Cumulative Outline
Lecture 1. History
- The first 2000 years
- Stoichiometry Laws
- Conservation of Mass
- Law of Definite Proportions
- Law of Multiple Proportions
Lecture 2. History
- Law of Multiple Proportions illustrated
- 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"
Lecture 3. Energies
- Kinetic energy
- Potential energy (and forces)
- Internal energies (rotation and vibration)
- Light
- H-atom line spectra (emission and absorbtion)
Rutherford's atomic model
Mass Spectroscopy
- Ions
- Mass spectrometer
- Isotopes
Problems with some results of physical measurements
- Line spectra
- Photoelectric Effect
- Blackbody Radiation (and the ultraviolet catastrophe)
Lecture 4. (Old Quantum Theory)
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
- 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
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, orbitals
- n, principal quantum number
- l, angular momentum or shape quantum number
- ml, magnetic or orientation quantum number
Electron "spin"
ms, spin quantum number
Energies and geometries
Lecture 6. More outcomes of wave-particle duality
- (Heisenberg's) Uncertainty Principle
- 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
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
- Configuration sequences
Lecture 8. The Periodic Table (continued)
- Electron configurations (exceptions)
- Sizes
- Isoelectronic species
- Transition metal ions
Electron Configurations and Ionization Energies
- First ionization energies
- Ionization energy and effective nuclear charge
- Trends across a row
Review for Exam I
Lecture 10. Electron Configurations and Ionization Energies
- Second and third ionization energies
- Electron affinities
- Electronegativity
Valence electrons and electron dot structures in atoms
Lewis Structures
- Valence electrons (Main groups)
- Octet Rule
Lecture 11. Lewis Structures
Octet Rule
Lecture 12. Molecular Structure
Lewis Structures
Exceptions to the Octet Rule
- Incomplete octets
- Odd electron numbers
- Expanded octets (hypervalency)
Resonance
- Equivalent preferred contributors
Lecture 13. Lewis structures (continued)
Resonance
- Equivalent preferred contributors
- Bond order
Line structures
Reaction Heats
Lec ture 14. Lewis structures (continued)
- Dipole moments
- Partial ionic character
Molecular structure and acid strength
- (Binary Acids)
- pK values
Lecture 15. Polar bonds
Molecular Geometries
Lecture 16. Molecular Geometries (continued)
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 17. Oxoacids (continued)
- phosphorous oxoacids
- Carboxylic acids
Lecture 18. Review for Exam II
Lecture 19. Molecular Geometries
- Molecular dipoles from "bond" dipoles
- Geometrical isomers
Molecular orbitals (in "homonuclear diatomic molecules")
- Approximated by combinations of atomic orbitals
- Constructive and destructive interference effects
Lecture 20. 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
- "Sigma" bonding molecular orbital
- "Sigma" antibonding molecular orbital
- Building up electron configurations
- 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
Lecture 21. Quantum Theory of the Chemical Bond
Molecular orbitals (in "homonuclear diatomic molecules")
- Building up electron configurations
Molecular Orbitals
- Importance of energy match vs mismatch
- Importance of net overlap
Lecture 22. Quantum Theory of the Chemical Bond
Molecular Orbitals
- Heteronuclear diatomic molecules
Polyatomic Molecules
- Pure atomic orbitals don't work
- Hybrid atomic orbitals
Lecture 23. 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
Lecture 24. Molecular orbitals (localized, continued)
- Pi --> Pi* light absorption
- Strained bonds in small rings
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
- Comparison to Lewis structure resonance
- Continuing with excited states and bond orders
Benzene
Lecture 25. Molecular Orbitals (delocalized)
- Ozone
- Carbon dioxide
- Energies via particle-in-a-box
- Light-induced transitions
Lecture 26. Review for Exam III
Lecture 27. Molecular Orbitals (delocalized, continued)
- Metallic bonds
Gases
- Ideal Gases
- Ideal Gas Law
- Dalton's Law of Partial Pressures
- Real Gases
- Excluded volume
- Intermolecular attractions
Lecture 28. Intermolecular Interactions
Gases
- Real Gases
- Excluded volume
- Intermolecular attractions
- Van der Waals equation
Induced dipoles
- Polarizability
- Van der Waals interactions
- Permanent dipoles
- Temporary (induced) dipoles
- Boiling points, melting points, densities
- Effects of size
- Effects of shape
Lecture 29. Intermolecular Interactions (condensed phases)
- Van der Waals interactions
Liquids and Solids
- Hydrogen Bonding
Lecture 30. Intermolecular Interactions
- Molecular Basis of Solubility
Lecture 31. Oxidation numbers
Transition Metal Chemistry
- Tramsition metal ion electron configurations
- Coordination complexes
Lecture 32. Transition metal complexes
Stereoisomers
- Geometrical isomers
- Square planar geometries
- Octahedral geometries
Optical isomers
Observations to explain
- Colors
- Stability
- Magnetic behavior
Crystal Field theory
Lecture 33. Transition Metal Complexes
- Crystal Field Theory
- Weak field vs strong field
- Spectrochemical series
- Octahedral geometry
Review for Exam IV
Lecture 34. Transition metals
- Distorting the octahedral geometry
- Square Planar geometry
- Tetrahedral geometry
Lecture 35. Transition Metals
- Hemoglobin
Lecture 36. Hemoglobin