and the pH Scale		43:12
			Sorenson pH	43:46
			Neutral Water	44:48
			Acid and Base pH	46:24
			pH Scale (Acid and Alkaline)	47:30
		Additional Example 1		5:53
	pH Calculations, Polyprotic Acids			60:09
		Intro		0:00
		pH in a Solution of a Weak Acid		0:45
			Vinegar (Acetic Acid)	1:00
			Example: pH of Acetic Acid Solution	2:34
		pH in a Solution of a Weak Base		9:42
			Ammonia	9:48
			Example: pH of Pyridine Solution	11:46
		Salts of Weak Acids with Strong Bases		17:15
			Example: Acetic Acid and Sodium Hydroxide	17:55
		Salts of Weak Bases with Strong Acids		20:55
			Example: Ammonia and Hydrochloric Acid	21:13
		Conjugate Acid Base Pairs: Ka and Kb		22:58
			Example: Acetic Acid Ionization	23:06
		Polyprotic Acids: Successive Ka Values		28:50
			Example: Diprotic Acid (Sulfuric Acid)	29:13
			Example: Tripotic Acid (Phosphoric Acid)	29:28
		pH in a Polyprotic Acid Solution		41:02
			Example: Phosphoric Acid Solution pH	41:21
		Salts of Polyprotic Acids		47:32
			Examples: TSP, Tartaric Acid	47:45
		Additional Example 1		6:15
	Titrations, Indicators, Buffers			66:19
		Intro		0:00
		Titration and Analysis		0:43
			Equipment: Burets, Pipet, Stopcock, Volumetric Flask	1:38
			Molarity	4:04
		Strong Acid-Strong Base Titration		6:16
			Example: Sodium Hydroxide and Hydrochloric Acid	7:04
		Weak Acid-Strong Base Titration		16:45
			Example: Acetic Acid and Sodium Hydroxide	17:06
		pH Meter		28:48
			pH Electrode: Logarithmic Change to Hydronium	29:19
		Indicators		32:10
			Example: Indicator and Hydronium	33:21
			Phenolphthalein	34:07
			Methyl Orange	35:12
		Theory and Choice of Indicators		39:19
			Indicator Visibility if Factor of 10	40:45
		Buffers		42:47
			What is a Buffer Solution?	46:08
			Acetate Buffer and Ammonium Buffer	47:16
			Example: Buffer Effects	48:26
		Buffer Regions in Titrations		51:38
			Example: Acetic Acid and Sodium Hydroxide	51:48
		Practical Buffers		55:17
			Example: Acetic Acid and Acetate Ion (pH Range)	55:27
		Additional Example 1		7:51
XIX. Solubility
	Solubility Product Constant, Precipitation			59:36
		Intro		0:00
		Equilibrium in Saturated Salt Solution		1:12
			Example: Silver Chloride	1:50
			Ksp (Solubility Product Constant)	4:12
		Solubility Product Constant		6:19
			Example : Lead Iodide	6:31
		Limitations of the Solubility Product		9:06
			Low Solubility	9:23
			Complexes that are Soluble	11:31
		Ksp Values and Ion Concentrations		13:28
			Example: Silver Chloride	16:06
			Example: Lead Chloride	19:22
		Precipitation of Salts		23:56
			Example: Silver Bromide and Copper Bromide	25:31
		Common Ion Effect		31:52
			Example: Lead Sulfate	32:11
			Le Chatelier's Principle	39:30
		Common Ion Solubility		42:37
			Example: Lead Chloride in Sodium Chloride Solution	42:46
		Acids, Bases, and Solubility Equilibria		48:32
			Example: Lead Carbonate	48:46
			Lle Chatelier's Principle	54:26
		Group Separation and Qualitative Analysis of Metal Ions		55:09
			Examples	56:25
		Additional Example 1		5:42
XX. Enthalpy and Entropy
	Enthalpy, Entropy, Second Law of Thermodynamics			53:51
		Intro		0:00
		Factors Affecting Equilibrium Constants		1:15
			Spontaneous Reaction	2:17
			Temperature Effects	4:50
		State Functions: Enthalpy and Entropy		6:17
			Example: Methane and Chlorine	8:32
			Hess's Law	10:36
			Entropy	10:55
		Statistical Interpretation of Entropy		13:24
			Boltzmann Entropy Equation	13:33
			Reversible Change	16:24
			Example: Water and Ice	16:55
		Third Law of Thermodynamics		20:06
			Nernst	20:31
		Entropies of Gases, Liquids, and Solids		23:16
			Example: Entropy Values	25:17
		Entropy Values from Enthalpy/Temperature		28:55
			Example: Water (Graph)	29:34
		Entropy Changes in Phase Changes		32:33
			Melting (Fusion)	32:41
			Example: Water Melting	33:15
		Second Law of Thermodynamics		34:21
			Example: Hydrogen and Oxygen	37:20
			Statement of Second Law (Spontaneous/Reversible)	39:28
		Reactant Favored and Product Favored Equilibria		41:10
			Reactant or Product Favored	41:48
			Converse	45:15
		Limitations of Applying the Second Law to Equilibria		46:57
			Delta S	47:30
XXI. Gibbs' Function
	Gibbs' Function, Equilibrium			61:10
		Intro		0:00
		The Gibbs' Function		0:35
			Values of Delta G	4:57
		The Gibbs' Function and K		9:11
			Gibbs' Function Change (Free Energy)	11:06
			Values of Gibbs' Function Standard Change	14:17
		Calculation of K from ThermoDynamic Data		15:46
			Example: Nitrogen Dioxide to Dinitrogen Tetroxide	16:01
		Calculation of K		24:32
			Example: Diamond to Graphite	24:46
		Calculation of K		31:33
			Example: Ammonia	31:38
		Temperature Changes: Gibbs' Function and K		38:12
			Estimating Gibbs' Function Values at Temperatures	40:04
		Temperature Changes		42:29
			Example: Oxide of Iron and Carbon	42:49
		Additional Example 1		8:26
XXII. Redox Reactions
	Balancing Redox Reactions, Half Reactions			67:26
		Intro		0:00
		Oxidation and Reduction Review		0:58
			Example: Sodium and Chlorine	1:05
		Determining Oxidation Numbers		5:43
			Rules for Assigning Oxidation Numbers	8:02
		Oxidation Number Assignment		11:25
			Examples: Various	11:42
		Balancing Half Reactions		18:26
			Example: Half Reactions	21:22
			Example: Zinc in Hydrochloric Acid	22:34
		Combining Half Reactions Into Complete Reactions		24:32
			Example: Zinc	24:40
			Spectator Ions	26:10
		Half Reactions in Acidic and Basic Solutions		28:38
			Example: Permanganate	29:18
		Balancing Redox Reactions		36:34
			Example: Determination of Iron	37:22
		Balancing Redox Reactions		45:54
			Example: Lead Dioxide and Chloride Ion	46:12
		Additional Example 1		5:14
		Additional Example 2		9:28
XXIII. Electrochemistry
	Electrochemical Cells, Half-Cell Potentials			67:52
		Intro		0:00
		Electricity from Chemical Reactions		0:29
			Galvani Volta: Current Electricity	0:40
			Voltaic Pile (Battery)	3:33
			Potato Clock	4:35
		Daniell Cell		5:56
			Oxidation of Zinc, Reduction of Copper	6:46
			Spontaneous Overall Reaction	8:25
			Anode and Cathode	9:20
		Current Electricity Fundamentals		11:34
			Electric Charge: Coulomb	11:46
			Electric Current: Ampere	12:33
			Volt	14:43
			Ohm's Law	16:16
		Galvanic Cell		17:41
			Salt Bridge	19:35
		Cell Potential and Work		20:56
			Joules	21:40
			Coulombs	22:27
		Hydrogen Electrode		22:53
			Breakdown	24:12
		Half-Cell Potentials		29:24
			Example: Zinc and Standard Hydrogen Electrode (SHE)	30:50
		Electrochemical Series		35:04
			Example: Aluminum Reducing Iron Ion	38:26
		Nernst Equation		41:46
			Faraday	42:09
			Example: Concentration Cell (Copper Ions)	46:39
		Nernst Equation: pH Meter		52:24
			Example: Potential and pH	53:21
		Nernst Equation: Ion Concentrations		56:11
		Additional Example 1		5:19
		Additional Example 2		5:12
	Practical Batteries, Electrolysis			62:06
		Intro		0:00
		Primary Batteries		0:54
			Leclanche Dry Cell	1:03
			Alkaline Cell	4:34
		Fuel Cell		6:53
			Overall Reaction	8:24
		Secondary Batteries		13:47
			Car Battery	14:04
		Electrolysis		18:41
			Aluminum Plant	19:14
			Chromium Plating	22:42
		Sodium Chloride		24:08
			Example: Metallic Na	24:20
			Example: Bleach	28:38
		Faraday's Laws		32:22
			Example: Aluminum Electrolysis	34:54
		Corrosion of Iron		41:24
			Example: Iron Galvanic Cell	44:34
		Protection of Iron Against Corrosion		46:55
			Coating of Tin Cans	47:18
		Additional Example 1		4:45
XXIV. Radioactivity
	Radioactivity, Nuclear Equations, Mass Energy Equivalence			40:35
		Intro		0:00
		Radioactivity Pioneers		0:36
			Becquerel	2:20
			Curie	1:53
			Rutherford	2:38
			Soddy	2:55
		Alpha, Beta, and Gamma Radiation		3:46
			Three Types of Emission	4:28
		Transmutation and Nuclear Equations		7:01
			Decay of Uranium	8:07
		Balancing Nuclear Equations		13:08
			Example: Chromium	13:19
			Example: Radium	15:56
		Synthesis of New Isotopes and Elements		18:47
			Example: Nitrogen and Alpha Particles	19:44
			Example: Uranium and Carbon Nuclei	21:41
		Mass Changes in Nuclear Transformations		23:55
			Mass and Energy Equivalence (e=mc2, Einstein)	24:39
		Mass-Energy Transformations		28:35
			Example: Uranium	28:38
		Stability of Nuclei and Binding Energy		33:11
			Nucleons	33:34
			Example: Deuterium and Helium	33:51
		Curve of Binding Energy; Fission and Fusion		35:53
	Radioactive Decay, Half-Life, Nuclear Reactions			56:12
		Intro		0:00
		First Order Nuclear Decay		0:41
			Example: Uranium	2:01
			Rate Constant	3:42
			Integrated Rate Equation	3:52
			Half-Life	5:14
		Half-Lives and Rate Constants		6:09
			Examples: Various	6:14
		Radioactive Dating: Rocks		9:18
			Example: Rock with Uranium and Lead	10:53
		Radioactive Dating: Carbon-14		17:27
			Example: Shroud of Turin	20:54
			Example: Wooden Staff	22:31
		Nuclear Fusion in Stars		27:22
			Example: Reaction in Sun	29:21
		Nuclear Weapons		32:24
			Example: Uranium Isotope	34:14
		Nuclear Power		38:52
			Nuclear Power Usage	42:30
		Nuclear Wastes and Their Disposal		45:03
		Additional Example 1		5:33
XXV. Miscellaneous
	Organic Structures, Isomers, Functional Groups			68:32
		Intro		0:00
		Saturated Hydrocarbons C-1 to C-4		1:41
			Acyclic	2:38
			Example: Methane, Ethane, Propane	3:28
			Isomers	7:19
		Acyclic Saturated Hydrocarbons C-5 Isomers		10:27
			Example: Pentanes	10:40
		Alkenes and Ring Compounds		14:56
			Alkenes	15:34
			Example: Ethene, Ethylene	16:25
			Example: Propene Isomers	19:19
		Geometric Isomers of Alkenes		24:13
			Example: 2-Butene	24:34
			Trans and Cis	26:27
		Optical Isomers		28:45
			Example: Carbon Atom	33:49
		Functional Groups: Alcohols and Caboxylic Acids		39:11
			Alcohols	39:27
			Carboxylic Acids	41:41
		Functional Groups: Esters and Ethers		44:10
			Esters (Ethyl Acetate)	44:27
			Ethers (Diethylether)	46:14
		Functional Groups: Aldehydes and Ketones		47:48
			Examples	47:59
		Amines		51:01
		Amide Group		54:24
		Peptides and Proteins		56:02
		Additional Example 1		9:41
	Chemistry and the Environment			50:13
		Intro		0:00
		Global Climate Change		1:41
			Greenhouse Gases	3:49
		Greenhouse Gases and Climate Change		6:53
			Last 100 Years	9:11
		Water Pollution: Eutrophication		12:59
			Example: Fertilizers	15:41
		Water Pollution: Organic Pollutants		9:15
			Chlorinated Hydrocarbons (DDT)	19:30
			Dioxins and Phthalates	20:58
		Water Pollution: Heavy Metal Pollutants		23:58
			Examples: Lead, Chromium, Arsenic	24:17
		Radiation in the Environment		24:35
			Thresholds	39:20

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States of Matter, Intermolecular Forces, Gases and Gas laws

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Advanced Placement Chemistry

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	Chemistry by Chang, 10th Edition, Solutions Manual Author: Raymond Chang ISBN: 73226742 Publisher: McGraw-Hill Science/Engineering/Math Year: 2009 This book is the solutions manual for Chemistry by Raymond Chang, 10th edition.