Learning objectives
the corse objectives include giving the student those instuemtns necessary for understanding the basic features and behaviour of matter and teaching the student the basic principles of physics and chemistry and the solving of stechiometric problems
Course unit content
<br />1) definition of system and environment, isolated, closed and open systems; 2) definition of state functions; 3) energy: kinetic and potential energy; heat and work; enthalpy; free energy and enthropy. 4) the atomo: protons, neutrons, electrons; eletronic structure: quantum theory; 5) the periodic table; 6) chemical bonds: ionic bond, covalent bond (Lewis’s theory, Valence bond theory and molecular orbital theory): molecular form: hydrogen bond: van der waals and London’s dispersion interactions; 7) chemical reactions: stechiometric caclulations; 8) the gas state: the ideal gas and real gases; 9) the liquid state: evaporation and vapor pressure; boiling temperature and its variation with pressure; 10) solid state: sublimation and vapore pressure: melting temperaO2; 12) solution state: solutes and solvents: enthralpic and enthropic balances during the solution process: solubility, the ideal solution and real solutions: Rault’s law and Henry’s law: state diagramms of acqueous solutions with non volatile solutes; fractionated distillation; 13) chemical equilibrium: homogeneous and hetereogeneous equilibria, definition of activity: Kc, Kp, reaction quotient Q; principle of mobile equilibrium; 14) acids and bases according to Arrhenius, Bronstead and Lewis; forces of acids and bases; solution equilibrium: Ka, Kb, pH; hydrolysis; buffer solutions, acid/base titration; indicators; 15) insoluble and solubility equilibria: Kps; 16) thermodynamics: first principle: dU and dH: calorimetry; bond, formation and combustion enthalpies, Hess’s law; second principle: definition of enthropy and its physical meaning; relationship bewteen G,H and S; definition of ÄGr and Q: extent of reactions: “ÄH driven ” “ÄS driven” reactions; 17) electrochemistry: the electrochemical cells; the Nernst equation; relationship between ÄGr and the potential difference between the half cells: concentration cells; the pH-meter; electrolysis; 18) chemical kinetics: kinetic equations; reaction order and its determination; zero, I° and II° reaction orders; half-life; elementary reactions and reaction meccanisms; collision theory; 20) inorganic chemistry: hydrogen, nitrogen oxygen sulphur, phosphoros, halogens and principle transtion elements.
Bibliography
<br /><br />P.W. Atkins, L. Jones: Chimica Generale, Zanichelli (1998);<br />S. S. Zumdahl: Chimica, Zanichelli (1993)<br />P. Michelin Lausarot, G. A. Vaglio: Stechiometria per la Chimica Generale, Piccin (2005)<br />Gianluigi Ingletto: Esercizi di Chimica, UNI.NOVA (2006)
Teaching methods
<br />lectures and practicals<br />written and oral examination
