CHEM 114: Introductory Chemistry

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This is a lecture and laboratory course that covers the fundamental concepts of chemistry. This course assumes no previous knowledge of chemistry, presenting both chemical problem solving and laboratory skills. This course is intended primarily to prepare students for CHEM 131.

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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: The Chemical World
  7. 1.1: The Scope of Chemistry
  8. 1.2: Chemicals Compose Ordinary Things
  9. 1.3: Hypothesis, Theories, and Laws
  10. 1.4: The Scientific Method- How Chemists Think
  11. 1.5: A Beginning Chemist- How to Succeed
  12. 2: Measurement and Problem Solving
  13. 2.1: Taking Measurements
  14. 2.2: Scientific Notation- Writing Large and Small Numbers
  15. 2.3: Significant Figures- Writing Numbers to Reflect Precision
  16. 2.4: Significant Figures in Calculations
  17. 2.5: The Basic Units of Measurement
  18. 2.6: Problem Solving and Unit Conversions
  19. 2.7: Solving Multistep Conversion Problems
  20. 2.8: Units Raised to a Power
  21. 2.9: Density
  22. 2.10: Numerical Problem-Solving Strategies and the Solution Map
  23. 2.11: Taking Measurements
  24. 2.E: Measurement and Problem Solving (Exercises)
  25. 3: Matter and Energy
  26. 3.1: In Your Room
  27. 3.2: What is Matter?
  28. 3.3: Classifying Matter According to Its State- Solid, Liquid, and Gas
  29. 3.4: Classifying Matter According to Its Composition
  30. 3.5: Differences in Matter- Physical and Chemical Properties
  31. 3.6: Changes in Matter- Physical and Chemical Changes
  32. 3.7: Conservation of Mass- There is No New Matter
  33. 3.8: Energy
  34. 3.9: Energy and Chemical and Physical Change
  35. 3.10: Temperature- Random Motion of Molecules and Atoms
  36. 3.11: Temperature Changes- Heat Capacity
  37. 3.12: Energy and Heat Capacity Calculations
  38. 3.E: Exercises
  39. 4: Atoms and Elements
  40. 4.1: Experiencing Atoms at Tiburon
  41. 4.2: Indivisible- The Atomic Theory
  42. 4.3: The Nuclear Atom
  43. 4.4: The Properties of Protons, Neutrons, and Electrons
  44. 4.5: Elements- Defined by Their Numbers of Protons
  45. 4.6: Looking for Patterns- The Periodic Law and the Periodic Table
  46. 4.7: Ions- Losing and Gaining Electrons
  47. 4.8: Isotopes- When the Number of Neutrons Varies
  48. 4.9: Atomic Mass- The Average Mass of an Element’s Atoms
  49. 5: Molecules and Compounds
  50. 5.1: Sugar and Salt
  51. 5.2: Compounds Display Constant Composition
  52. 5.3: Chemical Formulas- How to Represent Compounds
  53. 5.4: A Molecular View of Elements and Compounds
  54. 5.5: Writing Formulas for Ionic Compounds
  55. 5.6: Nomenclature- Naming Compounds
  56. 5.7: Naming Ionic Compounds
  57. 5.8: Naming Molecular Compounds
  58. 5.9: Naming Acids
  59. 5.10: Nomenclature Summary
  60. 5.11: Formula Mass- The Mass of a Molecule or Formula Unit
  61. 6: Chemical Composition
  62. 6.1: How Much Sodium?
  63. 6.2: Counting Nails by the Pound
  64. 6.3: Counting Atoms by the Gram
  65. 6.4: Counting Molecules by the Gram
  66. 6.5: Chemical Formulas as Conversion Factors
  67. 6.6: Mass Percent Composition of Compounds
  68. 6.7: Mass Percent Composition from a Chemical Formula
  69. 6.8: Calculating Empirical Formulas for Compounds
  70. 6.9: Calculating Molecular Formulas for Compounds
  71. 7: Chemical Reactions
  72. 7.1: Grade School Volcanoes, Automobiles, and Laundry Detergents
  73. 7.2: Evidence of a Chemical Reaction
  74. 7.3: The Chemical Equation
  75. 7.4: How to Write Balanced Chemical Equations
  76. 7.5: Aqueous Solutions and Solubility- Compounds Dissolved in Water
  77. 7.6: Precipitation Reactions- Reactions in Aqueous Solution That Form a Solid
  78. 7.7: Writing Chemical Equations for Reactions in Solution- Molecular, Complete Ionic, and Net Ionic Equations
  79. 7.8: Acid–Base and Gas Evolution Reactions
  80. 7.9: Oxidation–Reduction Reactions
  81. 7.10: Classifying Chemical Reactions
  82. 7.11: The Activity Series
  83. 8: Quantities in Chemical Reactions
  84. 8.1: Climate Change- Too Much Carbon Dioxide
  85. 8.2: Stoichiometry
  86. 8.3: Making Molecules- Mole-to-Mole Conversions
  87. 8.4: Making Molecules- Mass-to-Mass Conversions
  88. 8.5: Limiting Reactant, Theoretical Yield, and Percent Yield
  89. 8.6: Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants
  90. 8.7: Enthalpy- A Measure of the Heat Evolved or Absorbed in a Reaction
  91. 9: Electrons in Atoms and the Periodic Table
  92. 9.1: Blimps, Balloons, and Models of the Atom
  93. 9.2: Light- Electromagnetic Radiation
  94. 9.3: The Electromagnetic Spectrum
  95. 9.4: The Bohr Model- Atoms with Orbits
  96. 9.5: The Quantum-Mechanical Model- Atoms with Orbitals
  97. 9.6: Quantum-Mechanical Orbitals and Electron Configurations
  98. 9.7: Electron Configurations and the Periodic Table
  99. 9.8: The Explanatory Power of the Quantum-Mechanical Model
  100. 9.9: Periodic Trends- Atomic Size, Ionization Energy, and Metallic Character
  101. 10: Chemical Bonding
  102. 10.1: Bonding Models and AIDS Drugs
  103. 10.2: Representing Valence Electrons with Dots
  104. 10.3: Lewis Structures of Ionic Compounds- Electrons Transferred
  105. 10.4: Covalent Lewis Structures- Electrons Shared
  106. 10.5: Writing Lewis Structures for Covalent Compounds
  107. 10.6: Resonance- Equivalent Lewis Structures for the Same Molecule
  108. 10.7: Predicting the Shapes of Molecules
  109. 10.8: Electronegativity and Polarity - Why Oil and Water Don’t Mix
  110. 11: Gases
  111. 11.1: Extra-Long Straws
  112. 11.2: Kinetic Molecular Theory- A Model for Gases
  113. 11.3: Pressure- The Result of Constant Molecular Collisions
  114. 11.4: Boyle’s Law- Pressure and Volume
  115. 11.5: Charles’s Law- Volume and Temperature
  116. 11.6: Gay-Lussac's Law- Temperature and Pressure
  117. 11.7: The Combined Gas Law- Pressure, Volume, and Temperature
  118. 11.8: Avogadro’s Law- Volume and Moles
  119. 11.9: The Ideal Gas Law- Pressure, Volume, Temperature, and Moles
  120. 11.10: Mixtures of Gases- Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen
  121. 11.11: Gases in Chemical Reactions
  122. 12: Liquids, Solids, and Intermolecular Forces
  123. 12.1: Interactions between Molecules
  124. 12.2: Properties of Liquids and Solids
  125. 12.3: Intermolecular Forces in Action- Surface Tension and Viscosity
  126. 12.4: Evaporation and Condensation
  127. 12.5: Melting, Freezing, and Sublimation
  128. 12.6: Types of Intermolecular Forces- Dispersion, Dipole–Dipole, Hydrogen Bonding, and Ion-Dipole
  129. 12.7: Types of Crystalline Solids- Molecular, Ionic, and Atomic
  130. 12.8: Water- A Remarkable Molecule
  131. 13: Solutions
  132. 13.1: Prelude - Tragedy in Cameroon
  133. 13.2: Solutions- Homogeneous Mixtures
  134. 13.3: Solutions of Solids Dissolved in Water- How to Make Rock Candy
  135. 13.4: Solutions of Gases in Water- How Soda Pop Gets Its Fizz
  136. 13.5: Solution Concentration- Mass Percent
  137. 13.6: Solution Concentration- Molarity
  138. 13.7: Solution Dilution
  139. 13.8: Solution Stoichiometry
  140. 13.9: Freezing Point Depression and Boiling Point Elevation- Making Water Freeze Colder and Boil Hotter
  141. 13.10: Osmosis- Why Drinking Salt Water Causes Dehydration
  142. 14: Acids and Bases
  143. 14.1: Sour Patch Kids and International Spy Movies
  144. 14.2: Acids- Properties and Examples
  145. 14.3: Bases- Properties and Examples
  146. 14.4: Molecular Definitions of Acids and Bases
  147. 14.5: Reactions of Acids and Bases
  148. 14.6: Acid–Base Titration- A Way to Quantify the Amount of Acid or Base in a Solution
  149. 14.7: Strong and Weak Acids and Bases
  150. 14.8: Water- Acid and Base in One
  151. 14.9: The pH and pOH Scales- Ways to Express Acidity and Basicity
  152. 14.10: Buffers- Solutions That Resist pH Change
  153. Back Matter
  154. Index
  155. Index
  156. Glossary
  157. Detailed Licensing