Chem 10 - Chemistry for Allied Health Majors

by Todd Clements

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This textbook is intended for the first semester of a two-semester general, organic, and biochemistry course. It covers the general chemistry portion and introduces some of the organic chemistry portion, but does not cover biochemistry.

Description from LibreTexts.

Publisher
Mt. San Antonio College
Subjects
Chemistry
Licence
CC BY-NC-SA, as LibreTexts states it. Non-commercial use only.
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. Licensing
  3. TitlePage
  4. InfoPage
  5. Table of Contents
  6. Licensing
  7. 1: Numbers and Measurements
  8. 1.1: Chemistry - The Central Science
  9. 1.2: Physical Quantities - Units and Scientific Notation
  10. 1.3: Measuring Mass, Length, and Volume
  11. 1.4: Measurement and Significant Figures
  12. 1.5: Rounding Off Numbers
  13. 1.6: Problem Solving - Unit Conversions and Estimating Answers
  14. 1.7: Density and Specific Gravity
  15. 2: Matter and Energy
  16. 2.1: Prelude to Energy and Chemical Processes
  17. 2.2: States of Matter
  18. 2.3: Classification of Matter
  19. 2.4: Temperature, Heat, and Energy
  20. 2.5: Phase Changes
  21. 2.6: Changes of State Calculations
  22. 3: Elements, Atoms and the Periodic Table
  23. 3.1: Chemical Elements and Symbols
  24. 3.2: Atomic Theory and the Structure of Atoms
  25. 3.3: Elements and Atomic Number
  26. 3.4: Isotopes and Atomic Weight
  27. 3.5: The Periodic Table
  28. 3.6: Some Characteristics of Different Groups
  29. 3.7: Electronic Structure of Atoms
  30. 3.8: Electron Configurations
  31. 3.9: Electron Configurations and the Periodic Table
  32. 3.10: Electron-Dot Symbols
  33. 4: Ionic Compounds
  34. 4.1: Ions
  35. 4.2: Ions and the Octet Rule
  36. 4.3: Ions of Some Common Elements
  37. 4.4: Periodic Properties and Ion Formation
  38. 4.5: Naming Monoatomic Ions
  39. 4.6: Polyatomic Ions
  40. 4.7: Ionic Bonds
  41. 4.8: Formulas of Ionic Compounds
  42. 4.9: Naming Ionic Compounds
  43. 4.10: Some Properties of Ionic Compounds
  44. 4.11: H⁺ and OH⁻ Ions - An Introduction to Acids and Bases
  45. 5: Covalent Compounds
  46. 5.1: Covalent Bonds
  47. 5.2: Covalent Bonds and the Periodic Table
  48. 5.3: Multiple Covalent Bonds
  49. 5.4: Coordinate Covalent Bonds
  50. 5.5: Characteristics of Molecular Compounds
  51. 5.6: Molecular Formulas and Lewis Structures
  52. 5.7: Drawing Lewis Structures
  53. 5.8: The Shapes of Molecules
  54. 5.9: Polar Covalent Bonds and Electronegativity
  55. 5.10: Polar Molecules
  56. 5.11: Naming Simple Covalent Compounds
  57. 6: Chemical Reactions and Quantities
  58. 6.1: Chemical Reactions - Examples of Chemical Change
  59. 6.2: Chemical Equations and the Conservation of Matter
  60. 6.3: Balancing Chemical Equations
  61. 6.4: Precipitation Reactions and Solubility Guidelines
  62. 6.5: Acids, Bases, and Neutralization Reactions
  63. 6.6: Redox Reactions
  64. 6.7: The Mole and Avogadro’s Number
  65. 6.8: Gram-Mole Conversions
  66. 6.9: Mole Relationships and Chemical Equations
  67. 6.10: Mass Relationships and Chemical Equations
  68. 6.11: How Do Chemical Reactions Occur? Reaction Rates
  69. 6.12: Effects of Temperature, Concentration, and Catalysts on Reaction Rates
  70. 6.13: Reversible Reactions and Chemical Equilibrium
  71. 7: Gases, Liquids, and Solids
  72. 7.1: States of Matter and Their Changes
  73. 7.2: Intermolecular Forces
  74. 7.3: Gases and Pressure
  75. 7.4: Boyle’s Law - The Relation between Volume and Pressure
  76. 7.5: Charles’s Law- The Relation between Volume and Temperature
  77. 7.6: Gay-Lussac's Law- The Relationship Between Pressure and Temperature
  78. 7.7: The Combined Gas Law
  79. 7.8: Avogadro’s Law - The Relation between Volume and Molar Amount
  80. 7.9: Partial Pressure and Dalton's Law
  81. 7.10: Liquids
  82. 7.11: Solids
  83. 8: Solutions
  84. 8.1: Mixtures and Solutions
  85. 8.2: The Solution Process
  86. 8.3: Solubility
  87. 8.4: The Effect of Temperature on Solubility
  88. 8.5: The Effect of Pressure on Solubility - Henry’s Law
  89. 8.6: Units of Concentration
  90. 8.7: Dilution
  91. 8.8: Ions in Solution - Electrolytes
  92. 8.9: Properties of Solutions
  93. 8.10: Osmosis and Osmotic Pressure
  94. 8.11: Dialysis
  95. 9: Acids and Bases
  96. 9.1: Acids and Bases Definitions
  97. 9.2: Acid and Base Strength
  98. 9.3: Water as Both an Acid and a Base
  99. 9.4: Measuring Acidity in Aqueous Solutions- The pH Scale
  100. 9.5: Working with [H+], [OH-] and pH
  101. 9.6: Acid and Base Equivalents
  102. 9.7: Buffer Solutions
  103. 10: Introduction to Organic Chemistry
  104. 10.1: The Nature of Organic Molecules
  105. 10.2: The Structure of Organic Molecules - Alkanes and Their Isomers
  106. 10.3: Drawing Organic Structures
  107. 10.4: Naming Alkanes
  108. 10.5: Properties of Alkanes
  109. 10.6: Reactions of Alkanes
  110. 10.7: Cycloalkanes
  111. 10.8: Drawing and Naming Cycloalkanes
  112. 10.9: Drawing organic molecules from a name
  113. 10.10: Families of Organic Molecules - Functional Groups
  114. 11: Nuclear Chemistry
  115. 11.1: Nuclear Reactions
  116. 11.2: The Discovery and Nature of Radioactivity
  117. 11.3: Stable and Unstable Isotopes
  118. 11.4: Nuclear Decay
  119. 11.5: Radioactive Half-Life
  120. 11.6: Detecting and Measuring Radiation
  121. 11.7: Artificial Transmutation
  122. 11.8: Nuclear Fission and Nuclear Fusion
  123. Back Matter
  124. Index
  125. Glossary
  126. Detailed Licensing