Lubbock Christian University: CHE 1305 Introductory Chemistry

by Jessica Rogers

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Publisher
Lubbock Christian University
Subjects
Chemistry
Licence
CC BY-NC-SA 4.0, as LibreTexts states it. Non-commercial use only.
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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. 1: The Chemical World
  6. 1.1: The Scope of Chemistry
  7. 1.2: Chemicals Compose Ordinary Things
  8. 1.3: The Basic Units of Measurement
  9. 1.4: Taking Measurements
  10. 1.5: Scientific Notation - Writing Large and Small Numbers
  11. 1.6: Significant Figures - Writing Numbers to Reflect Precision
  12. 1.7: Problem Solving and Unit Conversions
  13. 1.8: Problem Solving and Unit Conversions
  14. 1.9: Solving Multistep Conversion Problems
  15. 1.10: Density
  16. 2: Atoms
  17. 2.1: Cutting Alumimun until you get Atoms
  18. 2.2: Indivisible: The Atomic Theory
  19. 2.3: The Properties of Protons, Neutrons, and Electrons
  20. 2.4: Elements: Defined by Their Number of Protons
  21. 2.5: Counting Nails by the Pound
  22. 2.6: Counting Atoms by the Gram
  23. 3: Isotopes
  24. 3.1: Isotopes - When the Number of Neutrons Varies
  25. 3.2: Atomic Mass: The Average Mass of an Element’s Atoms
  26. 3.3: The Discovery of Radioactivity
  27. 3.4: The Effects of Radiation on Life
  28. 3.5: Types of Radioactivity - Alpha, Beta, and Gamma Decay
  29. 3.6: Natural Radioactivity and Half-Life
  30. 3.7: Radiocarbon Dating: Using Radioactivity to Measure the Age of Fossils and Other Artifacts
  31. 3.8: Radioactivity in Medicine
  32. 4: Ions
  33. 4.1: Ions - Losing and Gaining Electrons
  34. 4.2: The Bohr Model - Atoms with Orbits
  35. 4.3: Representing Valence Electrons with Dots
  36. 4.4: Lewis Structures of Ionic Compounds: Electrons Transferred
  37. 4.5: The Electromagnetic Spectrum
  38. 5: Periodic Table
  39. 5.1: Looking for Patterns: The Periodic Table
  40. 5.2: The Explanatory Power of the Quantum-Mechanical Model
  41. 6: Ionic Bonds
  42. 6.1: Writing Formulas for Ionic Compounds
  43. 6.2: Naming Ionic Compounds
  44. 7: Covalent Bonds
  45. 7.1: Covalent Lewis Structures: Electrons Shared
  46. 7.2: A Molecular View of Elements and Compounds
  47. 7.3: Electronegativity and Polarity: Why Oil and Water Don’t Mix
  48. 7.4: Naming Molecular Compounds
  49. 7.5: Nomenclature Summary
  50. 7.6: Chemical Formulas: How to Represent Compounds
  51. 7.7: Formula Mass: The Mass of a Molecule or Formula Unit
  52. 7.8: Counting Molecules by the Gram
  53. 8: Matter Classification
  54. 8.1: What is Matter?
  55. 8.2: Classifying Matter According to Its State: Solid, Liquid, and Gas
  56. 8.3: Classifying Matter According to Its Composition
  57. 8.4: Differences in Matter: Physical and Chemical Properties
  58. 8.5: Changes in Matter: Physical and Chemical Changes
  59. 8.6: Conservation of Mass - There is No New Matter
  60. 9: Chemical Reactions
  61. 9.1: Chemical Equations
  62. 9.2: Classifying Chemical Reactions
  63. 9.3: Oxidation–Reduction Reactions
  64. 10: Amounts in Chemical Reactions
  65. 10.1: Stoichiometry
  66. 10.2: How to Write Balanced Chemical Equations
  67. 10.3: Mole-to-Mole Conversions
  68. 10.4: Making Molecules: Mole to Mass (or vice versa) and Mass-to-Mass Conversions
  69. 11: Energy
  70. 11.1: Energy and Chemical and Physical Change
  71. 11.2: Energy
  72. 11.3: Temperature: Random Motion of Molecules and Atoms
  73. 11.4: Temperature Changes - Heat Capacity
  74. 11.5: Energy and Heat Capacity Calculations
  75. 11.6: Phase Changes
  76. 11.7: Evaporation and Condensation
  77. 11.8: Melting, Freezing, and Sublimation
  78. 12: Gases
  79. 12.1: Kinetic Molecular Theory: A Model for Gases
  80. 12.2: Pressure: The Result of Constant Molecular Collisions
  81. 12.3: Boyle’s Law: Pressure and Volume
  82. 12.4: Charles’s Law: Volume and Temperature
  83. 12.5: Gay-Lussac's Law: Temperature and Pressure
  84. 12.6: Avogadro’s Law: Volume and Moles
  85. 12.7: The Combined Gas Law: Pressure, Volume, and Temperature
  86. 12.8: Mixtures of Gases: Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen
  87. 13: Concentration of Solutions
  88. 13.1: Solutions: Homogeneous Mixtures
  89. 13.2: Solutions of Solids Dissolved in Water: How to Make Rock Candy
  90. 13.3: Solutions of Gases in Water
  91. 13.4: Solution Concentration: Mass Percent
  92. 13.5: Solution Dilution
  93. 13.6: Solution Dilution
  94. 13.7: Aqueous Solutions and Solubility: Compounds Dissolved in Water
  95. 13.8: Ionic Equations - A Closer Look
  96. 14: Separation of Solutions
  97. 14.1: Colloids
  98. 14.2: Osmosis
  99. 15: Acids and Bases
  100. 15.1: Acids: Properties and Examples
  101. 15.2: Bases: Properties and Examples
  102. 15.3: Acid and Base Indicators
  103. 15.4: Molecular Definitions of Acids and Bases
  104. 15.5: Acid–Base Titration
  105. 15.6: Strong and Weak Acids and Bases
  106. 15.7: Water - Acid and Base in One
  107. 15.8: The pH and pOH Scales - Ways to Express Acidity and Basicity
  108. 16: Reactions of Acids and Bases
  109. 16.1: Reactions of Acids and Bases
  110. 16.2: Buffers: Solutions That Resist pH Change
  111. 16.3: Acid–Base and Gas Evolution Reactions
  112. Back Matter
  113. Index
  114. Glossary