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CHEM 1000 - Introductory Chemistry I

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CHEM 1000 - Introductory Chemistry I

Textbook Maps are an attempt to recreate that for existing textbooks to facilitate adoption. Faculty do not need to recreate the wheel to generate a LibreText for their class and can peruse the existing LibreTexts; then they can be adapted to that instructor’s specific desires. These Textmaps are complemented by the Modules in the Core.

Chemistry
Author
Budhi
Publisher
Eastern Wyoming College
Source
LibreTexts
License
CC BY-NC-SA
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 182 sections
  1. 01: The Chemical World
  2. 1.1: The Scope of Chemistry
  3. 1.2: Chemicals Compose Ordinary Things
  4. 1.3: Hypothesis, Theories, and Laws
  5. 1.4: The Scientific Method - How Chemists Think
  6. 1.5: A Beginning Chemist - How to Succeed
  7. 1.6: Exercises
  8. 02: Measurement and Problem Solving
  9. 2.01: Taking Measurements
  10. 2.02: Scientific Notation - Writing Large and Small Numbers
  11. 2.03: Significant Figures - Writing Numbers to Reflect Precision
  12. 2.04: Significant Figures in Calculations
  13. 2.05: The Basic Units of Measurement
  14. 2.06: Problem Solving and Unit Conversions
  15. 2.07: Solving Multistep Conversion Problems
  16. 2.08: Units Raised to a Power
  17. 2.09: Density
  18. 2.10: Numerical Problem-Solving Strategies and the Solution Map
  19. 2.11: Measurement and Problem Solving (Exercises)
  20. 03: Matter and Energy
  21. 3.01: In Your Room
  22. 3.02: What is Matter
  23. 3.03: Classifying Matter According to Its State: Solid Liquid and Gas
  24. 3.04: Classifying Matter According to Its Composition
  25. 3.05: Differences in Matter: Physical and Chemical Properties
  26. 3.06: Changes in Matter - Physical and Chemical Changes
  27. 3.07: Conservation of Mass - There is No New Matter
  28. 3.08: Energy
  29. 3.09: Energy and Chemical and Physical Change
  30. 3.10: Temperature - Random Motion of Molecules and Atoms
  31. 3.11: Temperature Changes - Heat Capacity
  32. 3.12: Energy and Heat Capacity Calculations
  33. 3.13: Exercises
  34. 04: Atoms and Elements
  35. 4.1: Cutting Alumimun until you get Atoms
  36. 4.2: Indivisible - The Atomic Theory
  37. 4.3: The Nuclear Atom
  38. 4.4: The Properties of Protons, Neutrons, and Electrons
  39. 4.5: Elements: Defined by Their Number of Protons
  40. 4.6: Looking for Patterns: The Periodic Table
  41. 4.7: Ions - Losing and Gaining Electrons
  42. 4.8: Isotopes - When the Number of Neutrons Varies
  43. 4.9: Atomic Mass: The Average Mass of an Element’s Atoms
  44. 05: Molecules and Compounds
  45. 5.01: Sugar and Salt
  46. 5.02: Compounds Display Constant Composition
  47. 5.03: Chemical Formulas: How to Represent Compounds
  48. 5.04: A Molecular View of Elements and Compounds
  49. 5.05: Writing Formulas for Ionic Compounds
  50. 5.06: Nomenclature: Naming Compounds
  51. 5.07: Naming Ionic Compounds
  52. 5.08: Naming Molecular Compounds
  53. 5.09: Naming Acids
  54. 5.10: Nomenclature Summary
  55. 5.11: Formula Mass: The Mass of a Molecule or Formula Unit
  56. 06: Chemical Composition
  57. 6.1: How Much Sodium?
  58. 6.2: Counting Nails by the Pound
  59. 6.3: Counting Atoms by the Gram
  60. 6.4: Counting Molecules by the Gram
  61. 6.5: Chemical Formulas as Conversion Factors
  62. 6.6: Mass Percent Composition of Compounds
  63. 6.7: Mass Percent Composition from a Chemical Formula
  64. 6.8: Calculating Empirical Formulas for Compounds
  65. 6.9: Calculating Molecular Formulas for Compounds
  66. 07: Chemical Reactions
  67. 7.01: Grade School Volcanoes, Automobiles, and Laundry Detergents
  68. 7.02: Evidence of a Chemical Reaction
  69. 7.03: Chemical Equations
  70. 7.04: How to Write Balanced Chemical Equations
  71. 7.05: Aqueous Solutions and Solubility - Compounds Dissolved in Water
  72. 7.06: Precipitation Reactions
  73. 7.07: Writing Chemical Equations for Reactions in Solution- Molecular, Complete Ionic, and Net Ionic Equations
  74. 7.08: Acid–Base and Gas Evolution Reactions
  75. 7.09: Oxidation–Reduction Reactions
  76. 7.10: Classifying Chemical Reactions
  77. 7.11: The Activity Series: Predicting Spontaneous Redox Reactions
  78. 08: Quantities in Chemical Reactions
  79. 8.1: Climate Change - Too Much Carbon Dioxide
  80. 8.2: Stoichiometry
  81. 8.3: Mole-to-Mole Conversions
  82. 8.4: Making Molecules: Mole to Mass (or vice versa) and Mass-to-Mass Conversions
  83. 8.5: Limiting Reactant and Theoretical Yield
  84. 8.6: Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants
  85. 8.7: Enthalpy Change is a Measure of the Heat Evolved or Absorbed
  86. 09: Electrons in Atoms and the Periodic Table
  87. 9.01: Blimps, Balloons, and Models of the Atom
  88. 9.02: Light is Visible Electromagnetic Radiation
  89. 9.03: The Electromagnetic Spectrum
  90. 9.04: The Bohr Model - Atoms with Orbits
  91. 9.05: The Quantum-Mechanical Model: Atoms with Orbitals
  92. 9.06: Quantum-Mechanical Orbitals and Electron Configurations
  93. 9.07: Electron Configurations and the Periodic Table
  94. 9.08: The Explanatory Power of the Quantum-Mechanical Model
  95. 9.09: Periodic Trends: Atomic Size, Ionization Energy, and Metallic Character
  96. 9.10: Electrons in Atoms and the Periodic Table (Exercises)
  97. 10: Chemical Bonding
  98. 10.1: Bonding Models and AIDS Drugs
  99. 10.2: Representing Valence Electrons with Dots
  100. 10.3: Lewis Structures of Ionic Compounds: Electrons Transferred
  101. 10.4: Covalent Lewis Structures: Electrons Shared
  102. 10.5: Writing Lewis Structures for Covalent Compounds
  103. 10.6: Resonance - Equivalent Lewis Structures for the Same Molecule
  104. 10.7: Predicting the Shapes of Molecules
  105. 10.8: Electronegativity and Polarity: Why Oil and Water Don’t Mix
  106. 11: Gases
  107. 11.01: Extra-Long Straws
  108. 11.02: Kinetic Molecular Theory: A Model for Gases
  109. 11.03: Pressure: The Result of Constant Molecular Collisions
  110. 11.04: Boyle’s Law: Pressure and Volume
  111. 11.05: Charles’s Law: Volume and Temperature
  112. 11.06: Gay-Lussac's Law: Temperature and Pressure
  113. 11.07: The Combined Gas Law: Pressure, Volume, and Temperature
  114. 11.08: Avogadro’s Law: Volume and Moles
  115. 11.09: The Ideal Gas Law: Pressure, Volume, Temperature, and Moles
  116. 11.10: Mixtures of Gases - Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen
  117. 11.11: Gases in Chemical Reactions
  118. 12: Liquids Solids and Intermolecular Forces
  119. 12.1: Interactions between Molecules
  120. 12.2: Properties of Liquids and Solids
  121. 12.3: Surface Tension and Viscosity
  122. 12.4: Evaporation and Condensation
  123. 12.5: Melting, Freezing, and Sublimation
  124. 12.6: Intermolecular Forces: Dispersion, Dipole–Dipole, Hydrogen Bonding, and Ion-Dipole
  125. 12.7: Types of Crystalline Solids
  126. 12.8: Water - A Remarkable Molecule
  127. 13: Solutions
  128. 13.01: Prelude - Tragedy in Cameroon
  129. 13.02: Solutions: Homogeneous Mixtures
  130. 13.03: Solutions of Solids Dissolved in Water: How to Make Rock Candy
  131. 13.04: Solutions of Gases in Water
  132. 13.05: Solution Concentration: Mass Percent
  133. 13.06: Solution Concentration: Molarity
  134. 13.07: Solution Dilution
  135. 13.08: Solution Stoichiometry
  136. 13.09: Freezing Point Depression and Boiling Point Elevation
  137. 13.10: Osmosis
  138. 14: Acids and Bases
  139. 14.01: Sour Patch Kids and International Spy Movies
  140. 14.02: Acids: Properties and Examples
  141. 14.03: Bases: Properties and Examples
  142. 14.04: Molecular Definitions of Acids and Bases
  143. 14.05: Reactions of Acids and Bases
  144. 14.06: Acid–Base Titration
  145. 14.07: Strong and Weak Acids and Bases
  146. 14.08: Water - Acid and Base in One
  147. 14.09: The pH and pOH Scales - Ways to Express Acidity and Basicity
  148. 14.10: Buffers are Solutions that Resist pH Change
  149. 15: Chemical Equilibrium
  150. 15.01: Life is Controlled Disequilibrium
  151. 15.02: The Rate of a Chemical Reaction
  152. 15.03: The Idea of Dynamic Chemical Equilibrium
  153. 15.04: The Equilibrium Constant - A Measure of How Far a Reaction Goes
  154. 15.05: Heterogeneous Equilibria: The Equilibrium Expression for Reactions Involving a Solid or a Liquid
  155. 15.06: Calculating and Using Equilibrium Constants
  156. 15.07: Disturbing a Reaction at Equilibrium: Le Châtelier’s Principle
  157. 15.08: The Effect of a Concentration Change on Equilibrium
  158. 15.09: The Effect of a Volume Change on Equilibrium
  159. 15.10: The Effect of Temperature Changes on Equilibrium
  160. 15.11: The Solubility-Product Constant
  161. 15.12: The Path of a Reaction and the Effect of a Catalyst
  162. 16: Oxidation and Reduction
  163. 16.1: The End of the Internal Combustion Engine?
  164. 16.2: Oxidation and Reduction: Some Definitions
  165. 16.3: Oxidation States - Electron Bookkeeping
  166. 16.4: Balancing Redox Equations
  167. 16.5: The Activity Series: Predicting Spontaneous Redox Reactions
  168. 16.6: Batteries: Using Chemistry to Generate Electricity
  169. 16.7: Electrolysis: Using Electricity to Do Chemistry
  170. 16.8: Corrosion: Undesirable Redox Reactions
  171. 17: Radioactivity and Nuclear Chemistry
  172. 17.01: Diagnosing Appendicitis
  173. 17.02: The Discovery of Radioactivity
  174. 17.03: Types of Radioactivity: Alpha, Beta, and Gamma Decay
  175. 17.04: Detecting Radioactivity
  176. 17.05: Natural Radioactivity and Half-Life
  177. 17.06: Radiocarbon Dating: Using Radioactivity to Measure the Age of Fossils and Other Artifacts
  178. 17.07: The Discovery of Fission and the Atomic Bomb
  179. 17.08: Nuclear Power: Using Fission to Generate Electricity
  180. 17.09: Nuclear Fusion: The Power of the Sun
  181. 17.10: The Effects of Radiation on Life
  182. 17.11: Radioactivity in Medicine