Fall 2008 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 Slides 1. History [Chapter 2]

• The first 2000 years
• Stoichiometry Laws

·        

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

• Law of Multiple Proportions illustrated
• Dalton's Postulates and Atomic Theory
• Dalton's "Postulate of Simplicity"

Lecture Slides 2. History

• Law of Combining Volumes
• Avogadro's Law [p. 188]
• Cannizzaro's Stoichiometric Analyses
• Early recognition of "Periodicity"

Energies [Chapter 8]

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

Lecture Slides 3.

Problems with some results of physical measurements [Chapter 8]

• 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

(Old Quantum Theory)

Physics puzzles "solved" by quantization (continued)
Line spectra, Bohr's Planetary Model, quantized angular momentum [Section 8.4]

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

Lecture Slides 4. (Old Quantum Theory)

(New Quantum Theory)

• deBroglie and wave-particle duality of matter (Section 8.5)

Wave Nature of Matter

• Particle-in-a-box

• one dimension
• two dimenstions
• three dimensions
• Schrodinger wave equation (concept), amplitude squared = local probability densities (Section 8.6)

• Schrodinger's Wave Equation applied to the hydrogen atom [Section 8.7]
• • n, principal quantum number
  • l, angular momentum or shape quantum number
  • m_l, magnetic or orientation quantum number

Lecture Slides 5.

• Electron "spin"[Section 8.9]
• • m_s, spin quantum number

Geometries [8.8]

More outcomes of wave-particle duality

• (Heisenberg's) Uncertainty Principle [p.298]

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

Lecture Slides 6. More outcomes of wave-particle duality

• (Heisenberg's) Uncertainty Principle [p.298]

• • 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 [Section 8.10]

Many-electron systems

• (Pauli) Exclusion Principle [p. 317]
• Effective nuclear charge [p. 316]
• Photoelectron spectra of atoms

Lecture Slides 7. Many-electron systems

• Effective nuclear charge
• Photoelectron spectra of atoms
• Electron configuration
• Hund's rules for most stable configurations
• paramagnetism
• Excited states

Lecture Slides 8. The Periodic Table (continued)

• Electron configurations (exceptions) [8.11, 9.2]
• Sizes [9.3]
• Isoelectronic species
• Transition metal ions

Lecture Slides 9. Exam I Review

Lecture Slides 10.

• Ionization energies [9.4]
• Second and third ionization energies
• Electron Affinity [9.5]
• Valence electrons and electron dot structures in atoms [10.1]
• Electronegativity [10.3]

Lecture Slides 11.

Electronegativity [10.3]

Molecular Structure [10.1]

• Lewis Structures
• Valence electrons (Main groups)
• Ionic compounds

Lecture Slides 12. Molecular Structure

Lewis Structures [10.4]

• Bond order
• Structural isomers
• Formal charge and preferred structures

Lecture Slides13. Molecular Structure

Exceptions to the Octet Rule [10.6]

• Odd electron numbers
• Expanded octets (hypervalency)

Resonance (Benzene puzzles)

Resonance [10.5]

• Equivalent preferred contributors
• Bond order

Lecture Slides14. Lewis structures

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

Dipole moments and partial ionic character

Lecture Slides 15.

Line Structures

Acid strengths and pK's

• Binary Acids
• Oxoacids
• Resonance stabilization

Lecture Slides 16. Molecular structure and acid strength

Oxoacids (continued)

• Carboxylic acids

Molecular Geometries

VSEPR Model [10.7]

• Steric number (and coordination number)
• Electronic geometries
• (Ideal) Molecular geometries
• Central atom with lone pairs

Lecture Slides 17. Molecular Geometries

VSEPR Model

Distortions from ideal geometries

• effect of lone pairs vs bonding pairs
• effect of multiple bonds
• effect of lone single electrons
• Effect of electronegativity differences

Lecture Slides 18. Review for Exam II

Lecture Slides 19 .Molecular Geometries

Dipole Moments in Polyatomic Molecules

• Rigidity about double bond
• Molecular dipoles from "bond" dipoles
• Geometrical isomers
• Free and restricted rotations about bonds

Quantum Theory of the Chemical Bond

Molecular orbitals (in "homonuclear diatomic molecules" [11.5]

Approximated by combinations of atomic orbitals

 

Lecture Slides 20 Quantum Theory of the Chemical Bond

Molecular orbitals (in "homonuclear diatomic molecules")

• Approximated by combinations of atomic orbitals
• Constructive and destructive interference effects
• 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 Slides 21 Quantum Theory of the Chemical Bond

Molecular Orbitals

• Importance of energy match vs mismatch
• Importance of net overlap
• Heteronuclear diatomic molecules

Lecture Slides 22 Quantum Theory of the Chemical Bond

Quantum Theory of the Chemical Bond

Molecular Orbitals

• Polyatomic molecules (Localized bonds)
  • Hybrid atomic orbitals

Lecture Slides 23 Molecular Orbitals in Polyatomic Molecules (Localized Bonds)

• Molecular orbitals from combinations of hybrid atomic orbitals
• Free rotations, restricted rotations, strained bonds

Molecular Orbitals in Polyatomic Molecules (Delocalized Bonds) [11.6]

• partial bond order per electron

Lecture Slides 24 Molecular Orbitals in Polyatomic Molecules (Delocalized Bonds)

• 1, 3 butadiene excited states
• benzene
• ozone
• Particle-in-a-box model for energy states

Lecture Slides 25 Molecular Orbitals in Polyatomic Molecules (Delocalized Bonds continued)

• Particle-in-a-box model
• Molecular basis of vision
• Metallic bonds [11.7]

Lecture Slides 26 Review for Exam III

Lecture Slides 27 Intermolecular Interactions

• Gases [6.1-6.4]
• Ideal Gases
  • Ideal Gas Law
  • Dalton's Law of Partial Pressures
• Real Gases [6.9]
  • Excluded volume
  • Intermolecular attractions
  • Van der Waals equation
• Intermolecular attractions [12.5]
  • Induced dipoles

Lecture Slides 28 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
• Hydrogen bonds [12.6]

Lecture Slides 29. Intermolecular Interactions

• Hydrogen Bonding
• Molecular Basis of Solubility

Lecture Slides 30.

Oxidation numbers

Transition Metal Chemistry

• Tramsition metal ion electron configurations
• Coordination complexes
• Isomers

Lecture Slides 31. 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 [24.5]

Lecture Slides 32. Transition Metal Complexes

• Crystal Field theory

• • Distorting the octahedral geometry
  • Square Planar geometry
  • Tetrahedral geometry

• Ligand Bonding to central ion's hybrid orbitals

Lecture Slides 33. Review for Exam IV

Lecture Slides 34. Proteins and Amino acids

• Amino acids
• alpha amino carboxylic acids
• zwitterions
• side groups (polar vs nonpolar)
• peptide bond
• polypeptides and proteins

• • primary structure
    combinations
  • secondary structure

  • • disulfide links
    • hydrogen bonds
    • peptide link pi-bond character

  • tertiary structure

• Hemoglobin (start)

Lecture Slides 35. Hemoglobin

• Bonding of heme to O₂ vs CO
• Role of protein in hemoglobin