CHEM 1020 - General Chemistry I

by Budhi

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Publisher
Eastern Wyoming College
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: Matter, Measurement, and Problem Solving
  7. 1.1: Atoms and Molecules
  8. 1.2: The Scientific Approach to Knowledge
  9. 1.3: The Classification of Matter
  10. 1.4: Physical and Chemical Changes and Properties
  11. 1.5: Energy: A Fundamental Part of Physical and Chemical Change
  12. 1.6: The Units of Measurement
  13. 1.7: The Reliability of a Measurement
  14. 1.8: Solving Chemical Problems
  15. 1.9: Matter, Measurement, and Problem Solving (Exercises)
  16. 2: Atoms and Elements
  17. 2.1: Brownian Motion - Evidence for Atoms
  18. 2.2: Early Ideas about the Building Blocks of Matter
  19. 2.3: Modern Atomic Theory and the Laws That Led to It
  20. 2.4: The Discovery of the Electron
  21. 2.5: 2.5 The Structure of The Atom
  22. 2.6: Protons, Neutrons, and Electrons in Atoms
  23. 2.7: Finding Patterns - The Periodic Law and the Periodic Table
  24. 2.8: The Average Mass of an Element’s Atoms
  25. 2.9: Molar Mass - Counting Atoms by Weighing Them
  26. 2.10: Atoms and Elements (Exercises)
  27. 3: Molecules, Compounds and Chemical Equations
  28. 3.1: Hydrogen, Oxygen, and Water
  29. 3.2: Chemical Bonds
  30. 3.3: Representing Compounds: Chemical Formulas and Molecular Models
  31. 3.4: An Atomic-Level Perspective of Elements and Compounds
  32. 3.5: Ionic Compounds: Formulas and Names
  33. 3.6: Molecular Compounds: Formulas and Names
  34. 3.7: Summary of Inorganic Nomenclature
  35. 3.8: Composition of Compounds
  36. 3.9: Determining a Chemical Formula from Experimental Data
  37. 3.10: Writing and Balancing Chemical Equations
  38. 3.11: Organic Compounds
  39. 3.12: Molecules, Compounds and Chemical Equations (Exercises)
  40. 4: Chemical Reactions and Aqueous Reactions
  41. 4.1: Global Warming and the Combustion of Fossil Fuels
  42. 4.2: How Much Carbon Dioxide?
  43. 4.3: 4.3 Limiting Reactant, Theoretical Yield, and Percent Yield
  44. 4.4: Solution Concentration and Solution Stoichiomentry
  45. 4.5: Types of Aqueous Solutions and Solubility
  46. 4.6: Precipitation Reactions
  47. 4.7: Representing Aqueous Reactions: Molecular, Ionic, and Complete Ionic Equations
  48. 4.8: Acid-Base and Gas-Evolution Reactions
  49. 4.9: Oxidation-Reduction Reactions
  50. 5: Gases
  51. 5.1: Water from Wells: Atmospheric Pressure at Work
  52. 5.2: Pressure: The Result of Particle Collisions
  53. 5.3: The Simple Gas Laws: Boyle’s Law, Charles’s Law and Avogadro’s Law
  54. 5.4: The Ideal Gas Law
  55. 5.5: Applications of the Ideal Gas Law: Molar Volume, Density and Molar Mass of a Gas
  56. 5.6: Mixtures of Gases and Partial Pressures
  57. 5.7: Gases in Chemical Reactions: Stoichiometry Revisited
  58. 5.8: Kinetic Molecular Theory: A Model for Gases
  59. 5.9: Mean Free Path, Diffusion, and Effusion of Gases
  60. 5.10: Real Gases: The Effects of Size and Intermolecular Forces
  61. 5.11: Gases (Exercises)
  62. 6: The Quantum-Mechanical Model of the Atom
  63. 6.1: Schrödinger's Cat
  64. 6.2: The Nature of Light
  65. 6.3: Atomic Spectroscopy and The Bohr Model
  66. 6.4: The Wavelength Nature of Matter
  67. 6.5: Quantum Mechanics and The Atom
  68. 6.6: The Shape of Atomic Orbitals
  69. 6.7: The Quantum-Mechanical Model of the Atom (Exercises)
  70. 7: Periodic Properties of the Elements
  71. 7.1: Nerve Signal Transmission
  72. 7.2: The Development of the Periodic Table
  73. 7.3: Electron Configurations: How Electrons Occupy Orbitals
  74. 7.4: Electron Configurations, Valence Electrons, and the Periodic Table
  75. 7.5: The Explanatory Power of the Quantum-Mechanical Model
  76. 7.6: Periodic Trends in the Size of Atoms and Effective Nuclear Charge
  77. 7.7: Ions- Configurations, Magnetic Properties, Radii, and Ionization Energy
  78. 7.8: Electron Affinities and Metallic Character
  79. 7.9: Examples of Periodic Chemical Behavior
  80. 7.10: Periodic Properties of the Elements (Exercises)
  81. 8: Chemical Bonding I: Lewis Structures
  82. 8.1: Bonding Models and AIDS Drugs
  83. 8.2: Types of Chemical Bonds
  84. 8.3: Representing Valance Electrons with Dots
  85. 8.4: Ionic Bonding
  86. 8.5: Covalent Bonding: Lewis Structure
  87. 8.6: Electronegativity and Bond Polarity
  88. 8.7: Lewis Structures
  89. 8.8: Resonance and Formal Charge
  90. 8.9: Exceptions to the Octet Rule
  91. 8.10: Bond Energies and Bond Lengths
  92. 8.11: Bonding in Metals
  93. 8.12: Chemical Bonding I (Exercises)
  94. 9: Chemical Bonding II: Valance Bond Theory and Molecular Orbital Theory
  95. 9.1: Artificial Sweeteners
  96. 9.2: VSEPR Theory - The Five Basic Shapes
  97. 9.3: VSPER Theory: The Effect of Lone Pairs
  98. 9.4: VSPER Theory - Predicting Molecular Geometries
  99. 9.5: Molecular Shape and Polarity
  100. 9.6: Valence Bond Theory: Orbital Overlap as a Chemical Bond
  101. 9.7: Valence Bond Theory: Hybridization of Atomic Orbitals
  102. 9.8: Molecular Orbital Theory: Electron Delocalization
  103. 10: Liquids, Solids, and Intermolecular Forces
  104. 10.1: Water in Zero Gravity
  105. 10.2: Solids, Liquids, and Gases: A Molecular Comparison
  106. 10.3: Intermolecular Forces: The Forces that Hold Condensed Phases Together
  107. 10.4: Intermolecular Forces in Action: Surface Tension, Viscosity, and Capillary Action
  108. 10.5: Vaporization and Vapor Pressure
  109. 10.6: Sublimation and Fusion
  110. 10.7: Heating Curve for Water
  111. 10.8: Phase Diagrams
  112. 10.9: Water - An Extraordinary Substance
  113. Back Matter
  114. Index
  115. Glossary
  116. Detailed Licensing