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Oregon Institute of Technology: CHE 202 General Chemistry II

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Oregon Institute of Technology: CHE 202 General Chemistry II

Electronic structure of atoms, periodic trends, chemical bonding, molecular geometry, intermolecular forces, phase transitions, and properties of solutions. Emphasis on engineering applications.

Chemistry
Author
Addie Clark
Publisher
Oregon Institute of Technology
Source
LibreTexts
License
CC BY-NC-SA
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 62 sections
  1. Unit 1: The Quantum World
  2. 1.1: The Nature of Light
  3. 1.1: The Nature of Light (Problems)
  4. 1.2: Atomic Spectroscopy and the deBroglie Wavelength
  5. 1.2: Atomic Spectroscopy and the deBroglie Wavelength (Problems)
  6. Unit 2: Electrons in Atoms
  7. 2.1: Coulomb's Law and the Electrostatic Potential
  8. 2.1: Coulomb's Law and the Electrostatic Potential (Problems)
  9. 2.2: Atomic Orbitals and Quantum Numbers
  10. 2.2: Atomic Orbitals and Quantum Numbers (Problems)
  11. 2.3: Atomic Orbitals and the Bohr Model
  12. 2.3: Atomic Orbitals and the Bohr Model (Problems)
  13. Unit 3: Periodic Patterns
  14. 3.1: Electron Configurations
  15. 3.1: Electron Configurations (Problems)
  16. 3.2: Trends in Size
  17. 3.2: Trends in Size (Problems)
  18. 3.3: Trends in Ionization Energy
  19. 3.3: Trends in Ionization Energy (Problems)
  20. 3.4: Trends in Electron Affinity and Metallic Character
  21. 3.4: Trends in Electron Affinity and Metallic Character (Problems)
  22. Unit 4: Lewis Structures
  23. 4.1: Lewis Dot Diagrams
  24. 4.1: Lewis Dot Diagrams (Problems)
  25. 4.2: Lewis Structures
  26. 4.2: Lewis Structures (Problems)
  27. 4.3: Formal Charge and Oxidation State
  28. 4.3: Formal Charge and Oxidation State (Problems)
  29. Unit 5: The Strength and Shape of Covalent Bonds
  30. 5.1: Covalent Bond Formation and Strength
  31. 5.1: Covalent Bond Formation and Strength (Problems)
  32. 5.2: Molecular Shape
  33. 5.2: Molecular Shape (Problems)
  34. 5.3: Valence Bond Theory and Hybrid Orbitals
  35. 5.3: Valence Bond Theory and Hybrid Orbitals (Problems)
  36. Unit 6: Molecular Polarity
  37. 6.1: Electronegativity and Polarity
  38. 6.1: Electronegativity and Polarity (Problems)
  39. 6.2: Molecular Shape and Polarity
  40. 6.2: Molecular Shape and Polarity (Problems)
  41. 6.3: Intermolecular Forces
  42. 6.3: Intermolecular Forces (Problems)
  43. Unit 7: Intermolecular and Intramolecular Forces in Action
  44. 7.1: Surface Tension, Viscosity, and Capillary Action
  45. 7.1: Surface Tension, Viscosity, and Capillary Action (Problems)
  46. 7.2: Vapor Pressure
  47. 7.2: Vapor Pressure (Problems)
  48. 7.3: Ionic Bond Formation and Strength
  49. 7.3: Ionic Bond Formations and Strength (Problems)
  50. Unit 8: Solutions and Phase Changes
  51. 8.1: Heating Curves and Phase Changes
  52. 8.1: Heating Curves and Phase Changes (Problems)
  53. 8.2: Solubility and Intermolecular Forces
  54. 8.2: Solubility and Intermolecular Forces (Problems)
  55. 8.3: Concentrations of Solutions
  56. 8.3: Concentrations of Solutions (Problems)
  57. Unit 9: Semiconductors
  58. 9.1: Bond Types and Molecular Orbital Theory
  59. 9.1: Bond Types and Molecular Orbital Theory (Problems)
  60. 9.2: The Solid State of Matter
  61. 9.2: The Solid State of Matter (Problems)
  62. 9.3: Structure and General Properties of the Metalloids