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Ministry of Education and Science of Ukraine V. N. Karazin Kharkiv National University Department of Physical Chemistry Program of the course MEDICAL CHEMISTRY For the first-year students of the School of Medicine. (credit-module system) Kharkiv – 2015 Working program for the subject “Medical Chemistry” for the first-year students of the School of Medicine. Lecturers of the course: Dr. Sci., Professor Natalya A. Vodolazkaya, Ph. D., Ass. Professor Sergey V. Eltsov Total hours: lectures – 20, practice – 50 The program is approved by the meeting of Department of Physical Chemistry Protocol No.1, 26 August 2015 Head of the Physical Chemistry Department N. O. Mchedlov-Petrossyan Approved by the Methodical Commission of the School of Chemistry Protocol No.2, 24 September 2015 Head of the Commission O. I. Yurchenko 2 Course Program Module 1. “Acid-base equilibria and complex formation in biological liquids”. 1. Biogenic s- and p- block elements: biological role, application in medicine. Introduction to the structure of matter. Electronic structure of chemical elements. Periodic table. Valence electrons and oxidation numbers. Oxidation state of chemical element. Balancing redox equations. Biological role of redox reactions. sand p- block chemical elements and their properties. Metals and nonmetals. Molecules and ions. Classification of biogenic elements. Macrominerals. 2. Biogenic d- block elements: biological role, application in medicine. Electronic structure of d-elements. Typical chemical properties of transition metals. Biological activity and medical application of d-elements. Biocomplexes of Fe, Co, Cu, and Zn. Toxic properties of transition metals. 3. Chemical bonding. Chemical bonding. Chemical bonds: covalent, ionic, metallic. Electronegativity. Types of complex compounds. Chemical bonds in complex compounds. Central ion and coordination sphere. Stability constants. Complex formation in biological systems. 4. Solutions. Electrolytic dissociation. The dissolving process and solubility. Solvation and hydration. Expression of the solution concentration: mass and volume percents, molar fraction, molarity, molality. Electrolytic dissociation, electrolytes. Strong and weak electrolytes. The degree of dissociation and dissociation constant. Ostwald’s dilution law. 5. Acid-base equilibrium in biological liquids. General properties of acids and bases. Hydronium and hydroxide ions. Acid dissociation constant and base dissociation constant. The neutralization reactions. The law of equivalents. Acid-base indicators. The methods of the volumetric analysis. Acid-base titration, equivalence point. Titration curve and the equivalence point. 6. Dissociation of water, pH scale. Buffer solutions. Ion product of water. pH scale and methods of pH determination. pH of biological liquids. Hydrolysis of salts. Buffer solutions. Mechanism of buffer action. Henderson–Hasselbalch equation. 7. Colligative properties of solutions. Colligative properties of solutions: vapour pressure lowering (Raoult’s law), elevation of boiling point and depression of freezing point of the solution, osmosis. Osmotic pressure, vant Hoff’s equation. Biological role of osmosis. Cryoscopy, ebullioscopy, osmometry and their using in biomedical investigations. 3 Practice for the 1-st module 1. Introduction to the course “Medical chemistry”. Safety rules. 2. Seminar No.1. Biogenic s- and p- block elements: biological role, application in medicine. 3. Laboratory exercise No.1. Properties and qualitative reactions of some important anions Test according to the material of seminar No.1. 4. Seminar No.2. Biogenic d- block elements: biological role, application in medicine. 5. Laboratory exercise No.2. Properties and qualitative reactions of MnO −4 ion and some important cations Test according to the material of seminar No.2. 6. Seminar No.3. Complex formation in biological systems. 7. Laboratory exercise No.3. Preparation of complex compounds. Test according to the material of seminar No.3. 8. Seminar No.4. Solutions. Electrolytic dissociation. 9. Laboratory exercise No.4. Preparation of solutions and acid-base titration. Test according to the material of seminar No.4. 10. Seminar No.5. Dissociation of water, pH scale. Buffer solutions. Colligative properties of solutions. Laboratory exercise No.5. Determination of the pH value of solutions 11. by indicator method. Test according to the material of seminar No.5. 12. Final test for the 1-st module. 4 Module 2. Equilibrium in biological systems at the phase interface 1. Chemical thermodynamics. Thermochemistry First law of thermodynamics. Exothermic and endothermic processes. Functions of state. Enthalpy and Hess’s law. Thermodynamic equilibrium. Second law of thermodynamics. Entropy, Gibbs energy and Helmholtz energy. Endergonic and exergonic processes in the organism. Thermodynamics conjugation. 2. Kinetics of biochemical processes Main concepts of chemical kinetics: the rate of chemical reaction, reaction rate constant, homogeneous and heterogeneous systems. Mass action law. Molecularity and the reaction order. Kinetic equations for zero-, first-, and second- order reactions. Temperature dependence of the reaction rate. Mechanism of catalysis. Peculiarities of enzyme catalysis. Michaelis-Menten theory of enzyme catalysis. 3. Electrochemical phenomena in biological processes Electrochemistry. Voltage of electrochemical cell. Electrode potential. Nernst’s equation. Diffuse membrane potential. Biopotentials. Diffusion and membrane potentials. The varieties of the electrodes: gas electrodes, 1-st type electrodes, 2-nd type electrodes, glass electrodes, ion-selective electrodes. Potentiometry. Potentiometric determination of the pH values of solutions. Potentiometric titration. 4. Adsorption. Chromatography Phenomenon of adsorption. Isoterms of adsorption. Langmuir’s theory of adsorption. Selective adsorption. Adsorption therapy: hemosorption, enterosorption, and application therapy. Chromatographic analysis. 5. Colloidal solutions Colloidal state of substance. Dispersing medium and dispersed phase. Classification of colloidal systems. Molecular-kinetic properties of colloidal systems. Electrokinetic phenomena. Stability and coagulation of the dispersed systems. 6. Properties of polymer solutions Structure of biopolymers. Protein isoelectric state. Swelling and dissolution of polymers. Gelation. Donnan’s membrane equilibrium. 5 Practice for the 2-nd module 1. Introduction to the module 2. Safety rules. 2. Seminar No.1. Chemical thermodynamics. 3. Laboratory exercise No.1. Determination of the integral heat of solution of a salt. Test according to the material of seminar No.1. 4. Seminar No.2. Chemical kinetics. 5. Laboratory exercise No.2. Determination of the rate constant of the chemical reaction. Test according to the material of seminar No.2. 6. Seminar No.3. Electrochemistry: galvanic cells. 7. Laboratory exercise No.3. Pothentiometric titration. Test according to the material of seminar No.3. 8. Seminar No.4. Colloidal systems. 9. Laboratory exercise No.4. Preparation of hydrophobic colloidal systems. Test according to the material of seminar No.4. 10. Seminar No.5. Stability and coagulation of colloidal systems. Adsorption. 11. Laboratory exercise No.5. Determination of a coagulation threshold. Test according to the material of seminar No.5. 12. Final test for the 2-nd module. 6 References General 1. Chang R. Chemistry. 10-th edition. NY: McGraw-Hill, 2010. 1170 p. 2. Chemistry: the central science. 12-th edition / Brown T.L., LeMay H.E., Bursten B.E. et al. – Glenview: Pearson Education, Inc. 2012. 1195 p. 3. Atkins P., de Paola J. Physical chemistry for the life sciences. 2-nd edition. NY: W. H. Freeman Publishers, 2011. 590 p. 4. Myers D. Surfaces, interfaces, and colloids: principles and applications. 2nd edition. New York: John Wiley & Sons, Inc., 1999. 493 p. 5. S. V. Eltsov, N. A. Vodolazkaya. Practical Medical Chemistry: manual / − Kh.: V. N. Karazin Kharkiv National University, 2015. 188 p. 6. Medical Chemistry: Theory and laboratory exercises for the first module: manual / Eltsov S. V., Vodolazkaya N. A., Voroshylova I. V. et al. Kharkiv: V. N. Karazin Kharkiv National University, 2013. 40 p. 7. Eltsov S.V., Vodolazkaya N.A. Physical and сolloid сhemistry in the сourse “medical сhemistry”. Theory and laboratory exercises. Kharkiv: V. N. Karazin Kharkiv National University, 2012. 132 p. Additional 1. Silberberg M.S. Chemistry: The molecular nature of matter and change. 5th edition. NY: McGraw-Hill, 2009. 1221 p. 2. Allen J.P. Biophysical chemistry. Blackwell publishing, 2008. 492 p. 3. Mortimer R.G. Physical chemistry. 3-d edition. Elsevier, 2008. 1385 p. 4. Walstra P. Physical chemistry of food. New York: Marcel Dekker, 2003. 807 p. 5. Haynie D.T. Biological thermodynamics. Cambridge university press, 2008. 422 p. 6. Leidler K. J. Physical chemistry with biological applications. Benjamin/Cummings publishing, 1978. 586 p. 7. Shaw D.J. Introduction to colloid and surface chemistry. Fourth edition. Oxford: Butterworth-Heinemann. 1992. 306 p. 8. Eltsov S.V., Vodolazkaya N.A. Laboratory exercises on physical and colloid chemistry. Kharkiv: V. N. Karazin Kharkiv National University, 2010. 46 p. 9. Medical Chemistry: module II. Physical and Сolloid Сhemistry. Laboratory exercises and tasks. / Nikitina N.A., Markov V.V., Boichenko A.P. et al. Kharkiv: V. N. Karazin Kharkiv National University, 2012. 80 p. 7 Marking for module 1 and 2 Work Laboratory exercise: а) working during experiment b) writing of the experiment and results in copybook Working during seminar Test according to the seminar material Final test Total: Mark а) 5 points b) 5 points 5 points 10 points 75 points 50 points = 5 lab. exercises per 10 points 25 points = 5 seminars per 5 points 50 points = 5 tests per 10 points 75 points = final test All: up to 200 points Points Traditional mark 200 – 180 excellent 179 – 150 good 149 – 120 satisfactory 119 – 0 unsatisfactory Final mark of the course is average of the marks for the 1-st and the 2-nd modules. Lecturer of the course Natalya A. Vodolazkaya 8