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Professor Goldwhite

Professor Goldwhite

Periodic Table, Electronic Configurations, Ionic Bond

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Table of Contents

Section 1: Introduction
Introduction to Chemistry

47m 38s

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
-1
Additional Example 2
-2
Section 2: Atoms
Atomic Theory and Measurement

1h 2m 38s

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
-1
Additional Example 2
-2
The Chemist's Atom

22m 20s

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
Section 3: Significant Figures
Significant Figures and the Mole

51m 6s

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
-1
Additional Example 2
-2
Section 4: Equations and Formulas
Balancing Equations, Limiting Reagents, Percentage Yield

58m 17s

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
-1
Additional Example 2
-2
Empirical and Molecular Formulas

1h 1m 11s

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
-1
Additional Example 2
-2
Section 5: Chemical Reactions
Classifying Chemical Reactions

42m 43s

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

1h 3m 47s

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
-1
Section 6: Electromagnetic Radiation
Electromagnetic Radiation Quantum Theory

1h 3m 35s

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
-1
Section 7: Periodic Table and Bonding
Periodic Table, Electronic Configurations, Ionic Bond

1h 13m 12s

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
-1
Additional Example 2
-2
Covalent Bond, Lewis Structures, Molecular Orbitals

1h 17m 27s

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
-1
Additional Example 2
-2
Shapes of Molecules and Hybridization

1h 11m 19s

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
-1
Additional Example 2
-2
Section 8: States of Matter
States of Matter, Intermolecular Forces, Gases and Gas laws

1h 1m 12s

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
-1
Additional Example 2
-2
Section 9: Gases
Partial Pressure, Real Gases, Atmospheric Pollution

1h 1m 12s

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
-1
Section 10: Phases
Vapor Pressure, Boiling Point, Phase Diagrams

56m 58s

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
Section 11: Solids
Types of Solids, X-Ray Diffraction, Unit Cells

57m 30s

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
-1
Section 12: Carbon
Carbon Allotropes, Band Theory of Solids

52m 34s

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
Section 13: Solutions
Solutions, Henry's Law, Concentration Equations

1h 5m 40s

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
-1
Section 14: Colligative Properties
Colligative Properties, Colloids, Surfactants

1h 10m 42s

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
-1
Additional Example 2
-2
Section 15: Kinetics
Kinetics, Rate Laws, Reaction Mechanism

1h 8m 48s

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
-1
Additional Example 2
-2
Section 16: Temperature Effects
Temperature Effects, Reaction Rate Theory, Catalysis

1h 2m 56s

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
-1
Section 17: Equilibrium
Physical and Chemical Equilibrium, Equilibrium Law, Le Chatelier's Principle

1h 10m 47s

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
-1
Additional Example 2
-2
Section 18: Acids and Bases
Acids and Bases: Strong and Weak, pH

1h 41s

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
-1
pH Calculations, Polyprotic Acids

1h 9s

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
-1
Titrations, Indicators, Buffers

1h 6m 19s

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
-1
Section 19: Solubility
Solubility Product Constant, Precipitation

59m 36s

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
-1
Section 20: Enthalpy and Entropy
Enthalpy, Entropy, Second Law of Thermodynamics

53m 51s

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
Section 21: Gibbs' Function
Gibbs' Function, Equilibrium

1h 1m 10s

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
-1
Section 22: Redox Reactions
Balancing Redox Reactions, Half Reactions

1h 7m 26s

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
-1
Additional Example 2
-2
Section 23: Electrochemistry
Electrochemical Cells, Half-Cell Potentials

1h 7m 52s

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
-1
Additional Example 2
-2
Practical Batteries, Electrolysis

1h 2m 6s

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
-1
Section 24: Radioactivity
Radioactivity, Nuclear Equations, Mass Energy Equivalence

40m 35s

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

56m 12s

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
-1
Section 25: Miscellaneous
Organic Structures, Isomers, Functional Groups

1h 8m 32s

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
-1
Chemistry and the Environment

50m 13s

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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