Chemistry explains the world around us. Everything we can see, and many things that we cannot, are made up of chemical elements and molecules. No one knows the ways in which chemistry shapes our world better than Dr. Harold Goldwhite. His experience on the History Channel coupled with over 45+ years teaching transform his lectures into an informative and fascinating journey. Dr. Goldwhite’s comprehensive syllabus is perfect for standard and accelerated one year chemistry courses. He covers everything from Atomic Theory, Chemical Reactions, Bonds, Kinetics, Acids and Bases, and Thermodynamics to Electrochemistry and Radioactivity. Dr. Goldwhite received his Ph.D and B.A. from the University of Cambridge.
| 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 |
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Electrochemical Cells, Half-Cell Potentials |
67:52 |
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Intro |
0:00 | |
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Electricity from Chemical Reactions |
0:29 | |
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| Galvani Volta: Current Electricity |
0:40 | |
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| Voltaic Pile (Battery) |
3:33 | |
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| Potato Clock |
4:35 | |
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Daniell Cell |
5:56 | |
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| Oxidation of Zinc, Reduction of Copper |
6:46 | |
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| Spontaneous Overall Reaction |
8:25 | |
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| Anode and Cathode |
9:20 | |
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Current Electricity Fundamentals |
11:34 | |
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| Electric Charge: Coulomb |
11:46 | |
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| Electric Current: Ampere |
12:33 | |
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| Volt |
14:43 | |
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| Ohm's Law |
16:16 | |
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Galvanic Cell |
17:41 | |
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| Salt Bridge |
19:35 | |
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Cell Potential and Work |
20:56 | |
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| Joules |
21:40 | |
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| Coulombs |
22:27 | |
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Hydrogen Electrode |
22:53 | |
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| Breakdown |
24:12 | |
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Half-Cell Potentials |
29:24 | |
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| Example: Zinc and Standard Hydrogen Electrode (SHE) |
30:50 | |
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Electrochemical Series |
35:04 | |
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| Example: Aluminum Reducing Iron Ion |
38:26 | |
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Nernst Equation |
41:46 | |
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| Faraday |
42:09 | |
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| Example: Concentration Cell (Copper Ions) |
46:39 | |
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Nernst Equation: pH Meter |
52:24 | |
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| Example: Potential and pH |
53:21 | |
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Nernst Equation: Ion Concentrations |
56:11 | |
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Additional Example 1 |
5:19 | |
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Additional Example 2 |
5:12 | |
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Practical Batteries, Electrolysis |
62:06 |
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Intro |
0:00 | |
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Primary Batteries |
0:54 | |
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| Leclanche Dry Cell |
1:03 | |
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| Alkaline Cell |
4:34 | |
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Fuel Cell |
6:53 | |
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| Overall Reaction |
8:24 | |
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Secondary Batteries |
13:47 | |
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| Car Battery |
14:04 | |
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Electrolysis |
18:41 | |
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| Aluminum Plant |
19:14 | |
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| Chromium Plating |
22:42 | |
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Sodium Chloride |
24:08 | |
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| Example: Metallic Na |
24:20 | |
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| Example: Bleach |
28:38 | |
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Faraday's Laws |
32:22 | |
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| Example: Aluminum Electrolysis |
34:54 | |
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Corrosion of Iron |
41:24 | |
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| Example: Iron Galvanic Cell |
44:34 | |
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Protection of Iron Against Corrosion |
46:55 | |
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| Coating of Tin Cans |
47:18 | |
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Additional Example 1 |
4:45 | |
| XXIV. Radioactivity |
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Radioactivity, Nuclear Equations, Mass Energy Equivalence |
40:35 |
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Intro |
0:00 | |
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Radioactivity Pioneers |
0:36 | |
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| Becquerel |
2:20 | |
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| Curie |
1:53 | |
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| Rutherford |
2:38 | |
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| Soddy |
2:55 | |
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Alpha, Beta, and Gamma Radiation |
3:46 | |
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| Three Types of Emission |
4:28 | |
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Transmutation and Nuclear Equations |
7:01 | |
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| Decay of Uranium |
8:07 | |
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Balancing Nuclear Equations |
13:08 | |
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| Example: Chromium |
13:19 | |
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| Example: Radium |
15:56 | |
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Synthesis of New Isotopes and Elements |
18:47 | |
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| Example: Nitrogen and Alpha Particles |
19:44 | |
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| Example: Uranium and Carbon Nuclei |
21:41 | |
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Mass Changes in Nuclear Transformations |
23:55 | |
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| Mass and Energy Equivalence (e=mc2, Einstein) |
24:39 | |
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Mass-Energy Transformations |
28:35 | |
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| Example: Uranium |
28:38 | |
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Stability of Nuclei and Binding Energy |
33:11 | |
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| Nucleons |
33:34 | |
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| Example: Deuterium and Helium |
33:51 | |
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Curve of Binding Energy; Fission and Fusion |
35:53 | |
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Radioactive Decay, Half-Life, Nuclear Reactions |
56:12 |
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Intro |
0:00 | |
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First Order Nuclear Decay |
0:41 | |
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| Example: Uranium |
2:01 | |
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| Rate Constant |
3:42 | |
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| Integrated Rate Equation |
3:52 | |
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| Half-Life |
5:14 | |
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Half-Lives and Rate Constants |
6:09 | |
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| Examples: Various |
6:14 | |
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Radioactive Dating: Rocks |
9:18 | |
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| Example: Rock with Uranium and Lead |
10:53 | |
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Radioactive Dating: Carbon-14 |
17:27 | |
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| Example: Shroud of Turin |
20:54 | |
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| Example: Wooden Staff |
22:31 | |
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Nuclear Fusion in Stars |
27:22 | |
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| Example: Reaction in Sun |
29:21 | |
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Nuclear Weapons |
32:24 | |
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| Example: Uranium Isotope |
34:14 | |
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Nuclear Power |
38:52 | |
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| Nuclear Power Usage |
42:30 | |
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Nuclear Wastes and Their Disposal |
45:03 | |
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Additional Example 1 |
5:33 | |
| XXV. Miscellaneous |
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Organic Structures, Isomers, Functional Groups |
68:32 |
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Intro |
0:00 | |
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Saturated Hydrocarbons C-1 to C-4 |
1:41 | |
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| Acyclic |
2:38 | |
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| Example: Methane, Ethane, Propane |
3:28 | |
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| Isomers |
7:19 | |
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Acyclic Saturated Hydrocarbons C-5 Isomers |
10:27 | |
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| Example: Pentanes |
10:40 | |
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Alkenes and Ring Compounds |
14:56 | |
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| Alkenes |
15:34 | |
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| Example: Ethene, Ethylene |
16:25 | |
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| Example: Propene Isomers |
19:19 | |
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Geometric Isomers of Alkenes |
24:13 | |
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| Example: 2-Butene |
24:34 | |
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| Trans and Cis |
26:27 | |
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Optical Isomers |
28:45 | |
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| Example: Carbon Atom |
33:49 | |
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Functional Groups: Alcohols and Caboxylic Acids |
39:11 | |
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| Alcohols |
39:27 | |
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| Carboxylic Acids |
41:41 | |
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Functional Groups: Esters and Ethers |
44:10 | |
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| Esters (Ethyl Acetate) |
44:27 | |
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| Ethers (Diethylether) |
46:14 | |
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Functional Groups: Aldehydes and Ketones |
47:48 | |
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| Examples |
47:59 | |
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Amines |
51:01 | |
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Amide Group |
54:24 | |
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Peptides and Proteins |
56:02 | |
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Additional Example 1 |
9:41 | |
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Chemistry and the Environment |
50:13 |
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Intro |
0:00 | |
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Global Climate Change |
1:41 | |
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| Greenhouse Gases |
3:49 | |
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Greenhouse Gases and Climate Change |
6:53 | |
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| Last 100 Years |
9:11 | |
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Water Pollution: Eutrophication |
12:59 | |
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| Example: Fertilizers |
15:41 | |
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Water Pollution: Organic Pollutants |
9:15 | |
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| Chlorinated Hydrocarbons (DDT) |
19:30 | |
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| Dioxins and Phthalates |
20:58 | |
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Water Pollution: Heavy Metal Pollutants |
23:58 | |
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| Examples: Lead, Chromium, Arsenic |
24:17 | |
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Radiation in the Environment |
24:35 | |
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| Thresholds |
39:20 | |