12758 - Biochemical Propaedeutics

Learning outcomes

Students should acquire a basic knowledge in the field of general and inorganic chemistry (structure of elements and compounds; thermodynamics, kinetics, equilibria; solutions; structure, properties and reactivity of inorganic and bioinorganic compounds); these concepts are helpful and adequate in view of acquiring professional competence. Such objectives, addressed to the requirements for the veterinary profession, represent the basis for the comprehension of biological phenomena and the principles of fundamental methodologies of investigation.

Course contents

Recall of the concepts of general and inorganic chemistry addressed to the biomedical field: systems, matter, energy and aggregation states; atomic structure: subatomic particles, interaction of light energy with matter, notion of spectrophotometry, electronic configuration, periodical properties, classification of elements (periodic table); chemical binding: theories on the formation of bonds, strong chemical bonds (polar and non-polar covalent bond, ionic bond, crystal ionic lattice and lattice forces, dative or coordination bond), metallic bond (crystal metallic lattice and properties of metals);  weak bonds and their biological functions (e.g. hydration, hydrogen bond, van der Waals forces); energy of chemical bonds (The first principle of thermodynamics and Hess’s law,  introductory remarks on calorimeter); stechiometry: the law of conservation of mass, balancing chemical reactions with and without electron transfer; acids and bases (Arrhenius, Broensted-Lowry, Lewis); chemical properties of the elements especially of that with biological role (inorganic e bioinorganic chemistry); molecular geometry: basal concepts,  types of hybrids of biological interest and geometrical shape of simple inorganic molecules; coordination complexes and their biological role; chemical kinetics and equilibrium, factors which affect them and bases of enzyme kinetics; solutions: ways of expressing concentration, solubility and hydrophobic bond, solubility of gases (Henry’s law and Bunsen coefficients); partition coefficient and introductory notions on chromatographic techniques; colligative properties of electrolytes and non-electrolytes, especially osmotic pressure, coefficients of activity and ionic strength, chemical and physical equilibria, homogeneous and heterogeneous equilibria in water solutions of biological role: electrolytic dissociation and strength of electrolytes, common-ion effect, ionic product of water, pH and acid and alkali solutions, acid-base equilibria (buffers, buffers in blood, hydrolysis, pH indicators, acid-base titration, ampholytes, isoionic and isoelectric pHs and introduction to electrophoresis) solubility product, notions of electrochemistry: Nernst equation,  concentration electrochemical battery, pHmeter; Donnan equilibrium and membrane potential; colloids: overview.

Readings/Bibliography

Raggi A., Chimica generale per le scienze biomediche, ETS, Pisa.

Silvestroni P., Chimica generale con elementi di inorganica, Ed. Veschi, Masson, Milano (1989).

Binaglia L., Giardina B., Chimica e Propedeutica Biochimica, McGraw-Hill (MI) (1999).

Viviani R., Elementi di Biochimica, Tomo I e II. UTET, Torino (1984-1985).

Teaching methods

Lessons are illustrated by means of transparencies, models of atoms and molecules. The course will be accompanied by exercises.

Assessment methods

The final exam consists of an oral examination.

Teaching tools

Transparency projector, traditional blackboard with chalks, PC, atomic and molecular models, laboratories.

Office hours

See the website of Anna Borgatti