Fall 2007 Cumulative Outline

(This will slide around abit as the semester proceeds to accommodate shifts in emphasis. After each lecture, the "Lecture X" hyperlink will connect to that lecture's slide collection. Previews may be found via the "Main Index" under "Preview". When lecture material has corresponding text material, the Chapter and possible Section are indicated in [green]. Be aware that parts of the outline may have no corresponding reading in the text. (For example, in Lecture 2, Cannizzaro's Stochiometric Analyses does not get mentioned in the reading.)

Lecture 1. History [Chapter 1]

• The first 2000 years
• Stoichiometry Laws

• • Conservation of Mass
  • Law of Definite Proportions
  • Law of Multiple Proportions

• Law of Multiple Proportions illustrated

Lecture 2. History [Chapter 1]

• Dalton's Postulates and Atomic Theory
• Dalton's "Postulate of Simplicity"
• Law of Combining Volumes
• Avogadro's Law
• Cannizzaro's Stoichiometric Analyses
• Early recognition of "Periodicity"
  

Energies [Chapter 4]

• Kinetic energy
• Potential energy (and forces)
• Internal energies (rotation and vibration)
• Light
• H-atom line spectra (emission and absorbtion)

Lecture 3.

Problems with some results of physical measurements [Chapter 4]

• Line spectra
• Photoelectric Effect
• Blackbody Radiation (and the ultraviolet catastrophe)

Physics puzzles "solved" by quantization [Chapter 4]

• Blackbody radiation, Planck, E=hv, energy jumps
• Photoelectric Effect, Einstein, the photon
• Line spectra, Bohr's Planetary Model, quantized angular momentum

Lecture 4. (Old Quantum Theory)

Physics puzzles "solved" by quantization (continued)

• Line spectra, Bohr's Planetary Model, quantized angular momentum [Section 4.3]

• • discrete orbit radii
  • quantized energy states
  • absorbtion and emission photons between states

(New Quantum Theory)

• deBroglie and wave-particle duality of matter
• Schrodinger wave equation (concept), amplitude squared = local probability densities

Particle-in-a-box model [Section 4..6]

Lecture 5.

Wave Nature of Matter

• Particle-in-a-box

• one dimension
• two dimenstions
  three dimensions

• Schrodinger's Wave Equation applied to the hydrogen atom [4.5, 5.1]
  
  • n, principal quantum number
  • l, angular momentum or shape quantum number
  • m_l, magnetic or orientation quantum number

• Electron "spin"[5.1]
  • m_s, spin quantum number

Energies and geometries [5.1]

Lecture 6. More outcomes of wave-particle duality

• (Heisenberg's) Uncertainty Principle [4.4]

• • simultaneous precise measurements restrictions
  • paths or orbits of particles are not legitimate topics of discussion

• Radial density distributions and electron density plots

• • screening and penetration of electrons in the same shell

Many-electron systems

• (Pauli) Exclusion Principle [5.3]

Lecture 7. Many-electron systems

• (Pauli) Exclusion Principle
• Effective nuclear charge
• Photoelectron spectra of atoms
• Electron configuration
• Hund's rules for most stable configurations
• paramagnetism

Lecture 8. The Periodic Table (continued)

• Electron configurations (exceptions)
• Sizes
• Isoelectronic species
• Transition metal ions

Lecture 9. Review for Exam I

Lecture 10. Electron Configurations (continued)

• Second and third ionization energies
• Electron Affinity
• Valence electrons and electron dot structures in atoms

Lecture 11.

Electronegativity

Molecular Structure

• Lewis Structures
• Valence electrons (Main groups)
  Octet Rule

Lecture 12. Molecular Structure

Lewis Structures

• Structural isomers
• Formal charge and preferred structures

Exceptions to the Octet Rule

• Incomplete octets

Lecture 13. Molecular Structure

Exceptions to the Octet Rule

• Odd electron numbers
• Expanded octets (hypervalency)

Resonance (Benzene puzzles)

Resonance

• Equivalent preferred contributors
• Bond order

Lecture 14. Lewis structures

• Examples
• More on resonance and bond orders
• Reaction Heats

Dipole moments and partial ionic character

Lecture 15.

Line Structures

Acid strengths and pK's

• Binary Acids
• Oxoacids

Lecture 16. Molecular structure and acid strength

Oxoacids (continued)

• Resonance stabilization
• Importance of Lewis structure
• Carboxylic acids

Molecular Geometries

VSEPR Model

• Steric number (and coordination number)
• Electronic geometries
• (Ideal) Molecular geometries

Lecture 17. Molecular Geometries

VSEPR Model

Central atom with lone pairs

Distortions from ideal geometries

• effect of lone pairs vs bonding pairs
• effect of multiple bonds

• effect of lone single electrons

Lecture 18. Review for Exam II

Lecture 19. Molecular Geometries

• Effect of electronegativity differences
• Rigidity about double bond
• Molecular dipoles from "bond" dipoles
• Geometrical isomers

Lecture 20.

Molecular geometry

Restricted vs free rotation about bonds

Quantum Theory of the Chemical Bond

Molecular orbitals (in "homonuclear diatomic molecules")

• Approximated by combinations of atomic orbitals
• Constructive and destructive interference effects
• Combining 1s atomic orbitals

Lecture 21.

Quantum Theory of the Chemical Bond

Molecular orbitals (in "homonuclear diatomic molecules")

• "Sigma" bonding molecular orbital
• "Sigma" antibonding molecular orbital

• Bond order and properties
• Combining 2s atomic orbitals

• • "Sigma" bonding molecular orbital
  • "Sigma" antibonding molecular orbital

• Combining 2p atomic orbitals

• • "Sigma" bonding molecular orbital
  • "Sigma" antibonding molecular orbital
  • "Pi" bonding molecular orbitals
  • "Pi" antibonding molecular orbitals

• Building up electron configurations

Lecture 22. Molecular Orbitals

• Building up electron configurations
• Importance of energy match vs mismatch
• Importance of net overlap
• Heteronuclear diatomic molecules

Lecture 23. Quantum Theory of the Chemical Bond

Molecular Orbitals

• Polyatomic molecules
• Hybrid atomic orbitals

Lecture 24. Quantum Theory of the Chemical Bond

Molecular Orbitals in Polyatomic Molecules

• Molecular orbitals from combinations of hybrid atomic orbitals

The rigid double bond

The freely rotating single sigma bond

Strained bonds

Delocalized bonding

Lecture 25. Molecular orbitals (delocalized)

1,3 butadiene example

Orbitals delocalized over more than two atoms

Bond order determination from electron configuration

Partial bond order per electron

Review for Exam III (start)

Lecture 26. Review for Exam III (complete)

Lecture 27.

Delocalized molecular orbitals

• excited states of 1,3 butadiene
• benzene
• ozone
• Carbon dioxide
• Energies via particle-in-a-box
• Light-induced transitions

Lecture 28.

Delocalized Molecular Orbitals (continued)

Metallic bonds

Lecture 29. Intermolecular Interactions

• Ideal Gases
• Real Gases

• • Excluded volume
  • Intermolecular attractions

Lecture 30. Intermolecular Interactions (condensed phases)

• Induced dipoles
  • Polarizability
• Van der Waals interactions
  • Permanent dipoles
  • Temporary (induced) dipoles
  • Boiling points, melting points, densities
    • Effects of size
    • Effects of shape

Lecture 31. Intermolecular Interactions

• Liquids and Solids
  • Hydrogen Bonding
• Molecular Basis of Solubility

Lecture 32. Oxidation numbers

Transition Metal Chemistry

• Tramsition metal ion electron configurations
• Coordination complexes
• Isomers

Lecture 33. Transition metal complexes

• Structural Isomers
• Stereoisomers

• • Geometrical isomers
  • Square planar geometries
  • Octahedral geometries
  • Optical isomers

• Observations to explain
  • Colors
  • Magnetic Properties
  • Stability
• Crystal Field Theory

Lecture 34.

Transition Metal Complexes

Crystal Field theory (Octahedral geometry)

• Weak field vs strong field
• Spectrochemical series

Square planar and tetrahedral geometries

Lecture 35. Transition Metal Complexes

Bond formation

Lecture 36. Ionic radii

Hemoglobin