Aerospace engineering

The course aims to provide the methodological approach and basic concepts for the study of the transformations of matter (atomic and molecular structure, thermodynamic and kinetic aspects). Phenomenological content will also be addressed, for example state diagrams, acid-base balances, electrochemical processes. The intent is to guide the student in understanding the close correlation between the microscopic structure of matter and its not only chemical-physical properties. The exercises will explore some of the topics covered in class with numerical examples. Detailed Syllabus: Elements, Materials, and stoichiometry Fundamental particles in an atom. Atomic number and mass number. Nuclides, isotopes and elements. Relative atomic mass of a nuclide and an item. Mole. Substances, molecular formulas and units of the formula. Molecular masses and masses on its formal. Elemental composition of a compound and its formula minimum. Amount of substance and Avogadro constant. Molar mass. Quantitative representation of a chemical reaction. Reagents in stoichiometric proportions, in the absence and in excess. Elements, Substances and Stoichiometric Calculations (8 hours) Fundamental particles in an atom. Atomic number and mass number. Nuclides, isotopes and elements. Relative atomic mass of a nuclide and an element. Mole. Substances, chemical formulas. Relative molecular masses and relative formal masses. Elemental composition of a compound and its minimum formula. Amount of substance and Avogadro's constant. Molar mass. Representation quantity of a chemical reaction. Reactants in stoichiometric proportions, in defect and in excess. Electronic Structure of Atoms and Periodic Classification of Elements (6 hours) The discovery of elementary particles. Wave model – corpuscular of light. Atomic spectra. Blackbody emission spectrum. Photoelectric effect. Bohr's quantum model of the hydrogen atom. Heisenberg's uncertainty principle. De Broglie's formula. Quantum numbers. Quantum-wave model of the hydrogen atom: orbitals and their shape. Electronic structure of polyelectronic atoms: Pauli exclusion principle and maximum multiplicity. Periodic table, main periodic properties of the elements and their trend: Ionization energy, electron affinity, electronegativity, atomic radius. The chemical bond - Molecular structures and geometries (8 hours) Covalent bond. Single, double and triple bonds. Dative link. Polarity in atomic bonds. Polar and non-polar molecules: dipole moment. Lewis structures. Resonance. Ionic bond: lattice energy. Valence bond theory. Hybrid orbitals. VSEPR theory. Intermolecular forces: ion-dipole, dipole-dipole, hydrogen bonding, London dispersion forces. Molecular orbitals (outline). Metallic bond. States of Oxidation of Elements and Redox Reactions (6 hours) Oxidation state of an element in a compound. Nomenclature. Variation of the oxidation state of an element: oxidation, reduction and redox reactions (in aqueous solution). Balancing of redox chemical equations with the ion-electronic method. States of Aggregation of Matter (8 hours) gaseous state. Macroscopic properties of gases. Ideal gas: gas laws and equation of state. Gaseous mixtures: molar fractions, partial pressures. Real gases, van der Waals equation and Andrews diagrams. Kinetic theory of gases. liquid state. Macroscopic properties of liquids. Vapor pressure, temperature effect. Evaporation and boiling. Solutions (liquid): passage of a solid or liquid species into solution. Ideal solutions. Concentration of solutes, dilution and mixing of solutions. solid state. Classification of solids. Crystalline solids, Bravais lattices. Ionic solids, lattice energy. Covalent solids. Molecular solids. Metallic solids. Bond in solids. Macroscopic properties. Allotropy and polymorphism Energetics of physico-chemical transformations (9 hours) Thermodynamic systems: state of equilibrium, reversible and irreversible transformations. 1st law of thermodynamics. Heat in constant volume and constant pressure transformations: the enthalpy state function. Thermal effect in chemical reactions: thermochemical equation. Standard states of substances. Standard molar enthalpy of formation. Additivity of thermochemical equations (Hess law). The entropy state function. The free energy state function (or Gibbs function). Criteria of spontaneity and equilibrium in chemical reactions and phase transformations. Free energy and useful work. Equilibria between different phases of chemically non-reacting substances (12 hours) Single component systems: Heating/cooling curves. Equilibria between different phases of the same substance: Clausius-Clapeyron equation. State diagrams, general information. State diagram of water. Two-component systems: Liquid-vapour mixture equilibrium: Raoult's law and related isotherm and isobaric diagrams of ideal and non-ideal solutions (positive and negative deviations); distillation. Azeotropic blends. Transition of liquid-solid state. Miscible solid solutions in the liquid state and in the solid state (isobar diagrams and heating/cooling curves). Eutectic and refrigeration mixtures (isobar diagrams and heating/cooling curves). Phase rule and its applications to systems with one or more chemically non-interacting components. Composition of solutions and their properties (5 hours) Expressions of the concentration of solutions (Molarity, molality, mole fraction, weight percentage) and transitions between different units. Colligative properties: lowering of the vapor pressure of a solution. Cryoscopy, Ebullioscopy, Osmosis. Chemical Kinetics: general information (2 hours) Reaction speed. Reaction mechanism: elementary reactions and multistep reactions. Kinetic law. Influence of temperature on the reaction rate: activation energy. Transition state theory and activated complex. Homogeneous and heterogeneous catalysis (outlines). Reaction equilibria in homogeneous and heterogeneous systems (7 hours) General information on homogeneous and heterogeneous chemical equilibria. Equilibrium constant of a homogeneous and/or heterogeneous reaction. Influence of change in composition, pressure or volume on equilibrium at constant temperature. Relationship between equilibrium constant and free energy; influence of temperature on equilibrium (van't Hoff equations). Ionic equilibria in aqueous solution (7 hours) The law of chemical equilibrium for reactions in solution. Constant of a reaction in solution. The self-ionization reaction of water and its standard constant. Definition of acid and base according to Arrhenius, Bronsted-Lowry. Neutral, acidic and basic solutions: pH. Calculation of the pH of diluted solutions of solutes consisting of strong acids and bases, monoprotic weak acids and bases, salt hydrolysis. Buffer solutions (only with weak monoprotic acids and their strong base salts). Solubility of salts, solubility product; common ion effect. Electrochemical potentials and corrosion phenomena (12 hours) Redox half-reactions and their balancing with the ionic-electronic method. Possibility of conversion of "chemical energy" into "electrical energy" and vice versa in electrochemical devices. Potential and standard potential of a galvanic semi-element. Table of standard redox couple reduction potentials and its applications. Electrolysis: electrolysis of water and of molten salts. Faraday's laws. Electrolytic refining of metals (Cu). Metal corrosion (galvanic and differential aeration mechanism) and passivation. Corrosion protection methods.

The student who accesses this course does not need specific prerequisites relating to the knowledge of the fundamental principles of Chemistry. The lessons will be held in Italian, therefore it is necessary to understand the Italian language in order to profitably follow the course and to be able to use the teaching material provided. It is important to master the following preliminary knowledge: • Fundamental concepts of elementary algebra, use of powers and logarithms, methods for the resolution of first and second degree equations and systems of linear equations. Elements of mathematical analysis (limits, derivatives, integrals, functions) • Elements of physics (mechanics, thermodynamics, electromagnetism).

Teoria: M. SCHIAVELLO-L. PALMISANO: Fondamenti di Chimica (quinta Edizione) - Ed. EdiSES P. Atkins, L. Jones, L. Laverman: Fondamenti di Chimica Generale - Zanichelli II ed. P. Silvestroni, Fondamenti di Chimica - XI edizione - casa ed. ambrosiana (È comunque possibile utilizzare altrii testi di Chimica di livello universitario) Per le esercitazioni di Stechiometria: - R. Michelin, P. Sgarbossa, M. Mozzon, A. Munari; CHIMICA - TEST ED ESERCIZI - Casa Editrice Ambrosiana - Stechiometria; F. Cacace, M. Schiavello; Bulzoni Editore - Stechiometria - Un avvio allo studio della chimica -Bertini, Luchinat, Mani, Ravera - Casa Editrice Ambrosiana - Esercizi di Chimica Generale; Alessandro Del Zotto; ed. EdiSES

The course has the following organization: • explanation of the topics in the classroom • resolution of numerical problems in the classroom • self-assessment tests The student will find on the e-learning platform the slides and teaching material (examination procedures, program, recommended texts) useful for the preparation of the exam. It is understood that the slides are a guide to the exam topics, but can never replace the recommended texts and lectures given by the teacher. The student can ask the teacher additional explanation on appointment.

Recommended. Attendance aims to improve the quality of learning and to give a track record for the exam. Students who cannot attend the lessons can download the detailed program and the teaching materials from the e-learning website, and receive assistance from the teacher.

The exam consists of a written test with numerical exercises and open theoretical questions. The exams take place at the end of the course during the exam periods provided for by the university teaching regulations, while ongoing tests are excluded in order not to interfere with the conduct and regular attendance of the semester's lessons. The written test consists in solving 3-4 stoichiometry problems and 4-5 theoretical questions on topics and problems covered in class.. The duration of the test is between 1 hour and a half and two hours depending on the number of questions / exercises. It is possible to consult the Periodic Table of the Elements and a form provided by the teacher. The test is considered passed if the student correctly completes at least 50% of the exercises and if he answers at least 50% of the questions correctly. The weight of the exercises and theoretical questions for the purposes of the overall assessment are equivalent. Exercises and questions cover the entire study program and are designed to ensure that the student has acquired the basic concepts of General Chemistry and has also acquired the ability to apply them to the main topics covered in the course. The purpose of the exam also consists in verifying the level of understanding and deepening on the subject exposed during the course. It also intends to evaluate the student's reasoning skills and the ability to summarize the arguments carried out in the vision of an organic framework of the subject.

- P. Silvestroni, Fondamenti di Chimica - XI edizione - casa ed. ambrosiana

The course has the following organization: • explanation of the topics in the classroom • resolution of numerical problems in the classroom • self-assessment tests The student will find on the e-learning platform the slides and teaching material (examination procedures, program, recommended texts) useful for the preparation of the exam. It is understood that the slides are a guide to the exam topics, but can never replace the recommended texts and lectures given by the teacher. The student can ask the teacher additional explanation on appointment.

Ionic equilibria in aqueous solution The law of equilibrium chemical reactions in solution. Standard constant of a reaction in solution. The reaction of water and its constant autoionizzazione standards. Solutions neutral, acidic or basic pH. Electrolytes in non-ionic and ionic structure of acids and bases, salts and anfoliti. Composition of balance. Calculating the pH of dilute solutions of solutes consisting of salts, acids and bases monoprotiche and solutions obtained by mixing solutions acido-forte/base strong, weak acid / strong base and strong base / weak acid. Buffer solutions. Equilibria in saturated solutions of sparingly soluble compounds. Solubility product. To common ion effect. Oxidation States of Elements and Redox Reactions Oxidation state of an element in a compound. Variation of the oxidation state of an element: oxidation, reduction and redox reactions (aqueous solution). Balancing chemical equations with the redox ion-electronic method. Electrochemical and corrosion potential Redox half reactions and balance them with the ionic-electronic method. Possibility of conversion of "chemical energy" to "electricity" and vice versa in electrochemical devices. Potential and standard potential of a galvanic half cells. Table of standard reduction potentials of redox couples and its applications. electrolysis. Electrolysis of H2O and in molten salts. Electrolytic refining of metals (Cu). Commercial cells. Fuel cells. Rechargeable cells. Corrosion of metals (galvanic mechanism and differential aeration) and passivation. Methods of corrosion protection.

Theory and exercises: M. SCHIAVELLO-L. PALMISANO: Fondamenti di Chimica (Fifth Edizione) -Ed. EdiSES for further insights: P. SILVESTRONI: Fondamenti di Chimica (11th Edition, managed by M. Pasquali, A. Latini)-Ed. Casa Editrice Ambrosiana