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Chemistry 305:Introduction to Chemistry

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Chemistry 305:Introduction to Chemistry

Chemistry
Author
Caitlin Zumalt
Publisher
American River College
Source
LibreTexts
License
CC BY-SA
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 111 sections
  1. 01: Unit 1
  2. 1.01: The Scope of Chemistry
  3. 1.02: The Scientific Method - How Chemists Think
  4. 1.03: Hypothesis Theories and Laws
  5. 1.04: Taking Measurements
  6. 1.05: The Basic Units of Measurement
  7. 1.06: Units Raised to a Power
  8. 1.07: Scientific Notation - Writing Large and Small Numbers
  9. 1.08: Significant Figures - Writing Numbers to Reflect Precision
  10. 1.09: Significant Figures in Calculations
  11. 1.10: Problem Solving and Unit Conversions
  12. 1.11: Solving Multi-step Conversion Problems
  13. 1.12: Density
  14. 1.13: Temperature - Random Motion of Molecules and Atoms
  15. 1.E: Measurement and Problem Solving (Exercises)
  16. 02: Unit 2
  17. 2.01: In Your Room
  18. 2.02: What is Matter
  19. 2.03: Classifying Matter According to Its StateSolid Liquid and Gas
  20. 2.04: Classifying Matter According to Its Composition
  21. 2.05: Differences in Matter- Physical and Chemical Properties
  22. 2.06: Changes in Matter - Physical and Chemical Changes
  23. 2.07: Conservation of Mass - There is No New Matter
  24. 2.08: Cutting Aluminum until you get Atoms
  25. 2.09: Indivisible - The Atomic Theory
  26. 2.10: The Nuclear Atom
  27. 2.11: The Properties of Protons Neutrons and Electrons
  28. 2.12: Elements- Defined by Their Number of Protons
  29. 2.13: Looking for Patterns - The Periodic Table
  30. 2.14: Ions - Losing and Gaining Electrons
  31. 2.15: Isotopes - When the Number of Neutrons Varies
  32. 2.16: Atomic Mass - The Average Mass of an Elements Atoms
  33. 2.17: Sugar and Salt
  34. 2.18: Compounds Display Constant Composition
  35. 2.19: Chemical Formulas - How to Represent Compounds
  36. 2.20: A Molecular View of Elements and Compounds
  37. 2.21: Writing Formulas for Ionic Compounds
  38. 2.22: Nomenclature- Naming Compounds
  39. 2.23: Naming Ionic Compounds
  40. 2.24: Naming Molecular Compounds
  41. 2.25: Naming Acids
  42. 2.26: Nomenclature Summary
  43. 03: Unit 3
  44. 3.01: Evidence of a Chemical Reaction
  45. 3.02: The Chemical Equation
  46. 3.03: How to Write Balanced Chemical Equations
  47. 3.04: Classifying Chemical Reactions
  48. 3.05: Aqueous Solutions and Solubility - Compounds Dissolved in Water
  49. 3.06: Precipitation Reactions
  50. 3.07: Writing Chemical Equations for Reactions in Solution- Molecular Complete Ionic and Net Ionic Equations
  51. 3.08: Prelude to Chemical Composition - How Much Sodium
  52. 3.09: Counting Nails by the Pound
  53. 3.10: Counting Atoms by the Gram
  54. 3.11: Counting Molecules by the Gram
  55. 3.12: Chemical Formulas as Conversion Factors
  56. 3.13: Mass Percent Composition of Compounds
  57. 3.14: Mass Percent Composition from a Chemical Formula
  58. 3.15: Calculating Empirical Formulas for Compounds
  59. 3.16: Calculating Molecular Formulas for Compounds
  60. 3.17: Making Pancakes- Relationships Between Ingredients
  61. 3.18: Making Molecules- Mole-to-Mole Conversions
  62. 3.19: Making Molecules- Mass-to-Mass Conversions
  63. 3.20: Stoichiometry
  64. 3.21: Limiting Reactant and Theoretical Yield
  65. 3.22: Limiting Reactant Theoretical Yield and Percent Yield from Initial Masses of Reactants
  66. 04: Unit 4
  67. 4.01: The Bohr Model - Atoms with Orbits
  68. 4.02: Quantum-Mechanical Orbitals and Electron Configurations
  69. 4.03: Electron Configurations and the Periodic Table
  70. 4.04: The Explanatory Power of the Quantum-Mechanical Model
  71. 4.05: Representing Valence Electrons with Dots
  72. 4.06: Lewis Structures of Ionic Compounds- Electrons Transferred
  73. 4.07: Covalent Lewis Structures- Electrons Shared
  74. 4.08: Writing Lewis Structures for Covalent Compounds
  75. 4.09: Resonance - Equivalent Lewis Structures for the Same Molecule
  76. 4.10: Predicting the Shapes of Molecules
  77. 4.11: Electronegativity and Polarity - Why Oil and Water Do not Mix
  78. 4.12: Kinetic Molecular Theory- A Model for Gases
  79. 4.13: Pressure - The Result of Constant Molecular Collisions
  80. 4.14: Boyles Law - Pressure and Volume
  81. 4.15: Charless Law- Volume and Temperature
  82. 4.16: Gay-Lussac's Law- Temperature and Pressure
  83. 4.17: The Combined Gas Law- Pressure Volume and Temperature
  84. 4.18: The Ideal Gas Law- Pressure Volume Temperature and Moles
  85. 4.19: Mixtures of Gases - Why Deep-Sea Divers Breathe a Mixture of Helium and Oxygen
  86. 05: Unit 5
  87. 5.01: Intermolecular Forces- Dispersion DipoleDipole Hydrogen Bonding and Ion-Dipole
  88. 5.02: Solutions - Homogeneous Mixtures
  89. 5.03: Solutions of Solids Dissolved in Water- How to Make Rock Candy
  90. 5.04: Specifying Solution Concentration- Mass Percent
  91. 5.05: Specifying Solution Concentration- Molarity
  92. 5.06: Solution Stoichiometry
  93. 5.07: Sour Patch Kids and International Spy Movies
  94. 5.08: Acids- Properties and Examples
  95. 5.09: Bases- Properties and Examples
  96. 5.10: Molecular Definitions of Acids and Bases
  97. 5.11: Reactions of Acids and Bases
  98. 5.12: AcidBase Titration
  99. 5.13: Strong and Weak Acids and Bases
  100. 5.14: Water - Acid and Base in One
  101. 5.15: The pH and pOH Scales - Ways to Express Acidity and Basicity
  102. 5.16: Carbon - A Versitile Atom
  103. 5.17: Hydrocarbons- Compounds Containing Only Carbon and Hydrocarbon
  104. 5.18: Alkanes- Saturated Hydrocarbons
  105. 5.19: Isomers- Same Formula Different Structure
  106. 5.20: Naming Alkanes
  107. 5.21: Alkenes and Alkynes
  108. 5.22: Functional Groups
  109. 5.23: Carbohydrates
  110. 5.24: Lipids
  111. 5.25: Proteins