Civil Engineering

Atomic structure, atomic symbols, atomic and mass numbers, isotopes, ions, periodic table and periodicity of physical magnitudes. Atomic mass, moles, molarity and other forms for expressing the concentration of solutions, dilutions, chemical reactions, chemical equations and equation balancing. Waves and particles, the shell model and periodic table, electron configurations, sizes of atoms and their ions, orbitals, quantum numbers and meaning, Hund’s rule and the Pauli principle, ionisation energie Valence electrons, covalent bonds, Lewis structures, bond lengths, electronegativity, partial and formal charges, orbital shape, molecular shape, polarity, the valence bond theory, hybrid atomic orbitals, double and triple bonds, molecular orbital theory, ionic bonds, introduction to metallic bonds, oxidation numbers. Temperature as a property of matter, states of matter, properties of gases, the ideal gas law, Dalton’s law of partial pressures, molecular kinetic theory. Deviation from a perfect gas. Energy and heat, the first principle of thermodynamics, state functions, reaction enthalpy, standard states, Hess’s law, enthalpy of formation. The structure of liquids, intermolecular forces, vapour pressure, melting, freezing and boiling points, colligative properties, osmotic pressure, solubility. Reactions that go to completion, equilibrium constant expression, reaction quotient, temperature effect, Le Châtelier’s principle, calculation of the equilibrium constant. Properties of acids and bases, definition according to Brønsted-Lowry, conjugated acid-base pairs, dissociation of water, pH, strength of acids and bases, pH calculation for weak and strong acids and bases, amphoteric compounds, salts and pH thereof, indicators. Recognising redox reactions, reaction stoichiometry and balancing, oxidating and reducing agents, voltaic cells, standard potentials, batteries, electrolytic cells, Faraday’s law, electrochemical cells in non-standard conditions, Nerst’s equation. Spontaneous processes, entropy and what it means, the second and third principle, standard entropy, Gibbs’ free energy, standard free energy, relationship between free energy and the equilibrium constant, dependency of equilibrium constants on temperature. Electrode systems. The half-reaction concept. Galvanic cells. The Nernst equation. Electrolysis Corrosion.

Mathematical, chemical and physical knowledge at secondary school level. It is necessary to have preliminary chemistry knowledge however chemistry course starts from the elementary concepts of this matter.

It is recommended any university text on General and Inorganic Chemistry eg T. L. Brown, H. E. LeMay, C. J. Murphy, P. Woodward, Fondamenti di Chimica, Casa Editrice EdiSES (with exercises) - I. Bertini, C. Luchinat, F. Mani, Chimica, Casa Editrice Ambrosiana per la stechiometria: - I. Bertini, C. Luchinat, F. Mani, Stechiometria, Casa Editrice Ambrosiana -Paola Michelin Lausarot, Gian Angelo Vaglio, Stechiometria per la Chimica Generale, Casa Editrice Piccin -P. D’Arrigo, A. Famulari, C. Gambarotti, M. Scotti, Chimica Esercizi e casi pratici Casa Editrice EdiSES

attendance not mandatory

Written and oral exam.

lectures and exercises in presence