* Load is given in academic hour (1 academic hour = 45 minutes)
COURSE GOALS: Detailed analysis of basic physical chemistry concepts in order to enable students to teach more elementary concepts at school level and to understand molecular structure, equilibria and rates of chemical processes.
LEARNING OUTCOMES AT THE LEVEL OF THE PROGRAMME:
1. KNOWLEDGE AND UNDERSTANDING
1.2. demonstrate a thorough knowledge and understanding of the fundamental concepts in chemistry
1.4. demonstrate a thorough knowledge and understanding of the most important chemistry laws and theories
1.5. demonstrate knowledge and understanding of basic experimental methods, instruments and methods of experimental data processing in physics and chemistry
2. APPLYING KNOWLEDGE AND UNDERSTANDING
2.2. describe important aspects of chemical change
2.3. apply stoichiometry
2.4. recognize and follow the logic of arguments, evaluate the adequacy of arguments and construct well supported arguments
5. LEARNING SKILLS
5.1. search for and use professional literature as well as any other sources of relevant information
LEARNING OUTCOMES SPECIFIC FOR THE COURSE:
After passing the exam student should be able to:
1. 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,
2. describe to procedure for solving the Schrödinger equation for the hydrogen atom and to explain the physical meaning of the solutions obtained,
3. 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,
4. describe the principles governing the nuclear magnetic resonance: NMR (chemical shifts and nuclear spin coupling),
5. explain and describe the energy changes during chemical reactions and physical processes,
6. name the factors that influence the spontaneity of chemical and physical processes,
7. describe the chemical equilibrium quantitatively,
8. describe the properties of electrolyte solutions and compare the structural models of strong electrolyte solutions (Debye&Hückel, Bjerrum, etc),
9. describe the changes in galvanic and electrolyte cells,
10. interpret quantitatively the rate of chemical reaction and corresponding parameters.
Introductory overview of physical chemisty. Hydrogen atom. Atomic orbitals. Spin and manyelectron atoms. Atomic spectra. Born-Oppenheimer aproximation. Molecular orbitals. Diatomic molecules. Correlation diagram. Hibridization. Hückel molecular orbitals. Electronic structure of crystals. Ligand field theory. Quantum chemistry in schools. Molecular spectra. Absorption, emission and scattering. Molecular rotations. Molecular vibrations. IR spectra. Electronic spectra. Lasers. Photoelectron spectra. Magnetic resonance. NMR. Spectroscopy in schools. Properties of gases. Ideal gas and real gases. Kinetic theory of gases. Distribution of molecular velocities and speeds. Collisions. Statistical mechanics. Boltzmann's law. Thermodynamics and temperature. First law: heat and work. Enthalpy. Extent of reaction and stoichiometry. Reaction enthalpies. Thermochemistry. Calorimetry. Temperature dependence of enthalpy. Adiabatic and isothermal work. Irreversibility and entropy. Probability and entropy. Entropy of mixing. Thermodynamic potentials. Gibbs energy. Fundamental equations. Dependence G(p) and G(T). Phase equilibria. Phase diagrams p(T). Partial molar quantities. Chemical potential. Colligative properties: krioscopy i ebulioscopy. Osmosis. Mixtures. Standard states. Relative activity. Chemical equilibrium. Coupled reactions. Solutions. Electrochemistry. Electrolyte solutions. Conductivity. Electrochemical cells. Nernst equation. Kinetics: definition of concepts. Rate laws. Mechanisms and rates. Temperature dependence of reaction rates. Theories of reaction rates. Catalysis.
REQUIREMENTS FOR STUDENTS:
Active participation in lectures and seminars. Homework.
GRADING AND ASSESSING THE WORK OF STUDENTS:
Tests and oral examination.
- P. W. Atkins: Elements of Physical Chemistry, 3. izd., Oxford University Press, Oxford 2001.
- T. Cvitaš, I. Planinić, N. Kallay: Rješavanje računskih zadataka u kemiji, II. dio, 2. izd., Hrvatsko kemijsko društvo, Zagreb, 2014., zbirka riješenih zadataka.
- I. N. Levine: Physical Chemistry, 6. izd., McGraw Hill, New York, 2009.
- P. W. Atkins, J. de Paula: Atkins' Physical Chemistry, 9. izd., Oxford University Press, Oxford 2010.
- T. Cvitaš, Fizikalna kemija, rkp. u pripremi i dijelom dostupan kao ftp download.
Fundamentals of Physics 2