Lectures 1. Chemical View of a Living Organism Introduction to medical chemistry. The relationships between chemistry to some other scientific and health-related disciplines. Chemical nomenclature of inorganic compounds. Classification of matter, physical and chemical properties of matter. Basic chemical calculations. 2. Structure of Matter - Chemical Bond I Structure of atoms, isotopes, the periodic table. Electronic structure of atoms (orbitals, shells, subshells, quantum numbers). Electron configurations, Pauli Exclusion Principle, Hund’s Rule, Build up Principle. Ionic bond: octet rule, the formation of ions, the polarizing effect of ions, deformation of ions, properties of ionic compounds, biologically important ions. 3. Structure of Matter - Chemical Bond II Covalent bond: formation of covalent bond, the bond energy, bond length, polarity of covalent bond, multiple covalent bonds. The hybridization theory, the shape of molecules. Coordinate covalent bond: formation, chelates, biological importance of some chelates in the organism. Van der Waals interactions. Relationship between the structure and biological function of the molecules. Analytical chemistry – Introduction Introduction to analytical chemistry, volumetric analysis, calculations in the volumetric analysis, and methods of the volumetric analysis. 4. Chemical Reactions in the Biological Systems I Classification of chemical reactions. Thermodynamics, thermodynamic system and equilibrium, kinds of thermodynamics process, internal energy, the first law of thermodynamics, enthalpy, entropy, and the second law of thermodynamics. Reversibility and irreversibility of reactions, spontaneous reactions. Thermochemistry - exothermic and endothermic reactions. Gibbs and Helmholtz energy, the transformation of free energy in a biological system. 5. Selected Parts of Applied Analytical Chemistry - Instrumental Analysis I Importance of redox reactions for the organism. Electrodes, types of electrodes, electrode potentials, Nernst equation, galvanic cell. Electrochemical determination of pH. Potentiometric titrations. Conductometric titrations. 6. Selected Parts of Applied Analytical Chemistry - Instrumental Analysis II The methods of biological material processing. Spectrophotometry - Lambert-Beer law, absorption spectra, calibration curve. Chromatographic methods, the quantitative and qualitative analysis in veterinary medicine. Chemical Reactions in the Biological Systems II Kinetics, reaction rate and factors that affect the rate. Reaction order and the molecularity, half-life of the reactions, and significance for medicine. Reaction mechanisms, catalysis. Chemical equilibrium, equilibrium constant. 7. Dispersive Systems True solutions, characteristics, properties. Colligative properties of solutions – vapour pressure, osmosis, diffusion. Acid and base theories, ionization of water, pH. Protolytic reactions and their biological importance. Dissociation equilibrium in weak electrolytes, the definition of pK. Buffer theory, Henderson–Hasselbalch equation, buffer capacity. Biological buffering systems and disorders in acid-base equilibrium in the organism. 8. Classification of Organic Compounds and Biochemically Important Reactions Molecular structure of organic compounds. Basic principles of IUPAC nomenclature, isomerism and its importance, inductive and mesomeric effects. Reactions of organic compounds in the living systems. The active site in the organic molecule - functional groups. Hydroxyderivatives (alcohols, phenols, enols): physical and chemical properties, biologically important reactions (oxidation, esterification), esters of phosphoric acid (AMP, ADP, ATP). 9. Oxocompounds (aldehydes, ketones): basic characteristics, physical and chemical properties, reactions important for the organism, and some representative compounds. Carbohydrates: classification, physical and chemical properties, stereoisomerism, important reactions (oxidation, reduction, forming of hemiacetals and acetals). Deoxysaccharides, aminosaccharides, glycosides, glycosidic bonds, oligosaccharides, and important disaccharides. Polysaccharides, classification, homoglycans (starch, glycogen, cellulose, dextran, inulin) and heteroglycans (hyaluronic acid, chondroitin sulphate, proteoglycans), biological function. 10. Carboxylic Acids and Their Functional Derivatives in the Body Classification, nomenclature, physical and chemical properties, biochemically important reactions. Characteristics of acid derivatives (salts - solubility, anhydrides – source of energy in the body, esters, amides), polycarboxylic acids, fatty acids. Lipids: classification, structure, properties, reactivity, biologically important compounds and reactions. Complex lipids, phospholipids, glycolipids. Biological membranes. 11. Substitutive Derivatives of Carboxylic Acids Classification, structure, properties, biochemically important reactions of hydroxy acids and oxoacids. Amino Acids, Peptides, Proteins Amino acids, structure, properties, reactivity. Formation and structure of peptides, biologically important peptides. Proteins, classification, primary, secondary, tertiary and quaternary structures, biological function, colloid character, isoelectric point, solubility, denaturation. 12. Organic Derivatives of Carbonic Acid in the Body Urea and its derivatives, ureides, biologically important compounds. Sulphur Organic Compounds Thiols, sulphides, thioethers, sulfonic acids, sulfonium salts, biologically important compounds. Sulphonamides in veterinary medicine. 13. Nitrogen Organic Compounds Amines - classification, reactions, biologically active amines, amides, amino alcohols and their derivatives. Heterocyclic compounds 5-membered and 6-membered heterocycles, classification, chemical properties biologically important compounds. Practical Exercises 1. Introduction The assessment of the study. Chemistry Laboratory Guidelines. Laboratory safety rules. Laboratory glassware. Basic chemical operations, sample preparation and procedures. 2. Chemical Nomenclature I Chemical nomenclature of inorganic compounds - binary compounds. Basic Calculations in Chemistry I Representation of solution composition - mass percentage, molar concentration. 3. Chemical Nomenclature II Chemical nomenclature of inorganic compounds - acids and salts Basic Calculations in Chemistry II Dilution of solutions Density Determination Practical Exercise No 1 and No 4: a) Preparation of 100 g 5% NaOH solution. Determination of density by a densitometer. b) Preparation of 100 ml 0.05 mol•dm-3 CuSO4•5H2O Determination of density by pycnometer. c) Preparation of diluted HCl from concentrated HCl in a volume ratio of 1:3. 4. Volumetric Analysis - Titrations Principle and classification of volumetric methods. The assessment of analytical results. Acid/base titrations. Practical Exercise No 5: a) Standardization of NaOH solution (acidimetry). b) Determination of HCl concentration and mass in the unknown sample (alkalimetry). 5. Redox Processes in the Living Organism Principle and classification of redox titrations. Manganometric titrations. Practical Exercise No 6: a) Standardization of KMnO4 solution. b) Manganometric determination of iron (II) concentration and mass in the unknown sample. 6th – 11th Week Complexometric Titrations Complexometric titration, classification of the methods. Practical Exercise No 7: a) Standardization of complexone III solution. b) Complexometric determination of Ca2+ mass in the unknown sample. Conductometry, Conductometric Titrations Principle of the method, conductivity of the solutions, conductometric titration. Practical Exercises No 8 and No 9: a) Preparation of the solutions: 0.5 mol•dm-3 NH4Cl 0.44 mol•dm-3 CH3COOH 0.5 mol•dm-3 HNO3 0.26 % Ba(OH)2 Measurement of conductivity of prepared solutions and assessment of conductivity according to chemical structure. b) Conductometric determination of HCl mass in the unknown sample (body fluid). pH of Solutions Acid-base properties of the solutions, pH definition, pH calculations. Colorimetric and potentiometric determinations of pH. Practical Exercise No 10: a) Preparation of the solutions: 1.5 % CH3COOH 0.05 mol•dm-3 NH4OH 0.2 mol•dm-3 Na2CO3 0.05 mol•dm-3 H2SO4 3.5 % citric acid pH measurement of prepared solutions using indicator paper and pH meter. b) Calculation of the theoretical pH value of prepared solutions. c) pH determination of egg, milk and drug solutions. Potentiometry, Potentiometric Titrations Principle, kinds of electrodes, potentiometric titration. Practical Exercise No 11: a) Potentiometric standardization of NaOH solution. b) Potentiometric determination of HCl concentration in an unknown sample (gastric juice). Spectrophotometric Analysis Lambert-Beer law. Qualitative and quantitative analysis, absorption and calibration curve. Practical Exercise No 12: a) Determination of KMnO4 absorption maximum. b) Spectrophotometrical determination of KMnO4 concentration in the unknown sample (industrial wastewater). Chromatography I Ion exchange chromatography - quantitative analysis Practical Exercise No 13 a) Preparation of HCl solution for stationary phase activation. b) Determination of NaCl mass in an unknown sample using the cation exchanger resin. Chromatography II Chromatographic methods classification. Qualitative analysis, determination of Rf value. Practical Exercise No 14: a) Analysis of sugar mixture by TLC. b) Separation of amino acids by PC. c) Separation of serum-neutral lipids by TLC. d) Size exclusion chromatography. 12. Master Practical Exercise 13. Master Test |
