Course code:
029B2		 Course name:
Physical Chemistry

Academic year:

2023/2024.

Attendance requirements:

001A2 / 101K2

ECTS:

7

Study level:

basic academic studies

Study program:

Biochemistry: 2. year, winter semester, compulsory course

Teachers:

Dragomir R. Stanisavljev, Ph.D.
full professor, Faculty for Physical Chemistry, Studentski trg 12-16, Beograd

Nemanja M. Gavrilov
associate professor, Faculty for Physical Chemistry, Studentski trg 12-16, Beograd

Assistant:

Maja M. Rankoviæ
assistant, Faculty for Physical Chemistry, Studentski trg 12-16, Beograd

Hours of instruction:

Weekly: four hours of lectures + three hours of labwork (4+0+3)

Goals:

The main goal of this course is to help biochemistry students acquire the essential general knowledge in the field, which should help them understand some of the courses in the later years of their studies. It introduces students to the basic physicochemical concepts and the determination of important variables.

Outcome:

Students will learn to thermodynamically describe and analyze systems in the conditions of the chemical equilibrium. They will become familiar with the basic irreversible processes, such as viscous processes, diffusion, sedimentation and electrophoresis. Students should be able to understand the atomic structure of matter and analyze time changes of systems.

Teaching methods:

Lectures, laboratory exercises.

Extracurricular activities:

—

Coursebooks:

Main coursebooks:

  1. Izabrana poglavlja fizičke hemije, Slobodan Anić, Dragomir Stanisavljev, Nikola Vukelić, Beograd 2007.
  2. Physical Chemistry, R. A. Alberty
  3. Physical Chemistry, P. Atkins
  4. Praktikum iz Opsteg kursa fizičke hemije
    Miroslav Ristić, Igor Pasti, Isidora Cekić-Lasković, Univerzitet u Beogradu, Fakultet za fizičku hemiju, Beograd, 2010.
  5. Zbirka zadataka iz fizičke hemije, U. Mioč, Beograd, 1988.

Supplementary coursebooks:

Lecture notes

Additional material:

http://helix.chem.bg.ac.rs/~saska/Fizicka_hemija_BH--1029B/

  Course activities and grading method

Lectures:

5 points (4 hours a week)

Syllabus:

  1. The introductory lecture. The basic physicochemical variables. The First Law of Thermodynamics. The state functions. Heat capacity.
  2. Reversible and irreversible processes. Thermochemistry.
  3. The Second Law of Thermodynamics. Calculation of entropy changes. Statistical meaning of entropy.
  4. Helmholtz and Gibbs free energy. Multicomponent systems. Equilibrium.
  5. The chemical potential in liquid and solid solutions. The phase equilibrium. One-component systems. The phase equilibrium - two-component systems. Colligative properties of solutions. Completely miscible liquids, vapor pressure-composition diagrams.
  6. Boiling point-composition diagrams. Immiscible liquids. Liquid-solid systems. Transport processes.
  7. The first progress test. Atomistic structure of matter. The Schrödinger equation. Wave function.
  8. A particle in a one-dimensional box. The quantum mechanical description of rotation and vibration. The spectra and structure of hydrogen-like atoms. The structure of multi-electron atoms.
  9. The spectra of multi-electron atoms. Atomic terms. The spectrum of helium. The structure of molecules. Rotational-vibrational spectra of two-atom molecules. Vibrations of polyatomic molecules.
  10. Electronic transitions in molecules. The vibrational structure of electronic transitions. Fluorescence. Phosphorescence. Predissociation. Electrical properties of molecules. Polarization. Molar refraction. Optical rotation.
  11. The second progress test. Characteristics of the atomic nucleus. Radioactive decay.
  12. Passage of radioactive rays through matter. Measuring radioactivity. Nuclear reactions. The fission. The application of isotopes.
  13. Chemical kinetics. The law of mass action. The connections between various types of rates in chemical kinetics. The dependence of the rate constant on temperature. The reaction order. Determination of the reaction order and rate constant.
  14. Collision theory. Transition state theory. Reactions in liquids. The influence of the solvent and ionic strength on rate constants.
  15. Complex chemical reactions. Parallel, reversible and consecutive reactions. The stationary state method. Catalysis. The mechanism of general and specific acid-base catalysis. The third progress test.

Labwork:

25 points (3 hours a week)

Syllabus:

  1. A progress test, calculations, an experiment: The heat of neutralization.
  2. A progress test, calculations, an experiment: Azeotropic mixtures.
  3. A progress test, calculations, an experiment: Determining relative molecular weight using the cryoscopic method.
  4. A progress test, calculations, an experiment: Testing Beer's Law.
  5. A progress test, calculations, an experiment: Determining the half-life. An alternative option: A scintillation counter.
  6. A progress test, calculations, an experiment: Determining the rate constant of the inversion of saccharose.

Written exam:

70 points