Download Ministry of Education and Science of the Ukraine

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
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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.
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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.
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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.
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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.
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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.
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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
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