A GUIDE TO DUKE UNIVERSITY'S PARTICIPATION IN THE US-EU EXCHANGE PROGRAM FOR CHEMISTRY STUDENTS, 1997-1998.

A. INFORMATION ABOUT DUKE UNIVERSITY

A.1. INTRODUCTION TO DUKE UNIVERSITY

Duke University has over 10,000 students enrolled in graduate and undergraduate degree programs. Since its beginning as Union Academy in 1838 the primary commitment of Duke University has been to the education of undergraduate students. In addition, Duke is recognized as one of the world's leading research institutions.

The combination of these two traditions gives Duke undergraduates an opportunity all too rare among major universities: the chance for undergraduates to work closely with professors who receive national and international recognition for their professional accomplishments. Last year, 88 percent of Duke's tenured and tenure-track professors taught undergraduate classes. Only ten percent of undergraduate courses have class sizes larger than 35 students.

Duke University places a strong emphasis on the importance of a cosmopolitan understanding of the world of ideas. With students from all 50 of the United States and over 40 foreign countries, Duke's 6,130 undergraduate students reflect a rich diversity of cultures. In addition, more than one third of Duke undergraduates study abroad during their undergraduate years, through participation in one of over 125 Duke-sponsored or other Duke-approved programs in foreign countries, from Australia to Zimbabwe.

Further information is available here.

A.2. Maps of Duke, Durham, NC and surrounding areas.

A.3. Academic Calendar current and projected.

A.4. LIVING AT DUKE

Duke is located in Durham, North Carolina, a city of 180,000 citizens. Durham is one of three cities which are known as "The Triangle" (Raleigh and Chapel Hill, the other points of The Triangle, are only a half-hour drive away from Durham). Recently, one of America's most popular publications, "Money Magazine", ranked The Triangle as the #1 best place to live in America.

Students invariably enjoy the pervasive politeness (known as "Southern Hospitality") of Triangle citizens, and the temperate climate of Durham, which is blessed with sunshine and warm weather, in the low 20 degrees, centigrade, most days of the year (although Durham does receive on average, one or two snowfalls a year, during the brief winter season).

In addition, the Triangle cities offer a rich diversity of cultural opportunities, from poetry readings to academic lectures from distinguished guest lecturers, to a wide selection of live music ranging from symphony concerts to jazz, rock&roll, and country-western bands.

With the 7,700 acre Duke forest being an integral part of the campus, and the Atlantic Ocean (to the east) and the Appalachian Mountain range (to the west) each being a two-and-a-half hour drive away, students have numerous opportunites for outdoor recreation.

The Duke campus is composed of dozens of beautiful gothic and Georgian-style, stone buildings. Ninety three percent of Duke undergraduates live in dormitories on the campus. A number of faculty members live in residence halls, and faculty offices and seminar rooms are also located in several dormitory houses. Educational, cultural, and outdoor adventure programming is planned and presented throughout the year. The goals of these various programs are to enhance the quality of intellectual and social life for the residents on campus, to facilitate student-faculty interaction outside of the formal classroom, and to develop a greater sense of community with the individual residence halls as well as within the University as a whole.

A.5. RESEARCH RESOURCES OF THE UNIVERSITY

As one of the pre-eminent science research centers in the United States, Duke University boasts research laboratories in all departments of the natural and social sciences and the School of Engineering as well as other facilities. In addition to the faculty, post-doctoral associates, technicians and graduate students who carry out research in the laboratories of the University, many undergraduate students are also involved in the research enterprise. The programs of research open to undergraduate students are found not only in the laboratories of the main campus in Chemistry, Physics, Biological and Medical sciences, but also in the specialized laboratories, including the Duke University Marine Laboratory in Beaufort, North Carolina; the Phytotron of the Southeastern Plant Environment Laboratories; the Duke Forest, adjacent to the campus; the Duke University Primate Center; the Triangle Universities Nuclear Laboratory; and the Free Electron Laser Laboratory.

The research laboratories of the Chemistry Department, located in the Gross Chemical Laboratory building, are described in detail in Section B.2.

Duke's library is the 19th largest in the America, with over four million volumes, plus nine million manuscripts. In addition to the main library, Duke has several separate libraries, including the Chemistry library, as well as ones for Mathematics-Physics, Divinity, Biology-Forestry, Engineering, Law, Medicine, Music and Business. Duke University, the University of North Carolina, and North Carolina State University also share a library data-base, which allows Duke students access to all three of these substantial library collections.

But of all the resources available to Duke students, the most invaluable is the distinguished faculty. The University faculty, numbering approximately 1,900, maintains a tradition of personal attention to students and devotion to research. Many members of the faculty are, and have been, cited for excellence in teaching and are elected to membership in national societies which honor the finest in scholarship and research. Leaders in their disciplines and their professional organizations, Duke's faculty, 97% of whom hold doctoral or equivalent degrees, are authors of significant books and articles. Many members of the Duke faculty also act as consultants to industry, government, and foundations.

A.6. FINANCIAL CONSIDERATIONS

Exchange students will be expected to live on the Duke campus. Room and board for the 1997-98 academic year are estimated to cost $6000- $8,000, and books and supplies are estimated to cost about $720. In addition, most students tend to spend an average of $3,000 for personal expenses, more or less, depending upon the student's lifestyle.

All foreign exchange students are required to have health insurance policy. Duke offers a policy which costs approximately $620 a year.

More information about Duke University is available in the Duke Bulletin, which is available upon request.

B. INFORMATION ABOUT THE CHEMISTRY DEPARTMENT

B.1. The ECTS COORDINATORS

B.2. GENERAL DESCRIPTION OF THE DEPARTMENT.

The Chemistry Department consists of twenty faculty whose interests span the fields of biological, analytical, inorganic, organic, physical and theoretical research. The Chemistry Library, lecture halls, class rooms, teaching laboratories and research laboratories, as well as the faculty and administrative offices of the Department are located in the P. M. Gross Chemical Laboratory on the Duke West Campus.

Although the majority of Duke undergraduates take the first year, "freshman" chemistry course, a smaller number continue on to the second year, organic, course and still fewer advance to the third year. Undergraduate chemistry courses in the third year, and particularly the fourth year, are populated almost exclusively by students studying to complete either a BA or BS degree in Chemistry. All of these BS degree candidates and some of the BA candidates include at least one year of research ("Independent Study", CHM 191-2 and 193-4) in their degree programs, usually in the fourth year. Approximately 25 BS and 24 BA Chemistry degrees are awarded each year, many with concentration in biochemistry or one of the other available concentrations. Advanced undergraduate students may also take one or more of the first year graduate level courses. This is an option for exchange students as well.

The graduate student population of the Department varies between 80 and 100. Required graduate courses are usually taken in the first year of graduate study, although advanced and special topics courses are sometimes taken beyond the first year. Most graduate students are in the PhD program, but a few will take MS degrees. After completing the required course work, the average PhD student spends 3-4 years carrying out research for the Dissertation. The Masters degree requires 1-2 years of work beyond the year of courses.

The typical research group in the Department, under the direction of one of the Faculty, comprises one or more postdoctoral research associates, several graduate students and senior undergraduates and often one or more visiting scholars. In addition to the support of the University, the research of the Department is supported by extensive external grants and contracts from the U. S. Government, from private foundations and from industry. Many research projects involve collaboration between faculty within the Department or with research groups in other departments and institutions.

The P. M. Gross Laboratory provides most of the facilities, equipment and instrumentation necessary to carry out chemical research in all fields of modern chemistry. Nuclear magnetic resonance facilities include a broad band Varian XL-300 and 600 MHz Unity, General Electric QE-300, GN-300 (25mm wide bore probe) and GN-500 frequency adjustable instruments, a JEOL FX-90Q, and two 60 MHz proton instruments. An ESR spectrometer, the Varian E-9, provides an excellent facility for research in electron spin resonance. Mass spectrometric service is provided by a Hewlett-Packard GC-MS system with HPLC/MS capability, and a new JEOL SX102A High Resolution MS has just been installed. The Chemistry Department houses the University Crystal Structure Center, which features an Enraf-Nonius CAD-4 automatic diffractometer. Numerous instruments of varying sophistication for photoacoustic, fluorescence, high resolution (Nicolet 8400) and routine (Bomen MB-100) FTIR, dispersive infrared, UV, Raman and ORD-CD spectroscopy are available; various laser sources, monochromators, and computerized data acquisition systems are associated with these systems. Some other significant research facilities include T-jump, stopped flow and diode array spectrometers for rapid kinetic studies, a circularly polarized luminescence spectrometer, electrochemical equipment, a scanning tunneling microscope, and an ultra dry lab facility. A variety of preparative and analytical gas and liquid chromatographs are also located in the building. Research in biological chemistry is facilitated by the availability of an autoclave, media prep room, and ultra centrifuges.

Computing facilities in chemistry include clusters of Sun UNIX workstations and Apple Macintosh computers. The UNIX cluster and many other computers associated with specific research groups are networked via Ethernet, which is linked to the university's fiber optic network. Among the resources available via the network is the North Carolina Supercomputing Center's Cray Y-MP8/464. In addition, the department has state-of-the-art computer/video projection systems in its lecture halls for incorporation of the latest computational research tools into the undergraduate chemistry curriculum.

The Department has a machine shop, an electronics shop, and a glass-blowing shop. The facilities of the Duke University Marine Laboratory on the coast at Beaufort, North Carolina, are available for specimen collecting and processing studies of chemicals of marine origin. The Department of Chemistry Library, with holdings of approximately 45,000 volumes, is also located in the P.M. Gross Chemical Labora- tory. The library receives 345 current scientific periodicals, 225 serial subscriptions and has computer facilities for complete information retrieval.

For those exchange students who are interested in combining research work with course work while on their exchange visits or for whom total concentration on research is the goal of their time at Duke, the descriptions of the backgrounds, fields, research programs and lists of recent publications of the faculty below will be of interest. Exchange students wishing to carry out research should communicate directly with the faculty member(s) whose research is of interest to them. Limitations on the space available to each research group require that these arrangements be made in advance and in parallel with other registration procedures.

The Chemistry Faculty: Research Interests

B.3. PROGRAMS OF STUDY


GRADUATE STUDY
Between 80 and 100 students are enrolled in the graduate program leading to degrees of Further information about the graduate program and application materials for the Graduate School are available on request.

UNDERGRADUATE STUDY

Courses at Duke University and Credit System

The University is on the semester system. Fall classes begin at the end of August or early in September and end before Christmas. The Spring semester begins in early January and ends at the end of April or early May. Although some courses are year long, each semester course is given a different number. In general, the second semester can be taken only after having passed the first semester.
The typical course load for a student is 4 courses per semester or 8 courses per year making the typical Duke course equivalent to 7.5 ECTS credits.

Degrees

Between 50 and 60 students are enrolled in the undergraduate program leading to degrees of An additional 50 to 60 students are pursuing a less rigorous degree in chemistry, the A.B. degree (Bachelor of Arts).

General Curriculum

During their 4 years of study, candidates for B.S. degrees are exposed to a traditional liberal arts experience which includes courses in at least 5 of 6 major areas: arts and literatures, civilizations, foreign languages, natural science, quantitative reasoning, and social sciences. A typical course load is 4 courses per semester or 8 courses per year. Generally a chemistry major takes 1 or 2 non-science courses per semester.

B.S. Chemistry Curriculum (science and math courses only)
Detailed course contents are given in the last section of this brochure.

First Year Curriculum Second Year Curriculum Third Year Curriculum Fourth Year Curriculum

B.4. THE DEPARTMENTAL GRADING SCALE

Passing grades are A (exceptional), B (superior), C (satisfactory), and D (low pass). These grades may be modified by a plus or a minus. the failing grade is F. A grade of Z may be assigned for the satisfactory completion of the first term of a two-course sequence, and the final grade for both courses is assigned at the end of the second course of the sequence.

Although the D grade represents a low pass, not more than two courses passed with D grades may be counted toward fulfilling continuation and graduation requirements.

A student may repeat any course in which he/she earns a grade of D+, D, D-, or F. The grade earned in the repeated course as well as the grade earned originally appear on the transcript, but only one is counted toward fulfilling continuation and graduation requirements.

In an "average" chemistry course, the average grade is B with about one-third of the students earning grades of A+, A, or A-; one-third earning grades of B+, B, or B-; and the remaining third earning grades below B-. About 1% of the class fails the course.

[The grading scale is consistent with the high quality of the Duke student body. Typically a matriculating class of 1600 students is selected from a pool of about 14,000 applicants. Roughly 90% of all matriculants rank in the top 10% of their high school graduating classes, while 75% of all matriculants rank in the top 5%.]

B.5. CONTENTS OF COURSES TAKEN BY CHEMISTRY MAJORS

(The contents given below are for the year 1996 and should be considered as representative only.)

BASIC CHEMISTRY COURSES

Chm 11L: Principles of Chemistry
(24 hrs lecture, 60 hrs lab/recitation, 1st semester, 1st year, 7.5 ECTS credits)
Continuous assessment of lecture, recitation, and lab work; comprehensive final examination.

Text: Masterton, W.L.; Hurley, C.N. Chemistry Principles and Reactions , 3rd Edition; Saunders, 1996.

Matter and Measurement (Types of matter, properties of matter, quantities, units, significant figures, conversions of units); Atoms, Molecules, Ions (Atomic theory, components of atom, introduction to periodic table, molecules and ions, formulas for ioninc compounds); Stoichiometry (atomic and formula masses, mole, mass relations in chemical formulas, mass relations in reactions); Reactions in Aqueous Solutions (Precipitation reactions, acid-base reactions, redox reactions, molarity, solution stoichiometry and quantitative analysis); Gases (measurements on gases, Ideal gas law, gas law calculations, stoichiometry of gaseous reactions, Dalton's Law, Kinetic Molecular Theory, real gases); Electronic Structure and the Periodic Table (Light, photon energies, atomic spectra, hydrogen atom, quantum numbers, energy levels, orbitals, electron configurations of atoms, orbital diagram of atoms and monatomic ions, periodic trends in atomic radii, ionization energies, electron affinities, and electronegativities); Covalent Bonding (Lewis structures, Octet Rule, VSEPR molecular geometry, polarity of molecules, hybridization of atomic orbitals, resonance); Thermochemistry (Heat flow, calorimetry, enthalpy, thermochemical equations, enthalpies of formation and Hess' Law, bond energy); Liquids and Solids (Intermolecular forces, network covalent, ionic, metallic solids, crystal structures and cubic unit cells, liquid-vapor equilibrium, phase diagrams of water and carbon dioxide); Solutions (types, concentration units, principles of solubility, colligative properties); Spectroscopy (Infrared, vibratory motions, IR active vibrations, identifying functional groups, "fingerprinting" molecules, ultraviolet, delocalization and wavelength of absorption, color).
Laboratory work emphasizes the scientific method and illustrates the concepts and principles discussed in lecture.

Math 31L: Laboratory Calculus
(36 hrs lecture, 24 hrs lab, 1st semester, 1st year, 7.5 ECTS credits)
Continuous assessment of lecture and lab work; comprehensive final examination.

Text: Smith, D.A.; Moore, L.C. The Calculus Reader; D.C. Heath, 1994.

Relationships (related variables, mathematical models, functions of time, functions as objects, inverse functions, accuracy of measurements); Rates of Change: Models of Growth (rates of change, derivative:instantaneous rate of change, symbolic calculation of derivatives:polynomial functions, exponential functions, modeling population growth, logarithms and representation of data); Initial Value Problems differential equations and initial values, a cooling body, a falling body, models for raindrops); Differential Calculus and Its Uses (derivatives and graphs, solving non-linear equations by linearization: Newton's Method, the product rule, the chain rule, analysis of reflection, derivatives of functions defined implicitly, the general power rule, differentials and Leibnitz notation); Applications of Euler's Method (Euler's method, modeling epidemics, modeling the evolution of prices in a simple economy); Periodic Motion (circular functions: sine and cosine, spring motion, pendulum motion). Labs utilize graphing calculators to illustrate topics covered in the lecture part of the course.

Chm 12L: Principles of Chemistry
(24 hrs lecture, 60 hrs lab/recitation, 2nd semester, 1st year, 7.5 ECTS credits)
Continuous assessment of lecture, recitation, and lab work; comprehensive final examination.

Text: Masterton, W.L.; Hurley, C.N. Chemistry Principles and Reactions , 3rd Edition; Saunders, 1996.

Rate of Reaction (Meaning of reaction rate, rate and concentration, integrated rate laws, activation energy, reaction rate and temperature, reaction mechanisms); Gaseous Chemical Equilibrium (equilibrium constant expression, determination of K, applications of K, Principle of LeChatelier with applications); Acids and Bases (Bronsted-Lowry model, water dissociation constant, pH and pOH, weak acids and bases and their dissociation constants, hydrolysis of salts); Acid-Base and Precipitation Reactions (Titrations and titration curves, buffers, precipitation equilibria); Complex Ions; Coordination Compounds (Composition of complex ions, geometry of complex ions, electronic structure and bonding in complex ions, crystal field theory); Spontaneity of Reaction (Three laws of thermodynamics, spontaneous processes, entropy, free energy, standard free energy change, non-standard state free energy changes, free energy change and equilibrium constant, coupled reactions); Electrochemistry (voltaic cells, standard state voltages, relation to K, Nernst relation, Latimer Diagrams, electrolytic cells, commercial cells); Nuclear Reactions nuclear stability, natural and artificial radioactivity, kinetics of radioactive decay, mass-energy relations, nuclear fission, nuclear fusion); Energy and the Environment (solar energy, fossil fuels, acid rain, smog, particulate matter, global warming, hydrogen as an alternative fuel).
Laboratory work emphasizes the scientific method and illustrates the concepts and principles discussed in lecture.

Math 32L: Laboratory Calculus
(36 hrs lecture, 24 hrs lab, 2nd semester, 1st year, 7.5 ECTS credits)
Continuous assessment of lecture and lab work; comprehensive final examination.

Text: Smith, D.A.; Moore, L.C. The Calculus Reader.; D.C. Heath, 1994.

From Raindrops to Rockets (raindrops, projectiles, escape velocity); Solutions of Initial Value Problems (natural vs. constrained growth, separation of variables, the logistic growth equation, the coalition model of population growth, discrete logistic growth); The Fundamental Theorem of Calculus (averaging continuous functions: the definite integral, evaluation of integrals, the indefinite integral, representation of functions, moments and centers of mass); Integral Calculus and its Uses numerical approximation of integrals, substitution: applying the chain rule to integrals, integral tables, representation of periodic functions, reliability theory, integration by parts, continuous probability: distribution and density functions, normal distributions, gamma distributions); Polynomial and Series Representations of Functions (Taylor polynomials and infinite series, series of constants, convergence of series, series calculations of the error function). Labs utilize graphing calculators to illustrate topics covered in the lecture part of the course.

Chm 151L: Organic Chemistry
(36 hrs lecture, 48 hrs lab, 1st semester, 2nd year, 7.5 ECTS credits)
Continuous assessment of lecture, recitation, and lab work; comprehensive final examination.

Text: Loudon, G.M. Organic Chemistry, 3rd edition; Benjamin, 1995.

Structure and Bonding (Ionic, covalent, polar covalent bonds, Lewis acids and bases, arrow formalism, structures of covalent substances, resonance structures); Electronic Structures of Atoms and Molecules (wave nature of electron, hydrogen atom, multielectron atoms, molecular orbitals, hybrid orbitals); Alkanes and functional groups (normal alkanes, structural isomers, alkane nomenclature, cycloalkanes, physical properties, conformations, elemental analysis, occurrence and uses of alkanes, alkyl radicals); Alkenes - equilibria and reaction rates (structure and bonding of alkenes, cis-trans isomerism, nomenclature, physical propeties, free energy and chemical equilibrium, addition of hydrogen halides to alkenes, rearrangement of carbocations, reaction rates, transition-state theory and Hammond's postulate, hydration of alkenes, catalysis); Addition Reactions of Alkenes (halogenation of alkenes, writing organic reactions, alkenes to alcohols, alkenes to glycols, ozonolysis, summary of eletrophilic addition reactions, hydrogenation of alkenes, addition of HBr, uses of alkenes, unsaturation number); Stereochemistry (Enantiomers and chirality, R,S system, physical properties of enantiomers, racemates, absolute configuration, diastereomers, meso compounds, conformational stereoisomers, Fischer projections, tetrahedral carbon atom); Cyclic Compounds, Stereochemistry of Chemical Reactions (relative stabilities of monocyclic alkanes, conformations of cyclohexane, monosubstituted cyclohexanes, disubstituted cyclohexanes, planar representation of cyclic compounds, bicyclic and polycyclic compounds, stereochemistry and chemical reactions, chirality in nature, stereochemistry of alkene addition reactions); Introduction to Alkyl Halides, Alcohols, Ethers, Thiols and Sulfides (nomenclature, structures, physical properties, polarity, hydrogen bonding, solvents in organic chemistry, review of Bronsted acidity and basicity, acidity of alcohols and thiols, basicity of alcohols and ethers, organometallic compounds, preparation); Substitution and Elimination Reactions of Alkyl Halides (equilibrium in nucleophilic substitution reactions, the SN2 reaction, the E2 reaction, the SN1 reaction, carbenes); Chemistry of Alcohols, Glycols, and Thiols (dehydration of alcohols, reactions of alcohols with hydrogen halides, sulfonate and inorganic ester derivatives of alcohols, reactions of alcohols with thionyl chlroide and phosphorus tribromide, oxidation of alcohols, redox in organic chemistry, biological oxidation of ethanol, chemical and stereochemical group equivalence, oxidation of thiols, synthesis of alcohols and glycols, design of organic synthesis); Chemistry of Ethers, Epoxides and Sulfides (synthesis of ethers, epoxides, and sulfides, cleavage of ethers and sulfides, nucleophilic substitution reactions of epoxides, oxonium and sulonium salts, neighboring group participation, oxidation of ethers and sulfides, organic synthesis); Infrared Spectroscopy and Mass Spectrometry (Introduction to Spectroscopy, IR spectroscopy, Functional-group IR absorptions, experimental aspects of IR, introduction to mass spectrometry); Nuclear Magnetic Resonance Spectroscopy (Introduction to NMR, NMR spectrum: chemical shift and integral, spin-spin splitting, high-field NMR, functional group NMR absorption, deuterium in proton NMR, NMR and dynamic systems, Carbon-13 NMR, solving structure problems with spectroscopy, newer uses of NMR); Chemistry of Alkynes (nomenclature, structure and bonding, physical properties, addition to the triple bond, conversion of alkynes to aldehydes and ketones, reduction of alkynes, acidity of 1-alkynes, organic synthesis using alkynes, pheromones, occurrence and use of alkynes).

Laboratory work illustrates the concepts and principles discussed in lecture.

Physics 51L or 53L: Introductory Physics
(36 hrs lecture and 30 hrs laboratory/recitation, 1st semester, 2nd year, 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Tipler, P.A. Physics, 3rd edition; Worth, 1991.

Mechanics (motion in one dimension, motion in two and three dimensions, Newton's laws, work and energy, systems of particles and the conservation of momentum, rotation, static equilibrium of a rigid body, gravity, mechanics of solids and fluids); Oscillations and Waves (oscillations, waves on a string, sound); Thermodynamics (temperature, heat and the First Law of Thermodynamics, availability of energy).

Biology 21L: Introduction to Organismal and Environmental Biology
(36 hrs lecture and 48 hrs laboratory, 2nd semester, 1st year, 7.5 ECTS credits)
Continuous assessment of lecture and laboratory work; comprehensive final examination.

Text: Curtis, H.; Barnes, N.S. Biology, 5th edition; Worth, 1989.

Origin and evolution of unicellular organisms and plants, evolutionary processes, physiology of animals and plants, basic principles of genetics including population genetics, and ecology.

Chm 152L: Organic Chemistry
(36 hrs lecture, 48 hrs lab, 2nd semester, 2nd year, 7.5 ECTS credits)
Continuous assessment of lecture, recitation, and lab work; comprehensive final examination.

Text: Loudon, G.M. Organic Chemistry, 3rd edition; Benjamin, 1995.

Dienes, Resonance, and Aromaticity (structure and stability of dienes, UV spectroscopy, Diels-Alder reaction, addition of HX to conjugated dienes, diene polymers, resonance, aromaticity); Chemistry of Benzene and Its Derivatives (Nomencalture of benzene derivatives, physical properties, spectroscopy, electrophilic aromatic substitution reactions of benzene and its derivatives, hydrogenation of benzene derivatives); Allylic and Benzylic Reactivity (allylic and benzylic carbocations - SN1 reactions, bromination, Grignard reagents, SN2 reactions, side-chain oxidation of alkylbenzenes, isoprene rule, biosynthesis of terpenes); Chemistry of Aryl Halides, Vinylic Halides, and Phenols(SN2 reactions, elimination reactions of vinylic halides, lack of reactivity of vinylic and aryl halides in SN1 and E1 reactions, nucleophilic substitution reactions of aryl halides, aryl and vinylic Grignard reagents, acidity of phenols, otrher reactions of phenols); Chemistry of Aldehydes and Ketones - Carbonyl Addition Reactions (Nomenclature of aldehydes and ketones, physical properties, spectroscopy, synthesis, reactions, basicity, reversible addition reactions, reduction, reactions with Grignard reagents, acetals and protecting groups, reactions with amines, reduction of carbonyl groups to methylene groups, Wittig synthesis, oxidation of aldehydes); Chemistry of Carboxylic Acids (nomenclature, structure and properties, spectroscopy, acidity and basicity, fatty acids, soaps, detergents, synthesis, reactions, esters, acid chlorides, anhydrides, reduction to alcohols, decarboxylation); Chemistry of Carboxylic Acid Derivatives (nomenclature, structure, physical properties, spectroscopy, basicity, reactions, hydrolysis, reactions with nucleophiles, reduction, organometallic reagents, synthesis, occurrence and uses); Chemistry of Enols,Enolate Ions, and a,b-Unsaturated Carbonyl Compounds (acidity, enolization of carbonyl compounds, halogenation, aldol condensation, condensation reactions of ester enolate ions, alkylation of ester enolate ions, biosynthesis of compounds derived from acetate, conjugate addition reactions, reduction, organometallic reagents, organic synthesis with conjugate addition reactions); Chemistry of Amines (nomenclature, structure and properties, spectroscopy, acidity and basicity, quaternary ammonium salts, alkylation and acylation reactions, Hofmann elimination, aniline derivatives, diazonium ions, synthesis of amines, occurrence and use); Amino Acids, Peptides, and Proteins (nomenclature, stereochemistry, UV spectra, acid-base properties, synthesis and optical resolution, reactions, reactions of peptides, synthesis of peptides, structures of peptides and proteins, enzymes, occurrence of peptides and proteins); Carbohydrates and Nucleic Acids Classification of sugars, structures of monosaccharides, mutarotation of sugars, base-catalyzed isomerization of sugars, glycosides, ether and ester derivatives of sugars, redox of sugars, synthesis, proof of glucose stereochemistry, disaccharides and polysaccharides, nucleosides, nucleotides, and nucleic acids).
Laboratory work illustrates the concepts and principles discussed in lecture.

Physics 52L or 54L: Introductory Physics
(36 hrs lecture and 30 hrs laboratory/recitation, 2nd semester, 2nd year, 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Tipler, P.A. Physics, 3rd edition; Worth, 1991

Electricity and Magnetism (electric field: discrete and continuous charge distributions, electric potential, capacitance, dielectrics, and electrostatic energy, electric current, direct-current circuits, the magnetic field, sources of the magnetic field, magnetic induction, magnetism in matter, alternating-current circuits, Maxwell's equations and electromagnetic waves); Optics (light, geometrical optics, optical instruments, inteference and diffraction); Modern Physics (relativity, origins of the quantum theory, quantum mechanics, atoms, molecules, solids, nuclei, elementary particles, astrophysics and cosmology).

Biology 22L: Introduction to Cellular, Developmental and Molecular Biology
(36 hrs lecture and 48 hrs laboratory, 2nd semester, 1st year, 7.5 ECTS credits)
Continuous assessment of lecture and laboratory work; comprehensive final examination.

Text: Curtis, H.; Barnes, N.S. Biology, 5th edition; Worth, 1989.

Introduction to animal diversity and development, principles underlying the cellular and molecular bases of organismal structure and function.

Chm 161: Physical Chemistry
(36 hrs lecture, 1st semester, 3rd year, 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Atkins, P.W. Physical Chemistry, 5th edition; W.H. Freeman and Comp., 1994.

The Properties of Gases (the perfect gas, real gases); The First Law: the concepts (the basic concepts, work and heat, thermochemistry); The First Law: the Machinery (state functions and exact differentials, work of adiabatic expansion); The Second Law: the Concepts (direction of spontaneous change, efficiencies of thermal processes, concentrating on the system: Helmholtz and Gibbs energies); The Second Law: the Machinery (combining the first and second laws, the chemical potential, real gases: the fugacity); Physical Transformations of Pure Substances (Phase diagrams, phase stability, phase transitions); The Properties of Simple Mixtures (the thermodynamic description of mixtures, the properties of solutions, activities); Chemical Equilibrium (spontaneous chemical reactions, the response of equilibria to the conditions, applications to selected systems); Equilibrium Electrochemistry (thermodynamic properties of ions in solution, electrochemical cells, applications of standard potentials); Molecules in Motion (molecular motion in gases, the motion of molecules and ions in liquids, diffusion); The Rates of Chemical Reactions (empirical chemical kinetics, accounting for the rate laws); The Kinetics of Complex Reactions (chain reactions, polymerization reactions, catalysis and oscillation); Molecular Reaction Dynamics (reactive encounters, activated complex theory, dynamics of molecular collisions).

The lab work related to this course is given as a separate course: Chm 163L.

Chm 163L: Physical Chemistry Laboratory
(48 hrs laboratory, 1st semester, 3rd year, 3.75 ECTS credits)
Continuous assessment of laboratory work including an emphasis on writing formal laboratory reports.

Text: Duke Staff; Physical Chemistry Laboratory; 1994.

Introduction to the MATLAB program, treatment of experimental error, solution calorimetry, kinetics of enzyme reactions: activity of tyrosinase, heat of combustion: bomb calorimeter, reaction kinetics as a function of temperature: conductance meter, liquid-vapor equilibrium for a pure liquid, solid-liquid equilibria in a two-component system.

Bch 227. Introductory Biochemistry
(36 hrs lecture, 1st semester, 3rd year, 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Lehninger, A.L.; Nelson, D.L.; Cox, M.M. Principles of Biochemistry, 2nd Edition; Worth, 1993.

Foundations of Biochemistry (the molecular logic of life, cells, biomolecules, water:its effect on dissolved biomolecules); Structure and Catalysis (amino acids and peptides, introduction to proteins, the three dimensional structures of proteins, enzymes, lipids, biological membranes and transport, carbohydrates, nucleotides and nucleic acids); Bioenergetics and Metabolism (principles of bioenergetics, glycolysis and catabolism of hexoses, the citric acid cycle, oxidation of fatty acids, amino acid oxidation and the production of urea, oxidative phosphorylation and photophosphorylation, carbohydrate biosynthesis, lipid biosynthesis, biosynthesis of amino acids, nucleotides, and related molecules, integration and hormonal regulation of mammalian metabolism).

Chm 162L: Physical Chemistry
(36 hrs lecture and 48 hrs laboratory, 2nd semester, 3rd year, 7.5 ECTS credits)
Continuous assessment of lecture and lab work; comprehensive final examination.

Text: Atkins, P.W. Physical Chemistry, 5th edition; W.H. Freeman and Comp., 1994.

Quantum Theory: Introduction and Principles (origins of quantum mechanics, dynamics of microscopic systems, quantum mechanical principle); Quantum Theory: Techniques and Applications (translational motion, vibrational motion, rotational motion); Atomic Structure and Atomic Spectra (structure and spectra of hydrogenic atoms, structure of many-electron atoms, spectra of complex atoms); Molecular Structure (Valence-bond theory, molecular orbital theory, molecular orbitals for polyatomic systems); Molecular Symmetry (symmetry elements of objects, character tables); Spectroscopy: Rotational and Vibrational Spectra (general features of spectroscopy, pure rotation spectra, vibrations of diatomic molecules, vibrations of polyatomic molecules); Spectroscopy: electronic transitions (characteristics of electronic transitions, fates of electronically excited states, lasers, photoelectron spectroscopy); Spectroscopy: Magnetic Resonance (Nuclear magnetic resonance, pulse techniques in NMR, electron spin resonance); Statistical Thermodynamics: the concepts (distribution of molecular states, internal energy and entropy, canonical partition function); Statistical Thermodynamics: the Machinery (fundamental relations, using statistical thermodynamics).
Laboratory work illustrates the concepts and principles discussed in lecture.

Biology 160: Principles of Cell Biology
(36 hrs lecture, 2nd semester, 3rd year, 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Alberts, A.; Bray, D.; Lewis, J.; Raff, M.; Roberts, K.; Watson, J.D. Molecular Biology of the Cell, 3rd edition; Garland, 1994.

This course focuses on the structure and function of cells and cell organelles and includes details of replication and expression of genetic information as they occur in eukaryotic cells in general, biosynthjesis and function of membrane components, the molecular basis for cell and organelle motility. Specific topics: anatomy of the cell, nuclear structure, transcription, RNA structure and processing, ribosome biosynthesis, translation, cellular localization of new proteins, intracellular trafficking, exocytosis and endocytosis, properties of plasma membranes, membrane proteins, transport through membranes, membranes and cellular energetics, mitochondria and chloroplasts, cytoskelton, mitosis and meiosis, regulation of the cell cycle, cancer, cell signalling, cell surface and multicellularity, mechanisms of early development, the immune system.

Biology 180: Principles of Genetics
(36 hrs lecture, 2nd semester, 3rd year, 7.5 ECTS credits)
Continuous assessment of lecture work.

Text: Griffiths, Miller, Suzuki, Lewontin and Gelbart An Introduction to Genetic Analysis, 5th edition; 1993.

General topics include: transmission genetics in eukaryotes, population and quantitative genetics, microbial genetics, and molecular and developmental genetics. Specific topics include: physical structure of DNA and chromosomes, segregation and independent assortment of genes, chromosome basis of heredity, basic eukaryotic chromosome mapping, tetrad analysis and other mapping techniques, changes in chromosome structure and number, population genetics, quantitative genetics, bacterial genetics, phage genetics, molecular mechanisms of recombination, genes as units of function, transcription, translation and the genetic code, molecular basis of DNA mutation, DNA repplication and repair, plasmids, episomes and transposable elements, extranuclear genomes, genetic engineering, gene regulation in bacteria and viruses, gene regulation in eukaryotes, developmental genetics in eukaryotes, human molecular genetics.

Bch 228. Introductory Biochemistry
(36 hrs lecture, 1st semester, 3rd year, 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Lehninger, A.L.; Nelson, D.L.; Cox, M.M. Principles of Biochemistry, 2nd Edition; Worth, 1993.

Information Pathways (Genes and chromosones, DNA metabolism, RNA metabolism, protein metabolism, regulation of gene expression, recombinant DNA technology).

Chm 131: Analytical Chemistry
(36 hrs lecture, 1st semester, 4th year, 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Skoog, D.A.; West, D.M.; Holler, F.J. Fundamentals of Analytical Chemistry; 7th edition, Saunders, 1996.

Introduction (Role of analytical chemistry in the sciences, steps in a typical quantitative analysis); Errors in Chemical Analysis (Determinate errors, gross errors, indeterminate errors, standard deviation, methods of reporting analytical data); Statistical Evaluation of Analytical Data (statistical treatment of indeterminate errors, uses of statistics); Potentiometric Methods (principles, reference electrodes, liquid-junction potentials, indicator electrodes, instruments for measuring cell potentials, direct potentiometric measurements, potentiometric titrations, determination of equilibrium constants from electrode potential measurements); Electrogravimetric and Coulometric Methods (effect of current on cell potentials, potential selectivity of eletrolytic methods, electrogravimetric methods, coulometric methods); Voltammetry (excitation signals in voltammerty, linear-scan voltammetry, pulse polarographic and voltammetric methods, stripping methods); Introduction to Spectroscopic Methods of Analysis (properties of electromagnetic radiation, the electromagnetic spectrum, absorption of radiation, emission of electromagnetic radiation); Instruments for Optical Spectroscopy (instrument components, spectroscopic instruments); Molecular Absorption Spectroscopy (UV and VIS absorption spectroscopy, IR absorption spectroscopy, automation of photometric and spectrophotometric methods); Molecular-Fluorescence Spectroscopy (theory of molecular fluorescence, effect of concentration on fluorescence intensity, fluorescence instruments, applications of fluorescence methods); Atomic Spectroscopy based on UV and VIS Radiation comparison of atomic and molecular spectroscopic methods, atomic spectroscopy based on flame atomization, atomic absorption methods with electrothermal atomizers, atomic emission methods based on atomization in plasmas); Introduction to Chromatographic Methods (description of chromatography, migration rates of solutes, efficiency of chromatographic columns, optimization of column performance, applications of chromatography); Gas-Liquid Chromatography (principles of gas-liquid chromatography, instruments for gas-liquid chromatography, liquid phases for gas-liquid chromatography, applications of gas-liquid chromatography); High-Performance Liquid Chromatography (instruments for high-performance liquid, high-performance partition chromatography, high-performance adsorption chromatogrpahy, high-performance ion chromatography, high-performance partition chromatography, high-performance size-exclusion liquid chromatography, comparison of high-performance liquid chromatography and gas-liquid chromatography, supercritical-fluid chromatography).
The lab work related to this course is given as a separate course: Chm 133L.

Chm 133L: Analytical Chemistry Laboratory
(63 hrs laboratory, 1st or 2nd semester, 4th year, 3.75 ECTS credits)
Continuous assessment of laboratory work including an emphasis on writing formal laboratory reports.

Text: Duke Staff Analytcal Chemistry Laboratory; 1995.

Review of quantitative laboratory techniques, quantitative analysis of multicomponent fluorescent mixtures using chemometric analysis, use of generalized standard addition method of simultaneous spectrophotometric analysis of a two-component mixture (UV), atomic spectrometry: determination of calcium and magnesium in a sand with statistical treatment of measurements, neutron activation analysis: simplex version, gas chromatography, cyclic voltammetry and chronocoulometry, high performance liquid chromatography, gas chromatography with a mass selective detector, scanning tunneling micrscopy.

Chm 117: Inorganic Chemistry
(36 hrs lecture, 2nd semester, 4th year, 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Shriver, D.F.; Atkins, P.W.; Langford, C.H. Inorganic Chemistry, 2nd edition; W.H. Freeman and Comp., 1994.

Atomic Structure (origin of the elements, structure of hydrogenic atoms, many-electron atoms, atomic parameters); Molecular Structure (electron-pair bonds, molecular orbitals of diatomic molecules, molecular orbitals of polyatomic molecules, molecular orbital theory of solids); Molecular Shape and Symmetry (origin of molecular shape, molecular symmetry, the symmetries of molecular vibrations); Structures of Solids (crystal structure, metals, ionic solids); Acids and Bases (Bronsted acidity, periodic trends in Bronsted acidity, Lewis definitions of acids and bases, reactions of Lewis acids and bases, heterogeneous acid-base reactions); d-Metal Complexes (structures and symmetries, bonding and electronic structure, reactions of complexes); Oxidation and Reduction (extraction of the elements, reduction potentials, redox stability in water, diagrammatic presentation of potential data: Latimer, Frost, and Pourbaix diagrams); The Metals s-block metals, d-block metals, elements of Group 12, p-block metals, f-block metals); Hydrogen and its Compounds (the element, classification and structures of compounds, synthesis and reactions of hydrogen compounds, electron-deficient hydrides of the boron group, electron-precise hydrides of the carbon group, electron rich compounds of Groups 15/V to 17/VII); Main-Group Organometallic Compounds (Classification, nomenclature, and structure, ionic and electron-deficient compounds of Groups 1, 2, and 12, electron deficient compounds of the boron group, electron-precise compounds of the carbon group, electron-rich compounds of the nitrogen group); Boron and Carbon Groups (boron group, carbon group); Nitrogen and Oxygen Groups (nitrogen group, oxygen group); Halogen and the Noble Gases (halogens, noble gases).

Also selected topics from the following: Electronic Spectra of Complexes (electronic spectra of atoms, electronic spectra of complexes, bonding and spectra of simple clusters); Reaction Mechanisms of d-Block Complexes (ligand substitution reactions, substitution in square-planar complexes, substitution in octahedral complexes, redox reactions, photochemical reactions); d- and f-Block Organometallic Compounds (bonding, d-block carbonyls, other organometallic compounds, metal-metal bonding and metal clusters); Catalysis (general principles, homogeneous, heterogeneous); Structures and Properties of Solids (general principles, prototypical oxides and fluorides, prototypical sulfides and related compounds); Bioinorganic Chemistry (pumps and transport proteins, enzyme exploiting acid catalysts, redox catalysts).

Chm 180L: Advanced Chemistry Laboratory
(63 hrs laboratory, 2nd semester, 4th year, 3.75 ECTS credits)
Continuous assessment of laboratory work including an emphasis on writing formal laboratory reports.

Text: Duke Staff Inorganic Chemistry Laboratory; 1995.

Preparation of a copper complex and study of solvatochroism, synthesis and resolution of optically active coordination complexes and preparation of a macrobicyclic complex, preparation of cobaloximes as vitamin B12 models, preparation of (arene)M(CO)3 complexes (M = Mo, Cr) : use of a high pressure autoclave, preparation of an organotin complex using a Grignard reagent, use of a glove bag for the preparation of [PCl4][SbCl6] and [P(C6H5)3Cl][SbCl6], preparation and reactions of [Mo(CO)4(bpy)] : an experiment in organometallic chemistry.

Chm 191, 192, 193, 194 : Independent Study
(May be taken 1st and/or 2nd semesters, 3rd and/or 4th years, 7.5 ECTS credits/course)
Continuous assessment of project culminating in a written senior thesis.

Independent Study (Chemistry 191-192) is an opportunity for the highly motivated advanced student to work closely with a faculty member and his or her research group on a research project. The Department considers this research important both for its educational benefits and for the advancement of basic knowledge in the field of chemistry. Over the past decade the research results of independent study students in the Department have appeared in numerous publications in major professional chemistry journals, with the undergraduate student being listed as a co-author.

Chemistry 191-192 is available as an option for both B.S. and A.B. majors. Students interested in Chemistry 191-192 should obtain from the Director of Undergraduate Studies a listing of research projects available in the Department. While it is not anticipated that the research project will be originated by the student, it is expected that the student will provide a high degree of independent thought and effort in the solution of the problem. For this reason it is essential that a student have a firm foundation in the principles and practices of chemistry before attempting an independent project. This background is obtained by completing the laboratory courses through Chemistry 163L. Students normally take Chemistry 191-192 during their senior year; however, a student having AP credits may begin Chemistry 191 earlier.

An independent study student in the Department of Chemistry is treated like a beginning graduate student in a faculty supervisor's research group. Specific requirements concerning the number of hours spent in a laboratory, participation in research group conferences, and related activities are determined by the research director. Chemistry 191-192 is graded research and, as such, it is expected to represent at least 25% of the student's academic load. Normally this represents a minimum of 15 hours per week in the laboratory.

There are four other requirements to be completed as part of the independent study of either the A.B. or B.S. major. The first is participation in an orientation program covering safety in the research laboratory, the use of the chemical library, use of facilities, keeping a research notebook, and ethics in science. The second is a paper describing the research accomplished during the year for submission to the faculty supervisor. The third is an oral presentation of the background of the research project and proposed method of solving the problem in a seminar early in the second semester of the project. The fourth is participation in the Department's annual undergraduate research Poster Session held in April. This event provides an opportunity for students to communicate their results to other students and the faculty. The Department views these requirements as important exercises in learning to handle chemicals in a safe and responsible manner, in correlating and analyzing experimental data, and in communicating results to other members of the scientific community.

In instances where a student has begun independent study early and the research has gone well, there exists a possibility for continuation in Independent Study using Chemistry 193-194, but only upon recommendation of the research director and approval of the Director of Undergraduate Studies. If a student is continuing, there should be consultation with the research director to determine whether the paper may be delayed until the end of the project, with only an interim report being submitted upon completion of Chemistry 192.

Chemistry majors may also elect to pursue independent study in another science department of Trinity College, in the School of Engineering, or in a basic science department in the School of Medicine. Students in a Specialization Program must have, in addition, prior approval of the chemical relevance of the research project from the Specialization Programs Coordinator.

Chm 195S, 196S, 197S, 198S: Seminar
(36 hrs class, 1st and/or 2nd semester, 4th year, 7.5 ECTS credits each)

Topics from various areas of chemistry, changing each year. For example, organic chemistry of biologically important compounds, chemical basis of pharmacology, bioinorganic chemistry, selected topics in physical chemistry of biological macromolecules.

ADVANCED COURSES

Advanced courses, particularly those numbered 300 and above, may not be offered every academic year. Exchange students interested in taking 300 level course(s) should contact the Chemistry Department at Duke early in their planning process to establish the availability of these course(s).

Chm 201.01: Molecular Spectroscopy
(13 hrs lecture, 2.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Harris, D.C.; Bertolucci, M.D. Symmetry and Spectroscopy; Oxford University Press, 1978.

Chemist's View of Group Theory (symmetry operations and molecules, groups, point groups, classification of molecules into point groups, matrix representatioon of symmetry operations, characters and character tables, decomposition of reducible representations and the direct product); Quantum Mechanics* (light, postulates of quantum mechanics, simple illustrations from quantum mechanics); Vibrational Spectroscopy introduction, infrared and Raman spectra, diatomic molecules, transitions between stationary states, normal modes of vibration of poyatomic molecules, selection rules and polarization, symmetry coordinates and normal modes, stretching mode analysis, assignment of real spectra, the resonance Raman effect, functional group analysis); Molecular Orbital Theory* (introduction, atoms, photoelectron spectroscopy, the LCAO molecular orbital model, diatomic molecules, polyatomic molecules, the Hückel method, transition metal complexes); Electronic Spectroscopy (introduction, molecular vibrations, basic notations, selection rules, electronic spectra of some diatomic molecules, fate of absorbed energy, single bonds, double bonds, and lone pairs, vibronic analysis, transition metal complexes).

*Background reading - review only.

Chm 201.03: NMR Spectroscopy
(13 hrs lecture, 2.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Becconsall, J.K Basic One- and Two Dimensional NMR Spectroscopy, 2nd Edition; VCH, 1993.

The Physical Basis of NMR Spectroscopy (introduction, nuclear angular momentum and magnetic moment, nuclei in a static magnetic field, basic principles of NMR experiment, the pulsed NMR method, spectral parameters: chemical shift, nuclear shielding, reference compounds, spin-spin coupling, indirect spin-spin coupling, coupling to one neighboring nucleus, coupling to two equivalent neighboring nuclei, coupling to three or more equivalent neighboring nuclei, multiplicity rules, coupling between three non-equivalent nuclei, order of a spectrum, couplings between protons and other nuclei, intensities of resonance signals, 1H signal intensities, 13C signal intensities, nuclides with I = 1/2, nuclides with I > 1/2); The Chemical Shift (introduction, 1H chemical shifts of organic compounds, 13C chemical shifts of organic compounds, relationships between spectrum and molecular structure); Indirect Spin Coupling (H,H coupling constants and chemical structure, C,H coupling constants and chemical structure, coupling mechanism, coupling of other nuclides); Spectrum Analysis and Calculations, Double Resonance Experiments, Assignment of 1H and 13C Signals, Relaxation (introduction, spin-lattice relaxation of 13C nuclei, spin-spin relaxation); One-Dimensional NMR Experiments introduction, simple pulse experiments, the J-modulated spin-echo experiment, signal enhancement by polarization transfer, the DEPT experiment, the one-dimensional INADEQUATE experiment); Two-Dimensional NMR Spectroscopy (introduction, the two-dimensional NMR experiment, two-dimensional J-resolved NMR spectroscopy, two-dimensional correlated NMR spectroscopy); The Nuclear Overhauser Effect introduction, theoretical background); Shift Reagents.

Chm 203.01: Foundations of Quantum Chemistry and Quantum Mechanics
(13 hrs lecture, 2.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Atkins, P.W. Molecular Quantum Mechanics, 3rdd Edition; Oxford, 1997.

Historical Introduction* (black-body radiation, heat capacities, the photoelectric effect, the Compton effect, atomic spectra, wave nature of matter, the uncertainty principle); The Schrödinger Equation (Heisenberg's suggestion, Hamilton's contribution, Schrödinger's Equation, Born's interpretation, quantization); The Properties of Operators (the postulates of quantum mechanics, Hermitian operators, the specific states: complementarity, the uncertainty principle, time evolution and conservation laws, matrices in quantum mechanics); Exact Solutions: Linear Motion (translational motion, potential barriers and tunnelling, particle in a box, the two-dimensional square well, the harmonic opscillator); Exact Solutions: Rotational Motion (particle on a ring, particle on a sphere, motion in a Coulomb field: the hydrogen atom, atomic orbitals).

*Background reading - review only.

Chm 203.02: Foundations of Quantum Chemistry and Quantum Mechanics: Approximate Methods.
(13 hrs lecture, 2.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Atkins, P.W. Molecular Quantum Mechanics, 3rd Edition; Oxford, 1997.

Techniques of Approximation (time-independent perturbation theory, perturbation theory for degenerate states, variation theory); Atomic Spectra and Atomic Structure (the structure of the helium atom); Molecular Structure (the Born-Oppenheimer approximation, the hydrogen molecule-ion, the molecular orbital method); Angular Momentum (the angular momentum operators, the shift operators, the eigenvalues of the angular momentum, the eigenfunctions of the angular momentum, spin); Atomic Spectra and Atomic Structure (the spectrum of helium and the Pauli principle, the periodic table, ionization energies, approximate atomic orbitals, self-consistent field fields); Molecular Structure (the valence bond method, comparison of the methods, the structures of diatomic molecules, the structures of polyatomic molecules, hybridization and bond angles, conjugated -systems).

Chm 203.03: Applications of Molecular Orbital Theory in Organic Chemistry
(13 hrs lecture, 2.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Fleming, I. Frontier Orbitals and Organic Chemical Reactions; Wiley, 1976.

Molecular Orbitals and Frontier Orbitals (chemical bonds: conjugation-Hückel theory, frontier orbitals: HUMO and LUMO); Ionic Reactions (the principle of hard and soft acids and bases (HSAB), ambident nucleophiles: charged nucleophiles: aromatic electrophilic substitution); Thermal Pericyclic Reactions (The Woodward-Hoffman rules: cycloaddition, the rates of cycloadditions, estimating energies and coefficients of the frontier orbitals of dienes and dienophiles, examples of regioselectivity: regioselectivity in 1,3-dipolar cycloadditions).

Chm 205.01: Structure and Reaction Dynamics.
(13 hrs lecture, 2.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Lowry, T.H.; Ruchardson, K.S. Mechanism and Theory in Organic Chemistry, 3rd Edition; Harper & Row, 1987.

Fundamentals of Physical Organic Chemistry (stereochemistry, linear-free-energy relationships, thermochemistry); Reactions of Carbonyl Compounds (hydration and acid-base catalysis, other simple additions, addition followed by elimination, addition of nitrogen nucleophiles, carboxylic acid derivatives, enols, enolates, and addition of carbon nucleophiles to C=O); Molecular Mechanics: Calculations and Techniques.

Chm 205.02: Stereochemistry of Organic Compounds.
(13 hrs lecture, 2.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Eliel, E.L.; Wilen, S.H.; Mander, L.N. Stereochemistry of Organic Compounds, 2nd Edition; Wiley, 1994.

Structure (consitution, configuration, conformation); Stereoisomers (nature of stereoisomers, enantiomers, diastereomers); Configuration (definitions: relative and absolute configuration, absolute configuration and notation); Separation of Stereoisomers, Resolution, Racemization (chemical separation of enantiomers via diastereomers); Heterotropic Ligands and Faces (Prostereoisomerism, Prochirality) (homotropic and heterotropic ligands and faces, heterotopicity and nuclear magnetic resonance, heterotropic ligands and faces in enzyme-catalyzed reactions); Conformation of Acyclic Molecules (conformation of ethane, butane, and other simple saturated acyclic molecules, conformation of unsaturated acyclic and miscellaneous compounds, conformation and reactivity: the Weinstein-Holness equation and the Curtin-Hammett principle); Configuration and Conformation of Cyclic Molecules (stereoisomerism and configurational nomenclature of ring compounds, conformational aspects of the chemistry of six-membered ring compounds); Stereoselective Syntheses (introduction: stereoselective synthesis, diastereoselective synthesis, enantioselective syntheses).

Chm 205.03: Kinetics, Mechanism, and Stereochemistry of Reactions of Coordination and Organometallic Compounds.
(13 hrs lecture, 2.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Miessler, G.L.; Tarr, D.A. Inorganic Chemistry ; Prentice Hall, 1991.

Chemistry of the Main Group Elements (general trends in main group chemistry, hydrogen, Group 1, Group 2, Group 13, Group 14, Group 15, Group 16, Group 17, Group 18); Coordination Chemistry III: Structures and Isomers (nomenclature, common structures, four- and six-coordinate preferences, isomerism); Coordination Chemistry IV: Reactions and Mechanisms (historical background, organic ligands and nomenclature, the 18-electron rule, ligands in organometallic chemistry, bonding between metal atoms and organic pi systems, complexes containing metal-carbon sigma bonds, spectral analysis and characterization of organometallic complexes); Organometallic Reactions and Catalysis (reactions involving gain or loss of ligands, reactions involving modification of ligands, organometallic catalysts, heterogeneous catalysts); Parallels between Main Group and Organometallic Chemistry (main group parallels with binary carbonyls complexes, the isobal analogy, cluster compounds).

Chm 207.01: Chemical Kinetics
(13 hrs lecture, 2.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Laidler, K.J. Chemical Kinetics; Harper and Row, 1987.

Basic Kinetic Concepts (reaction stoichiometry, rates of consumption and formation, extent of reaction, rate of reaction, volume change during a reaction, empirical rate equations, elementary, composite, and chain reactions, catalysis and inhibition, influence of temperature on reaction rates); Composite Reactions (types of composite reactions, rate equations for composite mechanisms, chain reactions); Theories of Reaction Rates (microscopic reversibility and detailed balance); Energy of Activation (statistical distribution of molecular energies, potential energy surfaces, ab initio calculations of potential energy surfaces, semiempirical calculations of potential energy surfaces, empirical treatments of activation energy); Theories of Reaction Rates (kinetic theory of collisions, rate theories based on thermodynamics, rate theories based on statistical mechanics, early dynamical theories of rates, conventional transition-state theory, applications, thermodynamic formulation of conventional transition-state theory, assumptions and limitations of conventional transition state theory, extensions of transition-state theory); Elementary Gas Phase Reactions (bimolecular reactions, trimolecular reactions, unimolecular reactions, combination and disproportionation reactions); Elementary Reactions in Solutions (solvent effects on reaction rates, factors determining reaction rates in solution, reactions between ions, ion-dipole and dipole-dipole reactions, influence of hydrostatic pressure, diffusion-controlled reactions); Analysis of Kinetic Results (reactions in flow systems, techniques for very fast reactions); Photochemical Reactions (Rotating-sector technique, flash photolysis).

Chm 207.02: Chemical Thermodynamics
(13 hrs lecture, 2.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Reid, C.E. Chemical Thermodynamics; McGraw-Hill Publishing Company, 1990.

Symbols, Units, and Mathematical Methods* (symbols and units, thermodynamic notation for partial derivatives, change of variable in differentiation, exact differentials and line lengths, homogeneous functions); Introduction and Basic Laws* (basic definitions, the First Law of Thermodynamics, enthalpy, thermal equilibrium, reversible and irreversible changes, intensive and extensive properties, the Second Law, statements of the Second Law, the Carnot cycle, practical consequences of the Second Law); Equilibrium and the Free Energy Functions (equilibrium at constant energy and volume, equilibrium at constant temperature and volume, equilibrium at constant temperature and pressure, some important general relations, properties of temperature, pressure and volume changes, stable, metastable, unstable, and neutral equilibria, nomenclature and units, the Clapeyron equation); Mixtures and Solutions (the chemical potential, partial molar quantities, equations of the Gibbs-Duhem type, the determination of partial molar quantities, relations among partial molar quantities, ideal mixtures); Chemical Equilibrium (fundamental equilibrium expression for a chemical reaction, the equilibrium constant, variation of equilibrium constant with temperature, calculation of equilibrium constants from calorimetric or spectrometric data); Statistical Thermodynamics general principles and definitions, the Boltzman H-Theorem, entropy postulate, distribution of systems in equilibrium, relation of the partition function to thermodynamic properties, the Einstein crystal model, changing the zero of the energy scale, factorization of the partition function, the ideal monatomic gas, diatomic gases, polyatomic gases, properties of ideal mixtures, the Debye crystal model, Planck's radiation equation, statistical thermodynamics and the Third Law, ortho- and para-hydrogen, statistical thermodynamics of solutions, statistical mechanics of chemical equilibrium); Gases (the thermodynamics of nonideal gases, standard states, fugacities of liquids and solids, experimental p-v-T data and the equation of state for real gases, the principle of corresponding states, the van der Waals equation); Mixtures and Solutions (non-ideal mixtures: rational activities, the colligative properties; the determination of solvent activities, solvent activity at other temperatures and pressures, applications of the Gibbs-Duhem equation to activities, the molal activity scale).

*Background reading - review only.

Chm 207.03: Structure Determination by X-ray Crystallography
(13 hrs lecture, 2.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Ladd, M.F.C.; Palmer, R.A. Structure Determination by X-ray Crystallography, 3rd Edition; Plenum Press, 1993.

Crystal Geometry I (introduction, the crystalline state: Miller indices, stereographic projection, external symmetry of crystals: two- and three-dimensional point groups); Crystal Geometry II (introduction, lattices: two-dimensional lattices: choice of unit cell, three-dimensional-lattices, families of planes and interplanar spacings, reciprocal lattice: truth of reciprocal lattice, rotational symmetries of lattices, space groups: two-dimensional space groups: plane groups related to 2mm: three-dimensional space groups: screw axes:glide planes: analysis of space-group symbol); Preliminary Examination of Crystals by Optical and X-ray Methods (introduction, polarized light, optical classification of crystals: uniaxial crystals: birefringence: biaxial crystals, direction of scattering of X-rays by crystals: Laue equations for X-ray scattering: Bragg's treatment of X-ray diffraction: equivalence of Laue and Bragg treatments of X-ray diffraction, X-ray techniques: Laue method:oscillation method: Ewald's construction: Weissenberg method: precession method, recognition of crystal system); Scattering of X-rays by Crystals (introduction, path difference, mathematical representation of a wave: amplitude and phase, combination of two waves, Argand diagram, combination of N waves, combined scattering of X-rays from the contents of the unit cell: phase difference: scattering by atoms, structure factor, intensity expressions, phase problem in structure analysis, applications of the structure factor equation: Friedell's law, structure factor for a centrosymmetric crystal: limiting conditions and systematic absences: determination of unit-cell type: structure factors and symmetry elements: limiting conditions from screw-axis symmetry: centrosymmetric zones: limiting conditions from glide-plane symmetry, preliminary structure analysis: practical determination of space groups); Fourier Transform Theory (structure solution methods in brief: use of heavy atoms); Techniques of X-ray Structure Determination (introduction, analysis of the unit-cell contents: special positions, methods of solving the phase problem: the Patterson function, heavy-atom method and partial Fourier synthesis); Schonflies' Symmetry Notation (alternating axis of symmetry, notation); Generation and Properties of X-rays (X-rays and white radiation, characteristics of X-rays, absorption of X-rays, filtered radiation).

Chm 300: Statistical Mechanics
(36 hrs lecture, 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Chandler, D. Introduction to Modern Statistical Mechanics ; Oxford, 1987.

Thermodynamics, Fundamentals (First law of thermodynamics and equilibrium, Second law, variational statement of Second law, application: thermal equilibrium and temperature, auxiliary functions and Legendre transforms, Maxwell relations, extensive functions and the Gibbs-Duhem equation, intensive functions); Conditions for Equilibrium and Stability (multiphase equilibrium, stability, application to phase equilibria, plane interfaces); Statistical Mechanics (the statistical method and ensembles, microcanonical ensemble and the rational foundation of thermodynamics, canonical ensemble, generalized ensembles and the Gibbs entropy formula, fluctuations involving uncorrelated particles, alternative development of equilibrium distribution functions); Non-Interacting (Ideal) Systems (occupation numbers, photon gas, phonon gas or fluctuations of atomic positions in a cold solid, ideal gases of real particles, electrons in metals, classical ideal gases, the classical limit, thermodynamics of an ideal gas of structureless classical particles, a dilute gas of atoms, dilute gas of diatomic molecules, chemical equilibria in gases); Statistical Mechanical Theory of Phase Transitions (Ising model, lattice gas, broken symmetry and range of correlations, mean field theory, variational treatment of mean field theory, renormalization group theory, RG theory for the two-dimensional Ising model); Classical Fluids (averages in phase space, reduced configurational distribution functions, reversible work theorem, thermodynamic properties from g(r), measurement of g(r) by diffraction); Statistical Mechanics of Non-Equilibrium Systems (systems close to equilibrium, Onsager's regression hypothesis and time correlation functions, chemical kinetics, self-diffusion, fluctuation-dissipation theorem, response functions, absorption, friction and Langevin equation).

Chm 302: Quantum Chemistry
(36 hrs lecture, 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Schatz, G.C.; Ratner, M.A. Quantum Mechanics in Chemistry; Prentice-Hall, 1994.

Review of Basic Concepts in Quantum Mechanics (fundamental definitions, eigenvalues and eigenfunctions, approximate methods, raising and lowering operators, two-body problems, electronic structure of atoms and molecules); Symmetry Considerations: Point Groups and Electronic Structure (group theory for point groups, applications of group theory to quantum mechanics, symmetry properties of many-electron wavefunctions); Symmetry Considerations: Continuous Groups and Rotations (introduction, continuous groups; the electronic structure of linear molecules, three-dimensional rotation group; angular momentum addition); Time-Dependent Quantum Mechanics (introduction, time-dependent Schrödinger equation; basis set solution, time-dependent perturbation theory, representations in quantum mechanics, transition probabilities per unit time); Interaction of Radiation with Matter (introduction, electromagnetic fields, interaction between matter and field, absorption and emission of light, light scattering); Occupation Number Representations (introduction, occupation number representation for harmonic molecular vibrations and quantized radiation fields, occupation number representations for electrons, Fermion field operators and second quantization, molecular electronic structure: model hamiltonians and occupation number representations, treatment of interacting electrons); Time-Dependent Approach to Spectroscopy: Electronic, Vibrational, and Rotational Spectra (introduction, thermal averages and imaginary time propagation, electronic spectra from time correlation functions, electronic spectra: time development of the correlation function approach, rotational, Raman, and magnetic resonance spectra, motional narrowing and stochastic motion); Density Matrices (introduction, density operators and density matrices: definitions and averages, representations and equations of motion, Examples: spin-1/2 particles, reduced density matrices, reduced density matrices for dynamical statistical systems, higher order corrections to the density matrix: pulsed spectroscopy.

Chm 306: Principles and Applications in Biophysical and Physical Chemistry
(24 or 36 hrs lecture, 5.0 or 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

The interrelationships between structure, function, and mechanisms of biological macromolecules, principles of dynamics (including kinetics, reactivity, and transport) and structure (including thermodynamics, NMR, fluoescence, CD spectroscopy, and other applicable biophysical techniques.

Chm 310: Electronic Structure and Spectroscopy of Transition metal Compounds
(24 hrs lecture, 5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Drago, R.S. Physical Methods for Chemists, 2nd Edition; Saunders, 1992.

Symmetry and Point Groups* (Definition of symmetry, symmetry elements, point groups, space symmetry); Group Theory and Character Tables* (rules for elements that constitute a group, group multiplication tables, summary of properties of vectors and matrices, representations: geometric transformations, character tables, non-diagonal representations, decomposition formula, direct products); General Introduction to Spectroscopy* (radiation, energies, atomic and molecular transitions, selection rules, relaxation and chemical exchange influences on spectral line width, determination of concentration, isobestic points, Job's method, fingerprinting); Electronic Absorption Spectroscopy* (vibrational and electronic energy levels in a diatomic molecule, potential energy curves and spectra, assignment of transitions, oscillator styrengths, transition moment integral, derivation of some selection rules, spectrum of formaldehyde, spin-orbit and vibronic coupling contributions to intensity, mixing d and p orbitals, magnetic dipole and electric quadrupole contributions to intensity, charge transfer transitions, polarized absorption spectra, applications, optical rotary dispersion, circular dichroism, and magnetocircular dichroism); Electron Paramagnetic Resonance Spectroscopy* (nuclear hyperfine splitting, anisotropic effects); The Electronic Structure and Spectra of Transition Metal Ions (electron-electron interactions and term symbols, spin-orbit coupling in free ions, effects of ligands on the d orbital energies, symmetry aspects of the d orbital splitting by ligands, double groups, Jahn-Teller effect, magnetic coupling in metal ion clusters, survey of the electronic spectra of Oh complexes, calculation of Dq and b for Oh Ni(II) complexes, effect of distortions on the d orbital energy levels, structural evidence from electronic spectrum, s and p bonding parameters from the spectra of tetragonal complexes, angular overlap model, electronic spectra of oxo-bridged dinuclear iron centers, intervalence electron transfer bands, photoreactions); Magnetism (types of magnetic behavior, Van Vleck's equation, applications of susceptibility measurements, intramolecular effects, high spin-low spin equilibria, measurement of magnetic susceptibilities, superparamagnetism); Electronic Paramagnetic Resonance Spectra of Transition Metal Ion Complexes (interpretation of the g-values, hyperfine couplings and zero field splittings, ligand hyperfine couplings, EPR spectra of first row transition metal ion complexes, EPR of metal clusters, double resonance and Fourier transform EPR techniques).

*Background reading - review only.

Chm 312: Chemistry of the Main Group Elements and Organometallic Chemistry of Transition Elements.
(24 hrs lecture, 5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Part I. Chemistry of the Main Group Elements.
Text: King, R.B. Inorganic Chemistry of Main Group Elements; VCH Publishers, 1995.

Preparations, bonding, structures, and reactivity of compounds of the main group elements with emphasis on members of the p-block groups. Specific topics include: Silicon, Germanium, Tin, Lead (general aspects, elements, anions and related binary compounds, hydrides and halides, silicates and related oxygen compounds, other oxygen compounds, organometallic derivatives, divalent compounds); Nitrogen (general aspects, isotopes and elemental nitrogen, nitrides, hydrogen compounds, oxides, oxoacids and oxoanions, nitrogen-halogen compounds); Phosphorus, Arsenic, Antimony, and Bismuth (general aspects, the elements, phosphides, arsenides, antimonides, and bismuthides, halides, oxides, sulfides and other chalcogenides, oxoacids and oxoanions, phosphorus-nitrogen compounds, organic derivatives, cationic chemistry in aqueous solutions); The Chalcogens (general aspects, the elements, compounds with O-O bonds, binary compounds of S and its heavier cogeners with H and metals, S-N compounds, halides, oxoacids and oxoanions, miscellaneous Se and Te compounds); Halogens and Noble Gases (general aspects, the elements, halides, halogen oxides, oxoacids and oxoanions, interhalogen and polyhalogen compounds: cations and anions, other halogen compounds, noble gas compounds); Boron (general aspects, the element and metal borides, boranes and related compounds, boron halides and their derivatives, B-O compounds, organoboron compounds, B-N derivatives); Aluminum, Gallium, Indium, and Thalium(general aspects, the elements and their alloys, aqueous solution chemistry of trivalent ions, oxygen derivatives of trivalent elements, halogen derivatives, hydride derivatives, other binary compounds, organometallic compounds, lower oxidation states than 3); The Alkali and Alkaline Earth Netals (general aspects, the elements, compounds, Be chemistry, Chemistry of Mg, Ca, Sr, and Ba); Zinc, Cadmium, and Mercury (general aspects, the elements, divalent compounds, organometallic compounds, oxidations states lower than 2).

Part II. Organometallic Chemistry of Transition Elements.

Text: Crabtree, R.H. Organometallic Chemistry of Transition Elements; 2nd Edition; Wiley, 1994.

Introduction (Werner complexes, the trans effect, soft versus hard ligands, the crystal field, the ligand field, back bonding, electroneutrality, types of ligands); General Properties of Organometallic Complexes (the 18-electron rule, limitations of the 18-electron rule, electron counting in reactions, oxidation state, coordination number and geometry, effects of complexation, different metals); Metal Alkyls, Aryls, and Hydrides and Related s-Bonded Ligands (the stability of transition metal alkyls and aryls, the preparation of metal alkyls, characterization and properties of metal alkyls, related s-bonded ligands, metal hydride complexes, bond strengths for classical s-bonding ligands); Carbonyls, Phosphine Complexes, and Ligand Subsitution Reactions (metal complexes of CO, RNC, CS, and NO, phosphines as ligands, dissociative substitution, the associative mechanism, redox effects, the I mechanism, and rearrangements in substitution, photochemical substitution, steric and solvent effects in substitution); Complexes of -Bound Ligands (alkene and alkyne complexes, allyl complexes, diene complexes, cyclopentadienyl complexes, complexes of arenes and other alicyclic ligands, metalacycles and isoelectronic and isolobal replacement, stability of polyene and polyenyl complexes); Oxidative Addition and Reductive Elimination (three-center additions, SN2 reactions, radical mechanisms, ionic mechanisms, reductive elimination, oxidative coupling and reductive cleavage); Insertion and Elimination reactions involving CO, insertions involving alkenes, other insertions, a,b, g, and d eliminations). Chm 314: Advanced Inorganic Reaction Mechanism
(24 hrs lecture, 5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Ligand substitution reactions at a transition metal center: introduction to mechanistic concepts; relationships between activation mode and entering group, leaving group, steric crowding and charge; interchange mechanism for octahedral complexes; experimental basis for dissociative, D, classification; mechanism of stereochemical rearrangement; application of stereochemical data to the elucidation of acid and base hydrolysis mechanisms in octahedral complexes; substitution reactions in square planar complexes; linear free energy relationships in substitution reactions of square planar complexes; mechanism of oxidation and reduction reactions; reactions and mechanisms of transition metal organometallic compounds.

Chm 320: Synthetic Organic Chemistry
(36 hrs lecture, 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Carey, F.A.; Sundberg, R.J. Advanced Organic Chemistry, part B: Reactions and Synthesis, 3rd Edition; Plenum Press, 1990.

Alkylation of Nucleophilic Carbon, Enolates and Enamines (generation of carbanions by deprotonation, regioselectivity and stereoselectivity in enolate formation, other means of generating enolates, alkylation of enolates, generation and alkylation of dianions, medium effects in the alkylation of enolates, oxygen versus carbon as the site of alkylation, alkylation of aldehydes, esters, amides, and nitriles, the nitrogen analogs of enols and enolates - enamines and imine anions, alkylation of carbon nucleophiles by conjugate addition); Reactions of Carbon Nucleophiles with Carbonyl Groups (aldol condensation, condensation reactions of imines and iminium ions, acylation of carbanions, the Wittig and related reactions, reactions of carbonyl compounds with a-trimethylsilyl carbanions, sulfur ylides and related nucleophiles, nucleophilic addition-cyclization); Functional Group Interconversion by Nucleophilic Substitution (conversion of alcohols to alkylating agents, introduction of functional groups by nucleophilic substitution at saturated carbon, nucleophilic cleavage of carbon-oxygen bonds in ethers and esters, interconversion of carboxylic acid derivatives); Electrophilic Addition to Carbon-Carbon Multiple Bonds (oxymercuration, electrophilic sulfur and selenium reagents, addition to double bonds via organoboranes); Reduction of Carbonyl and Other Functional Groups (addition of hydrogen, Group III hydride-donor reagents, Group IV hydride donors, hydrogen atom donors, dissolving-metal reductions, reductive deoxygenation of carbonyl groups); Cycloadditions, Unimolecular Rearrangments, and Thermal Eliminations (cycloaddition reactions, dipolar cycloaddition reactions, [2 + 2] cycloadditions and other reactions leading to cyclobutanes, photochemical cycloaddition reactions); Organometallic Compounds of Group I and II Metals (preparation and properties of organolithium and organomagnesium compounds, reactions organolithium and organomagnesium compounds); Reactions Involving the Transition Metals (reactions of organocopper intermediates, reactions involving organopalladium intermediates, reactions involving rhodium, iron, and cobalt); Carbon-Carbon Bond-Forming Reactions of Compounds of Boron, Silicon, and Tin (organoboron compounds, organosilicon compounds, organotin compounds); Reactions Involving Carbenes and Nitrenes (structure and reactivity of carbenes, generation of carbenes, addition reactions, insertion reactions, rearrangement reactions, related reactions, nitrenes and related intermediates, rearrangements to electron-deficient nitrogen); Oxidations (oxidation of alcohols to aldehydes, ketones, or carboxylic acids, addition of oxygen at C=C, cleavage of C=C, selective oxidative cleavages at other functional groups, oxidation of ketones and aldehydes, allylic oxidation, oxidations at unfunctionalized carbon); Multistep Syntheses (protective groups, synthetic equivalent groups, synthetic analysis and planning, control of stereochemistry, illustrative syntheses). Chm 322: Organic Reactive Intermediates.
(36 hrs lecture, 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

A discussion of reactive intermediates in organic chemistry: carbanions, carbenes, carbonium ions, free radicals, photochemical excited states and other reactive species.

Chm 326: Bioorganic Chemistry
(36 hrs lecture, 7.5 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Walsh, C. Enzymatic Reaction Mechanisms; Freeman, 1979.

An investigation of biochemical principles from the viewpoint of the organic chemist, fundamental and applied enzymology, enzyme inhibition, enzyme models, biosynthetic pathways, methodology for the study of biological transformations, molecular biology for organic chemists. Topics include: enzymes and enzymatic catalysis, acyl transfer to water: endopeptidases and exopeptidases, g-glutamyl transfers and amino transfers, phosporyl transfers, 1: phosphatases, ATpases and phosphodiesterases, kinases, nucleotidyl and pyrophosphoryl transfers, glycosyl transfers, enzymatic oxidations and reductions via apparent hydride transfers: nicotinamide coenzymes, flavin dependent dehydrogenases and oxidases, enzyme-catalyzed Aldol and Claisen condensations, enzymatic reactions requiring pyridoxal phosphate, enzymatic C1-group transfers requiring tetrahydrofolate or S-adenpsylmethinone, enzyme catalyzed alkylations involving prenyl-group transfer

Chm 330: Separation Science
(24 hrs lecture, 5.0 ECTS credits)
Continuous assessment of lecture work.

Fundamental separation chemistry; practical aspects of chromatographic methods.

Chm 334: Electroanalytical Chemistry
(24 hrs lecture, 5.0 ECTS credits)
Continuous assessment of lecture work.

Text: Brett, C.M.; Brett, A.M.O. Electrochemistry; Oxford University Press, 1993.

Introduction (basic electrical terms and concepts, electrode and electrochemical systems, general aspects of charge-transfer processes, reduction potentials and free energy, review of solution ionics: electrolytes and ionic strength: activity coefficients: standard states: development of the Nernst equation); Equilibrium Measurements (eletrochemical cell notation, redox reactions, calculation of cell potentials, batteries, fuel cells, sensors, potentiometry and ion-selective electrode: pH measurements and the glass electrode: cation-selective glass electrodes: solid-state membrane electrodes: ion-exchange and neutral carrier membranes: gas-sensing electrodes: potentiometric enzyme electrodes); Dynamic Electrochemical Measurements (review of basic kinetic expressions: the Arrhenius equation: the Butler-Volmer equation for electrode kinetics: the Tafel equation, mass transport to an electrode surface: diffusion: convection: migration, potential step and pulse techniques and their applications: chronoamperometry and chronocoulometry: normal pulse voltammetry: differential pulse and square wave voltammetry, polarography and anodic stripping voltammetry, cyclic voltammetry); Special Topics (ultramicroelectrodes, scanning probe microscopes: scanning tunneling microscopy: atomic force microscopy: other probe types: scanning electrochemical microscopy, spectroelectrochemistry, chemically-modified electrodes, biosensors).

Chm 336: Analytical Spectroscopy
(24 hrs lecture, 5.0 ECTS credits)
Continuous assessment of lecture work; comprehensive final examination.

Text: Ingle, J.D.; Crouch, S.R. Spectrochemical Analysis: Prentice Hall, 1988.

Spectrochemical Information (radiation/matter interactions, nature of spectrochemical analysis: types of analyses: samples: spectrochemical phenomena: analysis of real samples, expressions of analytical information: calibration data: atomic and molecular spectra: optimization of the response function, evaluation criteria in spectrochemical techniques: practical considerations: automation and multiple species capability: interferences and selectivity: figures of merit); Spectrochemical Measurements (complete spectrochemical measurement, expressions of optical intensity: radiometric system: photometric system, spectrochemical methods: emission spectroscopy: absorption spectroscopy: luminescence spectroscopy: scattering methods, selection of optical information: wavelength selection: other selection criteria); Methodology in Spectrochemical Analysis (external standard calibration, systematic errors in spectrochemical methods: matrix errors: calibration errors: sample acquisition, preparation, and measurement errors, random errors in spectrochemical errors: determination of standard deviation in concentration: statistical statements: other considerations, sensitivity and detection limit, techniques for minimization of systematic and random errors: separations: saturation, buffer, and masking methods: dilution, matrix match, and parametric methods: methods of standard additions: methods based on optical encoding: chemical selectivity: instrument correction methods, automated spectrochemical measurements); Introduction to Atomic Spectroscopy (sample introduction and atomization: nebulizers: free-atom formation after nebulization: free-atom formation with discrete sample introduction, interferences in atomic spectroscopy: blank: analyte, electronic states of atoms: quantum numbers: coupling schemes: term symbols: selection rules and atomic spectra: additional splitting effects: statistical weights and partition functions, spectral line profiles: lifetime broadening: Doppler broadening: other causes of broadening: overall line profiles, spectral line intensities: thermal emission: absorption: atomic fluorescence); Introduction to Molecular Spectroscopy (molecular spectra, rotational spectra, vibrational spectra: pure vibrational transitions: rotation-vibrational transitions, electronic absorption spectra of diatomic molecules: electronic states: electronic transitions, electronic absorption spectra of polyatomic molecules: electronic states and transitions: electronic spectra: electronic band shapes and intensities, luminescence spectra: processes of deactivation: quantum efficiencies and power yields: luminescence lifetimes: quenching and excited-state reactions: band shapes: structural effects: environmental effects: polarization of luminescence); Ultraviolet and Visible Molecular Absorption Spectrophotometry (instrumentation, signal and noise expressions, apparent deviations from Beer's Law, methodology and performance characteristics, applications); Molecular Luminescence Spectrometry (instrumentation, signal and noise expressions, molecular fluorescence spectrometry, molecular phosphorescence spectrometry, chemiluminescence, lifetime and polarization measurements).