Chem 1402:General Chemistry I

by Robert Belford

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This text builds upon a knowledge foundation in chemistry and offers inquiry into topics of scientific measurement, chemical nomenclatures, expressing qualitative and quantitative statements about chemistry reactions, qualitative atomic theory, electronic and molecular structure models, chemical periodicity, thermochemistry, gases, kinetics molecular theory, and nuclear chemistry.

Description from LibreTexts.

Publisher
University of Arkansas at Little Rock
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. Text
  2. Front Matter
  3. TitlePage
  4. InfoPage
  5. Table of Contents
  6. Licensing
  7. 1: Basic Concepts of Chemistry
  8. 1.1: Chemistry and its Methods
  9. 1.2: Sustainability and Green Chemistry
  10. 1.3: Classifying Matter
  11. 1.4: Elements
  12. 1.5: Compounds
  13. 1.6: Physical Properties
  14. 1.7: Physical and Chemical Changes
  15. 1.8: Energy- Some Basic Principles
  16. 2: Review of the Tools of Quantitative Chemistry
  17. 2.1: Units of Measurement
  18. 2.2: Making Measurements- Experimental Error, Accuracy, Precision, Standard Deviation and Significant Figures
  19. 2.3: Mathematics in Chemistry
  20. 2.4: Problem Solving by Dimensional Analysis
  21. 2.5: Graphs and Graphing
  22. 2.6: Algebra Review
  23. 3: Atoms, Molecules, and Ions
  24. 3.1: Atoms- Their Composition and Structure
  25. 3.2: Isotopes- Atomic Number and Atomic Mass Unit
  26. 3.3: Isotope Abundance and Atomic Weight
  27. 3.4: The Periodic Table
  28. 3.5: Chemical Compounds
  29. 3.6: Ionic Compounds and Formulas
  30. 3.7: Nomenclature
  31. 3.8: Atoms and the Mole
  32. 3.9: Calculations Determining the Mass, Moles and Number of Particles
  33. 3.10: Percent Composition
  34. 3.11: Empirical and Molecular Formulas
  35. 3.12: Hydrates
  36. 4: Chemical Reactions
  37. 4.1: Introduction to Chemical Equations
  38. 4.2: Types of Chemical Reactions
  39. 4.3: Balancing Chemical Equations
  40. 4.4: Aqueous Reactions
  41. 4.5: Acid-Base Reactions
  42. 4.6: Redox Reactions
  43. 5: Stoichiometry- Quantitative Information about Chemical Reactions
  44. 5.1: Stoichiometry
  45. 5.2: Limiting and Excess Reagents
  46. 5.3: Percent Yield
  47. 5.4: Measuring Concentrations of Solutions
  48. 5.5: pH scale for concentration of Acids and Bases
  49. 5.6: Stoichiometry of Reactions in Aqueous Solutions
  50. 5.7: Chemical Equations and Quantitative Analysis
  51. 5.8: Spectrophotometry
  52. 6: Energy and Chemical Reactions
  53. 6.1: Energy
  54. 6.2: Heat Capacity
  55. 6.3: Energy and Phase Transitions
  56. 6.4: First Law of Thermodynamics
  57. 6.5: Enthalpy Changes of Chemical Reactions
  58. 6.6: Calorimetry
  59. 6.7: Enthalpy Calculations
  60. 7: The Structure of Atoms
  61. 7.1: Electromagnetic Radiation
  62. 7.2: Quantization- Planck, Einstein, Energy, and Photons
  63. 7.3: Atomic Line Spectra and Niels Bohr
  64. 7.4: Wave-Particle Duality
  65. 7.5: The Modern View of Electronic Structure
  66. 7.6: The Shapes of Atomic Orbitals
  67. 7.7: Electron Spin and the Pauli Exclusion Principle
  68. 8: The Structure of Atoms and Periodic Trends
  69. 8.1: Orbitals of Polyelectronic Atoms
  70. 8.2: Electron Configurations of Atoms and Monatomic Ions
  71. 8.3: Atomic Properties and Periodic Trends
  72. 9: Bonding and Molecular Structure
  73. 9.1: Chemical Bond Formation- An Introduction
  74. 9.2: Covalent Bonding and Lewis Structures
  75. 9.3: Resonance
  76. 9.4: Formal Charge
  77. 9.5: Drawing Lewis Dot Structures
  78. 9.6: Molecular Geometries
  79. 9.7: Bond Polarity and Electronegativity (\(\chi\))
  80. 9.8: Bond and Molecular Polarity
  81. 9.9: Covalent Bond Properties- Order, Length, and Energy
  82. 9.10: Ionic Bonds
  83. 10: Orbital Hybridization and Molecular Orbitals
  84. 10.1: Orbitals and Theories of Chemical Bonding
  85. 10.2: Valence Bond Theory
  86. 10.3: Molecular Orbital Theory
  87. 11: Gases
  88. 11.1: Gas Properties
  89. 11.2: Gas Laws
  90. 11.3: Gas Phase Reactions
  91. 11.4: Gas Mixtures
  92. 11.5: Kinetic Molecular Theory of Gases
  93. 11.6: Diffusion and Effusion
  94. 11.7: Nonideal Gases
  95. 12: Intermolecular Forces and Liquids
  96. 12.1: States of Matter and Intermolecular Forces
  97. 12.2: Ion-Dipole Forces
  98. 12.3: Dipole-Dipole Forces
  99. 12.4: NonPolar Molecules and IMF
  100. 12.5: Hydrogen Bonds
  101. Back Matter
  102. Index
  103. Glossary
  104. Detailed Licensing
  105. Homework
  106. 1A: Basic Concepts of Chemistry
  107. 1B: Review of the Tools of Quantitative Chemistry
  108. 2: Atoms, Molecules, and Ions
  109. 3: Chemical Reactions
  110. 4: Stoichiometry: Quantitative Information about Chemical Reactions
  111. 4.1: Stoichiometry
  112. 4.2: Limiting and Excess Reagents
  113. 4.3 Percent Yield
  114. 4.4: Chemical Equations and Quantitative Analysis
  115. 4.5: Measuring Concentrations of Solutions
  116. 4.6: pH scale for Concentration of Acids and Bases
  117. 4.7 Stoichiometry of Reactions in Aqueous Solutions
  118. 4.8: Spectrophotometry
  119. 5: Energy and Chemical Reactions
  120. 5.1: Energy
  121. 5.2: Specific Heat Capacity
  122. 5.3: Energy and Phase Transitions
  123. 5.4: First Law of Thermodynamics
  124. 5.5: Enthalpy Changes of Chemcial Reactions
  125. 5.6: Calorimetry
  126. 5.7: Enthalpy Calculations
  127. 6: The Structure of Atoms
  128. 6.1: Electromagnetic Radiation
  129. 6.2: Quantization: Planck, Einstein, Energy, and Photons
  130. 6.3: Atomic Line Spectra and Niels Bohr
  131. 6.4: Particle-Wave Duality: Prelude to Quantum Mechanics
  132. 6.5: The Modern View of Electronic Structure: Quantum Mechanics
  133. 6.6: The Shapes of Atomic Orbitals
  134. 6.7: One More Electron Property: Electron Spin
  135. 7: The Structure of Atoms and Periodic Trends
  136. 7.1: The Pauli Exclusion Principle
  137. 7.2: Atomic Subshell Energies and Electron Assignments
  138. 7.3: Electron Configuration of Atoms
  139. 7.4: Electron Configuration of Ions
  140. 7.5: Atomic Properties and Periodic Trends
  141. 7.6: Periodic Trends and Chemical Properties
  142. 8: Bonding and Molecular Structure
  143. 8.1: Chemical Bond Formation: An Introduction
  144. 8.2: Covalent Bonding and Lewis Structures
  145. 8.3: Resonance
  146. 8.4: Formal Charge
  147. 8.5 Drawing Lewis Dot Structures
  148. 8.6 Molecular Geometries
  149. 8.7: Bond Polarity and Electronegativity
  150. 8.8: Bond and Molecular Polarity
  151. 8.9: Covalent Bond Properties
  152. 8.10: DNA, Revisited
  153. 9: Orbital Hybridization and Molecular Orbitals
  154. 9.1: Orbitals and Theories of Chemical Bonding
  155. 9.2: Valence Bond Theory
  156. 9.3: Molecular Orbital Theory
  157. 10: Gases
  158. 10.1: Gas Properties
  159. 10.2: Gas Laws
  160. 10.3: Gas Phase Reactions
  161. 10.4: Gas Mixtures
  162. 10.5: Kinetic Molecular Theory of Gases
  163. 10.6: Diffusion and Effusion
  164. 10.7: Non-ideal Gases
  165. Worksheets
  166. Chapters 1A and 1B Problem Sets
  167. Chapter 2 Problem Sets
  168. Chapter 3 Problem Sets
  169. Chapter 4 Problem Sets
  170. Chapter 5 Problem Sets
  171. Chapter 10 Problem Sets