MEDICINAL CHEMISTRY
Fall semester
Course coordinator: Prof. Anna Janecka
Department of Biomolecular Chemistry
Mazowiecka 6/8
Ph. +4842 272 57 06
e-mail: anna.janecka@umed.lodz.pl
Lectures
Practical classes
- 10 hours
- 20 hours
Textbook
General, Organic, and Biological Chemistry, K. Timberlake
Course Requirements
1. Class Attendance
Attendance is required at all classes.
Students that missed one or two class will have to write a quiz at the end of the
semester covering the material that they missed. Three absences will result in failure
of the course.
2. Quizzes
There will be a quiz each week consisting of 5 short questions covering the
material of the proceeding lecture.
Grading: Correct full answer to one question – 1 point
Maximal amount of points from one test – 5 points
3. Laboratory experiments:
Students will perform 4 experiments. Students will receive 3 points for each
experiment.
4. Test + calculations
At the end of the semester there will be a test (20 multiple choice questions) and 4
chemical calculations.
Grading:
1.5 points for each correct answer (30 points maximum)
2.5 points for each calculation (10 points maximum)
5. Final grade
A final grade will include the following elements:
a. weekly tests
4x5 = 20
b. laboratory work
4x3 = 12
c. test + calculations
40
max total
72
grading:
72-66 points – grade 5
65-60 points – grade 4.5
59-55 points – grade 4
54-49 points – grade 3.5
48-43 points – grade 3
42 and less - grade 2 (unsatisfactory)
Lecture topics
1. Structure of matter. Elements and symbols. Elements necessary for life. Structure of
atom, fundamental particles, mass number and atomic number, atomic mass unit, isotopes.
Arrangement of electrons in the atom, energy levels, electron configuration, shapes of
orbitals, Periodic table of elements. Valence electrons, electron-dot structure.
Chemical bonds and molecular structure. Molecules and compounds. Octet rule, ionic
bonds, ionic compounds, common cations and mono- and polyatomic anions, writing
formulas of ionic compounds, naming ionic compounds, reactions of ionic compounds.
Covalent bonds, electronegativity, nonpolar and polar covalent bonds.
2. Oxidation, reduction – definitions, oxidation number, redox reactions, balancing redox
reactions. Oxidizing and reducing agents. Practical use of redox reactions.
Chemical kinetics and equilibrium. Energy in chemical reactions. Reaction rate, factors
which influence the rate of a chemical reaction Homogeneous and heterogeneous catalysis.
Enzymes as catalysts. Equilibrium in chemical systems. Equilibrium constant. Le Chatelier’s
principle.
3. Solutions. Water – physical constants based on water. States of water. Structure of water.
Hydrogen bonding. Surface tension. Solutions, factors affecting solubility. Electrolytes and
non-electrolytes, ionization, strong and weak electrolytes, percent ionization and ionization
constant. Acids and bases, amphiprotic ions. Ionization constant of acids and bases. Salts,
hydrolysis of salts.
Acid-base equilibria. Ionization of water, definition and calculation of pH.
Buffer solutions – the mechanism of action. Buffer capacity. Titration curves.
Diffusion and osmosis. Diffusion. Colligative properties – osmosis. Osmotic pressure.
Chemical calculations. Calculating concentration (molar and percent), pH of solutions,
osmotic pressure.
4. Hydrocarbons (part 1)– Structure of alkanes, Homologous series, common alkyl groups,
IUPAC nomenclature. Hybridization of carbon atoms. Cycloalkanes. Properties and basic
reactions of alkanes. Conformations of alkanes and cycloalkanes.
5. Hydrocarbons (part 2) -.alkenes, alkines. Structural isomers, cis/trans isomers in alkenes
and cycloalkanes. Benzene, special properties of aromatic compounds. Substituted benzene.
Polycyclic aromatic compounds – carcinogens. Heterocyclic compounds.