Italian

No prerequisites required.

Theory lessons, 48 hours

The course aims to provide the foundation for a correct understanding and interpretation of chemical phenomena, upon which the technologies in use in engineering are based. The course is directed to the knowledge of the structure and properties of matter, creating a link between the microscopic and macroscopic world.

The course provides the skills needed to apply the knowledge acquired to the analysis and to the comprehension of chemical problems, through the use of laws and methods which represent the foundation of the chemical phenomena. These capabilities will be acquired by the student with the development of suitable exercises requiring the use of models and methodologies described in the lectures.

The course is designed to stimulate and emphasize connections with the other disciplines, with the aim to improve the learning and communication capacities through the mastery of the basic scientific terminology.

Matter and structure of matter: substances, properties, systems, phases and transformations. The language of chemistry. Symbols, formulas, equations. The quantitative bases. The mass conservation law and of mass - energy. Atomic mass unit. The concepts of relative atomic mass, molecular mass, mole, equivalent mass. The Avogadro Number. The atom. Nucleus and electrons. Atomic number and mass number. The atom structure. The Rutherford experiment. The Heisemberg uncertainty principle and the De Broglie equation. Quantization and quantum numbers. The orbitals. The periodic system of the elements and periodic properties. Atomic radius, atomic volume, ionization energy, electronic affinity, electronegativity, metallic character. The chemical bond according to the Valence Bond theory. Bonding energy, angle and distance. The model of ionic bonding and the Lattice Energy. The covalent bond: the hybridization of the orbitals and molecular geometry; dipole moment and polar molecules. Bonding in metals and electrical conductivity in materials: conductors, semiconductors and insulators; doping examples. The intermolecular bonding: hydrogen bonds, Van der Waals and London interactions. The states of matter. Solid state: ionic solids, covalent, molecular and metallic. Crystal lattices. Properties and defects in crystals. Liquids and liquid solutions: vapor pressure, ideal and real solutions; concentration expressions: molarity, normality, molar fraction, percentages by volume and weight, parts per million. Gases: the ideal gas model and the state equation. The liquefaction of gases. Real gases and their state equations. The chemical transformations. Elements of thermodynamics: reversible and irreversible transformations. The First Principle of Thermodynamics and Thermochemistry: Internal Energy and Enthalpy. Enthalpy and Standard Enthalpy of reaction, of Formation, Combustion, Solution, and phase transition. The Hess law. Spontaneity of a process and Gibbs free energy. Chemical Equilibrium and equilibrium constant. The Van't Hoff isotherm. The Le Chatelier principle. Homogeneous equilibria in gas phase and in solution. Ionic equilibrium in aqueous solution: the concept of acid and base; the pH. Salts: hydrolysis and product solubility. Heterogeneous equilibria. Equilibria between phases. Phase diagrams for one and two components. The Clausius-Clapeyron equation. Cooling curves. The Gibbs Rule Phases. Elements of electrochemical thermodynamics. Batteries: the theory of the electrical double layer; electromotive force of a battery and Nernst equation. Reference electrodes and redox potentials. The phenomenon of corrosion in metals. Electrolysis and Faraday's laws: electromotive force and overvoltage.

The assessment takes place through a written and an oral test within the same scheduled exam.
In the written test, students must deal with stoichiometry problems and
answer to selected theoretical questions.
In the oral exam students are asked to discuss their written test, and to
present the main concepts of basic chemistry developed within the
course.

In the course of the exams, students must demonstrate their basic
chemical knowledge, and must be able to develop appropriate reasoning
for their applications; they must also demonstrate sufficient capabilities
to synthesize and clearly present ideas, concepts and possible solutions
to basic chemical problems typical in engineering.

Marks are expressed on a scale of 30/30, with eventual praise.

The final mark arises from the average of the written and oral exams.
The maximum vote, equal to thirty points (cum laude) out of thirty, is
assigned to students who demonstrate, in both exams, full capability in
the interpretation of the basic chemical phenomena and to set logical
processes for the understanding of basic chemical problems related to
engineering.
The minimum mark, equal to eighteen points out of thirty, is assigned to
students who demonstrate sufficient capability of interpretation of the
basic chemical phenomena, and to set logical processes for the
understanding of basic chemical problems related to engineering

P. Zanello, R. Gobetto, R. Zanoni, “Conoscere la Chimica”, Ambrosiana R. H. Petucci, F. G. Herring, J. D. Madura, C. Bissonnette, “Chimica Generale”, Piccin F. Nobile, P. Mastrorilli, "La Chimica di Base", Ambrosiana P. Atkins, L. Jones, “Principi di Chimica”, Zanichelli R. A. Michelin, A. Munari, "Fondamenti di Chimica" CEDAM
P. Michelin Lausarot, G.A. Vaglio, "Stechiometria per la Chimica Generale" PICCIN
Materiale didattico elettronico disponibile su piattaforma Moodle di Ateneo https://learn.univpm.it/course/view.php?id=7995

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