General Chemistry I

by Lisa K Kendhammer

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Publisher
California State University, Chico
Subjects
Chemistry
Licence
CC BY-NC-SA 4.0, as LibreTexts states it. Non-commercial use only.
Who can read
Tweens profiles and older, judged from its title and subjects

Contents

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  1. Front Matter
  2. TitlePage
  3. InfoPage
  4. Table of Contents
  5. Licensing
  6. 1: Intro to Chem
  7. 1.1: The Scientific Approach to Knowledge
  8. 1.2: The Classification of Matter
  9. 1.3: Physical and Chemical Changes and Properties
  10. 2: Measurement and Experimentation in Science
  11. 2.1: The Units of Measurement
  12. 2.2: The Reliability of a Measurement
  13. 2.3: Solving Chemical Problems
  14. 2.E: Matter, Measurement, and Problem Solving (Exercises)
  15. 3: Atomic Theory
  16. 3.1: Finding Patterns - The Periodic Law and the Periodic Table
  17. 3.2: Early Ideas about the Building Blocks of Matter
  18. 3.3: Modern Atomic Theory and the Laws That Led to It
  19. 3.4: The Discovery of the Electron
  20. 3.5: The Structure of The Atom
  21. 3.6: Protons, Neutrons, and Electrons in Atoms
  22. 3.7: The Average Mass of an Element’s Atoms
  23. 3.8: Molar Mass - Counting Atoms by Weighing Them
  24. 3.E: Atoms and Elements (Exercises)
  25. 4: Chemical Formulas, Equations, and Mass Relationships
  26. 4.1: Writing and Balancing Chemical Equations
  27. 4.2: Representing Compounds- Chemical Formulas and Molecular Models
  28. 4.3: Organic Compounds
  29. 4.4: Functional Groups
  30. 4.5: Composition of Compounds
  31. 4.6: How Much Carbon Dioxide?
  32. 4.7: Limiting Reactant, Theoretical Yield, and Percent Yield
  33. 5: Ions, Salts, and Molecules
  34. 5.1: Chemical Bonds
  35. 5.2: An Atomic-Level Perspective of Elements and Compounds
  36. 5.3: Molecular Compounds- Formulas and Names
  37. 5.4: Ionic Compounds- Formulas and Names
  38. 5.5: Summary of Inorganic Nomenclature
  39. 5.E: Molecules, Compounds and Chemical Equations (Exercises)
  40. 6: Aqueous Applications- Redox
  41. 6.1: Oxidation-Reduction Reactions
  42. 7: Aqueous Applications- Precipitation
  43. 7.1: Types of Aqueous Solutions and Solubility
  44. 7.2: Precipitation Reactions
  45. 7.3: Representing Aqueous Reactions- Molecular, Ionic, and Complete Ionic Equations
  46. 8: Aqueous Applications- Acids and Bases including Gas Evolution
  47. 8.1: Acid-Base and Gas-Evolution Reactions
  48. 8.2: Representing Aqueous Reactions- Molecular, Ionic, and Complete Ionic Equations
  49. 8.3: Solution Concentration and Solution Stoichiomentry
  50. 9: The Interaction of Light with Matter
  51. 9.1: The Nature of Light
  52. 9.2: Atomic Spectroscopy and The Bohr Model
  53. 9.E: The Quantum-Mechanical Model of the Atom (Exercises)
  54. 10: Atomic Theory and Electronic Structure
  55. 10.1: The Wavelength Nature of Matter
  56. 10.2: Quantum Mechanics and The Atom
  57. 10.3: The Shape of Atomic Orbitals
  58. 10.4: Electron Configurations- How Electrons Occupy Orbitals
  59. 10.5: Electron Configurations, Valence Electrons, and the Periodic Table
  60. 10.6: Ions- Configurations, Magnetic Properties, Radii, and Ionization Energy
  61. 10.E: Periodic Properties of the Elements (Exercises)
  62. 10.E: The Quantum-Mechanical Model of the Atom (Exercises)
  63. 11: Periodic Trends and the Formation of Salts
  64. 11.1: The Explanatory Power of the Quantum-Mechanical Model
  65. 11.2: Periodic Trends in the Size of Atoms and Effective Nuclear Charge
  66. 11.3: Ions- Configurations, Magnetic Properties, Radii, and Ionization Energy
  67. 11.4: Electron Affinities and Metallic Character
  68. 11.5: Examples of Periodic Chemical Behavior
  69. 11.6: Ionic Bonding
  70. 11.7: Electronegativity and Bond Polarity
  71. 11.E: Periodic Properties of the Elements (Exercises)
  72. 12: Covalent Bonding- Shape and Structure
  73. 12.1: Types of Chemical Bonds
  74. 12.2: Representing Valance Electrons with Dots
  75. 12.3: Covalent Bonding- Lewis Structure
  76. 12.4: Lewis Structures
  77. 12.5: Resonance and Formal Charge
  78. 12.6: Exceptions to the Octet Rule
  79. 12.7: Bond Energies and Bond Lengths
  80. 12.8: VSEPR Theory - The Five Basic Shapes
  81. 12.9: VSPER Theory- The Effect of Lone Pairs
  82. 12.10: VSPER Theory - Predicting Molecular Geometries
  83. 12.11: Molecular Shape and Polarity
  84. 12.12: Intermolecular Forces- The Forces that Hold Condensed Phases Together
  85. 12.13: Intermolecular Forces in Action- Surface Tension, Viscosity, and Capillary Action
  86. 12.14: Valence Bond Theory- Orbital Overlap as a Chemical Bond
  87. 12.15: Valence Bond Theory- Hybridization of Atomic Orbitals
  88. 12.E: Chemical Bonding I (Exercises)
  89. 13: Chemical Energy
  90. 13.1: The Nature and Types of Energy
  91. 13.2: Quantifying Heat and Work
  92. 13.3: The First Law of Thermodynamics
  93. 13.4: Enthalpy- The Heat Evolved in a Chemical Reaction at Constant Pressure
  94. 13.5: Enthalpies of Reaction from Standard Heats of Formation
  95. 13.6: Constant Volume Calorimetry- Measuring ΔU for Chemical Reactions
  96. 13.7: Constant Pressure Calorimetry- Measuring ΔH for Chemical Reactions
  97. 13.8: Bond Energies and Bond Lengths
  98. 13.9: Relationships Involving Enthalpy of Reactions
  99. 13.10: Heating Curve for Water
  100. 13.11: Phase Diagrams
  101. 13.12: Energy Use and The Environment
  102. 14: Gas Laws
  103. 14.1: Kinetic Molecular Theory- A Model for Gases
  104. 14.2: Pressure- The Result of Particle Collisions
  105. 14.3: The Simple Gas Laws- Boyle’s Law, Charles’s Law and Avogadro’s Law
  106. 14.4: The Ideal Gas Law
  107. 14.5: Applications of the Ideal Gas Law- Molar Volume, Density and Molar Mass of a Gas
  108. 14.6: Mixtures of Gases and Partial Pressures
  109. 14.7: Gases in Chemical Reactions- Stoichiometry Revisited
  110. 14.8: Mean Free Path, Diffusion, and Effusion of Gases
  111. 14.9: Real Gases- The Effects of Size and Intermolecular Forces
  112. 14.E: Gases (Exercises)
  113. Back Matter
  114. Index
  115. Glossary
  116. Detailed Licensing
  117. Detailed Licensing