Teaching - UniCamillus

Chemistry and introductory biochemistry (objectives)

The main aim of this course is to allow the students to learn the major chemical and physical principles which govern organism life. The course will further cover the study of the composition of inorganic and organic compounds as well as the reactions they undergo.
These aims will be pursued through interactive frontal lectures, exercise-sessions designed to optimize learning and to maximize the student skill in recognizing and solving a given medicinal chemistry task.
LEARNING OUTCOMES

Knowledge and understanding

The medicinal chemistry course is aimed at allowing the students to learn the chemical, physical
and molecular bases of main principles and laws of molecular chemistry and biochemistry.
At the end of the course the student is expected to become able to identify the composition of inorganic compounds present in nature and how they interact and react each other during patho-physiological processes in human body. The student is asked to learn the water-based reactions, acid-base theories, and their role in maintaining the homeostasis.
The course is further organized to provide the students the basis of the chemistry of Carbon, i.e. organic chemistry, with a special focus on how organic compounds are structurally arranged and how they react to form the building blocks of life.

Applying knowledge and understanding

The student will learn how to apply the knowledge acquired during the course to the clinical tasks his/her profession is expected to deal with. This will allow the student to recognize critical diagnostic items and prognostic outcomes by deciphering how a given chemical and metabolic alteration turns out into a pathological condition. At the end of the course, the student will be able to apply this knowledge to the specific clinical area he/she will dedicate his/her medical activity.

Communication skills

The student will be asked to be able to discuss orally the subjects which are part of this course syllabus. He/She will be further asked to learn the right scientific terminology.

Making judgements

Specific attention will be paid to let the students improve the critical capacity when studying key chemical processes which underscore metabolic reaction of living organisms with clinical relevance. The students are expected to learn how critical is to bear a solid conceptual knowledge of each specific clinical task.

Code

90216

Language

ENG

Type of certificate

Profit certificate

Credits

Scientific Disciplinary Sector Code

BIO/10

Contact Hours

Type of Activity

Basic compulsory activities

Teacher	Tundo Grazia Raffaella (syllabus) General Chemistry Introduction remarks. Periodic table of elements and inorganic nomenclature. Atom: atom models, atomic particles: proton, neutron, electron. Isotopes. Electrons and atom electronic configuration. The quantum-mechanical model of the atom. Quantum numbers and orbitals. Auf-bau. Chemical bonds. Matter states. Gas: ideal gas law. Absolute temperature and its relation with mean molecular speed. Mixture of gases; Dalton law. Liquids. Vapor pressure of a liquid. Solids: structural characteristics of covalent, ionic, molecular and metallic solids. Thermodynamics. Thermodynamic potentials; enthalpy, Hess law, entropy. Free energy: relationship with enthalpy and entropy. Solutions. Concentrations of solutions: dilution and mixing of solutions. Vapor pressure of a solution (Raoult’s law). Solubility of gases in liquids: Henry law. Chemical equilibrium. Equilibrium in gaseous phase. Expression of equilibrium constant. Kp and Kc relationship. Equilibrium influencing factors. Homogeneous and heterogeneous equilibrium. Solutions of electrolytes. Strong and weak electrolytes: dissociation grade. Colligative properties of electrolyte solutions. Van't Hoff binomial. Acid and bases following Arrhenius, Bronsted and Lowry definitions. Strong and weak acid and bases. Dilution law of Ostwald. pH in strong and weak acid and base solutions. Buffers. Acid-base titrations. Heterogeneous systems. Equilibria of slightly soluble ionic compounds. The solubility-product constant. The effect of a common ion. Kinetic. Kinetic introduction, activated complex theory, activation energy. Kinetic equations and reaction order. Relationship between kinetic constant and activation energy (Arrhenius energy). Relationship between kinetic constants and equilibrium constants. Electrochemistry. Redox reactions and chemical potentials. Oxidation number. Redox reactions and their balance. Redox standard potentials. Nerst equation. Electromotive force potential of a cell. Half-cell. Chemical and concentration cells. Introductory Biochemistry Carbon atom hybridization. Sp3, Sp2, Sp hybridization and their geometry. Hydrocarbons. Saturated hydrocarbons (arenes): alkanes, cicloalkanes. Nomenclature. Conformational isomerism and geometric isomerism (cis-trans). Unsaturated hydrocarbons: alkenes and alkynes. Nomenclature. Addiction reactions to alkenes. Markovnikov rule. Alkynes addiction. Aromatic compounds. Benzene structure: resonance model. Aromatic compounds nomenclature. Polycyclic aromatic hydrocarbons. Alcohols, phenols, thiols. Nomenclature. Alcohols and phenols in comparison. Aldehydes and ketones. Nomenclature. Carbonylic group. Acetals and hemiacetals formation. Keto-enol tautomerism. Aldol condensation. Carboxylic acids and their derivatives. Nomenclature. Carboxylic acid derivatives: esters and amides. Esterification mechanisms. Glycerol triesters. Ammines and other nitrogen compounds. Classification and nomenclature of ammines. Comparation between ammines and amides. Stereoisomerism. Chirality. Enantiomers. Polarized light. Diastereoisomers. Meso compounds. Racemic mixtures. Carbohydrates. Definition, classification and nomenclature. Monosaccharides. Monosaccharides chirality. Fisher projections. Amino acids, proteins. Structure and properties of aminoacids. Peptide Bond. Nucleotides and nucleosides. Nomenclature, structure and properties. (reference books) Peter Atkins , Loretta Jones, Leroy Laverman Chemical Principles: The Quest for Insight Chemistry by M.S. Silderberg, McGraw-Hill International Edition. Katherine J Denniston, Joseph J Topping and Robert L Caret. General, Organic & Biochemistry. 7th Ed. 2010. McGraw-Hill Higher Education.
Dates of beginning and end of teaching activities	From to
Delivery mode	Traditional
Attendance	Mandatory
Evaluation methods	Written test Oral exam

Teacher	Sbardella Diego (syllabus) The main aim of this course is to allow the students to learn the major chemical and physical principles which govern organism life. The course will further cover the study of the composition of inorganic and organic compounds as well as the reactions they undergo. These aims will be pursued through interactive frontal lectures, exercise-sessions designed to optimize learning and to maximize the student skill in recognizing and solving a given medicinal chemistry task. (reference books) Peter Atkins , Loretta Jones, Leroy Laverman Chemical Principles: The Quest for Insight Chemistry by M.S. Silderberg, McGraw-Hill International Edition. Katherine J Denniston, Joseph J Topping and Robert L Caret. General, Organic & Biochemistry. 7th Ed. 2010. McGraw-Hill Higher Education.
Dates of beginning and end of teaching activities	From to
Delivery mode	Traditional
Attendance	Mandatory
Evaluation methods	Written test Oral exam