Brandeis University, 2007-2008
Chemistry 15
Judith Herzfeld
Professor of Biophysical Chemistry
herzfeld@brandeis.edu
Stage II: Classroom Exercises
1.1
Scope
Scientific notation
Units
Significant figures
1.3
Evolution
Types of mass/energy
Dissipation
2.1
Nucleogenesis & Nuclear Chemistry
Fundamental particles
Isotopes
Nuclear reactions
Nuclear binding energies
Radio decay kinetics
2.3
Atomic and Molecular Structure (pre-quantum)
Periodic properties & the Octet Rule
Types of bonding
Lewis structures
VSEPR
2.5
Stoichiometry
Composition
Balanced equations & extent of reaction
Limiting reagent & maximum yield
Mass action, the equilibrium constant, & equilibrium yield
2.7
Gases
Pressure
Ideal Gas Law
Chemical equilibrium in gases, Kp
Kinetic Theory
Molecular velocities
Non-ideality
2.9
Condensed phases
Intermolecular forces
Phase changes
Phase diagrams for pure substances
Equilibria between pure phases
vapor pressure
Solutions & solution composition
Phase equilibria of solutes
solubilities
extraction
Phase equilibria of solvents
colligative properties
Simultaneous phase equlibria of solute and solvent
distillation
3.1
Aqueous solutions & ionic reactions
Solvation by water
Proton Transfer reactions
Electrolyte strength
Net ionic equations
Stoichiometry of ionic reactions
3.3
Acid-base equilibria
Proton Transfer Equilibrium Constants & Composition Diagrams
Degree of Dissociation in Solution
Self-ionization of Water
pH Scale
Acid, Basic & Neutral Salts
Buffers
Titration
3.5
Dissolution-precipitation equilibria
Solubility Product
Solubility in Water
Common Ion Effect
Solubility in Acid
Analytical Separations
4.1
Wave-Particle Duality
Electromagnetic radiation (Maxwell, photons)
Wave properties of traveling particles
Discreteness of Atomic Spectra
Wave properties of confined particles (quantized states)
4.3
Atomic Orbitals and Periodicity
Atomic orbitals
Aufbau
Periodic properties of the elements
4.5
Covalent Bonding
Molecular orbitals
Diatomic molecules
Hybrid orbitals and polyatomic molecules
Multiple bonds
4.7
Coordination complexes
5.1
First Law of Thermodynamics
Energy and enthalpy
Heat capacity and calorimetry
Thermochemistry
Heats of formation
Bond enthalpies
5.3
Second Law of Thermodynamics
Reversible and irreversible processes
Gibbs Free Energy
Temperature dependence of equilibrium
5.5
Kinetics
Elementary reactions and rate constants
Transition state and activation energy
Temperature dependence of rate constants
Multi-step reactions and coupled reactions
Rate laws
6.1
Industrial Chemistry
Silicate products
Metallurgy
Dyes and pigments
Nitrogen fixation
Petroleum chemistry
Polymer chemistry
6.3
Electrochemistry
Oxidation-reduction reactions
Galvanic cells
Cell potentials
Electrolysis
6.5
Environmental Chemistry
Element cycles
Anthropogenic disturbances
Remediation
Green chemistry
