Chemical Engineering

The program has been divided into three modules each lasting one month. First Module: THE STRUCTURE OF THE MATTER - Fundamental particles of the atom. - Atomic number and mass number of the atom. - Nuclides, isotopes and chemical elements. - Relative atomic mass. - The bulk as a unit of measurement of the quantity of substance and the Avogadro number. ELECTRONIC STRUCTURE OF THE ATOMS AND PERIODIC CLASSIFICATION OF THE ELEMENTS - The Bohr model of the hydrogen atom. - Heisenberg's uncertainty principle. - De Broglie equation and outline of wave treatment. - The atomic orbitals. - Construction of the electronic structure of an atom in its fundamental state: Pauli exclusion principle and maximum multiplicity of Hund. Periodic classification of the elements. Ionization energy, electronic affinity and metallic character of an element. - Atomic radius. CHEMICAL BONDS - MOLECULAR STRUCTURES AND GEOMETRIES - Concept of bonding and binding energy - Atomic (or covalent) bonding. - Double and triple simple atomic bonds. Dative (or coordination) atomic bonds. - Electronegativity of the elements. - Polarity in atomic bonds. Polar and non-polar molecules. - The ionic bond. - The hybridization of atoms and the geometries of molecules. - The metallic bond. SUBSTANCES AND STATIC-CALCULATIONS - Elemental composition of a chemical compound and its minimum formula. - Molecular formulas and units of formula. - Formal relative masses. - Molar mass of a substance. - Quantitative representation of a chemical reaction: stoichiometric (or chemical) equation. - Balancing of a chemical equation. Reagents in stoichiometric or non stoichiometric proportions. Return of a reaction. OXIDATION STATES OF REDOX ELEMENTS AND REACTIONS - Oxidation state of an element in a compound. - Correlation between oxidation states of the elements and their periodic classification. - Variation of the oxidation state of an element: oxidation, reduction and redox reactions. Balancing of redox chemical equations. Redox couple. STATE OF AGGREGATION OF MATTER Gaseous state. Macroscopic properties of gases. Ideal gas and state equation. Kinetic theory of gases. Application of the law of gases in chemistry. Gaseous mixtures: molar fractions, partial pressures, molecular mass (average). - Real gas and Van der Waals equation. - Liquefaction of gases and critical state. Solid state. Ionic solid, solid molecular, solid covalent metal solids. Liquid state. Evaporation and solidification of liquids. Solutions (liquid): solvent and solute (gaseous, solid and liquid), concentration of solutions and concept of saturation. Second Module: CHEMICAL THERMODYNAMICS Thermodynamic and environmental systems: state variables (intensive and extensive), status functions. - Thermodynamic equilibrium, reversible and irreversible transformations. - Mechanical work in thermodynamic transformations. - 1st Principle of thermodynamics. The heat in the transformations at constant volume and in those at constant pressure: the function of state, enthalpy. - Thermal effect in chemical reactions: thermochemical equation. - Standard states of substances. - Additivity of thermochemical equations (Hess law). - 2nd Principle of thermodynamics: the function of entropy state. The entropy at absolute zero (3rd Principle of thermodynamics). - The free energy status function (or Gibbs function). - Criteria for spontaneity and balance in chemical reactions and phase transformations. - The chemical potential. - Variation of the free energy of the system in the progressive advancement of a reaction until equilibrium. - Law of chemical equilibrium: standard (equilibrium) constant of a reaction. Dependence of the equilibrium constant from the temperature: Van t'Hoff equation. The yield of a reaction. EQUILIBRIUM BETWEEN DIFFERENT PHASES OF CHEMICALLY NON-REAGENT SUBSTANCES Single-component systems; - Equilibrium between different phases of the same substance: Clausius equation - Clapeyron. Water status diagram. Fully miscible two-component systems. - Liquid-vapor equilibrium: Raoult's law. Isothermal diagrams "vapor pressure - composition of the liquid phase and the equilibrium phase". Isobar diagrams "boiling temperature - composition of the liquid phase and the equilibrium phase". Distillation. Fully immiscible or partially miscible two-component systems. - Concept of immiscibility and chemical aspect of the phenomenon. Constant distribution of a substance in two immiscible liquids. - Partial miscibility and miscibility gap for liquids and solids. PROPERTY OF SOLUTIONS OF NON-ELECTROLYTE AND ELECTROLYTE SOLUTS Colligative properties: Lowering the vapor pressure of the solvent in passing from pure solvent to solution; lowering the freezing temperature and raising the boiling point of a solution. - Cooling curves, eutectic and peritectic diagrams of solutions and alloys. - The electrical conduction of electrolytic solutions: conductivity, equivalent conductivity and limite equivalent conductivity. Third Module IONIC EQUILIBRIUM IN WATER SOLUTION The law of chemical equilibrium for reactions in solution (Kc). The reaction of self-ionization of the water and its reaction constant (Kw). Definition of acid and base according to Arrhenius. Acid-base reaction according to Bronsted and Lewis. Neutral, acid and basic solutions: pH. Calculation of the pH of solutions of acids, bases, and salts. Calculation of pH of mixtures of acids, bases and strong acid with strong base: neutralization. Low soluble electrolytes: solubility and solubility product (Kso) ELETTROCHIMICA - Semi-redox reactions and their balance with the ionic-electronic method. - Redox reactions and the possibility of converting "chemical energy" into "electricity" and vice versa into electrochemical devices. - The Nernst equation. - Electromotive force of a galvanic element. - Electrode potential and standard electrode potential of a semi-element. - Semi-standard element of hydrogen. - Table of potential reduction standards of redox couples, oxidizing and reducing power of redox pairs. CHEMICAL KINETICS Notes on the reaction speed.

Good basic scientific training (chemical-physical-mathematical).

Main book: Fondamenti di Chimica P. Silvestroni XI edizione a cura di M. Pasquali e A. Latini Casa Editrice Ambrosiana CEA For the part of numerical exercises, the following test is recommended: Problemi di Chimica M. Pasquali e A. Dell'Era Casa editrice Esculapio

The course is provided for the 1st semester of the 1st year. The course is divided into three parts: - The first part concerns the structure of matter; we start from the electronic structure of atoms, the periodic classification of the elements to arrive at explaining the chemical bonds and molecular structures; very important in this context are the stoichiometric calculations of the chemical reactions. At the end of this first part, the states of aggregation of matter are studied: the gaseous state, solid, and liquid. - The second part is entirely focused on chemical thermodynamics, from the thermal effect linked to chemical reactions as thermodynamic transformations, to the law of chemical equilibrium, and its dependence on temperature. Subsequently, the balances between the different states of aggregation of the matter are dealt with both for pure substances and for mixtures of these. Important in this context is the numerical exercises related to the properties of non-electrolyte and electrolyte solutions, including aspects of conductivity. - The third part concerns practical applications of the concepts of equilibrium, in particular, the ionic equilibria in aqueous solution and the electrodic equilibria realized in the batteries. Particular attention will be paid to corrosion phenomena and energy storage systems. Also in this phase numerical exercises are foreseen for the practical consolidation of the theoretical concepts. The course ends by addressing the kinetic aspects of chemical reactions.

Attendance is not compulsory even if it is strongly recommended to take part in lessons due to the complexity of some topics and the vastness of the program.

The student must perform four stoichiometry exercises covering all the topics of the program. The oral exam can be done or by asking open questions in written form and/or a traditional oral. Much weight is given to the interconnections of the various topics in order to ascertain the ability of the student to rationalize and connect the various problems.

Chimica Generale e Inorganica A cura di P. Tagliatesta Fondamenti di Chimica " P. Chiorboli Principi dell’equilibrio chimico " K. Denbigh Valence " McWeeny- Coulson

The course is provided for the 1st semester of the 1st year. The course is divided into three parts: - The first part concerns the structure of matter; we start from the electronic structure of atoms, the periodic classification of the elements to arrive at explaining the chemical bonds and molecular structures; very important in this context are the stoichiometric calculations of the chemical reactions. At the end of this first part, the states of aggregation of matter are studied: the gaseous state, solid, and liquid. - The second part is entirely focused on chemical thermodynamics, from the thermal effect linked to chemical reactions as thermodynamic transformations, to the law of chemical equilibrium, and its dependence on temperature. Subsequently, the balances between the different states of aggregation of the matter are dealt with both for pure substances and for mixtures of these. Important in this context is the numerical exercises related to the properties of non-electrolyte and electrolyte solutions, including aspects of conductivity. - The third part concerns practical applications of the concepts of equilibrium, in particular, the ionic equilibria in aqueous solution and the electrodic equilibria realized in the batteries. Particular attention will be paid to corrosion phenomena and energy storage systems. Also in this phase numerical exercises are foreseen for the practical consolidation of the theoretical concepts. The course ends by addressing the kinetic aspects of chemical reactions.