CHEM 2000: Chemistry for Engineers

by Scott Sinex, Scott Johnson, Joshua Halpern

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Publisher
Prince George's Community 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. Preface
  7. Creative Commons Copyright and the Source of this Book
  8. Unit 1: Atomic Structure
  9. Chapter 1: Introduction
  10. Chapter 1.1: The Atom
  11. Chapter 1.2: Isotopes and Atomic Masses
  12. Chapter 1.3: The Nucleus and Radioactivity
  13. Chapter 1.4: The Mole and Molar Mass
  14. Chapter 2: Atomic Structure
  15. Chapter 2.1: Wave - Particle Duality
  16. Chapter 2.2: Atomic Orbitals and Their Energies
  17. Chapter 2.3: Building Up The Periodic Table
  18. Chapter 2.4: Electronic Structure of the Transition Metals
  19. Chapter 2.5: Atomic Spectra and Models of the Atom
  20. Chapter 2.6: End of Chapter Material
  21. Chapter 3: The Periodic Table
  22. Chapter 3.1: Sizes of Atoms and Ions
  23. Chapter 3.2: Energetics of Ion Formation
  24. Chapter 3.3: The Chemical Families
  25. Chapter 3.4: The History of the Periodic Table
  26. Chapter 3.5: End of Chapter Material
  27. Unit 2: Molecular Structure
  28. Chapter 4: Chemical Bonding
  29. Chapter 4.0: What is a Chemical Bond?
  30. Chapter 4.1: Ionic Bonding
  31. Chapter 4.2: Lattice Energies in Ionic Solids
  32. Chapter 4.3: Lewis Electron Dot Symbols
  33. Chapter 4.4: Lewis Structures and Covalent Bonding
  34. Chapter 4.5: Exceptions to the Octet Rule
  35. Chapter 4.6: Properties of Covalent Bonds
  36. Chapter 4.7: Properties of Polar Covalent Bonds
  37. Chapter 4.8: Metallic Bonding
  38. Chapter 4.9: End of Chapter Material
  39. Chapter 5: Molecular Geometry
  40. Chapter 5.0: Molecular Geometry
  41. Chapter 5.1: Predicting the Geometry of Molecules
  42. Chapter 5.2: Localized Bonding and Hybrid Orbitals
  43. Chapter 5.3 Delocalized Bonding and Molecular Orbitals
  44. Chapter 5.4: Polyatomic Systems, Multiple Bonds, Resonance
  45. Chapter 5.5: Naming Organic Molecules
  46. Chapter 5.6: End of Chapter Material
  47. Unit 3: States of Matter
  48. Chapter 6: Gases
  49. Chapter 6.1: Gaseous Elements and Compounds
  50. Chapter 6.2: Gas Pressure
  51. Chapter 6.3: The Ideal Gas Law
  52. Chapter 6.4: The Combined Gas Law
  53. Chapter 6.5: Gas Mixtures
  54. Chapter 6.6: The Kinetic Theory of Gases
  55. Chapter 6.7: Mean Free Path
  56. Chapter 7: Fluids
  57. Chapter 7.0: Introduction
  58. Chapter 7.1: Real Gases
  59. Chapter 7.2: Intermolecular forces
  60. Chapter 7.3: Unique Properties of Liquids
  61. Chapter 7.4: Vapor Pressure
  62. Chapter 7.5: Changes of State
  63. Chapter 7.6: Critical Temperature and Pressure
  64. Chapter 7.7: Phase Diagrams
  65. Chapter 7.8: Liquid Crystals
  66. Chapter 7.9: End of Chapter Material
  67. Chapter 8: Solids
  68. Chapter 8.1: Crystalline and Amorphous Solids
  69. Chapter 8.2: Arrangement of Atoms in Crystals
  70. Chapter 8.3: Stucture of Simple Binary Compounds
  71. Chapter 8.4: Crystal Defects
  72. Chapter 8.5: Bonding and Properties of Solids
  73. Chapter 8.6: Metals and Semiconductors
  74. Chapter 8.7: Superconductors
  75. Chapter 8.8: Polymers
  76. Chapter 8.9: Modern Materials
  77. Chapter 8. 10: End of Chapter Material
  78. Chapter 9: Solutions
  79. Chapter 9.1: Forming Soutions
  80. Chapter 9.2: Solubility and Structure
  81. Chapter 9.3: Units for Concentration
  82. Chapter 9.4:Temperature and Pressure Effects
  83. Chapter 9.5: Colligative Properties
  84. Chapter 9.6: Aggregate Particles
  85. Chapter 9.7: End of Chapter Materials
  86. Unit 4: Nomenclature and Reactions
  87. Chapter 10: Nomenclature
  88. Chapter 10.0: Introduction
  89. Chapter 10.1: Molecular Representations and Formula
  90. Chapter 10.2: Chemical Formulas
  91. Chapter 10.3: Naming Ionic Compounds
  92. Chapter 10.4: Naming Covalent Compounds
  93. Chapter 10.5: Acids and Bases
  94. Chapter 10.6: End of Chapter Material
  95. Chapter 11: Stoichiometry
  96. Chapter 11.1: Again the Mole
  97. Chapter 11.2: Empirical and Molecular Formulas
  98. Chapter 11.3: Chemical Equations
  99. Chapter 11.4: Stoichiometry
  100. Chapter 11.5: Stoichiometry Involving Gases
  101. Chapter 11.6: Types of Chemical Reactions
  102. Chapter 11.7: End of Chapter Material
  103. Chapter 12: Aqueous Reactions
  104. Chapter 12.1: Preparing Solutions
  105. Chapter 12.2: Stoichiometry of Reactions in Solution
  106. Chapter 12.3: Ionic Equations
  107. Chapter 12.4: Precipitation Reactions
  108. Chapter 12.5: Acid Base Reactions
  109. Chapter 12.6: The Chemistry of Acid Rain
  110. Chapter 12.7: Oxidation-Reduction Reactions
  111. Chapter 12.8: End of Chapter Material
  112. Unit 5: Kinetics and Equilibria
  113. Chapter 13: Chemical Kinetics
  114. Chapter 13.1: Factors that Affect Reaction Rates
  115. Chapter 13.2: Reaction Rates and Rate Laws
  116. Chapter 13.3: Methods of Determining Reaction Order
  117. Chapter 13.4: Using Graphs to Determine Rate Laws, Rate Constants and Reaction Orders
  118. Chapter 13.5: Half Lives and Radioactive Decay Kinetics
  119. Chapter 13.6: Reaction Rates - A Microscopic View
  120. Chapter 13.7: The Collision Model of Chemical Kinetics
  121. Chapter 13.8: Catalysis
  122. Chapter 13.9: End of Chapter Materials
  123. Chapter 14: Chemical Equilibrium
  124. Chapter 14.1: The Concept of Chemical Equilibrium
  125. Chapter 14.2: The Equilibrium Constant
  126. Chapter 14.3: Solving Equilibrium Problems
  127. Chapter 14.4: Non-equilibrium Conditions
  128. Chapter 14.5: Factors That Affect Equilibrium
  129. Chapter 14.6: Controlling the Products of Reactions
  130. Chapter 14.7: End of Chapter Materials
  131. Unit 6: Thermo and Electrochemistry
  132. Chapter 15: First Law Thermochem
  133. Chapter 15.0: Introduction
  134. Chapter 15.1 Energy Changes in Chemical Reactions
  135. Chapter 15.2: The First Law of Thermodynamics
  136. Chapter 15.3: Enthalpy and Reactions
  137. Chapter 15.4: Hess's Law
  138. Chapter 15.5: Heats of Formation
  139. Chapter 15.6: Enthalpies of Solution
  140. Chapter 15.7: Fossil Fuels
  141. Chapter 15.8: Calorimetry
  142. Chapter 15.9: End of Chapter Material
  143. Chapter 16: Entropy and Free Energy
  144. Chapter 16.1: The Second Law of Thermodynamics
  145. Chapter 16.2: Entropy Changes and the Third Law of Thermodynamics
  146. Chapter 16.3: Free Energy
  147. Chapter 16.4: Spontaneity and Equilibrium
  148. Chapter 16.5: Comparing Thermodynamics and Kinetics
  149. Chapter 16.6: End of Chapter Material
  150. Chapter 17: Electrochemistry
  151. Chapter 17.0: Introduction
  152. Chapter 17.1: Describing Electrochemical Cells
  153. Chapter 17.2: Standard Potentials
  154. Chapter 17.3: Comparing Strengths of Oxidants and Reductants
  155. Chapter 17.4: Electrochemical Cells and Thermodynamics
  156. Chapter 17.5: Commercial Galvanic Cells
  157. Chapter 17.6: Corrosion
  158. Chapter 17.7: Electrolysis
  159. Chapter 17.8: End of Chapter Materials
  160. Unit 7: Nuclear Chemistry
  161. Chapter 18: Nuclear Chemistry
  162. Chapter 18.0: Introduction
  163. Chapter 18.1: The Components of the Nucleus
  164. Chapter 18.2: Nuclear Reactions
  165. Chapter 18.3: The Interaction of Nuclear Radiation with Matter
  166. Chapter 18.4: Thermodynamic Stability of the Atomic Nucleus
  167. Chapter 18.5: Applied Nuclear Chemistry
  168. Chapter 18.6: The Origin of the Elements
  169. Chapter 18.7: End of Chapter Material
  170. Back Matter
  171. Index
  172. Glossary
  173. Detailed Licensing