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UBC Introductory Chemistry

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UBC Introductory Chemistry

Chemistry
Author
Jeanette Leeuwner
Publisher
University of British Columbia
Source
LibreTexts
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 125 sections
  1. 01: Units and Measure
  2. 1.01: Scientific Notation - Writing Large and Small Numbers
  3. 1.02: Significant Figures - Writing Numbers to Reflect Precision
  4. 1.03: Significant Figures in Calculations
  5. 1.04: The Basic Units of Measurement
  6. 1.05: Problem Solving and Unit Conversions
  7. 1.06: Solving Multistep Conversion Problems
  8. 1.07: Units Raised to a Power
  9. 02: Naming and Composition
  10. 2.01: A Molecular View of Elements and Compounds
  11. 2.02: Writing Formulas for Ionic Compounds
  12. 2.03: Nomenclature- Naming Compounds
  13. 2.04: Naming Ionic Compounds
  14. 2.05: Naming Molecular Compounds
  15. 2.06: Naming Acids
  16. 2.07: Nomenclature Summary
  17. 2.08: Formula Mass- The Mass of a Molecule or Formula Unit
  18. 2.09: Counting Atoms by the Gram
  19. 2.10: Counting Molecules by the Gram
  20. 2.11: Chemical Formulas as Conversion Factors
  21. 2.12: Mass Percent Composition of Compounds
  22. 2.13: Mass Percent Composition from a Chemical Formula
  23. 2.14: Calculating Empirical Formulas for Compounds
  24. 2.15: Calculating Molecular Formulas for Compounds
  25. 03: Reactions and Stoichiometry
  26. 3.01: Chemical Equations
  27. 3.02: How to Write Balanced Chemical Equations
  28. 3.03: Stoichiometry
  29. 3.04: Mole-to-Mole Conversions
  30. 3.05: Making Molecules- Mole to Mass (or vice versa) and Mass-to-Mass Conversions
  31. 3.06: Limiting Reactant and Theoretical Yield
  32. 3.07: Limiting Reactant Theoretical Yield and Percent Yield from Initial Masses of Reactants
  33. 3.08: Enthalpy Change is a Measure of the Heat Evolved or Absorbed
  34. 04: Gases
  35. 4.01: Kinetic Molecular Theory- A Model for Gases
  36. 4.02: Pressure- The Result of Constant Molecular Collisions
  37. 4.03: Boyles Law- Pressure and Volume
  38. 4.04: Charless Law- Volume and Temperature
  39. 4.05: Gay-Lussac's Law- Temperature and Pressure
  40. 4.06: The Combined Gas Law- Pressure Volume and Temperature
  41. 4.07: Avogadros Law- Volume and Moles
  42. 4.08: The Ideal Gas Law- Pressure Volume Temperature and Moles
  43. 4.09: Mixtures of Gases - Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen
  44. 05: Solutions
  45. 5.01: Aqueous Solutions and Solubility - Compounds Dissolved in Water
  46. 5.02: Precipitation Reactions
  47. 5.03: Writing Chemical Equations for Reactions in Solution- Molecular Complete Ionic and Net Ionic Equations
  48. 5.04: Solution Concentration- Molarity
  49. 5.05: Solution Dilution
  50. 5.06: Solution Stoichiometry
  51. 06: Atomic Structure and Periodic Trends
  52. 6.01: The Properties of Protons Neutrons and Electrons
  53. 6.02: Elements- Defined by Their Number of Protons
  54. 6.03: Looking for Patterns- The Periodic Table
  55. 6.04: Ions - Losing and Gaining Electrons
  56. 6.05: Isotopes - When the Number of Neutrons Varies
  57. 6.06: Atomic Mass- The Average Mass of an Elements Atoms
  58. 6.07: The Quantum-Mechanical Model- Atoms with Orbitals
  59. 6.08: Quantum-Mechanical Orbitals and Electron Configurations
  60. 6.09: Electron Configurations and the Periodic Table
  61. 6.10: The Explanatory Power of the Quantum-Mechanical Model
  62. 6.11: Periodic Trends- Atomic Size Ionization Energy and Metallic Character
  63. 07: Bonding and Intermolecular Forces
  64. 7.01: Representing Valence Electrons with Dots
  65. 7.02: Lewis Structures of Ionic Compounds- Electrons Transferred
  66. 7.03: Covalent Lewis Structures- Electrons Shared
  67. 7.04: Writing Lewis Structures for Covalent Compounds
  68. 7.05: Resonance - Equivalent Lewis Structures for the Same Molecule
  69. 7.06: Predicting the Shapes of Molecules
  70. 7.07: Electronegativity and Polarity- Why Oil and Water Dont Mix
  71. 7.08: Interactions between Molecules
  72. 7.09: Evaporation and Condensation
  73. 7.10: Melting Freezing and Sublimation
  74. 7.11: Intermolecular Forces- Dispersion DipoleDipole Hydrogen Bonding and Ion-Dipole
  75. 08: Organic Chemistry
  76. 8.01: Drawing Chemical Structures
  77. 8.02: Alkanes- Saturated Hydrocarbons
  78. 8.03: Alkenes and Alkynes
  79. 8.04: Hydrocarbon Reactions
  80. 8.05: Aromatic Hydrocarbons
  81. 8.06: Functional Groups
  82. 8.07: Alcohols
  83. 8.08: Aldehydes and Ketones
  84. 8.09: Carboxylic Acids and Esters
  85. 8.10: Ethers
  86. 8.11: Amines
  87. 8.12: Isomers
  88. 09: Reaction Kinetics
  89. 9.01: Rate of a Chemical Reaction
  90. 9.02: The Rate Law- The Effect of Concentration on Reaction Rate
  91. 9.03: The Integrated Rate Law- The Dependence of Concentration on Time
  92. 9.04: The Effect of Temperature on Reaction Rate
  93. 9.05: Reaction Mechanisms
  94. 9.06: Catalysis
  95. 10: Acids and Bases
  96. 10.01: Acids- Properties and Examples
  97. 10.02: Bases- Properties and Examples
  98. 10.03: Molecular Definitions of Acids and Bases
  99. 10.04: Reactions of Acids and Bases
  100. 10.05: AcidBase Titration
  101. 10.06: Strong and Weak Acids and Acid Ionization Constant (left( K texta right))
  102. 10.07: Strong and Weak Bases and Base Ionization Constant (left( K textb right))
  103. 10.08: Relationship between Ka Kb pKa and pKb
  104. 10.09: Calculating Ka and Kb
  105. 10.10: Water - Acid and Base in One
  106. 10.11: The pH and pOH Scales - Ways to Express Acidity and Basicity
  107. 10.12: Buffers are Solutions that Resist pH Change
  108. 11: Chemical Equilibrium
  109. 11.01: The Concept of Dynamic Equilibrium
  110. 11.02: The Equilibrium Constant (K)
  111. 11.03: Expressing the Equilibrium Constant in Terms of Pressure
  112. 11.04: Calculating the Equilibrium Constant From Measured Equilibrium Concentrations
  113. 11.05: Heterogenous Equilibria - Reactions Involving Solids and Liquids
  114. 11.06: The Reaction Quotient- Predicting the Direction of Change
  115. 11.07: Finding Equilibrium Concentrations
  116. 11.08: Le Chateliers Principle- How a System at Equilibrium Responds to Disturbances
  117. 12: Oxidation and Reduction
  118. 12.01: Oxidation States - Electron Bookkeeping
  119. 12.02: Oxidation and Reduction- Some Definitions
  120. 12.03: Balancing Oxidation-Reduction Equations
  121. 12.04: Voltaic (or Galvanic) Cells- Generating Electricity from Spontaneous Chemical Reactions
  122. 12.05: Standard Reduction Potentials
  123. 12.06: Batteries- Using Chemistry to Generate Electricity
  124. 12.07: Electrolysis- Driving Non-spontaneous Chemical Reactions with Electricity
  125. 12.08: Corrosion- Undesirable Redox Reactions