Mechanical Engineering for the Green Transition

STECHIOMETRIC ELEMENTS, SUBSTANCES AND CALCULATIONS. Structure of the atom. Core structure. Nucleons. Radioactive decay. Fusion and nuclear fission. Atomic number and mass number of an atom. Isotope nuclei and chemical elements. Relative atomic mass of a nuclide and an element. Substances, molecular formulas. Relative molecular masses. Elemental composition of a compound and its minimum formula. Avogadro's constant. Molar mass of a substance. Quantitative representation of a chemical reaction, stoichiometric (or chemical) equation. Reagents in stoichiometric proportions, in defect and in excess. Indirect analysis. ELECTRONIC STRUCTURE OF ATOMS AND CLASSIFICATION PERIODIC OF THE ELEMENTS. Electromagnetic radiation. Bohr's atomic model. Body wave pattern of light. Absorption and emission spectrum of atoms. Heisenberg's principle. The atom according to wave mechanics (orbitals, energy levels, quantum numbers). Schrödinger equation. Construction of the electronic structure of an atom in its ground state: principle of minimum energy, Pauli exclusion principle and maximum multiplicity (or Hund). Electronic construction of the atoms of the elements in their ground state: periodic classification of the elements. Ionization energy, electron affinity and metallic character of an element. CHEMICAL LINKS - MOLECULAR STRUCTURES AND GEOMETRIES. Atomic bond (or covalent): valence bond and molecular orbital theory (outline). Atomic radius, bond distance, bond energy and Morse curve. Simple, double and triple atomic bonds. Polarity in atomic bonds. Polar and non-polar molecules: dipolar moments. Electronegativity of the elements. Ionic bond: lattice energy, Madelung constant. Geometry of molecules: hybrid orbitals. Resonance. Delocalized bonds and electrons (benzene). Metallic bond, properties of metals. Electronic conductors, semiconductors and insulators. Intermolecular dipole-dipole forces (Van der Waals), hydrogen bond, London dispersion forces. Structural formulas. STATES OF OXIDATION OF THE ELEMENTS AND REDOX REACTIONS. Oxidation state of an element in a compound. Correlation between the oxidation states of the elements and their periodic classification. Change in the oxidation state of an element: oxidation, reduction and redox reactions. Balancing of redox chemical equations with electronic method. STATES OF AGGREGATION OF MATTER. Solid state. Macroscopic properties of (crystalline) solids. Ionic solids, molecular solids, mononuclear and heteronuclear covalent solids, metallic solids. Liquid state: Macroscopic properties of liquids. Gaseous state. Macroscopic properties of gases. Ideal gas and equation of state. Application of the gas law. Dalton's law. Real gases and Van der Waals equation. Gas mixtures: molar fractions, partial pressures. NOTES OF CHEMICAL THERMODYNAMICS. System, environment, universe. Endothermic and exothermic reactions. 1st, 2nd and 3rd law of thermodynamics: internal energy, enthalpy, entropy, free energy. Law of Hess. Spontaneity criterion of a transformation (entropy and free energy). BALANCES BETWEEN PHASES. One-component systems: State changes for a one-component system; Clapeyron equation. State diagrams of water and carbon dioxide, vapor pressure, boiling temperature. Two-component systems: Raoult's law, positive and negative deviations. Solutions of non-volatile and non-electrolyte solutes: Colligative properties. Variation in the vapor pressure of the solvent in the pure solvent-diluted solution passage. Variation of the boiling temperature and freezing of the solvent due to the addition of non-volatile and non-electrolyte solute. Osmotic pressure. GASEOUS REACTION BALANCES IN HOMOGENEOUS AND HETEROGENEOUS SYSTEMS. Equilibrium constant of a reaction Kp. Read model (or limit laws) of the chemical equilibrium for homogeneous systems (in the gas phase) and for heterogeneous systems. Gas dissociation: degree of dissociation. Effects on the composition of an equilibrium system caused: a) by a change in the quantity of components. b) from a change in pressure or volume c) from a change in temperature (enthalpy of reaction, Van't Hoff equation). IONIC BALANCES IN WATER SOLUTION. The law of chemical equilibrium for reactions in solution. Standard constant of a reaction Kc in solution. The ionization reaction of water and its self-protolysis constant Kw. Neutral, acidic and basic solutions: pH. Electrolytes with non-ionic and ionic structure: acids and bases (Brønsted-Lowry and Lewis), salts. Inductive effect on the strength of acids. Leveling effect of water. Degree of dissociation. Equilibrium composition and calculation of the pH of "dilute" solutions of acidic, basic and saline solutes. Colliga property tives of electrolyte solutions. ELECTROCHEMISTRY. Balancing of redox reactions with the ionic-electronic method. Galvanic cells; f.e.m. of cell, standard potentials, Nernst equation. Concentration batteries; fuel cells, lead accumulator, commonly used batteries. Corrosion. Electrolysis.

No request

Books: R.Bertani, M.Dettin, M.Mozzon, P.Sgarbossa Fondamenti di Chimica per le Tecnologie - EdiSES or other universitary book about General Chemistry Libri di esercizi : Pasquali Dell'Era - Problemi di Chimica - Esculapio oppure Paterno Parsi Pintauer Gelmini Hilts - Esercizi svolti Chimica Generale - Piccin

The course is organized with lectures, using computerized means and slides. The lectures will be presented with examples of exercises to be carried out in the classroom for providing an overview of some applications of the concepts developped during the lessons, for acquiring the tools for the written exam

Attendance is higly suggested as it is the basic course of the degree course

Written test by 30 questions (multiple answers) plus two exercies of chemistry in 1,5 hour will be held, considering the arguements approached during the course.

The course is organized with lectures, using computerized means and slides. The lectures will be presented with examples of exercises to be carried out in the classroom for providing an overview of some applications of the concepts developped during the lessons, for acquiring the tools for the written exam

STECHIOMETRIC ELEMENTS, SUBSTANCES AND CALCULATIONS. Structure of the atom. Core structure. Nucleons. Radioactive decay. Fusion and nuclear fission. Atomic number and mass number of an atom. Isotope nuclei and chemical elements. Relative atomic mass of a nuclide and an element. Substances, molecular formulas. Relative molecular masses. Elemental composition of a compound and its minimum formula. Avogadro's constant. Molar mass of a substance. Quantitative representation of a chemical reaction, stoichiometric (or chemical) equation. Reagents in stoichiometric proportions, in defect and in excess. Indirect analysis. ELECTRONIC STRUCTURE OF ATOMS AND CLASSIFICATION PERIODIC OF THE ELEMENTS. Electromagnetic radiation. Bohr's atomic model. Body wave pattern of light. Absorption and emission spectrum of atoms. Heisenberg's principle. The atom according to wave mechanics (orbitals, energy levels, quantum numbers). Schrödinger equation. Construction of the electronic structure of an atom in its ground state: principle of minimum energy, Pauli exclusion principle and maximum multiplicity (or Hund). Electronic construction of the atoms of the elements in their ground state: periodic classification of the elements. Ionization energy, electron affinity and metallic character of an element. CHEMICAL LINKS - MOLECULAR STRUCTURES AND GEOMETRIES. Atomic bond (or covalent): valence bond and molecular orbital theory (outline). Atomic radius, bond distance, bond energy and Morse curve. Simple, double and triple atomic bonds. Polarity in atomic bonds. Polar and non-polar molecules: dipolar moments. Electronegativity of the elements. Ionic bond: lattice energy, Madelung constant. Geometry of molecules: hybrid orbitals. Resonance. Delocalized bonds and electrons (benzene). Metallic bond, properties of metals. Electronic conductors, semiconductors and insulators. Intermolecular dipole-dipole forces (Van der Waals), hydrogen bond, London dispersion forces. Structural formulas. STATES OF OXIDATION OF THE ELEMENTS AND REDOX REACTIONS. Oxidation state of an element in a compound. Correlation between the oxidation states of the elements and their periodic classification. Change in the oxidation state of an element: oxidation, reduction and redox reactions. Balancing of redox chemical equations with electronic method. STATES OF AGGREGATION OF MATTER. Solid state. Macroscopic properties of (crystalline) solids. Ionic solids, molecular solids, mononuclear and heteronuclear covalent solids, metallic solids. Liquid state: Macroscopic properties of liquids. Gaseous state. Macroscopic properties of gases. Ideal gas and equation of state. Application of the gas law. Dalton's law. Real gases and Van der Waals equation. Gas mixtures: molar fractions, partial pressures. NOTES OF CHEMICAL THERMODYNAMICS. System, environment, universe. Endothermic and exothermic reactions. 1st, 2nd and 3rd law of thermodynamics: internal energy, enthalpy, entropy, free energy. Law of Hess. Spontaneity criterion of a transformation (entropy and free energy). BALANCES BETWEEN PHASES. One-component systems: State changes for a one-component system; Clapeyron equation. State diagrams of water and carbon dioxide, vapor pressure, boiling temperature. Two-component systems: Raoult's law, positive and negative deviations. Solutions of non-volatile and non-electrolyte solutes: Colligative properties. Variation in the vapor pressure of the solvent in the pure solvent-diluted solution passage. Variation of the boiling temperature and freezing of the solvent due to the addition of non-volatile and non-electrolyte solute. Osmotic pressure. GASEOUS REACTION BALANCES IN HOMOGENEOUS AND HETEROGENEOUS SYSTEMS. Equilibrium constant of a reaction Kp. Read model (or limit laws) of the chemical equilibrium for homogeneous systems (in the gas phase) and for heterogeneous systems. Gas dissociation: degree of dissociation. Effects on the composition of an equilibrium system caused: a) by a change in the quantity of components. b) from a change in pressure or volume c) from a change in temperature (enthalpy of reaction, Van't Hoff equation). IONIC BALANCES IN WATER SOLUTION. The law of chemical equilibrium for reactions in solution. Standard constant of a reaction Kc in solution. The ionization reaction of water and its self-protolysis constant Kw. Neutral, acidic and basic solutions: pH. Electrolytes with non-ionic and ionic structure: acids and bases (Brønsted-Lowry and Lewis), salts. Inductive effect on the strength of acids. Leveling effect of water. Degree of dissociation. Equilibrium composition and calculation of the pH of "dilute" solutions of acidic, basic and saline solutes. Colliga property tives of electrolyte solutions. ELECTROCHEMISTRY. Balancing of redox reactions with the ionic-electronic method. Galvanic cells; f.e.m. of cell, standard potentials, Nernst equation. Concentration batteries; fuel cells, lead accumulator, commonly used batteries. Corrosion. Electrolysis.

No request

Books: R.Bertani, M.Dettin, M.Mozzon, P.Sgarbossa Fondamenti di Chimica per le Tecnologie - EdiSES or other universitary book about General Chemistry Libri di esercizi : Pasquali Dell'Era - Problemi di Chimica - Esculapio oppure Paterno Parsi Pintauer Gelmini Hilts - Esercizi svolti Chimica Generale - Piccin

The course is organized with lectures, using computerized means and slides. The lectures will be presented with examples of exercises to be carried out in the classroom for providing an overview of some applications of the concepts developped during the lessons, for acquiring the tools for the written exam

Attendance is higly suggested as it is the basic course of the degree course

Written test by 30 questions (multiple answers) plus two exercies of chemistry in 1,5 hour will be held, considering the arguements approached during the course.

The course is organized with lectures, using computerized means and slides. The lectures will be presented with examples of exercises to be carried out in the classroom for providing an overview of some applications of the concepts developped during the lessons, for acquiring the tools for the written exam