Chapter 7 Lecture Outline

The Pauli Exclusion Principle

  1. Periodic Table

  2. Energy Level Diagram

  3. Quantum Numbers

    Principal Quantum Number n 1, 2, 3, 4 ... Shell Row of Periodicc Table
    Angular Momentum l 0, 1, 2.. n-1 Orbital Shape (or type)_(t Block of table (s, p, d, f)
    Magnetic ml -l... +l Orbital Direction Which s, p, d, or f orbital
    Spin ms +1/2 or -1/2 Electron Spin

  4. Orbital Box Diagram

  5. Spectroscopic Notation (ie: [Ne] 3s2 3p4

Atomic Subshell Energies and Electron Assignments

  1. n + l order

  2. n vs. l table with diagonals

  3. periodic table
    1. s = row
    2. p = row
    3. d = row -1
    4. f = row -2

Electron Configurations of the Atoms

See Table 7.3 on page 310
  1. Lithium
  2. Oxygen
  3. Scandium
  4. Chromium
  5. Copper
  6. Zinc
  7. Lanthanum ([Xe] 5d1 6s2)
  8. Cerium ([Xe] 4f1 5d1 6s2)
  9. Praseodynium ([Xe] 4f3 6s2)

Electron Configurations of Ions

  1. Lithium
  2. Oxygen
  3. Copper (II)
  4. Copper (III)

Atomic Properties and Periodic Trends

  1. Atomic Size (Overhead)

  2. Ion Size (Overhead)

  3. Ionization Energy (Overhead)
    1. Mg -> Mg1+ ( Internet © Saunders, 1997)
    2. Mg1+ -> Mg2+( Internet © Saunders, 1997)
    3. Mg2+ -> Mg3+( Internet © Saunders, 1997)
    4. Review Common Monoatomic Ions (Figure 3.10, p 115):

  4. Electron Affinity (Overhead) ( Internet © Saunders, 1997)

Periodic Trends and Chemical Properties

  1. Na (s) + 1/2 Cl2 (g) -> NaCl (s) ( Internet © Saunders, 1997)

  2. 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)

  3. Energy of Ion Pair Formation

  4. Lattice Energy

  5. Forming Ionic Solids ( Internet © Saunders, 1997)
  6. Formation of LiF using Thermodynamics Data
    Reaction [delta]H (kJ/mole)
    Li (s) -> Li(g) 159.4
    1/2 F2 (g) > F (g) 79.5
    Li (g) -> Li1+ (g) + 1 e- 5.39172 eV
    (1 eV = 96.485 kJ/mole)
    F (g) + e- -> F1- (g) -328
    Li (s) + 1/2 F2 (g) -> LiF (g) -332.6
    Li (s) + 1/2 F2 (g) -> LiF (s) -616.9

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