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Electronic stucture of atoms. The Bohr theory. Heisemberg uncertainty principle. The nature of the light. Photoelectric effect. The de Broglie relation. Schrodinger equation. Atomic orbital shapes. Electron configurations and periodicity. Chemical bonds. Atomic weight and molecular weight. The mole concept. Electronegativity. Metals and nonmetals. Covalent, polar-covalent, ionic bond. Hybrid orbitals. The resonance concept. Delocalizated bonding. Metal bond. Inter-molecular bonds. Molecular geometry Chemical thermodynamics. The first low of thermodynamics. Hess’ law. Spontaneity of chemical reactions. Entropy. The second law of thermodynamic. Free energy and useful work. Free energies and equilibrium. States of matter. The ideal gas. The combined gas law. Dalton’s law of partial pressures. Kinetic molecular theory. The real gases Vapor pressures of liquids. Cristalline solids. Liquid crystals. Heating and cooling curves. Changes of states. Clausius-Clapeyron equation. Phase diagrams. Chemical Kinetics. Rate laws. Reaction orders. The Arrhenius equation. Reaction mechanism. Catalysts. Chemical equilibrium. The equilibrium constant. Thermodynamics and chemical equilibrium The pressure and the temperature in the chemical equilibrium. Acids and bases. Acid-base equilibria in aqueous solution. Ionization of water and pH. Dissociation of weak electrolites. Buffers. Hydrolysys. Acid-base indicators. Properties of the solutions. Concentration units. Rault’s law. Fractional distillation. Colligative properties of the solutions.

Basic notions of mathematics.

a book on Stoichiometry - N. J. Tro, Chimica, Casa Editrice Edises (with exercises) - Chimica Generale – Petrucci, Herring, madura, Bissonnette – Piccin (2013) (with exercises) - T. L. Brown, H. E. LeMay, C. J. Murphy, P. Woodward, Fondamenti di Chimica, Casa Editrice Edises (with exercises)

Lessons if possible in person, otherwise in blended or online mode.

No obligation to attend

Written and oral ezam, if possible in person, otherwise online.

Lessons in classroom

ELEMENTS, SUBSTANCES, AND STOICHIOMETRIC CALCULATIONS. Structure of the atom. Structure of the nucleus. Nucleons. Radioactive decay. Nuclear fusion and fission. Atomic number and mass number of an atom. Isotopic nuclides 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 empirical formula. Avogadro's constant. Molar mass of a substance. Quantitative representation of a chemical reaction, stoichiometric (or chemical) equation. Reactants in stoichiometric proportions, in deficit and excess. Indirect analysis. ELECTRONIC STRUCTURE OF ATOMS AND PERIODIC CLASSIFICATION OF ELEMENTS. Electromagnetic radiation. Bohr's atomic model. Wave-particle duality of light. Absorption and emission spectrum of atoms. Heisenberg's principle. The atom according to wave mechanics (orbitals, energy levels, quantum numbers). Schrödinger's equation. Construction of the electronic structure of an atom in its ground state: principle of minimum energy, Pauli exclusion principle, and Hund's rule of maximum multiplicity. Electronic construction of the atoms of elements in their ground state: periodic classification of elements. Ionization energy, electron affinity, and metallic character of an element. CHEMICAL BONDS - STRUCTURES AND MOLECULAR GEOMETRIES. Atomic (or covalent) bond: valence bond theory and molecular orbital theory (briefly). Atomic radius, bond distance, bond energy, and Morse curve. Single, double, and triple atomic bonds. Polarity in atomic bonds. Polar and non-polar molecules: dipole moments. Electronegativity of 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. OXIDATION STATES OF ELEMENTS AND REDOX REACTIONS. Oxidation state of an element in a compound. Correlation between oxidation states of elements and their periodic classification. Variation of the oxidation state of an element: oxidation, reduction, and redox reactions. Balancing redox chemical equations using the electronic method. STATES OF AGGREGATION OF MATTER. Solid state. Macroscopic properties of solids (crystalline). 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 state equation. Application of gas law. Dalton's law. Real gases and Van der Waals equation. Gaseous mixtures: molar fractions, partial pressures. BASICS OF CHEMICAL THERMODYNAMICS. System, environment, universe. Endothermic and exothermic reactions. 1st, 2nd, and 3rd principles of thermodynamics: internal energy, enthalpy, entropy, free energy. Hess's law. Criterion of spontaneity of a transformation (entropy and free energy). PHASE EQUILIBRIA. Single-component systems: State transitions for a single-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 solutes and non-electrolytes: Colligative properties. Variation of solvent vapor pressure in the transition from pure solvent to dilute solution. Variation of boiling and freezing temperatures of the solvent by adding non-volatile and non-electrolyte solute. Osmotic pressure. CHEMICAL KINETICS. Reaction rate. Reaction order. Arrhenius equation. Reaction mechanisms. Catalysis. GASEOUS REACTION EQUILIBRIA IN HOMOGENEOUS AND HETEROGENEOUS SYSTEMS. Equilibrium constant of a reaction Kp. Model laws (or limit laws) of chemical equilibrium for homogeneous systems (in gaseous phase) and for heterogeneous systems. Gaseous dissociation: degree of dissociation. Effects on the composition of an equilibrium system caused by: a) variation in the quantity of components, b) variation in pressure or volume, c) variation in temperature (reaction enthalpy, Van't Hoff equation). IONIC EQUILIBRIA IN AQUEOUS SOLUTION. Chemical equilibrium law for reactions in solution. Standard constant of a reaction Kc in solution. Ionization reaction of water and its autoprotolysis constant Kw. Neutral, acidic, and basic solutions: pH. Non-ionic and ionic electrolytes: acids and bases (Brønsted-Lowry and Lewis), salts. Inductive effect on acid strength. Leveling effect of water. Degree of dissociation. Equilibrium composition and pH calculation of "dilute" solutions of acidic, basic, and saline solutes. Colligative properties of electrolyte solutions. ELECTROCHEMISTRY. Balancing redox reactions using the ionic-electronic method. Galvanic cells; cell emf, standard potentials, Nernst equation. Concentration cells; fuel cells, lead-acid accumulator, common batteries. Corrosion. Electrolysis.

Basic knowledge of mathematics, physics and chemistry are required.

To support the slides provided by the instructor and used during classroom lessons, any university chemistry textbook is suitable for studying the topics covered in the course. Below, as an example, are some titles: Fondamenti di Chimica - Silvestroni (11th ed., 2020, Casa Editrice Ambrosiana) Fondamenti di Chimica - Michelin, Munari (1st ed., 2019, Casa Editrice Ambrosiana) Fondamenti di Chimica - Brown, LeMay, Bursten, Murphy, Woodward, Stoltzfus (4th ed., 2018, EdiSES) Chimica Generale - Laird (1st ed., 2010, McGraw-Hill) Chimica, Test ed Esercizi - Michelin, Sgarbossa, Mozzon, Munari (1st ed., 2018, Casa Editrice Ambrosiana)

Attendance is not mandatory but recommended.

Through Midterm Exams: 2 written midterm exams that will contribute respectively 40% (first exam) and 60% (second exam) to the overall grade. Through Single Exam: A single written exam that will contribute 100% to the overall grade. At the student's request, there will be the possibility to take an additional oral interview.

The Course is divided into a series of lectures (in person and/or remotely) using the projection of slides. There are also several hours dedicated to exercises. The slides used to support the lessons are available during the entire duration of the Course on the Professor's website, together with self-assessment tests.