Course Summary:
A continuation of Chemical Concepts, Systems and Practices I, emphasizing molecular and macroscopic approaches to chemical systems with examples concerned with life sciences (Turner) or energy and the environment (Farrar). Topics covered include: Chemical kinetics, electrochemistry, thermodynamics, properties of atoms, atomic structure, and chemical bonding. In addition to course lectures, there is a three hour laboratory every week, a 50 minute laboratory/lecture and a 50 minute recitation. You must register for the laboratory/lecture and laboratory (linked) prior to the start of the semester. Recitations will be assigned in the main lecture during the first week of classes.

Course Topics:

1. Energy Conservation
   1. Heat, work, energy, and the First Law
   2. Thermodynamic processes: cyclic processes
   3. Optimizing the work you do: Reversible and irreversible processes
   4. Thermodynamic Efficiency
2. Spontaneous Processes
   1. Spontaneous chemical reactions. Entropy and entropy changes. Definition of entropy, S. Definition of Second Law via S. Entropy changes: for heating objects, entropy change for reversible isothermal expansion.
   2. Molecular Disorder: Statistical interpretation of S. The Third Law of thermodynamics.
   3. Spontaneity in Chemical Reactions. The Gibbs Free Energy G and Chemical Equilibria. Standards states, Gibbs Free Energy changes and Keq.
3. Electrical Energy from Chemical Reactions
   1. Electrical energy from atoms: Redox reactions. The Nernst equation.
   2. Electrochemical cells and fuel cells: Energy from batteries. Light into electrical energy. Energy storage in H2 via water splitting. The hydrogen economy.
   3. Electrolysis in aqueous and non-aqueous systems
   4. Energy Consumption in Industrial Electrochemical Processes: Aluminum production and the Hall process.
4. Chemical Kinetics: Atmospheric Chemistry
   1. Principles gas phase chemical kinetics: rate laws and mechanisms
   2. Stratospheric removal of O3: NOx vs. Cl from CFC's CFC, chlorine photochemistry
   3. Catalysis: Homogeneous and heterogeneous catalysis, surface kinetics: ClONO2, HCl reservoirs
   4. Photochemical pollution
5. Sources of energy: nuclei
   1. The Atomic Theory: Modern evidence for electrons and the nucleus. Rutherford scattering.
   2. The nucleus: Isotopes and mass spectrometry revisited. Nuclear processes. Nuclear decay by emission of particles and radiation.  Radioactive decay and first order kinetics.
   3. Energy from nuclear reactions: E = mc2. Nuclear thermochemistry.
   4. Fission and fusion.
6. Energy from atoms
   1. Quantum Theory: deBroglie waves, Heisenberg Uncertainty Principle, the Schrödinger equation. One-electron atoms. Many-electron atoms. Pauli Principle, Aufbau Principle, Hund's rules
   2. Atomic properties and the Periodic Table.
7. Chemical Stability and Energetics: Chemical Bonds
   1. Lewis structures, ionic and covalent bonds and bond enthalpies; Bond polarity
   2. Molecular energy levels and spectroscopy; Simple molecular orbital concepts; Molecular shapes
   3. Greenhouse gases and global warming

Required Text:
Steven S. Zumdahl, Chemical Principles, Sixth Edition Houghton Mifflin, Boston, MA (2007)
ISBN-10: 061894690-X | ISBN-13: 9780618946907