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Fundamentals of Physical Chemistry

Code: 40361
ECTS: 12.0
Lecturers in charge: prof. dr. sc. Davor Kovačević
Lecturers: dr. sc. Tin Klačić - Seminar

Nikol Bebić , mag. chem. - Practicum
Katarina Jerin , mag. educ. phys. et chem. - Practicum
Katarina Leko , mag. chem. - Practicum
dr. sc. Karlo Sović - Practicum
Take exam: Studomat
English level:


The lecturer is not able to offer courses in English at this time.

1. komponenta

Lecture typeTotal
Lectures 60
Practicum 60
Seminar 30
* Load is given in academic hour (1 academic hour = 45 minutes)
Physical quantities and units.
Zeroth law of thermodynamics. Work, heat and internal energy. First law of thermodynamics. Enthalpy.
Extent of chemical reaction, reaction quantities. Hess law. Calorimetry.
Second law of thermodynamics. Probability and entropy. Entropy of mixing.
Gibbs energy. G(p) and G(T) dependency.
Partial molar quantities. Thermodynamics potential. Chemical potential.
Standard states. Relative activities.
Changes of thermodynamics properties during mixing of fluids.
Dependency of Gibbs energy on extent of reaction. Equilibrium of chemical reaction.
Phase equilibrium. Phase diagram p(T).
Colligative properties.
Introduction to electrochemistry.
Electrolyte solutions. Transport number. Conductivity.
Ion-ion interactions.
Nernst equations. Galvanic cells. Full cells and corrosion.
Introduction to chemical kinetics.
Chemical kinetics: Basic definitions. Rate of reaction and simple rate laws. Reaction mechanisms.
Temperature dependency of reaction rate.
Catalysis. Enzyme catalysis. Collision theory and activated complex theory.
Black body radiation Photoelectric effect. The spectra of hydrogen atom. Models of atom.
Wave-particle duality. The uncertainty principle.
Principles of quantum mechanics. Harmonic oscillator. Particle in a box.
Hydrogen atom. Atomic orbitals. Spin and many-electron atoms
Atomic spectra
Born-Oppenheimer approximation. Valence bond theory. Molecular orbital theory. Hybridization. Hückels molecular orbitals Crystal electronic structure. Ligand field theory.
Molecular spectra. Absorption, emission and scattering of light.
Rotation spectroscopy. Vibration spectroscopy. Electronic transitions and electronic spectra.
Magnetic resonances
Laboratory exercises:
Conductometry 1; conductivity measurements, examination of conductometry cells
Conductometry 2; conductance of strong and weak electrolytes, Kohlrausch law, conductivity measurements
Potentiometry 1; pH measurements, glass electrode
Potentiometry 2; potentiometric titration
Spectrophotometry; UV-Vis spectrophotometry, Beer-Lambert law
Transport number of ions; independent ion migration, Hittorf method
Calorimetry; calorimeters, determination of enthalpy of neutralization
Chemical kinetics; kinetics of decomposition of hydrogen peroxide.
Learning outcomes:
After passing the exam student should be able to:
- describe the postulates of quantum mechanics, derive the Schrödinger equation for simple systems (particle in a box, harmonic oscillator) and to interpret the obtained results,
- describe to procedure for solving the Schrödinger equation for the hydrogen atom and to explain the physical meaning of the solutions obtained,
- distinguish between the absorption, emission and scattering of electromagnetic radiation and to state which information regarding the molecular structure can be deduced from rotational, vibrational and electronic spectra,
- describe the principles governing the nuclear magnetic resonance: NMR (chemical shifts and nuclear spin coupling)
- explain and describe the energy changes during chemical reactions and physical processes
- name the factors that influence the spontaneity of chemical and physical processes
- describe the chemical equilibrium quantitatively
- describe the properties of electrolyte solutions and compare the structural models of strong electrolyte solutions (Debye&Hückel, Bjerrum, etc)
- describe the changes in galvanic and electrolyte cells
- interpret quantitatively the rate of chemical reaction and corresponding parameters
After completing the laboratory course student should be able to:
- independently measure basic physico-chemical properties (pH, conductivity, absorbance, temperature, electromotive force, etc ...) using modern instrumentation and classical techniques
- collect and interpret the experimental results
- apply standard mathematical methods for solving the chemical problems and analysing the experimental results.
- apply various physico-chemical models for interpretation of experimental results
- analyse the experimental results regarding the reproducibility of measurements, sensitivity of measurements and predictable errors.
- analyse the factors that influence the obtained results.
  1. P. W. Atkins, J. de Paula: Elements of Physical Chemistry, 5th ed., Oxford University Press, Oxford 2009.
  2. T. Cvitaš, Fizikalna kemija, rkp. u pripremi i dijelom dostupan kao ftp download.
  3. T. Cvitaš, I. Planinić, N. Kallay: Rješavanje računskih zadataka u kemiji, II. dio, 2. izd., Hrvatsko kemijsko društvo, Zagreb, 2014., zbirka riješenih zadataka.
  4. N. Kallay, S. Žalac, D. Kovačević, T. Preočanin i A. Čop, Osnovni praktikum fizikalne kemije, Fizičko-kemijski Zavod, Kemijski odsjek, PMF, 2002.
  5. P. W. Atkins, Atkins' Physical Chemistry, 9. izd., Oxford University Press, Oxford, 2010.
  6. I. N. Levine, Physical Chemistry, 6. izd., McGraw Hill, New York 2009.
  7. R. J. Silbey, R. A. Alberty, M. G. Bawendi, Physical Chemistry, 5. izd., Wiley, New York 2008.
Prerequisit for:
Enrollment :
Passed : General and Inorganic Chemistry
Attended : Mathematics
Attended : Physics
3. semester
Mandatory course - Regular study - Molecular Biology
Consultations schedule: