Course description:
Physical Chemistry – the most powerful and useful theory in chemistry, may be defined as the science that describes the world in terms of atoms, molecules, and energies. CHEM 3412 is the second part of the one-year course in Physical Chemistry. Topics include thermodynamics of surfaces and electrochemical systems; kinetic theory of gases and kinetics of chemical reactions; fundamentals of quantum mechanics and quantum chemistry; statistical thermodynamics, theoretical foundations of spectroscopy.
Class schedule:
Lectures will be held two times a week: M,W 5.30-6.45 PM at room 69 Corrigan Hall
Textbook:
“Physical Chemistry”, by Ira, Levine 4-th or 5-th edition (McGraw-Hill).
Course Outline:
| Week | Day | Date | Reading | Lecture Topic | Homework |
|---|---|---|---|---|---|
Surface Thermodynamics and Electrochemistry. |
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| 1 | M | 1/14 | 13.1-13.3 Notes |
The interface region. Curved interfaces. Capillarity. |
|
| W | 1/16 | 13.4-13.5 Notes |
Thermodynamics of adsorption. | Problem Set 1. | |
| 2 | M | 1/21 | Martin Luter King, Jr. Day, No classes | ||
| W | 1/23 | 13.4-13.5 Notes |
Type of adsorption isotherms. | ||
| 3 | M | 1/28 | 13.6, Notes | Colloids. Molecular interactions in colloid systems. |
Due Problem Set 1 |
| W | 1/30 | 14.1.-14.6. | Electrochemical Systems. The Nernst equation. |
Problem Set 2. | |
| 4 | M | 2/4 | 14.7.-14.17 | Electromotive force. Batteries. The electric double layer. |
|
| W | 2/6 | Ch. 13, 14. | In class problems. | Due Problem Set 2. | |
| 5 | M | 2/11 | Exam 1 (Surface Thermodynamics, Electrochemistry) |
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Chemical Kinetics. |
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| W | 2/13 | 17.1-17.3 | Reaction rates. Reaction order. Consecutive and competing reactions. |
Problem set 3. | |
| 6 | M | 2/18 | President’s Day — University Closed | ||
| W | 2/20 | 17.4-17.7 | Determination of reaction parameters. Reaction mechanisms. Temperature dependence of rate constant. |
Due Problem set 3. Problem set 4. |
|
| 7 | M | 2/25 | 17.8-17.14 17.15-17.19 Notes |
Complex reactions. Chain reactions. Polymerization. Catalysis. |
|
| W | 2/27 | Notes 15.1-15.11 |
Maxwell distrubutions. Molecular collisions in gases. Barometric formula. |
Due Problem Set 4 Problem set 5. |
|
| 8 | M | 3/4 | 23.1-23.9 Notes |
Hard-Sphere Colision Theory of Gas-Phase Reactions.Potential energy surfaces. Activated complex theory. | Due Problem Set 5. |
| W | 3/6 | Ch. 15,17,23. | In class problems | ||
| 9 | M | 3/11 | Exam 2 (Chemical kinetics) | ||
Quantum Mechanics. Atomic and Molecular Structure. |
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| W | 3/13 | 18.1-18.8. | Quantum mechanics. The de Broglie hypothesis. Bohr theory. Shroedinger’s equation. |
Problem set 6 | |
| 10 | M | 3/18 | 18.8-18.16. | Particle in a box. Operators. Harmonical oscillator. Rigid rotator. |
|
| W | 3/20 | 19.1-19.5. | The hydrogen atom. Atomic Orbitals. |
Due Problem set 6 Problem set 7 |
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| 11 | M | 3/25 | Spring Break | ||
| W | 3/27 | Spring Break | |||
| 12 | M | 4/1 | 19.6-19.7 | Easter Monday (Class on Schedule). Many electron atoms and the Periodic table |
Due Problem set 7. Problem set 8. |
| W | 4/3 | 20.1-20.6 Notes |
Chemical bond. Molecular orbitals. | ||
| 13 | M | 4/8 | 20.7-20.14 | Quantum chemistry methods | Due Problem set 8 |
Statistical Thermodynamics |
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| W | 4/10 | 22.1-22.5 | Statistical Thermodynamics. The Canonical ensemble. The Boltzmann distribution law. |
Problem set 9 | |
| 14 | M | 4/15 | 22.6-22.9 | Statistical Thermodynamics of ideal gas | Due problem set 9 |
| W | 4/17 | 22.10-22.12 | Statistical Thermodynamics. Intermolecular forces. | . | |
| 15 | M | 4/22 | Ch. 18-20, 22. | Exam 3 (Quantum mechanics. Atomic and Molecular Structure. Statistical Thermodynamics). |
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Spectroscopy and Determination of Molecular Structures |
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| W | 4/24 | 21.1-21.11. | Spectroscopy. Electromagnetic Radiation. Rotational, vibrational and electronic spectra. Fluorescence. |
Problem Set 10 | |
| 16 | M | 4/29 | 21.12-21.17. Notes | NMR and EPR spectroscopy. Symmetry and molecular structures. X-ray diffractions |
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| W | 5/1 | Preparation for the Final Exam. In class problems. | Due Problem set 10. | ||
| 17 | M | 5/6 | Final Exam (Comprehensive), 150 min |
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| W | 5/8 | ||||
Lectures:
Lectures may not always follow the textbook in order to offer an alternative way of presentation of the subject.
Homework:
The best way to master the material is to solve problems. There will be total 10 homework problem sets. Please, note that you final score will have a significant impact from your homework. Homework is due on the day it is assigned before the class starts. No late homework will be accepted. Solutions for homework will be hand out after each due date.
Exams, and Grading:
There will be three mid-term one hour in class exams during the semester and final comprehensive exam at the end of the semester. The final grade will reflect the following distribution of course contributions.
| Mid-term exams | Three at 130 points | 50% | 390 |
| Final exam | 200 | 25% | 200 |
| Homework | 10 at 20 points | 25% | 200 |
| Total (max) | 100% | 790 |
The final letter grades will be calculated as follows:
- A>85%;
- B+>75%;
- B>70%;
- C+>65%;
- C>60%;
- D-60%-45%;
- F<45%
It is YOUR responsibility to follow university policies. Student dishonesty is troublesome for your classmates, your instructor, and for you. It is in everybody’s best interests that you work with integrity.
Sample exams will be handed out in lecture. Exam dates are:
The final exam will be held on Friday, December 17, 1999 at 10:05 am. The exam may NOT be rescheduled for a reasons such as holiday travel plans or family plans (if in doubt, ask your Dean). If you have too many exams scheduled within a 24 hour period and wish to reschedule your chemistry exam, please notify me by Thanksgiving.
Grades are not assigned on a curve and you are not competing with your classmates for a grade. Please recognize that these point allocations for lab/quiz activities are estimates; if for some reason something extra is added or something does not take place, the scale will be adjusted appropriately.
At the end of the semester, each person’s grade will be assigned as follows:
A: 730-800 points
AB: 710-729 points
B: 650-709 points
BC: 630-649 points
C: 560-629 points
D: 500-559 points
F: below 500 points
Physical chemical principles and their application to the chemical and life sciences. Topics include thermodynamics, chemical and biochemical kinetics, solution physical chemistry, surface chemistry, electrochemistry, quantum mechanical description of atomic and molecular structure, spectroscopic methods, statistical mechanics, transport processes, and macromolecular structure.