Madera Community College Introductory Chemistry v2

by Jamie MacArthur

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Publisher
Madera Community College
Subjects
Chemistry
Licence
Mixed licences (each page states its own), 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. TitlePage
  3. InfoPage
  4. Table of Contents
  5. Licensing
  6. 1: Basics of Measurement
  7. 1.1: Taking Measurements- Numbers and Units
  8. 1.1.1: Scientific Notation - Writing Large and Small Numbers
  9. 1.1.2: The Basic Units of Measurement
  10. 1.2: Significant Figures
  11. 1.2.1: Significant Figures - Writing Numbers to Reflect Precision
  12. 1.2.2: Significant Figures in Calculations
  13. 1.3: Conversions
  14. 1.3.1: Problem Solving and Unit Conversions
  15. 1.3.2: Solving Multi-step Conversion Problems
  16. 1.3.3: Units Raised to a Power
  17. 1.E: Measurements (Exercises)
  18. 2: Matter and Energy
  19. 2.1: What is Matter?
  20. 2.1.1: Classifying Matter According to Its State—Solid, Liquid, and Gas
  21. 2.1.2: Classifying Matter According to Its Composition
  22. 2.2: Properties and Changes of Matter
  23. 2.2.1: Differences in Matter- Physical and Chemical Properties
  24. 2.2.2: Changes in Matter - Physical and Chemical Changes
  25. 2.2.3: Conservation of Mass - There is No New Matter
  26. 2.3: Summary of Matter and Changes
  27. 2.4: Density
  28. 2.5: Temperature, Heat, and Energy
  29. 2.5.1: Energy
  30. 2.5.2: Energy and Chemical and Physical Change
  31. 2.5.3: Temperature - Random Motion of Molecules and Atoms
  32. 2.6: Heat Capacity
  33. 2.6.1: Temperature Changes - Heat Capacity
  34. 2.6.2: Energy and Heat Capacity Calculations
  35. 2.E: Matter and Energy (Exercises)
  36. 3: Elements and Compounds
  37. 3.1: Introduction to Atoms and Elements
  38. 3.1.1: Modern Understandings of Elements
  39. 3.1.2: Law of Conservation of Mass
  40. 3.1.3: Law of Definite Proportions
  41. 3.1.4: Law of Multiple Proportions
  42. 3.1.5: Dalton's Atomic Theory
  43. 3.2: Looking for Patterns - The Periodic Table
  44. 3.3: Electrons and Ions
  45. 3.3.1: Ions - Losing and Gaining Electrons
  46. 3.3.2: Ions - Monatomic and Polyatomic
  47. 3.3.3: Naming Ions
  48. 3.4: Compounds
  49. 3.4.1: Chemical Formulas - How to Represent Compounds
  50. 3.5: A Molecular View of Elements and Compounds
  51. 3.5.1: Recognizing Ionic Compounds
  52. 3.6: Ionic Compounds
  53. 3.6.1: Writing Formulas for Ionic Compounds
  54. 3.7: How to Name Compounds
  55. 3.7.1: Naming Ionic Compounds
  56. 3.7.2: Naming Molecular Compounds
  57. 3.7.3: Naming Acids
  58. 3.7.4: Nomenclature Summary
  59. 3.E: Atoms, Molecules, and Ions (Exercises)
  60. 4: The Mole Concept
  61. 4.1: Avogadro's Number
  62. 4.2: Conversions Between Moles and Atoms
  63. 4.3: Molar Mass
  64. 4.4: Conversions Between Moles and Mass
  65. 4.5: Conversions Between Mass and Number of Particles
  66. 4.6: Percent Composition
  67. 4.7: Determining Empirical Formulas
  68. 4.8: Percent of Water in a Hydrate
  69. 4.9: Determining Molecular Formulas
  70. 4.10: Mole Road Map
  71. 4.E: The Mole Concept (Exercises)
  72. 5: Chemical Reactions
  73. 5.1: Word Equations
  74. 5.2: Chemical Equations
  75. 5.3: Balancing Equations
  76. 5.4: Types of Reactions
  77. 5.4.1: Combination Reactions
  78. 5.4.2: Decomposition Reactions
  79. 5.4.3: Combustion Reactions
  80. 5.4.4: Single Replacement Reactions
  81. 5.4.5: Double Replacement Reactions
  82. 5.5: Predicting Reactions - Single and Double Replacement Reactions
  83. 5.6: Oxidation and Reduction
  84. 5.6.1: Oxidation and Reduction- Some Definitions
  85. 5.6.2: Determining Redox Reactions from Oxidation States
  86. 5.6.3: Applications of Redox Reactions
  87. 5.6.3.1: The Activity Series- Predicting Spontaneous Redox Reactions
  88. 5.6.3.2: Batteries- Using Chemistry to Generate Electricity
  89. 5.6.3.3: Corrosion - Undesirable Redox Reactions
  90. 5.6.3.4: Electrolysis- Using Electricity to Do Chemistry
  91. 5.E: Chemical Reactions (Exercises)
  92. 6: Introduction to Stoichiometry
  93. 6.1: Everyday Stoichiometry
  94. 6.2: Mole Ratios
  95. 6.3: Mass-Mole and Mole-Mass Stoichiometry
  96. 6.4: Mass-Mass Stoichiometry
  97. 6.5: Enthalpy Change is a Measure of the Heat Evolved or Absorbed
  98. 6.6: Stoichiometry Applications
  99. 6.6.1: Making Your Own Mole Road Map
  100. 6.6.2: Limiting Reactant
  101. 6.6.3: Theoretical Yield and Percent Yield
  102. 6.E: Introduction to Stoichiometry (Exercises)
  103. 7: Electrons and Chemical Bonding
  104. 7.1: Electromagnetic Radiation
  105. 7.2: Matter and Light and Quantum Mechanics
  106. 7.2.1: The Bohr Model - Atoms with Orbits
  107. 7.2.2: The Quantum-Mechanical Model- Atoms with Orbitals
  108. 7.3: Electron Configurations
  109. 7.4: Electron Configurations and the Periodic Table
  110. 7.5: The Octet Rule
  111. 7.5.1: Periodic Trends- Lewis dot Structures
  112. 7.5.2: Lewis Structures of Ionic Compounds- Electrons Transferred
  113. 7.5.3: Covalent Lewis Structures- Electrons Shared
  114. 7.6: Lewis Structures of Molecules
  115. 7.6.1: Exceptions to the Octet Rule
  116. 7.7: Resonance - Equivalent Lewis Structures for the Same Molecule
  117. 7.E: Electrons and Chemical Bonds (Exercises)
  118. 8: Molecules and Attractive Forces
  119. 8.1: Review Lewis Structures
  120. 8.2: Bond Polarity
  121. 8.3: Predicting the Shapes of Molecules
  122. 8.4: Molecular Polarity
  123. 8.5: Intermolecular Forces- Dispersion, Dipole–Dipole, Hydrogen Bonding
  124. 8.6: The Physical States
  125. 8.7: Phase Changes
  126. 8.7.1: The Relationship Between Phase Changes and Intermolecular Forces
  127. 8.7.2: Boiling, Evaporation and Condensation
  128. 8.7.3: Calculations for Phase Changes
  129. 8.7.4: Heating Curve for Water
  130. 8.8: Solutions - Homogeneous Mixtures
  131. 8.8.1: How Solutions Form
  132. 8.8.2: Electrolytes and Nonelectrolytes
  133. 8.8.3: Aqueous Solutions and Solubility - Compounds Dissolved in Water
  134. 8.E: Attractive Forces
  135. 9: Solids, Liquids, and Gases
  136. 9.1: Types of Crystalline Solids
  137. 9.2: Properties of Liquids
  138. 9.3: Pressure - The Result of Constant Molecular Collisions
  139. 9.4: Kinetic Molecular Theory- A Model for Gases
  140. 9.5: Simple Gas Laws
  141. 9.5.1: Boyle’s Law - Pressure and Volume
  142. 9.5.2: Charles’s Law- Volume and Temperature
  143. 9.5.3: Gay-Lussac's Law- Temperature and Pressure
  144. 9.5.4: Avogadro’s Law- Volume and Moles
  145. 9.6: The Ideal Gas Law
  146. 9.7: Mixtures of Gases
  147. 9.8: Solids, Liquids, and Gases (Exercises)
  148. 10: Aqueous Solutions
  149. 10.1: Solubility Trends
  150. 10.1.1: Solutions of Solids Dissolved in Water
  151. 10.1.2: Solutions of Gases in Water
  152. 10.2: Measures of Concentration
  153. 10.2.1: Percent Solutions
  154. 10.2.2: Solution Concentration- Molarity
  155. 10.3: Concentration Calculations
  156. 10.3.1: A Mole Map for Concentration
  157. 10.3.2: Solution Dilution
  158. 10.3.3: Solution Stoichiometry
  159. 10.3.4: Acid–Base Titration
  160. 10.4: Colligative Properties
  161. 10.4.1: Freezing Point Depression and Boiling Point Elevation
  162. 10.4.2: Osmosis
  163. 10.E: Solutions (Exercises)
  164. 11: Acids and Bases
  165. 11.1: Properties of Acids and Bases
  166. 11.1.1: Acids- Properties and Examples
  167. 11.1.2: Bases- Properties and Examples
  168. 11.2: Chemistry of Acids and Bases
  169. 11.2.1: Molecular Definitions of Acids and Bases
  170. 11.2.2: Reactions of Acids and Bases
  171. 11.2.3: Strong and Weak Acids and Bases
  172. 11.3: Acid-Base Equilibria
  173. 11.3.1: Water - Acid and Base in One
  174. 11.3.2: The pH and pOH Scales - Ways to Express Acidity and Basicity
  175. 11.3.3: Dynamic Equilibrium
  176. 11.4: Buffers are Solutions that Resist pH Change
  177. 11.E: Acids and Bases
  178. 12: Chemistry Applications- more stoichiometry and reaction prediction
  179. 12.1: Review Stoichiometry
  180. 12.2: Moles in the Ideal Gas Law
  181. 12.3: Limiting Reactant
  182. 12.4: Theoretical Yield, and Percent Yield
  183. 12.5: Precipitation Reactions
  184. 12.6: Writing Chemical Equations for Reactions in Solution- Complete Chemical, Complete Ionic, and Net Ionic Equations
  185. 12.E: Applications (Exercises)
  186. 13: Radioactivity and Nuclear Chemistry
  187. 13.1: Properties of Atoms
  188. 13.1.1: The Properties of Protons, Neutrons, and Electrons
  189. 13.1.2: Keeping Track of Subatomic Particles
  190. 13.2: Isotopes - When the Number of Neutrons Varies
  191. 13.3: Atomic Mass - The Average Mass of an Element’s Atoms
  192. 13.4: The Discovery of Radioactivity
  193. 13.5: Types of Radioactivity- Alpha, Beta, and Gamma Decay
  194. 13.6: Balancing Nuclear Equations
  195. 13.7: Natural Radioactivity and Half-Life
  196. 13.8: Applications of Nuclear Chemistry
  197. 13.8.1: Detecting Radioactivity
  198. 13.8.2: Radiocarbon Dating- Using Radioactivity to Measure the Age of Fossils and Other Artifacts
  199. 13.8.3: The Discovery of Fission and the Atomic Bomb
  200. 13.8.4: Nuclear Power- Using Fission to Generate Electricity
  201. 13.8.5: Nuclear Fusion- The Power of the Sun
  202. 13.8.6: The Effects of Radiation on Life
  203. 13.8.7: Radioactivity in Medicine
  204. 13.E: Nuclear Chemistry (Exercises)
  205. Back Matter
  206. Index
  207. Glossary
  208. Detailed Licensing
  209. Detailed Licensing