General Chemistry

General Chemistry

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Limitations of VSEPR Theory

65 of 80

65 of 80

Limitations of VSEPR Theory

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Classroom Contents

General Chemistry

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  1. 1 Introduction to Chemistry
  2. 2 Types of Matter: Elements, Compounds, and Mixtures
  3. 3 Measurement and Significant Figures
  4. 4 Scientific Notation and Dimensional Analysis
  5. 5 History of Atomic Theory
  6. 6 Nuclide Symbols: Atomic Number, Mass Number, Ions, and Isotopes
  7. 7 Balancing Chemical Equations
  8. 8 The Mole: Avogadro's Number and Stoichiometry
  9. 9 Limiting Reagents and Percent Yield
  10. 10 Elemental Analysis: Empirical and Molecular Formulas
  11. 11 Kinetic Molecular Theory and the Ideal Gas Laws
  12. 12 Wave-Particle Duality and the Photoelectric Effect
  13. 13 Bohr Model of the Hydrogen Atom
  14. 14 Quantum Mechanics of the Electron
  15. 15 Quantum Numbers, Atomic Orbitals, and Electron Configurations
  16. 16 The Periodic Table: Atomic Radius, Ionization Energy, and Electronegativity
  17. 17 The Chemical Bond: Covalent vs. Ionic and Polar vs. Nonpolar
  18. 18 Naming Ionic Compounds
  19. 19 Lewis Dot Structures
  20. 20 VSEPR Theory and Molecular Geometry
  21. 21 Intermolecular Forces and Boiling Points
  22. 22 Thermochemistry: Heat and Enthalpy
  23. 23 Hess's Law and Heats of Formation
  24. 24 Heat Capacity, Specific Heat, and Calorimetry
  25. 25 Phase Changes, Heats of Fusion and Vaporization, and Phase Diagrams
  26. 26 Solution Chemistry and Net Ionic Equations
  27. 27 Molarity and Dilution
  28. 28 Solubility and the Born-Haber Cycle
  29. 29 Molality and Colligative Properties
  30. 30 The Laws of Thermodynamics, Entropy, and Gibbs Free Energy
  31. 31 Kinetics: Initial Rates and Integrated Rate Laws
  32. 32 Energy Diagrams, Catalysts, and Reaction Mechanisms
  33. 33 Chemical Equilibria and Reaction Quotients
  34. 34 Le Chatelier's Principle
  35. 35 Valence Bond Theory, Hybrid Orbitals, and Molecular Orbital Theory
  36. 36 Acids and Bases, pH and pOH
  37. 37 Acid-Base Equilibria and Buffer Solutions
  38. 38 Acid-Base Titration
  39. 39 Oxidation-Reduction Reactions
  40. 40 Electrochemistry
  41. 41 Nuclear Reactions, Radioactivity, Fission and Fusion
  42. 42 Accuracy and Precision for Data Collection
  43. 43 Converting Between Temperature Scales (Celsius, Fahrenheit, and Kelvin)
  44. 44 Visualizing Molecular Geometry With 3D Software
  45. 45 Calculating Percent Error
  46. 46 Nomenclature of Oxyacids
  47. 47 Nomenclature of Hydrated Salts
  48. 48 Writing Chemical Equations in Words
  49. 49 The Law of Conservation of Matter
  50. 50 Expressing Concentration by Mass Percent
  51. 51 Calculating the Formulas of Hydrated Salts
  52. 52 What Are Electrolytes?
  53. 53 Calculating Ion Concentrations in Solution
  54. 54 Neutralization Reactions
  55. 55 Dalton's Law and Partial Pressures
  56. 56 What Are Standard Conditions?
  57. 57 Molar Gas Volume: Stoichiometry With Gases
  58. 58 Kinetic Molecular Theory and its Postulates
  59. 59 Temperature and Gas Solubility
  60. 60 Balancing Redox Reactions in Acidic and Basic Conditions
  61. 61 Pseudo Noble Gas Electron Configurations
  62. 62 Complex Ion Formation
  63. 63 Lattice Structures in Ionic Solids
  64. 64 Covalent Bond Energy and Length
  65. 65 Limitations of VSEPR Theory
  66. 66 Examples of s-p Mixing in Molecular Orbital Theory
  67. 67 Measuring Pressure With Barometers and Manometers
  68. 68 Non-Ideal Gases and the Van der Waals Equation
  69. 69 Viscosity, Cohesive and Adhesive Forces, Surface Tension, and Capillary Action
  70. 70 Types of Colloids and Their Properties
  71. 71 Solubility Product Constant (Ksp)
  72. 72 Predicting Precipitation With Ksp Values
  73. 73 Selective Precipitation
  74. 74 The Common Ion Effect
  75. 75 Coordination Compounds: Geometry and Nomenclature
  76. 76 Crystal Field Theory
  77. 77 Radiometric Dating: Carbon-14 and Uranium-238
  78. 78 Conductivity and Semiconductors
  79. 79 Spectrophotometry and Beer's Law
  80. 80 The Chemistry of Air Purification

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