CHEM 210: General Chemistry I, An "Atoms Up" Approach

by Camille Kaslan

Read here Read at LibreTextsPDF

This is the free digital textbook that accompanies CHEM 210: General College Chemistry I, which is first half of the two-semester college-level chemistry series offered at Cañada College. Curated and remixed via LibreTexts by Camille Kaslan, Fall 2023.

Description from LibreTexts.

Publisher
Cañada College
Subjects
Chemistry
Licence
CC BY 4.0, as LibreTexts states it
Who can read
Tweens profiles and older, judged from its title and subjects

Contents

LibreTexts writes equations in TeX, and here they show as TeX; the PDF has them typeset.

  1. Front Matter
  2. Table of Contents
  3. TitlePage
  4. InfoPage
  5. Table of Contents
  6. Licensing
  7. 1: Chemistry is the Science of Everything
  8. 1.1: Thinking Scientifically - The Scientific Method
  9. 1.2: Designing Experiments - What's Being Tested?
  10. 2: Matter - An Introduction
  11. 2.1: Classifications of Matter
  12. 2.2: Properties of Matter
  13. 2.3: Intensive vs. Extensive Properties
  14. 2.4: Changes in Matter
  15. 2.5: Energy - What Drives Changes in Matter
  16. 3: Units, Measurements, and Conversions
  17. 3.1: Base Units and Derived Units
  18. 3.2: Scientific Notation - Writing Large and Small Numbers
  19. 3.3: The Reliability of Measurement
  20. 3.4: Significant Figures - Approximating Uncertainty
  21. 3.5: Solving Chemical Problems - Dimensional Analysis
  22. 3.5.1: Metric and Imperial Unit Conversions
  23. 3.5.2: Compound Unit Conversion Factors - Density
  24. 3.5.3: Molar Mass and Avogadro's Number
  25. 4: Atoms and Elements
  26. 4.1: Evidence for Atoms - Brownian Motion
  27. 4.2: Early Ideas About the Building Blocks of Matter
  28. 4.2.1: Dalton's Atomic Theory
  29. 4.3: The Discovery of The Electron - The Plum Pudding Atomic Model
  30. 4.4: Discovery of the Proton - The Nuclear Atomic Model
  31. 4.5: The Subatomic Particles and Isotopes
  32. 4.5.1: Ions - Differences in Electrons
  33. 4.6: The Periodic Table of the Elements
  34. 5: The Quantum Model of the Atom
  35. 5.1: The Nature of Light and Electromagnetic Radiation
  36. 5.2: The Photoelectric Effect - Light as a Particle
  37. 5.3: Blackbody Radiation and The UV Catastrophe - Evidence of Quantization
  38. 5.4: The Bohr Model of The Atom
  39. 5.5: Wave-Particle Duality of Matter
  40. 5.6: The Wavefunction and Schrödinger's Equation
  41. 5.7: Atomic Orbitals and Quantum Numbers
  42. 5.7.1: Visualizing Atomic Orbitals as Probability Densities
  43. 6: Periodic Law and Periodic Properties of the Elements
  44. 6.1: The Development of The Periodic Table
  45. 6.2: Electron Configurations - The Quantum Model and Periodic Structure
  46. 6.3: Periodicity
  47. 6.4: Effective Nuclear Charge and Shielding
  48. 6.5: Periodic Trends
  49. 6.5.1: Periodic Trends in Ions
  50. 6.5.2: Electronegativity
  51. 7: Molecules and Compounds
  52. 7.1: Chemical Formulas - Atomic Ratios
  53. 7.2: Types of Compounds - Differences in Atomic Connections
  54. 7.3: Ionic Compounds - Names and Formulas
  55. 7.4: Covalent Compounds - Names and Formulas
  56. 7.5: Chemical Composition
  57. 7.5.1: Empirical Formulas
  58. 8: Chemical Bonding I - The Lewis Model
  59. 8.1: Lewis Symbols
  60. 8.2: Covalent Bonding and Lewis Dot Structures
  61. 8.2.1: Exceptions to Octet
  62. 8.3: Resonance Structures and Formal Charge
  63. 8.4: Polar Covalent Bonds
  64. 8.5: Bond Energies, Strengths, and Lengths
  65. 9: Chemical Bonding II - Advanced Bonding Models
  66. 9.1: Valence Bond Theory - Bonds as Orbital Overlaps
  67. 9.2: Hybridization and Hybrid Orbitals in VBT
  68. 9.3: Valence Shell Electron-Pair Repulsion (VSEPR) Theory
  69. 9.3.1: Lone Pairs and 3D Geometry
  70. 9.4: Molecular Geometry and Polarity
  71. 9.5: Molecular Orbital Theory
  72. 9.5.1: The Predictive Power of MO Theory - The Case of Oxygen
  73. 10: Chemical Reactions and Chemical Quantities
  74. 10.1: Chemical Reactions and Balanced Chemical Equations
  75. 10.1.1: Coefficients and Mole Ratios
  76. 10.2: General Types of Chemical Reactions
  77. 10.3: Mole Quantities
  78. 10.4: Stoichiometry
  79. 10.5: The Limiting Reactant, Theoretical Yield, and Percent Yield
  80. 11: Solutions, Concentration, and Dilution
  81. 11.1: Solutes and Solvents
  82. 11.2: Aqueous Solutions and Dissolution
  83. 11.2.1: Solute Dissociation Equations
  84. 11.2.2: Electrolyte Solutions
  85. 11.3: Solution Concentration - Molarity
  86. 11.4: Solution Preparation
  87. 12: Aqueous Reactions
  88. 12.1: Complete and Net Ionic Equations
  89. 12.2: Precipitation Reactions
  90. 12.3: Acids and Bases
  91. 12.3.1: Neutralization Reactions
  92. 12.4: Oxidation-Reduction Reactions
  93. 12.5: Stoichiometry of Aqueous Reactions
  94. 13: Thermochemistry
  95. 13.1: The Nature of Energy
  96. 13.2: The First Law of Thermodynamics
  97. 13.2.1: Heat and Work
  98. 13.3: Enthalpy, ΔH, and Heat of Reaction
  99. 13.3.1: Calorimetry
  100. 13.3.2: Hess' Law
  101. 13.3.3: Standard Enthalpy of Formation
  102. 13.4: Heat Transfer Involving Phase Changes
  103. 14: Gases and Gas Laws
  104. 15.1: Gas Pressure - a Result of Collisions
  105. 15.2: The Gas Laws
  106. 15.3: Other Gas Relationships
  107. 15.4: Ideal Gases and The Ideal Gas Law
  108. 15.5: Dalton's Law of Partial Pressures
  109. 15.5.1: Vapor Pressure
  110. 15.6: Ideal Gases and Real Gases
  111. 15.7: Gas Stoichiometry
  112. 15: Solids, Liquids, and Phase Changes
  113. 16.1: The Phases - Solids, Liquids, and Gases
  114. 16.2: Phase Changes
  115. 16.3: Phase Change Diagrams
  116. 16.4: Phase Diagrams
  117. 16.5: Intermolecular Forces
  118. 16.6: Properties of Liquids
  119. 16.7: Solids
  120. Back Matter
  121. Index
  122. Glossary
  123. Detailed Licensing