CHE 125: GOB Introductory Chemistry

by Erin O’Connell

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In this book you will be learning about the fundamental concepts of chemistry. These concepts are meant to help you understand more about the world around you, and to prepare you for the second semester of this course on organic and biochemistry. This is the first semester of two part course on nursing chemistry.

Description from LibreTexts.

Publisher
UW-Milwaukee/Washington County & Waukesha
Subjects
Chemistry
Licence
CC BY, 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: Chemistry as a Science
  7. 1.1: The Scope of Chemistry
  8. 1.2: Chemicals Compose Ordinary Things
  9. 1.3: Hypothesis, Theories, and Laws
  10. 1.4: The Scientific Method - How Chemists Think
  11. 2: Measurements and Density
  12. 2.1: Taking Measurements
  13. 2.2: Scientific Notation - Writing Large and Small Numbers
  14. 2.3: Significant Figures - Writing Numbers to Reflect Precision
  15. 2.4: Significant Figures in Calculations
  16. 2.5: The Basic Units of Measurement
  17. 2.6: Problem Solving and Unit Conversions
  18. 2.7: Solving Multistep Conversion Problems
  19. 2.8: Units Raised to a Power
  20. 2.9: Density
  21. 2.10: Dosage Calculations
  22. 3: Matter
  23. 3.1: In Your Room
  24. 3.2: What is Matter?
  25. 3.3: Classifying Matter According to Its State- Solid, Liquid, and Gas
  26. 3.4: Classifying Matter According to Its Composition
  27. 3.5: Differences in Matter- Physical and Chemical Properties
  28. 3.6: Changes in Matter - Physical and Chemical Changes
  29. 3.7: Conservation of Mass - There is No New Matter
  30. 3.E: Chemistry, Matter, and Measurement (Exercises)
  31. 4: Atoms, Elements, and the Periodic Table
  32. 4.1: Prelude to Elements, Atoms, and the Periodic Table
  33. 4.2: The Elements
  34. 4.3: Atomic Theory
  35. 4.4: Atomic Theory
  36. 4.5: Defining Isotopes
  37. 4.6: Atomic Masses
  38. 4.7: Arrangements of Electrons
  39. 4.8: Orbital Shape
  40. 4.9: The Periodic Table
  41. 4.10: Ions - Losing and Gaining Electrons
  42. 4.E: Elements, Atoms, and the Periodic Table (Exercises)
  43. 5: Compounds- Ionic and Covalent
  44. 5.1: Sugar and Salt
  45. 5.2: Compounds Display Constant Composition
  46. 5.3: Chemical Formulas- How to Represent Compounds
  47. 5.4: A Molecular View of Elements and Compounds
  48. 5.5: Writing Formulas for Ionic Compounds
  49. 5.6: Nomenclature- Naming Compounds
  50. 5.7: Naming Ionic Compounds
  51. 5.8: Naming Molecular Compounds
  52. 5.9: Naming Acids
  53. 5.10: Nomenclature Summary
  54. 5.11: Formula Mass- The Mass of a Molecule or Formula Unit
  55. 5.12: Moles, Molecular Formulas, and Calculating Empirical Formulas for Compounds
  56. 6: Chemical Bonding
  57. 6.1: Representing Valence Electrons with Dots
  58. 6.2: Lewis Structures of Ionic Compounds- Electrons Transferred
  59. 6.3: Covalent Lewis Structures- Electrons Shared
  60. 6.4: Writing Lewis Structures for Covalent Compounds
  61. 6.5: Resonance - Equivalent Lewis Structures for the Same Molecule
  62. 6.6: Predicting the Shapes of Molecules
  63. 6.7: Electronegativity and Polarity - Why Oil and Water Don’t Mix
  64. 7: Chemical Reactions
  65. 7.1: Prelude to Introduction to Chemical Reactions
  66. 7.2: Laws of Conservation : A Review
  67. 7.3: Evidence of a Chemical Reaction
  68. 7.4: Chemical Equations
  69. 7.5: How to Write Balanced Chemical Equations
  70. 7.6: Aqueous Solutions and Solubility - Compounds Dissolved in Water
  71. 7.7: Precipitation Reactions
  72. 7.8: Writing Chemical Equations for Reactions in Solution- Molecular, Complete Ionic, and Net Ionic Equations
  73. 7.9: Acid–Base and Gas Evolution Reactions
  74. 7.10: Oxidation-Reduction Reactions
  75. 7.11: Classifying Chemical Reactions
  76. 7.12: The Activity Series- Predicting Spontaneous Redox Reactions
  77. 8: Quantities in Chemical Reactions
  78. 8.1: Prelude to Quantities in Chemical Reactions
  79. 8.2: The Mole
  80. 8.3: Atomic and Molar Masses
  81. 8.4: Mole-Mass Conversions
  82. 8.5: Mole-Mole Relationships in Chemical Reactions
  83. 8.6: Mole-Mass and Mass-Mass Problems
  84. 8.E: Quantities in Chemical Reactions (Exercise)
  85. 8.S: Quantities in Chemical Reactions (Summary)
  86. 9: Solutions
  87. 9.1: Prelude to Solutions
  88. 9.2: Solutions
  89. 9.3: Concentration
  90. 9.4: The Dissolution Process
  91. 9.5: Properties of Solutions
  92. 9.E: Solutions (Exercises)
  93. 9.S: Solutions (Summary)
  94. 10: Equilibrium
  95. 10.1: The Rate of a Chemical Reaction
  96. 10.2: The Idea of Dynamic Chemical Equilibrium
  97. 10.3: The Equilibrium Constant - A Measure of How Far a Reaction Goes
  98. 10.4: Disturbing a Reaction at Equilibrium- Le Châtelier’s Principle
  99. 10.5: The Effect of a Concentration Change on Equilibrium
  100. 10.6: The Effect of a Volume Change on Equilibrium
  101. 10.7: The Effect of Temperature Changes on Equilibrium
  102. 10.8: The Path of a Reaction and the Effect of a Catalyst
  103. 11: Energy and Chemical Processes
  104. 11.1: Prelude to Energy and Chemical Processes
  105. 11.2: Energy and Its Units
  106. 11.3: Heat
  107. 11.4: Phase Changes
  108. 11.5: Bond Energies and Chemical Reactions
  109. 11.6: The Energy of Biochemical Reactions
  110. 11.E: Energy and Chemical Processes (Exercises)
  111. 11.S: Energy and Chemical Processes (Summary)
  112. 12: Solids, Liquids, and Gases
  113. 12.1: A Molecular Comparison of Gases, Liquids, and Solids
  114. 12.2: Kinetic-Molecular Theory
  115. 12.3: The Ideal Gas Equation
  116. 12.4: The Kinetic-Molecular Theory Explains the Behavior of Gases
  117. 12.5: Dalton's Law (Law of Partial Pressures)
  118. 12.6: Evaporation and Condensation
  119. 12.7: Intermolecular forces
  120. 13: Acids and Bases
  121. 13.1: Prelude to Acids and Bases
  122. 13.2: Arrhenius Definition of Acids and Bases
  123. 13.3: Brønsted-Lowry Definition of Acids and Bases
  124. 13.4: Water - Both an Acid and a Base
  125. 13.5: The Strengths of Acids and Bases
  126. 13.6: Buffers
  127. 13.E: Acids and Bases (Exercises)
  128. 13.S: Acids and Bases (Summary)
  129. 14: Organic Chemistry - Alkanes and Halogenated Hydrocarbons
  130. 14.1: Organic Chemistry
  131. 14.2: Structures and Names of Alkanes
  132. 14.3: Alkenes- Structures and Names
  133. 14.4: Alkynes
  134. 14.5: Branched-Chain Alkanes
  135. 14.6: Condensed Structural and Line-Angle Formulas
  136. 14.7: IUPAC Nomenclature
  137. 14.8: Physical Properties of Alkanes
  138. 14.9: Physical Properties of Alkenes
  139. 14.10: Chemical Properties of Alkanes
  140. 14.11: Chemical Properties of Alkenes
  141. 14.12: Halogenated Hydrocarbons
  142. 14.13: Cycloalkanes
  143. 14.14: Organic Chemistry - Alkanes and Halogenated Hydrocarbons
  144. 14.15: Organic Reactions
  145. 14.E: Organic Chemistry- Alkanes and Halogenated Hydrocarbons (Exercises)
  146. 14.S: Organic Chemistry- Alkanes and Halogenated Hydrocarbons (Summary)
  147. 14.S: Unsaturated and Aromatic Hydrocarbons (Summary)
  148. Back Matter
  149. Index
  150. Index
  151. Glossary
  152. Detailed Licensing