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Chem 1A: General Chemistry I

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Chem 1A: General Chemistry I

This course is designed for students who need a rigorous treatment of general chemistry at the freshman-level college or university. This course will focus on topics including but not limited to the fundamental principles of inorganic chemistry; nomenclature of inorganic compounds, chemical formulas, equations, and reactions; stoichiometry; structure of atoms, ions, and molecules and periodic table; oxidation-reduction and acid-base reactions; equilibrium; and gas laws.

Chemistry
Author
Julie Brown
Publisher
Woodland Community College
Source
LibreTexts
License
CC BY-NC-SA
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 118 sections
  1. 01: Matter Measurement and Problem Solving
  2. 1.01: Atoms and Molecules
  3. 1.02: The Scientific Approach to Knowledge
  4. 1.03: The Classification of Matter
  5. 1.04: Physical and Chemical Changes and Properties
  6. 1.05: Energy- A Fundamental Part of Physical and Chemical Change
  7. 1.06: The Units of Measurement
  8. 1.07: The Reliability of a Measurement
  9. 1.08: Solving Chemical Problems
  10. 1.E: Matter Measurement and Problem Solving (Exercises)
  11. 02: Atoms and Elements
  12. 2.01: Brownian Motion- Evidence for Atoms
  13. 2.02: Early Ideas about the Building Blocks of Matter
  14. 2.03: Modern Atomic Theory and the Laws That Led to It
  15. 2.04: The Discovery of the Electron
  16. 2.05: 2.5 The Structure of The Atom
  17. 2.06: 2.6 Subatomic Particles- Protons Neutrons and Electrons in Atoms
  18. 2.07: 2.7 Finding Patterns- The Periodic Law and the Periodic Table
  19. 2.08: 2.8 Atomic Mass- The Average Mass of an Elements Atoms
  20. 2.09: 2.9 Molar Mass- Counting Atoms by Weighing Them
  21. 2.10: 2.E - Atoms and Elements (Exercises)
  22. 03: Molecules Compounds and Chemical Equations
  23. 3.01: Hydrogen Oxygen and Water
  24. 3.02: Chemical Bonds
  25. 3.03: Representing Compounds- Chemical Formulas and Molecular Models
  26. 3.04: An Atomic-Level Perspective of Elements and Compounds
  27. 3.05: Ionic Compounds- Formulas and Names
  28. 3.06: Molecular Compounds- Formulas and Names
  29. 3.07: Summary of Inorganic Nomenclature
  30. 3.08: Composition of Compounds
  31. 3.09: Determining a Chemical Formula from Experimental Data
  32. 3.10: Writing and Balancing Chemical Equations
  33. 3.11: Organic Compounds
  34. 3.E: Molecules Compounds and Chemical Equations (Exercises)
  35. 04: Chemical Reactions and Aqueous Reactions
  36. 4.01: Global Warming and the Combustion of Fossil Fuels
  37. 4.02: 4.2 Reaction Stoichiometry- How Much Carbon Dioxide
  38. 4.03: 4.3 Limiting Reactant Theoretical Yield and Percent Yield
  39. 4.04: Solution Concentration and Solution Stoichiomentry
  40. 4.05: Types of Aqueous Solutions and Solubility
  41. 4.06: Precipitation Reactions
  42. 4.07: Representing Aqueous Reactions- Molecular Ionic and Complete Ionic Equations
  43. 4.08: Acid-Base and Gas-Evolution Reactions
  44. 4.09: Oxidation-Reduction Reactions
  45. 05: Gases
  46. 5.01: Water from Wells- Atmospheric Pressure at Work
  47. 5.02: Pressure- The Result of Particle Collisions
  48. 5.03: The Simple Gas Laws- Boyles Law Charless Law and Avogadros Law
  49. 5.04: The Ideal Gas Law
  50. 5.05: Applications of the Ideal Gas Law- Molar Volume Density and Molar Mass of a Gas
  51. 5.06: Mixtures of Gases and Partial Pressures
  52. 5.07: Gases in Chemical Reactions- Stoichiometry Revisited
  53. 5.08: Kinetic Molecular Theory- A Model for Gases
  54. 5.09: Mean Free Path Diffusion and Effusion of Gases
  55. 5.10: Real Gases- The Effects of Size and Intermolecular Forces
  56. 5.E: Gases (Exercises)
  57. 06: Thermochemistry
  58. 6.01: Light the Furnace- The Nature of Energy and Its Transformations
  59. 6.02: The First Law of Thermodynamics
  60. 6.03: The Nature of Energy
  61. 6.04: Quantifying Heat and Work
  62. 6.05: Constant Volume Calorimetry- Measuring U for Chemical Reactions
  63. 6.06: Enthalpy- The Heat Evolved in a Chemical Reaction at Constant Pressure
  64. 6.07: Constant Pressure Calorimetry- Measuring H for Chemical Reactions
  65. 6.08: Relationships Involving Enthalpy of Reactions
  66. 6.09: Enthalpies of Reaction from Standard Heats of Formation
  67. 6.10: Energy Use and The Environment
  68. 07: The Quantum-Mechanical Model of the Atom
  69. 7.01: Schrodinger's Cat
  70. 7.02: The Nature of Light
  71. 7.03: Atomic Spectroscopy and The Bohr Model
  72. 7.04: The Wavelength Nature of Matter
  73. 7.05: Quantum Mechanics and The Atom
  74. 7.06: The Shape of Atomic Orbitals
  75. 7.E: The Quantum-Mechanical Model of the Atom (Exercises)
  76. 08: Periodic Properties of the Elements
  77. 8.01: Nerve Signal Transmission
  78. 8.02: The Development of the Periodic Table
  79. 8.03: Electron Configurations- How Electrons Occupy Orbitals
  80. 8.04: Electron Configurations Valence Electrons and the Periodic Table
  81. 8.05: The Explanatory Power of the Quantum-Mechanical Model
  82. 8.06: Periodic Trends in the Size of Atoms and Effective Nuclear Charge
  83. 8.07: Ions- Configurations Magnetic Properties Radii and Ionization Energy
  84. 8.08: Electron Affinities and Metallic Character
  85. 8.09: Examples of Periodic Chemical Behavior
  86. 8.E: Periodic Properties of the Elements (Exercises)
  87. 09: Chemical Bonding I- Lewis Structures and Determining Molecular Shapes
  88. 9.01: Bonding Models and AIDS Drugs
  89. 9.02: Types of Chemical Bonds
  90. 9.03: Representing Valance Electrons with Dots
  91. 9.04: Ionic Bonding
  92. 9.05: Covalent Bonding- Lewis Structure
  93. 9.06: Electronegativity and Bond Polarity
  94. 9.07: Lewis Structures
  95. 9.08: Resonance and Formal Charge
  96. 9.09: Exceptions to the Octet Rule
  97. 9.10: Bond Energies and Bond Lengths
  98. 9.11: Bonding in Metals
  99. 9.E: Chemical Bonding I (Exercises)
  100. 10: Chemical Bonding II- Valance Bond Theory and Molecular Orbital Theory
  101. 10.01: Artificial Sweeteners
  102. 10.02: VSEPR Theory- The Five Basic Shapes
  103. 10.03: VSPER Theory- The Effect of Lone Pairs
  104. 10.04: VSPER Theory- Predicting Molecular Geometries
  105. 10.05: Molecular Shape and Polarity
  106. 10.06: Valence Bond Theory- Orbital Overlap as a Chemical Bond
  107. 10.07: Valence Bond Theory- Hybridization of Atomic Orbitals
  108. 10.08: Molecular Orbital Theory- Electron Delocalization
  109. 11: Chemical Equilibrium
  110. 11.01: Fetal Hemoglobin and Equilibrium
  111. 11.02: The Concept of Dynamic Equilibrium
  112. 11.03: The Equilibrium Constant (K)
  113. 11.04: Expressing the Equilibrium Constant in Terms of Pressure
  114. 11.05: Calculating the Equilibrium Constant From Measured Equilibrium Concentrations
  115. 11.06: Heterogenous Equilibria- Reactions Involving Solids and Liquids
  116. 11.07: The Reaction Quotient- Predicting the Direction of Change
  117. 11.08: Finding Equilibrium Concentrations
  118. 11.09: Le Chateliers Principle- How a System at Equilibrium Responds to Disturbances