Location, time, authorized pages: Lecture slides
Schedule of lectures
|Week||Date||Topic of lectures|
|Lecturer: Prof. Mária Sasvári|
|1||09:09||Introduction to Medical Chemistry. The chemical equilibrium.|
|09:10||Definition of pH and pOH, pH scale. pH of strong electrolytes|
|2||09:16||Acid-base theories. Acidic and basic ionization Constants (pKa and pKb).|
|09:17||Conductance of strong and weak electrolytes. pH of weak acids and bases. The common ion effect; effect of strong acids on the dissociation of weark acids.|
|3||09:23||Acid-base indicators. Ionization of polyprotic acids. Anionic and cationic hydrolysis. Calculation of pH of salts.|
|09:24||Buffers. Calculation of the pH of buffer solutions. The Henderson-Hasselbach equation. Buffer capacity.|
|4||09:30||The most important physiological buffer systems. The bicarbonate/carbonic acid system.|
|10:01||Conditions for precipitation of salt solutions. Solubility rules.|
|Lecturer: Dr. Nándor Müllner|
|5||10:07||Solutions. Gas mixtures. Henry,s law, Bunsen coefficient. Decompression sickness. Solubility of CO2 in blood serum.|
|10:08||Enthalpy change of the solution process and its relation to the solubility. Raoult‘s law. Laws of dilute solutions.|
|Lecturer: Dr. László Csanády|
|6||10:14||Chemical thermodynamics. First law of thermodynamics in chemistry. Enthalpy change of physical processes. Determination of reaction heat from combustion heat data. Bond energy.|
|10:15||Second law of thermodynamics in chemistry. Entropy content and entropy change. Gibbs free energy (or free enthalpy). Third law of thermodynamics. Free enthalpy changes in biochemistry and in redox reactions.|
|Lecturer: Dr. András Hrabák|
|7||10:21||Basics of chemical kinetics. Equilibrium constant. The thermodynamical and kinetic control of reactions.|
|10:22||Catalysis. Activation energy. Arrhenius equation. Enzymes as catalysts.|
|8||10:28||Complex ions and coordination compounds. Central ions and ligands. IUPAC nomenclature of coordination complexes. Stability exponent. Some biomedically important coordination complexes and chelating ligands.|
|10:29||Elements and inorganic coumpounds of biomedical importance.|
|Lecturer: Prof. Mária Sasvári|
|9||11:04||Electrochemistry. Electrode potential, cation and anion electrodes. The hydrogen electrode. The electromotive force of voltaic (galvanic) cells.|
|11:05||The electromotive force and the Gibbs free energy change of a reaction. The Nernst equation.|
|10||11:11||Concentration cells. Direction of a redox reaction. Non-polarizable electrodes.|
|Lecturer: Dr. Pál Bauer|
|11:12||Organic chemistry. Introduction, general structure of organic compounds. Hybridization of atomic orbitals. The hybrid states of carbon. Functional groups, general types of organic reactions.|
Isomerism: constitution, configuration, conformation. Stereochemistry, geometric isomerism, chirality, the D/L and R/S systems, prochirality.
The most important groups of organic compounds. Alkanes, structures, radical reactions.
Alkenes, their structures, properties, reactions. Alkynes: the triple bond. Aromatic compounds. Structure and reactions of benzene. Resonance stabilization in aromatic compounds. Huckel’s rule.
Reactions of the aromatic ring: Mechanism of electrophilic substitution of aromatic compounds. Effect of substituents of the aromatic ring on the reaction rate and product formation in further electrophilic substitution type of rections. Alkyl halides. Nucleopihilic substitutions: SN1 and SN2 rections.
|Lecturer: Dr. Attila Ambrus|
|13||12:02||Organic hydroxyl compounds. Classification, structures, reactions. Formation of ethers, esters.|
|12:03||Aldehydes, ketones. Reactions, nucleophilic addition.|
|14||12:09||Organic acids, classification, their properties, reactions.|
Nitrogen-containing organic compounds: amines, amides. Structures, reactions. Sulfur-containing organic compounds: classification, structures, reactions.