Chapter 2 Lecture Outline

Atomic Structure - Protons, Electrons, and Neutrons

  1. Democritus
  2. John Dalton; Atoms, Elements, and Compounds
  3. Lavoisier, Law of Conservation of Matter
  4. Proust, Law of Constant Composition or Law of Definit Proportions
  5. Atomic Model (video)
  6. Electricity (video)
  7. Radioactivity (video)
  8. The electron
    1. JJ Thompson (figure 2.4, and 2.5) Cathode Ray Tube (video)
    2. Millikan (figure 2.6) Oil Drop Experiment (video)
  9. Protons
  10. Neutrons (Chadwick)
  11. Rutherford, the Nucleus of the Atom (video)

Atomic Number and Atomic Mass

Subatomic Particles
Particle Charge Mass Symbol Significance
Proton +1 1 u  11p Atomic Number
Neutron 0 1 u 10n # neutron + # proton = isotope mass
Electron -1 0 u (0.0005485799 u) 0-1e charge of atom

Isotopes (protons, neutrons, electrons)

  1. Video
  2. Mass Spectrometry (overhead)
  3. High Resolution Mass Spectrometer
  4. Number of protons, neutrons, and electrons in examples

Atomic Weight (Periodic Table)

The Periodic Table

  1. Example of Periodic Trends, Alkali Metals reacting with water (The Chemistry Set CD-ROM)
    1. Lithium in Water (video clip)
    2. Sodium in Water (video clip)
    3. Potassium in Water (video clip)
    4. Rubidium in Water (video clip)
    5. Cesium in Water (video clip)

  2. Basic Outline
    1. Groups
    2. Periods
    3. Arrangement of Elements
    4. Reactivity

  3. Names of Regions
    1. Metals and Non-Metals
    2. Alkali Metals
    3. Alkaline Earth Metals
    4. Halogens
    5. Nobel Gas
    6. Main Group
    7. Transition Metals
    8. Inner Transition Metals
    9. Diatomic
    10. Metals/Non-Metals

  4. Properties of Groups and Periods
    1. Reactivity
    2. Physical Properties
    3. Oxide Formulas
    4. Hydrogen Formulas

  5. Electronic Basis for Similarity

Molecules, Compounds, and Formulas

  1. What is a molecule
  2. Molecular formulas
  3. Elements as Molecules
    1. Hydrogen Internet ©Saunders 1997)
    2. Carbon ( Internet ©Saunders 1997)
    3. Nitrogen ( Internet ©Saunders 1997)
    4. Oxygen ( Internet ©Saunders 1997)
    5. Fluorine ( Internet ©Saunders 1997)
    6. Phosphorous ( Internet ©Saunders 1997)
    7. Sulfur ( Internet ©Saunders 1997)
    8. Chlorine ( Internet ©Saunders 1997)
    9. Bromine ( Internet ©Saunders 1997)
    10. Iodine ( Internet ©Saunders 1997)

Ionic Compounds: Formulas, Names, and Properties

  1. Ionic Compounds
    1. Reaction of Na (s) and Cl2 (g)
      1. Video( Internet © Saunders 1997)
      2. Animation( Internet © Saunders 1997)

    2. Molten Salt Conducts ( Internet © Saunders 1997)

    3. Cleave KBr crystal ( Internet © Saunders 1997)

    4. Solvation of KMNO4
      1. Video( Internet © Saunders 1997)
      2. Animation( Internet © Saunders 1997)

  2. Charge of Ions from Periodic Table (Figure 3.7, page 87)

  3. Polyatomic Ions (Table 3.1, page 89)

  4. Chemical Nomenclature Handout

Molecular Compounds: Forumlas, Names, and Properties

  1. Formulas
    1. Molecular Formula
    2. Condensed Structural Formula
    3. Expanded Structural Formula
    4. Stereo Projection (Wedge)
    5. Molecular Model (Computer)

  2. Representing Compounds as above
    1. CO2 (*.pdb, CO2animations)
    2. Ethanol, CH3CH2OH (*.pdb )
    3. Caffeine, C8H10N4O2 (*.pdb)

  3. Chemical Nomenclature Handout

Adoms, Molecules, and the Mole

  1. The mole as a counting unit
    1. Definition of the mole
    2. 1 C-12 atom mass 12 u (unified atomic mass units)
    3. 1 mole C-12 mass 12 g
    4. 1 mole = 6.022136736 x 1023 items
    5. u atom-1 = g mole-1
  2. Avogadro's Number
  3. mole, mass, and quantity conversions

  1. Lecture Problems

Describing Compound Formulas

  1. Lecture Problems

Hydrated Compounds

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Widener University
Chester, PA 19013

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Last Updated Friday, May 25, 2001 1:59:43 PM