Chemistry 305:Introduction to Chemistry

by Caitlin Zumalt

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Publisher
American River College
Subjects
Chemistry
Licence
CC BY-SA, as LibreTexts states it
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: Unit 1
  7. 1.1: The Scope of Chemistry
  8. 1.2: The Scientific Method - How Chemists Think
  9. 1.3: Hypothesis, Theories, and Laws
  10. 1.4: Taking Measurements
  11. 1.5: The Basic Units of Measurement
  12. 1.6: Units Raised to a Power
  13. 1.7: Scientific Notation - Writing Large and Small Numbers
  14. 1.8: Significant Figures - Writing Numbers to Reflect Precision
  15. 1.9: Significant Figures in Calculations
  16. 1.10: Problem Solving and Unit Conversions
  17. 1.11: Solving Multi-step Conversion Problems
  18. 1.12: Density
  19. 1.13: Temperature - Random Motion of Molecules and Atoms
  20. 1.E: Measurement and Problem Solving (Exercises)
  21. 2: Unit 2
  22. 2.1: In Your Room
  23. 2.2: What is Matter?
  24. 2.3: Classifying Matter According to Its State—Solid, Liquid, and Gas
  25. 2.4: Classifying Matter According to Its Composition
  26. 2.5: Differences in Matter- Physical and Chemical Properties
  27. 2.6: Changes in Matter - Physical and Chemical Changes
  28. 2.7: Conservation of Mass - There is No New Matter
  29. 2.8: Cutting Aluminum until you get Atoms
  30. 2.9: Indivisible - The Atomic Theory
  31. 2.10: The Nuclear Atom
  32. 2.11: The Properties of Protons, Neutrons, and Electrons
  33. 2.12: Elements- Defined by Their Number of Protons
  34. 2.13: Looking for Patterns - The Periodic Table
  35. 2.14: Ions - Losing and Gaining Electrons
  36. 2.15: Isotopes - When the Number of Neutrons Varies
  37. 2.16: Atomic Mass - The Average Mass of an Element’s Atoms
  38. 2.17: Sugar and Salt
  39. 2.18: Compounds Display Constant Composition
  40. 2.19: Chemical Formulas - How to Represent Compounds
  41. 2.20: A Molecular View of Elements and Compounds
  42. 2.21: Writing Formulas for Ionic Compounds
  43. 2.22: Nomenclature- Naming Compounds
  44. 2.23: Naming Ionic Compounds
  45. 2.24: Naming Molecular Compounds
  46. 2.25: Naming Acids
  47. 2.26: Nomenclature Summary
  48. 3: Unit 3
  49. 3.1: Evidence of a Chemical Reaction
  50. 3.2: The Chemical Equation
  51. 3.3: How to Write Balanced Chemical Equations
  52. 3.4: Classifying Chemical Reactions
  53. 3.5: Aqueous Solutions and Solubility - Compounds Dissolved in Water
  54. 3.6: Precipitation Reactions
  55. 3.7: Writing Chemical Equations for Reactions in Solution- Molecular, Complete Ionic, and Net Ionic Equations
  56. 3.8: Prelude to Chemical Composition - How Much Sodium?
  57. 3.9: Counting Nails by the Pound
  58. 3.10: Counting Atoms by the Gram
  59. 3.11: Counting Molecules by the Gram
  60. 3.12: Chemical Formulas as Conversion Factors
  61. 3.13: Mass Percent Composition of Compounds
  62. 3.14: Mass Percent Composition from a Chemical Formula
  63. 3.15: Calculating Empirical Formulas for Compounds
  64. 3.16: Calculating Molecular Formulas for Compounds
  65. 3.17: Making Pancakes- Relationships Between Ingredients
  66. 3.18: Making Molecules- Mole-to-Mole Conversions
  67. 3.19: Making Molecules- Mass-to-Mass Conversions
  68. 3.20: Stoichiometry
  69. 3.21: Limiting Reactant and Theoretical Yield
  70. 3.22: Limiting Reactant, Theoretical Yield, and Percent Yield from Initial Masses of Reactants
  71. 4: Unit 4
  72. 4.1: The Bohr Model - Atoms with Orbits
  73. 4.2: Quantum-Mechanical Orbitals and Electron Configurations
  74. 4.3: Electron Configurations and the Periodic Table
  75. 4.4: The Explanatory Power of the Quantum-Mechanical Model
  76. 4.5: Representing Valence Electrons with Dots
  77. 4.6: Lewis Structures of Ionic Compounds- Electrons Transferred
  78. 4.7: Covalent Lewis Structures- Electrons Shared
  79. 4.8: Writing Lewis Structures for Covalent Compounds
  80. 4.9: Resonance - Equivalent Lewis Structures for the Same Molecule
  81. 4.10: Predicting the Shapes of Molecules
  82. 4.11: Electronegativity and Polarity - Why Oil and Water Do not Mix
  83. 4.12: Kinetic Molecular Theory- A Model for Gases
  84. 4.13: Pressure - The Result of Constant Molecular Collisions
  85. 4.14: Boyle’s Law - Pressure and Volume
  86. 4.15: Charles’s Law- Volume and Temperature
  87. 4.16: Gay-Lussac's Law- Temperature and Pressure
  88. 4.17: The Combined Gas Law- Pressure, Volume, and Temperature
  89. 4.18: The Ideal Gas Law- Pressure, Volume, Temperature, and Moles
  90. 4.19: Mixtures of Gases - Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen
  91. 5: Unit 5
  92. 5.1: Intermolecular Forces- Dispersion, Dipole–Dipole, Hydrogen Bonding, and Ion-Dipole
  93. 5.2: Solutions - Homogeneous Mixtures
  94. 5.3: Solutions of Solids Dissolved in Water- How to Make Rock Candy
  95. 5.4: Specifying Solution Concentration- Mass Percent
  96. 5.5: Specifying Solution Concentration- Molarity
  97. 5.6: Solution Stoichiometry
  98. 5.7: Sour Patch Kids and International Spy Movies
  99. 5.8: Acids- Properties and Examples
  100. 5.9: Bases- Properties and Examples
  101. 5.10: Molecular Definitions of Acids and Bases
  102. 5.11: Reactions of Acids and Bases
  103. 5.12: Acid–Base Titration
  104. 5.13: Strong and Weak Acids and Bases
  105. 5.14: Water - Acid and Base in One
  106. 5.15: The pH and pOH Scales - Ways to Express Acidity and Basicity
  107. 5.16: Carbon - A Versitile Atom
  108. 5.17: Hydrocarbons- Compounds Containing Only Carbon and Hydrocarbon
  109. 5.18: Alkanes- Saturated Hydrocarbons
  110. 5.19: Isomers- Same Formula, Different Structure
  111. 5.20: Naming Alkanes
  112. 5.21: Alkenes and Alkynes
  113. 5.22: Functional Groups
  114. 5.23: Carbohydrates
  115. 5.24: Lipids
  116. 5.25: Proteins
  117. Back Matter
  118. Index
  119. Glossary
  120. Detailed Licensing
  121. Detailed Licensing