Chemistry 1 - (9 cfu)

Prof. Chiara Massera Tel. 0521.905428 - Fax. 0521.905557
  E-mail. massera@unipr.it
 


Finalità

To give the foundamental knowledge about the atomic and molecular structure of matter, in order to interpret the chemical-physical properties and the transformations which can be useful in technical areas.

Programma

Historical development of atomic theory. Subatomic particles. Principles of stoichiometry
Electronic structure of atoms
Early atomic models: the Bohr atom; wave mechanical models. Multielectronic atoms and the Aufbau principle. Electron configurations of the elements in the periodic table. Periodic properties of the elements.
Chemical bonds
Ionic bond, covalent bond, electronic delocalization and resonance. Polar covalent bond. Electronegativity. Molecular geometry and polarity. Metal bond (band theory from MO model). Conductors, insulators and semiconductors. Van der Waals forces and hydrogen bond.
Nomenclature
Oxidation numbers, classification and nomenclature of inorganic compounds. Types of chemical equations.
Thermochemistry and thermodynamics
The First Law. Enthalpy. Heat of formation, thermochemical equations, Hess’s Iaw and enthalpy diagrams.
The gaseous state
Introduction. Equation of state of an ideal gas. Real gases. Kinetic theory. Partial pressure and partial volume. Gas Iiquefaction, critical temperature.
The Iiquid state
Introduction. Evaporation. Vapour tension and its dependence from the temperature. Relative humidity. Boiling. Sublimation. Fusion and solidification. H20 and C02 phase diagrams.
The solid state
Crystalline and amorfous solids. Crystal lattice and lattice planes. Primitive and non-primitive cells. X-ray diffraction. Covalent, ionic, molecular and metallic crystals. Polymorphism.
Solutions
Nature of solutions. Concentration of solutions. Raoult’s Iaw. Colligative properties of solutions.
The van’t Hoff coefficient.
Chemical equilibrium
Chemical equilibrium: the Iaw of mass action. The equilibrium constants Kp and Kc. Omogeneous and eterogeneous equilibrium. The Le Chatelier—Braun principle.
Equilibria in solution
Acids and bases: Arrhenius’ theory, the Brønsted-Lowry theory. Water autoionization. The ionic product of water. The pH scale
Electrochemistry
Electrolytic cells. Electrolysis and its applications. Stoichiometry of electrolysis. Galvanic cells. Stoichiometry of galvanic processes. Electrode potentials and electromotive force (emf) in standard conditions. Nernst equation. Applications. Corrosion.
Kinetics of reaction
Reaction rates. Rate Iaws and reaction order. Factors affecting reaction rates: radiations, concentration of reactants, temperature, catalysts. Temperature-dependence of reaction rates, Arrhenius equation, activated complex theory, activation energy. Catalysis. Catalytic converters.

Attività d'esercitazione

Exercises in preparation of the written exam.

Modalità d'esame

Written and oral exams.

Propedeuticità

None, but a good knowledge of mathematics is recommended.

Testi consigliati

A.M. Manotti Lanfredi, A. Tiripicchio, “Fondamenti di Chimica”, Ed. Ambrosiana, Milano
A.M. Manotti Lanfredi, “Appilcazioni di fondamenti chimici” , Ed. Pitagora, Bologna
F. Ugozzoli “La Chimica in Numeri”, Ed. Santa Croce, Parma


Ultimo aggiornamento: 08-02-2010


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