Fall 2011 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.

Lecture Slides 1. Introduction

Lecture Slides 2. 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"
• Avogadro's Law (Hypothesis) [p. 20]
• Cannizzaro's Stoichiometric Analyses

Lecture Slides 3. History

• Avogadro's Law (Hypothesis) [p. 20]
• Cannizzaro's Stoichiometric Analyses
• Early recognition of "Periodicity"

Energies

• Kinetic energy
• Potential energy (and forces)
• Internal energies (rotation and vibration)
• Light [Chapter 12]]
• H-atom line spectra (emission and absorbtion)

Masses

• Mass spectrometry [3.1]

Lecture Slides 4.

Problems with some results of physical measurements [Chapter 12]

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

Physics puzzles "solved" by quantization

• 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 12.4]

(New Quantum Theory)

• deBroglie and wave-particle duality of matter (Section 12.2)

Lecture Slides 5. (New Quantum Theory)

(New Quantum Theory)

• deBroglie and wave-particle duality of matter (Section 12.2)

Wave Nature of Matter

• Particle-in-a-box (Section 12.6)

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

• Schrodinger's Wave Equation applied to the hydrogen atom [Section 12.7]
• • n, principal quantum number
  • l, angular momentum or shape quantum number
  • m_l, magnetic or orientation quantum number

Lecture Slides 6. (New Quantum Theory)

Geometries [12.9]

More outcomes of wave-particle duality

• (Heisenberg's) Uncertainty Principle [p.539]

• • 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 [Section 12.10]

Lecture Slides 7.

Many-electron systems

• Effective nuclear charge [Section 12.11]
• Photoelectron spectra of atoms
• Hund's Rule [Section 12.13]
• Excited states
• Building the Periodic Table [Section 12.13]

Lecture Slides 8. The Periodic Table (continued)

• Building the Periodic Table
• Electron configurations (and exceptions)
• Sizes [pp. 577,8]
• Isoelectronic species
• Transition metal ions

Lecture Slides 9. Exam I Review

Lecture Slides 10. Periodic Table (continued)

• Ionization energies
• Electron affinities[12.15]
• Electronegativity [13.2]

Lecture Slides 11. Molecules

Lewis Structures [13.10]

• Valence electrons (Main groups)
• Octet Rule
• Structural isomers
• Formal charge and preferred structures [13.12]

Lecture Slides 12. Lewis Structures [13.10]

• Formal charge and preferred structures [13.12]
• Exceptions to the Octet Rule [13.12]
  • Incomplete octets
  • Odd electron numbers
  • Expanded octets (hypervalency)
• Resonance (Benzene puzzles)

Lecture Slides13. Molecular Structure

Resonance [13.12]

• Equivalent preferred contributors
• Bond order

Reaction Heats

Line Structures

Lecture Slides 14.

Partial Ionic character [13.3 and 13.6]

Acid strengths and pK's

• Binary Acids
• Oxoacids
• Resonance stabilization
• Carboxylic acids

Lecture Slides 15.

Acid strengths and pK's

• Carboxylic acids

Molecular Geometries

VSEPR Model [13.13]

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

Lecture Slides 16. Molecular Geometries

VSEPR Model [13.13]

Distortions from ideal geometries

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

Dipole Moments in Polyatomic Molecules

• Rigidity about double bond
• Molecular dipoles from "bond" dipoles
• Geometrical isomers

Lecture Slides 17.

Dipole Moments in Polyatomic Molecules

• Rigidity about double bond
• Molecular dipoles from "bond" dipoles
• Geometrical isomers

Start of review for Exam II

Lecture Slides 18. Review for Exam II

Lecture Slides 19. Quantum Theory of the Chemical Bond

Molecular orbitals (in "homonuclear diatomic molecules" [14.2]

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

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

• Combining 2p atomic orbitals

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

Lecture Slides 20. Quantum Theory of the Chemical Bond

Molecular orbitals (in "homonuclear diatomic molecules") [14.3]

• Molecular energy level diagrams
• Building up electron configurations
• Bond order

Lecture Slides 21. Quantum Theory of the Chemical Bond

Molecular Orbitals (factors to consider)

• Importance of energy match vs mismatch
• Importance of net overlap

Heteronuclear diatomic molecules [14.4]

Lecture Slides 22. Quantum Theory of the Chemical Bond

Molecular Orbitals

• Polyatomic molecules

• Hybrid atomic orbitals [14.1]

• Molecular orbitals from combinations of hybrid atomic orbitals
• The rigid double bond
• The freely rotating single sigma bond

Lecture Slides 23. Quantum Theory of the Chemical Bond

Molecular Orbitals in Polyatomic Molecules

• The rigid double bond
• The freely rotating single sigma bond
• 1,3 butadience and delocalized moleculal orbitals

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

• 1,3 butadiene and the use of "partial bond order per electron"
• benzene

Triatomic molecules

• Ozone
• Carbon dioxide

Energy levels and the particle-in-a-box model

• conjugated systems
• particle-in-a-box levels
• light absorption transitions
•  

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

Energy levels and the particle-in-a-box model

• conjugated systems
• particle-in-a-box levels
• light absorption transitions
• retinal
• Metallic bonds [pp. 797-8]

Lecture Slides 26. Review for Exam III (part I)

Lecture Slides 27. Review for Exam III (part II)

Lecture Slides 28. Intermolecular interactions

Ideal gases [5.3]

Real gases (Van der Waals) [5.10]

• Excluded volume effect
• Intermolecular attractions

Induced dipoles

• Polarizability

Lecture Slides 29. Intermolecular Interactions (condensed phases) [16.1, 2]

Van der Waals interactions

• Permanent dipoles
• Temporary (induced) dipoles
• Boiling points, melting points, densities

• Effects of size
• Effects of shape

Lecture Slides 30. Intermolecular Interactions (condensed phases)

Van der Waals interactions

• Hydrogen Bonding
• Molecular Basis of Solubility

Lecture Slides 31. Intermolecular Interactions

• Molecular Basis of Solubility

Oxidation Numbers

Lecture Slides 32.

Oxidation Numbers

Transition Metal Chemistry

• Tramsition metal ion electron configurations [19.1]
• Coordination complexes [19.3]
• Isomers [19.4]
  • Structural Isomers

• Stereoisomers [19.4]

• Geometrical isomers

• Square planar geometries
• Octahedral geometries

Lecture Slides 33. Transition metal complexes

Stereoisomers [19.4]

Optical isomers

Observations to explain

• Colors
• Magnetic Properties
• Stability

Crystal Field Theory [19.6]

Lecture Slides 34. 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 35. Transition Metal Complexes

Crystal Field theory

• Coordination number 2

Hemoglobin

• Bonding of heme Fe²⁺ to O₂ vs CO
• Sizes of transition metal ions
• Role of protein in hemoglobin

Lecture Slides 36. Review (part 1)

Lecture Slides 37. Review (part 2)