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Chem 100: Fundamentals of G(OB) Chemistry

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Chem 100: Fundamentals of G(OB) Chemistry

This course is a one-semester survey of general, organic, and biological chemistry for nursing and other health-related fields. Topics include general chemistry, organic chemistry, and biological chemistry as they apply to the human body. This course is intended for students majoring in nursing, nutrition, or allied health fields.

Chemistry
Author
Fred Garces
Publisher
San Diego Miramar College
Source
LibreTexts
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 167 sections
  1. 01: Chemistry Around Us
  2. 1.01: Prelude to Chemistry
  3. 1.02: Basic Definitions
  4. 1.03: What is Chemistry
  5. 1.04: Chemicals Compose Ordinary Things
  6. 1.05: Hypothesis Theories and Laws
  7. 1.06: The Scientific Method - How Chemists Think
  8. 1.07: Learning Chemistry
  9. 1.08: A Beginning Chemist - How to Succeed
  10. 1.09: Scientific Problem Solving
  11. 02: Measurements
  12. 2.01: The Basic Units of Measurement
  13. 2.02: Taking Measurements
  14. 2.2.01: Measurements in the Laboratory (Experiment)-Home Version
  15. 2.03: Scientific Notation - Writing Large and Small Numbers
  16. 2.04: Significant Figures - Writing Numbers to Reflect Precision
  17. 2.05: Significant Figures in Calculations
  18. 2.06: Problem Solving and Unit Conversions
  19. 2.07: Solving Multistep Conversion Problems
  20. 2.08: Numerical Problem-Solving Strategies and the Solution Map
  21. 2.09: Density
  22. 2.E: Measurement and Problem Solving (Exercises)
  23. 03: Matter and Energy
  24. 3.01: In Your Room
  25. 3.02: What is Matter
  26. 3.03: Classifying Matter According to Its State- Solid Liquid and Gas
  27. 3.04: Classifying Matter According to Its Composition
  28. 3.05: Differences in Matter- Physical and Chemical Properties
  29. 3.06: Changes in Matter - Physical and Chemical Changes
  30. 3.07: Conservation of Mass - There is No New Matter
  31. 3.08: Energy
  32. 3.09: Energy and Chemical and Physical Change
  33. 3.10: Temperature - Random Motion of Molecules and Atoms
  34. 3.11: Temperature Changes - Heat Capacity
  35. 3.12: Energy and Heat Capacity Calculations
  36. 3.13: Phase Changes
  37. 3.14: What Are Nutrients
  38. 3.15: The Broad Role of Nutritional Science
  39. 3.16: Serving Size
  40. 3.E: Matter and Energy (Exercises)
  41. 3.E: Nutrition and You (Exercises)
  42. 04: Atoms and Elements
  43. 4.01: Cutting Aluminum until you get Atoms
  44. 4.02: Indivisible - The Atomic Theory
  45. 4.03: The Nuclear Atom
  46. 4.04: The Properties of Protons Neutrons and Electrons
  47. 4.05: Elements- Defined by Their Number of Protons
  48. 4.06: Ions - Losing and Gaining Electrons
  49. 4.07: Isotopes - When the Number of Neutrons Varies
  50. 4.08: Atomic Mass - The Average Mass of an Elements Atoms
  51. 4.09: Arrangements of Electrons
  52. 4.10: Looking for Patterns - The Periodic Table
  53. 4.S: Elements Atoms and the Periodic Table (Summary)
  54. 05: Nuclear Chemistry
  55. 5.01: Prelude to Nuclear Chemistry
  56. 5.02: Radioactivity
  57. 5.03: Half-Life
  58. 5.04: Units of Radioactivity
  59. 5.05: Uses of Radioactive Isotopes
  60. 5.06: Nuclear Energy
  61. 5.E: Nuclear Chemistry (Exercises)
  62. 5.S: Nuclear Chemistry (Summary)
  63. 06: Molecules and Compounds
  64. 6.01: Sugar and Salt
  65. 6.02: Compounds Display Constant Composition
  66. 6.03: Chemical Formulas- How to Represent Compounds
  67. 6.04: A Molecular View of Elements and Compounds
  68. 6.05: Writing Formulas for Ionic Compounds
  69. 6.06: Nomenclature- Naming Compounds
  70. 6.07: Naming Ionic Compounds
  71. 6.08: Naming Molecular Compounds
  72. 6.09: Naming Acids
  73. 6.10: Nomenclature Summary
  74. 6.11: Bonding Models and AIDS Drugs
  75. 6.12: Representing Valence Electrons with Dots
  76. 6.13: Lewis Structures of Ionic Compounds- Electrons Transferred
  77. 6.14: Covalent Lewis Structures- Electrons Shared
  78. 6.15: Writing Lewis Structures for Covalent Compounds
  79. 6.16: Resonance - Equivalent Lewis Structures for the Same Molecule
  80. 6.17: Predicting the Shapes of Molecules
  81. 6.18: Electronegativity and Polarity- Why Oil and Water Dont Mix
  82. 07: Stoichiometry
  83. 7.01: Some Types of Chemical Reactions
  84. 7.02: Evidence of a Chemical Reaction
  85. 7.03: Chemical Equations
  86. 7.04: How to Write Balanced Chemical Equations
  87. 7.05: Climate Change - Too Much Carbon Dioxide
  88. 7.06: Stoichiometry
  89. 7.07: Counting Nails by the Pound
  90. 7.08: Counting Atoms by the Gram
  91. 7.09: Counting Molecules by the Gram
  92. 7.10: Chemical Formulas as Conversion Factors
  93. 7.11: Mole-to-Mole Conversions
  94. 7.12: Making Molecules- Mole to Mass (or vice versa) and Mass-to-Mass Conversions
  95. 7.13: Limiting Reactant and Theoretical Yield
  96. 7.14: Limiting Reactant Theoretical Yield and Percent Yield from Initial Masses of Reactants
  97. 7.15: Enthalpy Change is a Measure of the Heat Evolved or Absorbed
  98. 7.16: New Page
  99. 08: Gases
  100. 8.01: Extra-Long Straws
  101. 8.02: Kinetic Molecular Theory- A Model for Gases
  102. 8.03: Pressure- The Result of Constant Molecular Collisions
  103. 8.04: Boyles Law - Pressure and Volume
  104. 8.05: Charless Law- Volume and Temperature
  105. 8.06: Gay-Lussac's Law- Temperature and Pressure
  106. 8.07: The Combined Gas Law- Pressure Volume and Temperature
  107. 8.08: Avogadros Law- Volume and Moles
  108. 8.09: The Ideal Gas Law- Pressure Volume Temperature and Moles
  109. 8.10: Mixtures of Gases - Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen
  110. 09: Solutions
  111. 9.01: Prelude - Tragedy in Cameroon
  112. 9.02: Solutions - Homogeneous Mixtures
  113. 9.03: Solutions of Solids Dissolved in Water- How to Make Rock Candy
  114. 9.04: Solutions of Gases in Water
  115. 9.05: Solution Concentration- Mass Percent
  116. 9.06: Solution Concentration- Molarity
  117. 9.07: Solution Dilution
  118. 9.08: Solution Stoichiometry
  119. 9.09: Freezing Point Depression and Boiling Point Elevation
  120. 9.10: Osmosis
  121. 10: Kinetics and Equilibrium
  122. 10.01: Chemical Reaction Rate
  123. 10.02: Collision Theory
  124. 10.03: Activation Energy
  125. 10.04: Factors Affecting Reaction Rate
  126. 10.05: Catalysts
  127. 10.06: Rate Law and Specific Rate Constant
  128. 10.07: Order of Reaction
  129. 10.08: Rate-Determining Step
  130. 10.09: Chemical Equilibrium
  131. 10.10: Equilibrium Constant
  132. 10.11: Calculations with Equilibrium Constants
  133. 10.12: Le Chatelier's Principle
  134. 10.13: Effect of Concentration
  135. 10.14: Effect of Temperature
  136. 10.15: Effect of Pressure
  137. 10.16: Nonreversible Reactions
  138. 10.17: Le Chatelier's Principle and the Equilibrium Constant
  139. 10.18: Solubility Product Constant (left( K textsp right))
  140. 10.19: Conversion of Solubility to (K textsp)
  141. 10.20: Conversion of (K textsp) to Solubility
  142. 10.21: Predicting Precipitates
  143. 10.22: Common Ion Effect
  144. 11: Acids and Bases
  145. 11.01: Properties of Acids
  146. 11.02: Properties of Bases
  147. 11.03: Arrhenius Acids
  148. 11.04: Arrhenius Bases
  149. 11.05: Brnsted-Lowry Acids and Bases
  150. 11.06: Brnsted-Lowry Acid-Base Reactions
  151. 11.07: Lewis Acids and Bases
  152. 11.08: Ion-Product of Water
  153. 11.09: The pH Scale
  154. 11.10: Calculating pH of Acids and Bases
  155. 11.11: The pOH Concept
  156. 11.12: Strong and Weak Acids and Acid Ionization Constant (left( K texta right))
  157. 11.13: Strong and Weak Bases and Base Ionization Constant
  158. 11.14: Calculating Acid and Base Dissociation Constants
  159. 11.15: Calculating pH of Weak Acid and Base Solutions
  160. 11.16: Neutralization Reaction and Net Ionic Equations for Neutralization Reactions
  161. 11.17: Titration Experiment
  162. 11.18: Titration Calculations
  163. 11.19: Titration Curves
  164. 11.20: Indicators
  165. 11.21: Hydrolysis of Salts - Equations
  166. 11.22: Calculating pH of Salt Solutions
  167. 11.23: Buffers