Learning objectives
<br />To provide to the students of the first year the fundamental knowledgeof the general chemistry with a particular attention to the atomic, structure, to the chemical bond, to the states of the matter, to the termodinamic and kinetics features and to the acid-basic properties.
Prerequisites
None
Course unit content
<br />FUNDAMENTALS OF THE ATOMIC AND MOLECULAR THEORY<br />Physical states of the matter. Mass and energy. Atomic theory and structure. Atomic masses. Isotopes. Mole and Avogadro's number. Electromagnetic radiation. Quantum theory. Wave-particle duality. The Heisenberg uncertainty principle. The Schroedinger equation. Atomic orbitals and quantum numbers. The "aufbau" principle. Electronic configuration of the elements. The periodic table and the main periodical properties.<br />CHEMICAL BONDING<br />The ionic and covalent bonds. Lewis structures. Electronegativity. The shapes of molecules. The VSEPR theory. The Valence Bond and the Molecular Orbital theories. The metallic bond. The oxidation number. Chemical reactions. Oxidation-reduction reactions.<br />THE GASEOUS STATE <br />General properties. Ideal and real gases. The ideal gas law. Kinetic molecular theory. Real gases.<br />THE LIQUID STATE<br />General properties, liquefaction of gases, surface tension, vapour pressure. Boiling point.<br />THE SOLID STATE<br />General properties. Ionic, covalent, molecular and metallic crystalline solids. X-ray diffraction. Crystal systems. Unit cells. Polymorphism and isomorphism.<br />INTERMOLECULAR FORCES <br />Repulsive and attractive forces. Van der Waals forces. The hydrogen bond.<br />SOLUTIONS<br />Properties of solutions. Composition of solutions. Solutions of non-electrolytes. Dissolution mechanism. Solubility. Ideal and real solutions. Raoult's law. Colligative properties. Cryoscopy and ebullioscopy, osmosis and osmotic pressure.<br />THERMODINAMICS<br />State functions. The first law. Work and heat. Enthalpy. Termochemistry and applications. Entropy. The second law. The third law. <br />CHEMICAL EQUILIBRIUM<br />Equilibrium constants. Law of mass action. Homogeneous and heterogeneous equilibria. Phase diagram. The phase rule. Effects on the equilibrium constants ( Le Chatelier's principle). Gibbs free energy and equilibrium constant.<br />IONIC EQUILIBRIA<br />Acids and bases. The strength of acids and bases. Acidity constants. Polyprotic acids. Ionic product of water. pH and pOH. Calculation of pH. Hydrolysis. pH indicators. Buffer solutions. Amphoterism. Acid-base titration curves. Solubility product constant.<br />CHEMICAL KINETICS<br />Rates of chemical reactions. Reaction rates and concentrations. Dependence of concentrations on time. First-order and second-order reactions. Activation energy. Effect of temperature on rection rates. Reaction mechanisms. Homogeneous and heterogeneous catalysis.<br />
Full programme
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Bibliography
<br /> RECOMMENDED TEXT-BOOKS:<br /> <br />- R.H.Petrucci,W.S.Harwood,'Chimica Generale,Principi e Moderne Applicazioni',Ed.Piccin, Padova<br />- D. W. Oxtoby, N. H. Nachtrieb, 'Chimica Moderna', EDISES, Napoli<br />
Teaching methods
<br />Frontal lectures<br />Written and oral examinations
Assessment methods and criteria
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Other information
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