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CHEM 210 General Chemistry I

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CHEM 210 General Chemistry I

This course is the first half of a two-semester sequence in general chemistry intended for students pursuing majors in physical sciences, biological sciences and engineering. The topics include atomic theory, stoichiometry, chemical bonding, thermochemistry, periodicity, molecular geometry, gas laws, solution stoichiometry, intermolecular forces and selected topics covering redox and acid-base reactions.

Chemistry
Author
Sol Parajon Puenzo
Publisher
Cañada College
Source
LibreTexts
Language
EN
Category
Basic Sciences
Read online Download PDF (open licence)
Contents· 127 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: Expressing Numbers - Scientific Notation
  9. 1.08: The Reliability of a Measurement
  10. 1.09: Solving Chemical Problems
  11. 1.10: Matter Measurement and Problem Solving (Exercises)
  12. 02: Atoms and Elements
  13. 2.01: Brownian Motion - Evidence for Atoms
  14. 2.02: Early Ideas about the Building Blocks of Matter
  15. 2.03: Modern Atomic Theory and the Laws That Led to It
  16. 2.04: The Discovery of the Subatomic Particles
  17. 2.05: The Structure of The Atom
  18. 2.06: Protons Neutrons and Electrons in Atoms
  19. 2.07: Finding Patterns - The Periodic Law and the Periodic Table
  20. 2.08: The Average Mass of an Elements Atoms
  21. 2.09: Molar Mass - Counting Atoms by Weighing Them
  22. 2.10: Atoms and Elements (Exercises)
  23. 03: Molecules Compounds and Chemical Equations
  24. 3.01: Hydrogen Oxygen and Water
  25. 3.02: Representing Compounds- Chemical Formulas and Molecular Models
  26. 3.03: Lewis (Dot) Representation
  27. 3.04: A Molecular View of Elements and Compounds
  28. 3.05: Formation of Ions and Ionic Compounds
  29. 3.06: Ionic Compounds- Formulas and Names
  30. 3.07: Summary of Inorganic Nomenclature
  31. 3.08: Molecular Compounds- Formulas and Names
  32. 3.09: Formula Mass and the Mole Concept
  33. 3.10: Composition of Compounds
  34. 3.11: Determining a Chemical Formula from Experimental Data
  35. 3.12: Organic Compounds
  36. 3.13: Molecules Compounds and Chemical Equations (Exercises)
  37. 04: Chemical Reactions and Quantities
  38. 4.01: Carbon Dioxide and Climate Change
  39. 4.02: Writing and Balancing Chemical Equations
  40. 4.03: Limiting Reactant Theoretical Yield and Percent Yield
  41. 4.04: Reaction Stoichiometry- How Much Carbon Dioxide
  42. 4.05: Examples of Chemical Reaction- Combustion Alkali Metals and Halogens
  43. 4.06: Combustion Reactions
  44. 05: Introduction to Solutions and Aqueous Reactions
  45. 5.01: Prelude to Solutions
  46. 5.02: Solution Concentration and Solution Stoichiomentry
  47. 5.03: Solution Stoichiometry
  48. 5.04: Types of Aqueous Solutions and Solubility
  49. 5.05: Precipitation Reactions
  50. 5.06: Representing Aqueous Reactions- Molecular Ionic and Complete Ionic Equations
  51. 5.07: Acid-Base Reactions
  52. 5.08: Gas Evolution Reactions
  53. 5.09: Oxidation-Reduction Reactions
  54. 06: Gases
  55. 6.01: Water from Wells- Atmospheric Pressure at Work
  56. 6.02: Pressure- The Result of Particle Collisions
  57. 6.03: The Simple Gas Laws- Boyles Law Charless Law and Avogadros Law
  58. 6.04: The Ideal Gas Law
  59. 6.05: Applications of the Ideal Gas Law- Molar Volume Density and Molar Mass of a Gas
  60. 6.06: Mixtures of Gases and Partial Pressures
  61. 6.07: Gases in Chemical Reactions- Stoichiometry Revisited
  62. 6.08: Kinetic Molecular Theory- A Model for Gases
  63. 6.09: Mean Free Path Diffusion and Effusion of Gases
  64. 6.10: Real Gases- The Effects of Size and Intermolecular Forces
  65. 6.11: Gases (Exercises)
  66. 07: Thermochemistry
  67. 7.01: Light the Furnace- The Nature of Energy and Its Transformations
  68. 7.02: The Nature and Types of Energy
  69. 7.03: The First Law of Thermodynamics
  70. 7.04: Quantifying Heat and Work
  71. 7.05: Constant Volume Calorimetry- Measuring U for Chemical Reactions
  72. 7.06: Enthalpy- The Heat Evolved in a Chemical Reaction at Constant Pressure
  73. 7.07: Constant Pressure Calorimetry- Measuring H for Chemical Reactions
  74. 7.08: Relationships Involving Enthalpy of Reactions
  75. 7.09: Enthalpies of Reaction from Standard Heats of Formation
  76. 7.10: Energy Sources and the Environment
  77. 08: The Quantum-Mechanical Model of the Atom
  78. 8.01: Schrodinger's Cat
  79. 8.02: The Nature of Light
  80. 8.03: Atomic Spectroscopy and The Bohr Model
  81. 8.04: The Wavelength Nature of Matter
  82. 8.05: Quantum Mechanics and The Atom
  83. 8.06: The Shape of Atomic Orbitals
  84. 8.07: The Quantum-Mechanical Model of the Atom (Exercises)
  85. 09: Periodic Properties of the Elements
  86. 9.01: Nerve Signal Transmission
  87. 9.02: The Development of the Periodic Table
  88. 9.03: Electron Configurations- How Electrons Occupy Orbitals
  89. 9.04: Electron Configurations Valence Electrons and the Periodic Table
  90. 9.05: The Explanatory Power of the Quantum-Mechanical Model
  91. 9.06: Periodic Trends in the Size of Atoms and Effective Nuclear Charge
  92. 9.07: Ions- Configurations Magnetic Properties Radii and Ionization Energy
  93. 9.08: Electron Affinities and Metallic Character
  94. 9.09: Examples of Periodic Chemical Behavior
  95. 9.10: Periodic Properties of the Elements (Exercises)
  96. 10: Chemical Bonding I- Lewis Structures
  97. 10.01: Models and Funtionality of proteins
  98. 10.02: Types of Chemical Bonds
  99. 10.03: Representing Valance Electrons with Dots
  100. 10.04: Ionic Bonding
  101. 10.05: Covalent Bonding- Lewis Structure
  102. 10.06: Electronegativity and Bond Polarity
  103. 10.07: Lewis Structures
  104. 10.08: Resonance and Formal Charge
  105. 10.09: Exceptions to the Octet Rule
  106. 10.10: Bond Energies and Bond Lengths
  107. 10.11: Bonding in Metals
  108. 10.12: Chemical Bonding I (Exercises)
  109. 11: Chemical Bonding II- Valence Bond Theory and Molecular Orbital Theory
  110. 11.01: Artificial Sweeteners
  111. 11.02: VSEPR Theory - The Five Basic Shapes
  112. 11.03: VSPER Theory- The Effect of Lone Pairs
  113. 11.04: VSPER Theory - Predicting Molecular Geometries
  114. 11.05: Molecular Shape and Polarity
  115. 11.06: Valence Bond Theory- Orbital Overlap as a Chemical Bond
  116. 11.07: Valence Bond Theory- Hybridization of Atomic Orbitals
  117. 11.08: Molecular Orbital Theory- Electron Delocalization
  118. 12: Liquids Solids and Intermolecular Forces
  119. 12.01: Water in Zero Gravity
  120. 12.02: Solids Liquids and Gases- A Molecular Comparison
  121. 12.03: Intermolecular Forces- The Forces that Hold Condensed Phases Together
  122. 12.04: Intermolecular Forces in Action- Surface Tension Viscosity and Capillary Action
  123. 12.05: Vaporization and Vapor Pressure
  124. 12.06: Sublimation and Fusion
  125. 12.07: Heating Curve for Water
  126. 12.08: Phase Diagrams
  127. 12.09: Water - An Extraordinary Substance