CHEMICAL BASICS AND MECHANISMS OF RISK FACTORS
Learning outcomes of the course unit
Allow the student to learn and understand the basic principles of chemistry, the properties of the main chemical molecules of biological interest, the functional aspects and inter-relationships of biomolecules and, finally, the etiologic agents present in the environment that are responsible for disease manifestations and onset of tumors. These skills, combined with the acquisition of knowledge of medical terminology will be functional to understand the topics that will be taught in more specialized courses and for future employment.
Course contents summary
FONDAMENTI DI CHIMICA
The module can be divided into three parts. The first part covers topics of General Chemistry on elementary substances and chemical compounds, periodic table, chemical symbols of the elements, the definition and application of oxidation number, nomenclature of inorganic compounds and rules for balancing redox reactions and not redox. The second part concerns the structure of the atom, chemical bonding, and physical states of matter. The third and last part is the solutions, the chemical equilibrium, the buffer solutions and the pH.
After a brief introduction to the basic principles of Organic Chemistry, the main molecules of biological systems will be presented: carbohydrates, lipids, proteins and nucleic acids, and ATP as energy transporter (Structural Biochemistry).
In the second section main subject will be Metabolic Biochemistry with particular emphasis on bioenergetics, red-ox biological reactions, and cell metabolism.
Physical, chemical and biological causes of the disease. Environmental and nutritional pathology. Molecular and cellular oncology and the aetiology of cancer.
FONDAMENTI DI CHIMICA. Elementary substances and chemical compounds. Periodic Table. Chemical symbols of the elements. Chemical phenomena and physical phenomena. Chemically homogeneous and heterogeneous systems. The mixtures. Dalton's atomic theory. The atom as the fundamental unit of matter, through which chemical transformations occur. Lavoisier's law. The definition of mass and weight. The principle of Avogadro. Mass and atomic weight. The scale of atomic weights. Molecular Weight. Chemical formulas: quality and quantity information. Atomic mass units. Chemical symbols and formulas. Fundamental subatomic particles: proton, neutron and electron. Atomic number (Z) and mass number.
Definition and application of oxidation number. The oxidation numbers of the elements. Nomenclature of inorganic compounds: oxides and hydroxides. Preparation of hydroxides. The peroxides, basic oxides and anhydrides. IUPAC nomenclature, Stock and traditional for oxides, hydroxides and anhydrides. Acids and hydracids (IUPAC and traditional nomenclature) and oxoacids (traditional nomenclature). The salts and the reactions of salification: reactions of simple exchange and double exchange.
Rules for balancing redox and not redox reactions. Acidic and Basic substances. Equations: molecular and ionic equations.
Structure: electrical nature of matter, particle nature of electricity. Atomic model of Thomson and Rutherford. Isotopes and isobars. Elettromegnetica radiation. Planck Theory. Bohr atom. Dualism of wave - particle (De Broglie). Uncertainty principle of Heisenberg. Atomic orbitals and quantum numbers. Polyelectronic atoms. Aufbau: Hund's Rule and the Pauli exclusion principle. Periodic Table. Periodic properties: first ionization energy and electron affinity. Electronegativity. Metals and non-metals.
The chemical bond. Ionic and covalent bonding. Lewis theory. Octet rule. Expansion of the sphere of valence. Polar and non-polar covalent bond. Dative covalent bond. Calculation of the percentage of ionic character of a bond. Molecular geometry. VB theory or valence bond. Hybridization (e.g. carbon: sp3, sp2, sp). Weak bonds. Van der Waals forces: dipole-dipole forces, dipole forces - induced dipole, dipole forces instant - instant dipole. Hydrogen bond. Paramagnetic and diamagnetic molecules.
States of matter. Gaseous state. Equation of state of an ideal gas. Ideal gas laws: Boyle's law, Gay-Lussac I °, II ° Gay-Lussac, the Law of Dalton on gas mixtures. Real gases. Liquid state: Properties. Surface tension, evaporation, vapor pressure, boiling point. Changes of state. The solutions: dilute and concentrated. Ways to express the composition of a solution (% weight / weight; % weight / volume; % volume / volume; molarity, molality, ppm; ppb; molar fraction). Density of a solution. Dissolution of a solid ion in water. Solubility. Factors affecting solubility.
Ideal solutions. Raoult's law. Colligative properties of solutions. Strong electrolytes and weak electrolytes. Osmotic pressure. Colligative properties of electrolyte solutions. Solid state: crystalline solids and amorphous solids. Polymorphism and isomorphism. Comparison between diamond and graphite. Types of chemical transformations. Chemical equilibrium: the equilibrium constant. Mobile principle of balance.
Effect of change of temperature on the equilibrium constant. Factors affecting the position of equilibrium. Heterogeneous equilibria and solubility equilibria (solubility product constant). Acids and bases: Arrhenius theory, theory of Bronsred-Lowry, Lewis theory. The strength of acids and bases. Leveling effect of the water. Henderson-Hasselbach equation. The ionic product of water. The pH of a solution. Indicators. The pH measurement. pH values for some solutions. Buffer solutions. Hydrolysis. Conjugate acid-base pair. Relationship between Ka, K
Franco Ugozzoli, LEZIONI DI CHIMICA, Edizioni Santa Croce.
Le basi della biochimica di Champe Pamela C. - Harvey Richard - Ferrier Denise R. Editore: Zanichelli
Materiale integrativo elaborato dal docente è reperibile sul sito del Corso.
Pontieri G.M. Patologia Generale per i corsi di Laurea in Professioni Sanitarie. PICCIN III Edizione.
The topics will be covered in lectures using PowerPoint presentations and overhead transparencies illustrated with figures, data and comments to facilitate memorization and understanding of the concepts trying to involve the student so that he can be an active part of the lesson. The module "Foundations of Chemistry will be accompanied by exercises of chemical stoichiometry and in particular on the calculation of the concentrations of the solutions and related topics. The exercises will be conducted initially on the blackboard by the teacher and then by the students themselves.
Assessment methods and criteria
The assessment of the achievement of the objectives of the course provides an oral exam with written exercise. Through questions regarding the course content will be determined whether the student has achieved the goal of knowledge and understanding the content and if he has reached the goal of applying the acquired knowledge. The student at the end of the course, using the knowledge gained will need to demonstrate knowledge and understanding of the notions gained on all the topics.