B006262 - CHEMISTRY

The atomic model of matter. Periodic system. The chemical bond. Chemical compounds and their reactions; stoichiometry. Phase diagrams. Thermodynamics. Chemical equilibrium. Chemical kinetics. Electrochemistry. Basics of inorganic chemistry and essentials of organic chemistry.

Bertini, Luchinat, Mani, Chimica, Ed.Ambrosiana.
M.S. Silberberg, Chimica, McGraw-Hill.

Knowledge acquiredPhysicochemical fundaments of experimental techniques for the diagnosis in the filed of cultural heritage conservation. Physicochemical aspects of painting techniques, of deterioration phenomena in works of art and of the conservation methodologies.
Competences acquiredFor setting up measurements programme in relationship to the experimental techniques as above described in the knowledge acquired, and for the collection, analysis and interpretation of the results associated to these measurements. For individuating: materials constituting a work of art associated with the executive technique, variables determining the decay of a cultural object, most suitable materials/techniques involved in the conservative intervention.
Skills acquired (at the end of the course)Skills for: (i) applying physicochemical experimental techniques for which the students have acquired knowledge of the fundaments and specific competences to solve easy problems in diagnostics in the field of cultural heritage, (ii) correctly interpreting all the experimental results, (iii) working in a chemical laboratory, (iv) working in team, (v) orally exposing the results of a laboratory chemical experiment, (vi) orally exposing knowledge and competences acquired.

Courses recommended It is recommended to attend contemporarily the mathematics course.

Total hours of the course (including the time spent in attending lectures, seminars, private study, examinations, etc...): 225
Hours reserved to private study and other indivual formative activities: about 140
Contact hours for: Lectures (hours): 42
Contact hours for: Laboratory (hours): 42

Office hours:
Monday 3 p.m.-4 p.m.Friday 3 p.m.-4 p.m.

Written and oral final exam. Written tests are scheduled for mid-term assessments, which replace the final written exam.

The atomic model of matter. Gross atomic structure: atomic nucleus and electrons. Atomic number and mass number. Nuclides and isotopes. Mass atomic unit, nuclide masses on 12C scale, atomic weights, molecular weights, formula weights. The mole and Avogadro’s constant. Relationship between mass, molecular weight, number of moles. Nuclear chemistry. Nuclide distribution in nature. Nuclear binding energy and corresponding mass difference. Radioactive decay and half-life. Nuclear fusion and fission. Electronic structure of the atom. Quantization of microscopic systems. Electromagnetic radiation. Uncertainty principle. Hydrogen atom energy levels, quantum numbers, classification and symbols of hydrogenoid orbitals. Spin properties and quantum number. Many-electron atoms: energy order of orbital subshells, aufbau procedure and atomic electronic configurations.The periodic system of elements: periods, groups and principal and transition groups. Main periodic atomic properties: values of first ionization energy, of atomic (and ionic) radius and electron affinity as a function of atomic number. Relationships between atomic and ionic radii. Electronegativity, as a derived periodic property.The chemical bond. Covalent bond and factors determining its formation. Single covalent bond (σ bond), π bond and multiple bonds. Bond polarity. Octet configuration and octet expansion. Electronic structure (Lewis) formulas; resonance. Molecular geometry and VSEPR theory. Hybrid orbitals.The ionic bond, as a limit of covalent polar bond. Stabilizing factors for the ionic bond in the solid state. Lattice energy. Structures of ionic compounds. Metal bond: its nature and difference from bonds formed by non-metals. Connections between the nature of bond in solids (unlimited 3D covalent, covalent in molecules, ionic, metallic) and some properties of solids. The hydrogen bond. Weak intermolecular (Van der Waals) interactions. Overview of bonding in elements, along the periodic table. Oxidation numbers of atoms in compounds. Main classes of inorganic compounds (hydrides, oxides, hydroxides, oxoacids, salts, coordination compounds): trends in structure and bonding and (acid-base) reactivity. Main types of chemical reactions (precipitation, acid-base, redox), balancing procedures, stoicheiometric calculations. Gaseous, liquid and solid states of matter and transitions among them. The equation of state of perfect gases. Avogadro’s principle. Assumptions of the kinetic theory of gases. Range of molecular speeds. Ideal and real gases: pressure dependence of the compressibility coefficient. Some properties of the liquid state: surface tension, temperature dependence of viscosity. Vapour pressure; distinction between vaporization and boiling. Isoterms in the P/V diagram of a vapour-liquid system; critical parameters. Phase diagrams of one-component systems: water and carbon dioxide. Essentials about the solid state and some structures of solids.Nature of solutions and definitions of solute concentration. Solubility and saturation. Mechanisms of formation of solutions of solids in liquids. Solutions of gases. Colligative properties of solutions. Phase diagrams for two-component systems. Chemical equilibrium. Equilibrium in the gas phase and extension to solutions and heterogeneous conditions. Expression of the equilibrium constant. The Le Chatelier action-reaction principle and its applications; effects of changes in concentrations, pressure and temperature on the equilibrium conditions. Chemical thermodynamics. First and second principles of thermodynamics. State functions: internal energy, enthalpy, entropy and Gibbs free energy. Reaction and formation enthalpy changes. Trend of molar free energy value with temperature. Relationship between standard free energy change and equilibrium constant.Quantitative aspects of acidic and basic properties of substances. Brönsted-Lowry theory. Dissociation of acids and hydrolysis of bases in water. Definitions of the Ka and Kb constants. Fractional ionization. Water self-ionization and ionic product. Conjugate acids and bases. Polyprotic and amphiprotic species. Leveling effect of strong species. Relationship between the equilibrium constant of an acid-base reaction and the Ka and Kb values. Prediction of oxoacid strengths from their formula. Hydrolysis of salts.pH and pOH definitions and ranges of values. Calculation of pH/pOH values for solutions of weak or strong species and in presence of common-ion effects. Distribution curves: trends in concentrations as a function of pH. Buffer solutions: their nature and action, pH calculation. Acid-base titrations.Equilibrium in heterogeneous systems. Solubility product and Kps constant. Connection between Kps and molar solubility. Common-ion effects on solubility. Formation or dissolution of precipitates like hydroxides, carbonates and metal sulfides via pH changes. Complexation-aided dissolution or precipitation inhibition. Chemical kinetics. Definition of reaction rate. Initial rate reaction measurement. Order and molecularity of a reaction. First order reaction kinetics. Catalysis.Electrochemistry. Galvanic cell and cell potential. Standard reference electrode and standard reduction potentials. Reduction potentials and redox processes. Electrochemical series of metals. Dependence of cell potential on concentrations, Nernst equation. Electrolysis. Basic aspects of inorganic chemistry: main classes of inorganic compounds and information on properties of elements of outstanding interest and their compounds.Essentials of organic chemistry.