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CHEM 1020 - General Chemistry I

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CHEM 1020 - General Chemistry I

Chemistry
Author
Budhi
Publisher
Eastern Wyoming College
Source
LibreTexts
License
CC BY-NC-SA
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 107 sections
  1. 01: Matter Measurement and Problem Solving
  2. 1.1: Atoms and Molecules
  3. 1.2: The Scientific Approach to Knowledge
  4. 1.3: The Classification of Matter
  5. 1.4: Physical and Chemical Changes and Properties
  6. 1.5: Energy: A Fundamental Part of Physical and Chemical Change
  7. 1.6: The Units of Measurement
  8. 1.7: The Reliability of a Measurement
  9. 1.8: Solving Chemical Problems
  10. 1.9: 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: Protons, Neutrons, and Electrons in Atoms
  18. 2.07: Finding Patterns - The Periodic Law and the Periodic Table
  19. 2.08: The Average Mass of an Element’s Atoms
  20. 2.09: Molar Mass - Counting Atoms by Weighing Them
  21. 2.10: 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. 3.12: Molecules, Compounds and Chemical Equations (Exercises)
  35. 04: Chemical Reactions and Aqueous Reactions
  36. 4.1: Global Warming and the Combustion of Fossil Fuels
  37. 4.2: How Much Carbon Dioxide?
  38. 4.3: 4.3 Limiting Reactant, Theoretical Yield, and Percent Yield
  39. 4.4: Solution Concentration and Solution Stoichiomentry
  40. 4.5: Types of Aqueous Solutions and Solubility
  41. 4.6: Precipitation Reactions
  42. 4.7: Representing Aqueous Reactions: Molecular, Ionic, and Complete Ionic Equations
  43. 4.8: Acid-Base and Gas-Evolution Reactions
  44. 4.9: 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: Boyle’s Law, Charles’s Law and Avogadro’s 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. 5.11: Gases (Exercises)
  57. 06: The Quantum-Mechanical Model of the Atom
  58. 6.1: Schrödinger's Cat
  59. 6.2: The Nature of Light
  60. 6.3: Atomic Spectroscopy and The Bohr Model
  61. 6.4: The Wavelength Nature of Matter
  62. 6.5: Quantum Mechanics and The Atom
  63. 6.6: The Shape of Atomic Orbitals
  64. 6.7: The Quantum-Mechanical Model of the Atom (Exercises)
  65. 07: Periodic Properties of the Elements
  66. 7.01: Nerve Signal Transmission
  67. 7.02: The Development of the Periodic Table
  68. 7.03: Electron Configurations: How Electrons Occupy Orbitals
  69. 7.04: Electron Configurations, Valence Electrons, and the Periodic Table
  70. 7.05: The Explanatory Power of the Quantum-Mechanical Model
  71. 7.06: Periodic Trends in the Size of Atoms and Effective Nuclear Charge
  72. 7.07: Ions- Configurations, Magnetic Properties, Radii, and Ionization Energy
  73. 7.08: Electron Affinities and Metallic Character
  74. 7.09: Examples of Periodic Chemical Behavior
  75. 7.10: Periodic Properties of the Elements (Exercises)
  76. 08: Chemical Bonding I: Lewis Structures
  77. 8.01: Bonding Models and AIDS Drugs
  78. 8.02: Types of Chemical Bonds
  79. 8.03: Representing Valance Electrons with Dots
  80. 8.04: Ionic Bonding
  81. 8.05: Covalent Bonding: Lewis Structure
  82. 8.06: Electronegativity and Bond Polarity
  83. 8.07: Lewis Structures
  84. 8.08: Resonance and Formal Charge
  85. 8.09: Exceptions to the Octet Rule
  86. 8.10: Bond Energies and Bond Lengths
  87. 8.11: Bonding in Metals
  88. 8.12: Chemical Bonding I (Exercises)
  89. 09: Chemical Bonding II: Valance Bond Theory and Molecular Orbital Theory
  90. 9.1: Artificial Sweeteners
  91. 9.2: VSEPR Theory - The Five Basic Shapes
  92. 9.3: VSPER Theory: The Effect of Lone Pairs
  93. 9.4: VSPER Theory - Predicting Molecular Geometries
  94. 9.5: Molecular Shape and Polarity
  95. 9.6: Valence Bond Theory: Orbital Overlap as a Chemical Bond
  96. 9.7: Valence Bond Theory: Hybridization of Atomic Orbitals
  97. 9.8: Molecular Orbital Theory: Electron Delocalization
  98. 10: Liquids Solids and Intermolecular Forces
  99. 10.1: Water in Zero Gravity
  100. 10.2: Solids, Liquids, and Gases: A Molecular Comparison
  101. 10.3: Intermolecular Forces: The Forces that Hold Condensed Phases Together
  102. 10.4: Intermolecular Forces in Action: Surface Tension, Viscosity, and Capillary Action
  103. 10.5: Vaporization and Vapor Pressure
  104. 10.6: Sublimation and Fusion
  105. 10.7: Heating Curve for Water
  106. 10.8: Phase Diagrams
  107. 10.9: Water - An Extraordinary Substance