Chem 400: General Chemistry I

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CHEM 400 covers the fundamental principles and concepts of chemistry including chemical nomenclature, balancing reactions, stoichiometry, thermochemistry, acid/base and reduction/oxidation (redox) reactions. Also covered are theories addressing atomic and molecular structure and bonding, as well as the physical and chemical properties of gases, liquids, solids, and solutions, including intermolecular forces.

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Publisher
Sacramento City 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. 1: Matter, Measurement, and Problem Solving
  7. 1.1: Atoms and Molecules
  8. 1.2: The Scientific Approach to Knowledge
  9. 1.3: The Classification of Matter
  10. 1.4: Physical and Chemical Changes and Properties
  11. 1.5: Energy: A Fundamental Part of Physical and Chemical Change
  12. 1.6: The Units of Measurement
  13. 1.7: The Reliability of a Measurement
  14. 1.8: Solving Chemical Problems
  15. 1.E: Matter, Measurement, and Problem Solving (Exercises)
  16. 2: Atoms and Elements
  17. 2.1: Brownian Motion: Evidence for Atoms
  18. 2.2: Early Ideas about the Building Blocks of Matter
  19. 2.3: Modern Atomic Theory and the Laws That Led to It
  20. 2.4: The Discovery of the Electron
  21. 2.5 The Structure of The Atom
  22. 2.6 Subatomic Particles: Protons, Neutrons, and Electrons in Atoms
  23. 2.7 Finding Patterns: The Periodic Law and the Periodic Table
  24. 2.8 Atomic Mass: The Average Mass of an Element’s Atoms
  25. 2.9 Molar Mass: Counting Atoms by Weighing Them
  26. 2.E : Atoms and Elements (Exercises)
  27. 3: Molecules, Compounds and Chemical Equations
  28. 3.1: Hydrogen, Oxygen, and Water
  29. 3.2: Chemical Bonds
  30. 3.3: Representing Compounds: Chemical Formulas and Molecular Models
  31. 3.4: An Atomic-Level Perspective of Elements and Compounds
  32. 3.5: Ionic Compounds: Formulas and Names
  33. 3.6: Molecular Compounds: Formulas and Names
  34. 3.7: Summary of Inorganic Nomenclature
  35. 3.9: Composition of Compounds
  36. 3.10: Determining a Chemical Formula from Experimental Data
  37. 3.11: Writing and Balancing Chemical Equations
  38. 3.12: Organic Compounds
  39. 3.E: Molecules, Compounds and Chemical Equations (Exercises)
  40. 4: Chemical Reactions and Aqueous Reactions
  41. 4.1: Global Warming and the Combustion of Fossil Fuels
  42. 4.2 Reaction Stoichiometry: How Much Carbon Dioxide?
  43. 4.3 Limiting Reactant, Theoretical Yield, and Percent Yield
  44. 4.4: Solution Concentration and Solution Stoichiomentry
  45. 4.5: Types of Aqueous Solutions and Solubility
  46. 4.6: Precipitation Reactions
  47. 4.7: Representing Aqueous Reactions: Molecular, Ionic, and Complete Ionic Equations
  48. 4.8: Acid-Base and Gas-Evolution Reactions
  49. 4.9: Oxidation-Reduction Reactions
  50. 5: Gases
  51. 5.1: Water from Wells: Atmospheric Pressure at Work
  52. 5.2: Pressure: The Result of Particle Collisions
  53. 5.3: The Simple Gas Laws: Boyle’s Law, Charles’s Law and Avogadro’s Law
  54. 5.4: The Ideal Gas Law
  55. 5.5: Applications of the Ideal Gas Law: Molar Volume, Density and Molar Mass of a Gas
  56. 5.6: Mixtures of Gases and Partial Pressures
  57. 5.7: Gases in Chemical Reactions: Stoichiometry Revisited
  58. 5.8: Kinetic Molecular Theory: A Model for Gases
  59. 5.9: Mean Free Path, Diffusion, and Effusion of Gases
  60. 5.10: Real Gases: The Effects of Size and Intermolecular Forces
  61. 5.E: Gases (Exercises)
  62. 6: Thermochemistry
  63. 6.1: Light the Furnace: The Nature of Energy and Its Transformations
  64. 6.3: The First Law of Thermodynamics
  65. 6.2: The Nature of Energy
  66. 6.4: Quantifying Heat and Work
  67. 6.4: Constant Volume Calorimetry: Measuring ΔU for Chemical Reactions
  68. 6.5: Enthalpy: The Heat Evolved in a Chemical Reaction at Constant Pressure
  69. 6.7: Constant Pressure Calorimetry: Measuring ΔH for Chemical Reactions
  70. 6.7: Relationships Involving Enthalpy of Reactions
  71. 6.8: Enthalpies of Reaction from Standard Heats of Formation
  72. 6.9: Energy Use and The Environment
  73. 7: The Quantum-Mechanical Model of the Atom
  74. 7.1: Schrödinger's Cat
  75. 7.2: The Nature of Light
  76. 7.3: Atomic Spectroscopy and The Bohr Model
  77. 7.4: The Wavelength Nature of Matter
  78. 7.5: Quantum Mechanics and The Atom
  79. 7.6: The Shape of Atomic Orbitals
  80. 7.E: The Quantum-Mechanical Model of the Atom (Exercises)
  81. 8: Periodic Properties of the Elements
  82. 8.1: Nerve Signal Transmission
  83. 8.2: The Development of the Periodic Table
  84. 8.3: Electron Configurations: How Electrons Occupy Orbitals
  85. 8.4: Electron Configurations, Valence Electrons, and the Periodic Table
  86. 8.5: The Explanatory Power of the Quantum-Mechanical Model
  87. 8.6: Periodic Trends in the Size of Atoms and Effective Nuclear Charge
  88. 8.7: Ions- Configurations, Magnetic Properties, Radii, and Ionization Energy
  89. 8.8: Electron Affinities and Metallic Character
  90. 8.9: Examples of Periodic Chemical Behavior
  91. 8.E: Periodic Properties of the Elements (Exercises)
  92. 9: Chemical Bonding I: Lewis Structures & Determining Molecular Shapes
  93. 9.1: Bonding Models and AIDS Drugs
  94. 9.2: Types of Chemical Bonds
  95. 9.3: Representing Valance Electrons with Dots
  96. 9.4: Ionic Bonding
  97. 9.5: Covalent Bonding: Lewis Structure
  98. 9.6: Electronegativity and Bond Polarity
  99. 9.7: Lewis Structures
  100. 9.8: Resonance and Formal Charge
  101. 9.9: Exceptions to the Octet Rule
  102. 9.10: Bond Energies and Bond Lengths
  103. 9.11: Bonding in Metals
  104. 9.E: Chemical Bonding I (Exercises)
  105. 10: Chemical Bonding II: Valance Bond Theory and Molecular Orbital Theory
  106. 10.1: Artificial Sweeteners
  107. 10.2: VSEPR Theory: The Five Basic Shapes
  108. 10.3: VSPER Theory: The Effect of Lone Pairs
  109. 10.4: VSPER Theory: Predicting Molecular Geometries
  110. 10.5: Molecular Shape and Polarity
  111. 10.6: Valence Bond Theory: Orbital Overlap as a Chemical Bond
  112. 10.7: Valence Bond Theory: Hybridization of Atomic Orbitals
  113. 10.8: Molecular Orbital Theory: Electron Delocalization
  114. 11: Liquids, Solids, and Intermolecular Forces
  115. 11.1: Water in Zero Gravity
  116. 11.2: Solids, Liquids, and Gases: A Molecular Comparison
  117. 11.3: Intermolecular Forces: The Forces that Hold Condensed Phases Together
  118. 11.4: Intermolecular Forces in Action: Surface Tension, Viscosity, and Capillary Action
  119. 11.5: Vaporization and Vapor Pressure
  120. 11.6: Sublimation and Fusion
  121. 11.7: Heating Curve for Water
  122. 11.8: Phase Diagrams
  123. 11.9: Water - An Extraordinary Substance
  124. 12: Solids and Modern Materials
  125. 12.1: Discovery of Graphene
  126. 12.2: X-Ray Crystallography
  127. 12.3: Unit Cells and Basic Structures
  128. 12.4: The Fundamental Types of Crystalline Solids
  129. 12.5: The Structure of Ionic Solids
  130. 12.6: Network Covalent Atomic Solids: Carbon and Silicates
  131. 12.7: Ceramics, Cement, and Glass
  132. 12.8: Crystalline Solids: Band Theory
  133. 12.9: Polymers and Plastics
  134. 13: Solutions
  135. 13.1: Thirsty Solutions: Why You Should Not Drink Seawater
  136. 13.2: Types of Solutions and Solubility
  137. 13.3: Energetics of Solution Formation
  138. 13.4: Solution Equilibrium and Factors Affecting Solubility
  139. 13.5: Expressing Solution Concentration
  140. 13.6: Colligative Properties: Freezing Point Depression, Boiling Point Elevation, and Osmosis
  141. 13.7: The Colligative Properties of Strong Electrolyte Solutions
  142. 13.8: Colloids
  143. 13.E: Solutions (Exercises)
  144. 14: Chemical Kinetics
  145. 14.1: Catching Lizards
  146. 14.2: Rate of a Chemical Reaction
  147. 14.3: The Rate Law: The Effect of Concentration on Reaction Rate
  148. 14.4: The Integrated Rate Law: The Dependence of Concentration on Time
  149. 14.5: The Effect of Temperature on Reaction Rate
  150. 14.6: Reaction Mechanisms
  151. 14.7: Catalysis
  152. 15: Chemical Equilibrium
  153. 15.1: Fetal Hemoglobin and Equilibrium
  154. 15.2: The Concept of Dynamic Equilibrium
  155. 15.3: The Equilibrium Constant (K)
  156. 15.4: Expressing the Equilibrium Constant in Terms of Pressure
  157. 15.5: Calculating the Equilibrium Constant From Measured Equilibrium Concentrations
  158. 15.5: Heterogenous Equilibria: Reactions Involving Solids and Liquids
  159. 15.7: The Reaction Quotient: Predicting the Direction of Change
  160. 15.8: Finding Equilibrium Concentrations
  161. 15.9: Le Châtelier’s Principle: How a System at Equilibrium Responds to Disturbances
  162. 16: Acids and Bases
  163. 16.1: Heartburn
  164. 16.2: The Nature of Acids and Bases
  165. 16.3: Definitions of Acids and Bases
  166. 16.4: Acid Strength and the Acid Dissociation Constant (Ka)
  167. 16.5: Autoionization of Water and pH
  168. 16.6: Finding the [H3O+] and pH of Strong and Weak Acid Solutions
  169. 16.7: Base Solutions
  170. 16.8: The Acid-Base Properties of Ions and Salts
  171. 16.9: Polyprotic Acids
  172. 16.10: Acid Strength and Molecular Structure
  173. 16.11: Lewis Acids and Bases
  174. 16.12: Acid rain
  175. 17: Aqueous Ionic Equilibrium
  176. 17.1: The Danger of Antifreeze
  177. 17.2: Buffers: Solutions That Resist pH Change
  178. 17.3: Buffer Effectiveness: Buffer Capacity and Buffer Range
  179. 17.4: Titrations and pH Curves
  180. 17.5: Solubility Equilibria and the Solubility Product Constant
  181. 17.6: Precipitation
  182. 17.7: Qualitative Chemical Analysis
  183. 17.8: Complex Ion Equilibria
  184. 17.E: Aqueous Ionic Equilibrium (Exercises)
  185. 18: Gibbs Energy and Thermodynamics
  186. 18.1: Nature’s Heat Tax: You Can’t Win and You Can’t Break Even
  187. 18.2: Spontaneous and Nonspontaneous Processes
  188. 18.3: Entropy and the Second Law of Thermodynamics
  189. 18.4: Entropy Changes Associated with State Changes
  190. 18.5: Heat Transfer and Changes in the Entropy of the Surroundings
  191. 18.6: Gibbs Energy
  192. 18.7: Entropy Changes in Chemical Reactions
  193. 18.8: Gibbs Energy Changes in Chemical Reactions
  194. 18.9: Gibbs Energy Changers for Non-Standard States
  195. 18.10: Gibbs Energy and Equilibrium
  196. 19: Electrochemistry
  197. 19.1: Pulling the Plug on the Power Grid
  198. 19.2: Balancing Oxidation-Reduction Equations
  199. 19.3: Voltaic (or Galvanic) Cells: Generating Electricity from Spontaneous Chemical Reactions
  200. 19.4: Standard Reduction Potentials
  201. 19.5: Cell Potential, Gibbs Energy, and the Equilibrium Constant
  202. 19.6: Cell Potential and Concentration
  203. 19.7: Batteries: Using Chemistry to Generate Electricity
  204. 19.8: Electrolysis: Driving Non-spontaneous Chemical Reactions with Electricity
  205. 19.9: Corrosion: Undesirable Redox Reactions
  206. 20: Radioactivity and Nuclear Chemistry
  207. 20.1: Diagnosing Appendicitis
  208. 20.2: The Discovery of Radioactivity
  209. 20.3: Types of Radioactivity
  210. 20.4: The Valley of Stability: Predicting the Type of Radioactivity
  211. 20.5: Detecting Radioactivity
  212. 20.6: The Kinetics of Radioactive Decay and Radiometric Dating
  213. 20.7: The Discovery of Fission: The Atomic Bomb and Nuclear Power
  214. 20.8: Converting Mass to Energy: Mass Defect and Nuclear Binding Energy
  215. 20.9: Nuclear Fusion: The Power of the Sun
  216. 20.10: Nuclear Transmutation and Transuranium Elements
  217. 20.11: The Effects of Radiation on Life
  218. 20.12: Radioactivity in Medicine and Other Applications
  219. 21: Organic Chemistry
  220. 21.1: Fragrances and Odor
  221. 21.2: Carbon: Why It Is Unique
  222. 21.3: Hydrocarbons: Compounds Containing Only Carbon and Hydrocarbon
  223. 21.4: Alkanes: Saturated Hydrocarbons
  224. 21.5: Alkenes and Alkynes
  225. 21.6: Hydrocarbon Reactions
  226. 21.7: Aromatic Hydrocarbons
  227. 21.8: Functional Groups
  228. 21.9: Alcohols
  229. 21.10: Aldehydes and Ketones
  230. 21.11: Carboxylic Acids and Esters
  231. 21.12: Ethers
  232. 21.13: Amines
  233. 22: Biochemistry
  234. 22.1: Diabetes and the Synthesis of Human Insulin
  235. 22.2: Lipids
  236. 22.3: Carbohydrates
  237. 22.4: Proteins and Amino Acids
  238. 22.5: Protein Structure
  239. 22.6: Nucleic Acids: Blueprints for Proteins
  240. 22.7: DNA Replication, the Double Helix, and Protein Synthesis
  241. 23: Chemistry of the Nonmetals
  242. 23.1: Insulated Nanowires
  243. 23.2: The Main-Group Elements: Bonding and Properties
  244. 23.3: The Most Common Matter: Silicates
  245. 23.4: Boron and Its Amazing Structures
  246. 23.5: Carbon, Carbides, and Carbonates
  247. 23.6: Nitrogen and Phosphorus: Essential Elements for Life
  248. 23.7: Oxygen
  249. 23.8: Sulfur: A Dangerous and Useful Element
  250. 23.9: Halogens: Reactive Chemicals with High Electronegativity
  251. 23.E: Chemistry of the Nonmetals (Exercises)
  252. 24: Metals and Metallurgy
  253. 24.1: Vanadium: A Problem and an Opportunity
  254. 24.2: The General Properties and Natural Distribution of Metals
  255. 24.3: Metallurgical Processes
  256. 24.4: Metal Structures and Alloys
  257. 24.5: Sources, Properties, and Products of Some of the 3d Transition Metals
  258. 25: Transition Metals and Coordination Compounds
  259. 25.1: The Colors of Rubies and Emeralds
  260. 25.2: Properties of Transition Metals
  261. 25.3: Coordination Compounds
  262. 25.4: Structure and Isomerization
  263. 25.5: Bonding in Coordinate Compounds
  264. 25.6: Applications of Coordination Compounds
  265. 25.E: Transition Metals and Coordination Compounds (Exercises)
  266. Back Matter
  267. Index
  268. Glossary
  269. Detailed Licensing