Mechanical Engineering

THE STRUCTURE OF MATTER - fundamental particles in an atom. - atomic number and mass number of an atom. - Nuclides, isotopes and chemical elements. - Relative atomic mass. - The mole as a measure of the amount of substance, and the Avogadro's number. Electronic structure of atoms AND PERIODIC CLASSIFICATION OF THE ELEMENTS - The Bohr model of the hydrogen atom. - uncertainty principle. - Equation of de Broglie - The atomic orbital. - Construction of the electronic structure of an atom. Pauli exclusion and the maximum multiplicity (or Hund) principles. Periodic Classification of the elements. Ionization energy, electron affinity and metallic character of an element. - Atomic radius. CHEMICAL BONDS - STRUCTURES AND MOLECULAR GEOMETRY - binding concept and the binding energy - The atomic bond (covalent). - atomic bonds simple double and triple. datives atomic bonds (or coordination). - Electronegativity of the elements. - Polarity in the atomic bonds. polar and non-polar molecules. - The ionic bond. - The hybridization of the atoms and molecules of geometries. - The metallic bonding. SUBSTANCES AND CALCULATIONS stoichiometric - Elemental composition of a chemical compound and its minimum formula. - Formulas and molecular units of formula. - related formal Masses. - Molar mass of a substance. - quantitative representation of a chemical reaction: stoichiometric equation (or chemical). - Balancing a chemical equation. Reagents in stoichiometric or non-stoichiometric proportions. Efficiency of a reaction. OXIDATION STATES OF ELEMENTS AND REACTIONS Redox - oxidation state of an element in a compound. - Correlation between oxidation states of the elements and their periodic classification. - Change the state of an element oxidation: oxidation, reduction and redox reactions. Balancing redox chemical equations. Redox couples. 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 gases and equation of Van der Waals. - liquefaction of gas and was critical. Solid state. ionic solids, molecular solids, solid metal covalent solids. Liquid State. Evaporation and solidification of liquids. Solutions (liquid): solvent and solute (gaseous, solid and liquid), concentration of the solutions and saturation concept. CHEMICAL THERMODYNAMICS thermodynamic and environmental systems: state variables (intensive and extensive), state functions. - The thermodynamic equilibrium, reversible and irreversible transformations. - Mechanical work in thermodynamic processes. - 1st law of thermodynamics. The heat at constant volume and in those transformations at constant pressure: the state function, enthalpy. - Thermal effect in chemical reactions: thermochemical equation. - standards of substances States. - Additivity of thermochemical equations (Hess Law). - 2nd law of thermodynamics: entropy function. The entropy at zero absolute (3rd principle of thermodynamics). - The free energy function (or Gibbs function). - Criteria of spontaneity and equilibrium in chemical reactions and phase transformations. - The chemical potential. - free energy of the system change in the progressive advancement of a reaction until equilibrium. - chemical equilibrium Law: standard constant (equilibrium) of a reaction. Dependence of the equilibrium constant on the temperature: equation Van t'Hoff. The yield of a reaction. BALANCE BETWEEN DIFFERENT LEVELS OF SUBSTANCES NOT CHEMICALLY REAGENTS Systems with a single component. - equilibria between different phases of the same substance: Clausius - Clapeyron. Diagram of state of water. Systems with two completely miscible components. - The vapor-liquid equilibrium: Raoult's law. isothermal Diagrams "vapor pressure - composition of the liquid phase and the vapor phase in equilibrium". isobars Diagrams "boiling temperature - composition of the liquid phase and the vapor phase in equilibrium". Distillation. completely immiscible or partially miscible two-component systems. - immiscibility Concept and chemical aspect of the phenomenon. distribution constant of a substance in two immiscible liquids. - Partial Miscibility and miscibility gap for liquids and solids. - colligative properties: Lowering of the solvent vapor pressure,passing from pure solvent to solution; lowering the freezing temperature and increasing the boiling temperature of a solution. - Cooling curves, eutectic and peritectic diagrams of solutions and alloys. - The electrical conductivity of electrolytic solutions: conductivity, equivalent conductivity and limit equivalent conductivity. IONIC EQUILIBRIUM IN SOLUTION The chemical equilibrium law for reactions in solution (Kc). The reaction of auto-ionization of water and its constant (Kw). Definition of acid and base according to Arrhenius. Acid-base reaction according to Bronsted and Lewis. Neutral solutions, acids and bases: pH. Calculation of pH of solutions of acids, bases and salts. Calculation of the pH of mixtures of acids, bases and strong acid with a strong base: neutralization. Electrolytes slightly soluble: solubility and solubility product (Kso) Electrochemistry - Semi redox reactions and their balancing with ionic-electronic method. - - The Nernst equation. - Electromotive force of a galvanic element. - potential electrode and the standard electrode potential of the semi elements. - standard hydrogen semi-element. - Table of standard reduction potentials, oxidizing power. Mention on CHEMICAL KINETICS

basic knowledge of math

Chimica generale e inorganica authors: Tagliatesta - Failla - Paolesse - Pasini - Pasquali - Valli Ed. Edi Ermes Fondamenti di chimica authors: Paolo Silvestroni Ed. Zanichelli Problemi di chimica authors: Mauro Pasquali Alessandro Dell'Era Ed. Esculapio

classroom lessons and training by periodic exercises in which students can perform exercises collaborating with each other and they can ask the teacher.

not required

written test and subsequent oral test. The written test will consist of 3-4 exercises and will last 2.5-3 hours. The oral test will be a question lasting about 30-40 minutes. The examinations will fall on the dates established by the university but there would be a kind of pre-test. To pass the exam it is necessary to obtain a mark not less than 18/30. The student must demonstrate to have acquired sufficient knowledge of the subjects.To achieve a score of 30/30 cum laude, the student must instead demonstrate that he has acquired excellent knowledge of all the topics of the course, being able to connect them in a logical and coherent way.

since the expected results are exclusively related to the acquisition of knowledge, lectures and periodic exercises will be carried out in which students are called to carry out exercises, collaborating with each other and asking the teacher.

THE STRUCTURE OF MATTER - fundamental particles in an atom. - atomic number and mass number of an atom. - Nuclides, isotopes and chemical elements. - Relative atomic mass. - The mole as a measure of the amount of substance, and the Avogadro's number. Electronic structure of atoms AND PERIODIC CLASSIFICATION OF THE ELEMENTS - The Bohr model of the hydrogen atom. - uncertainty principle. - Equation of de Broglie - The atomic orbital. - Construction of the electronic structure of an atom. Pauli exclusion and the maximum multiplicity (or Hund) principles. Periodic Classification of the elements. Ionization energy, electron affinity and metallic character of an element. - Atomic radius. CHEMICAL BONDS - STRUCTURES AND MOLECULAR GEOMETRY - binding concept and the binding energy - The atomic bond (covalent). - atomic bonds simple double and triple. datives atomic bonds (or coordination). - Electronegativity of the elements. - Polarity in the atomic bonds. polar and non-polar molecules. - The ionic bond. - The hybridization of the atoms and molecules of geometries. - The metallic bonding. SUBSTANCES AND CALCULATIONS stoichiometric - Elemental composition of a chemical compound and its minimum formula. - Formulas and molecular units of formula. - related formal Masses. - Molar mass of a substance. - quantitative representation of a chemical reaction: stoichiometric equation (or chemical). - Balancing a chemical equation. Reagents in stoichiometric or non-stoichiometric proportions. Efficiency of a reaction. OXIDATION STATES OF ELEMENTS AND REACTIONS Redox - oxidation state of an element in a compound. - Correlation between oxidation states of the elements and their periodic classification. - Change the state of an element oxidation: oxidation, reduction and redox reactions. Balancing redox chemical equations. Redox couples. 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 gases and equation of Van der Waals. - liquefaction of gas and was critical. Solid state. ionic solids, molecular solids, solid metal covalent solids. Liquid State. Evaporation and solidification of liquids. Solutions (liquid): solvent and solute (gaseous, solid and liquid), concentration of the solutions and saturation concept. CHEMICAL THERMODYNAMICS thermodynamic and environmental systems: state variables (intensive and extensive), state functions. - The thermodynamic equilibrium, reversible and irreversible transformations. - Mechanical work in thermodynamic processes. - 1st law of thermodynamics. The heat at constant volume and in those transformations at constant pressure: the state function, enthalpy. - Thermal effect in chemical reactions: thermochemical equation. - standards of substances States. - Additivity of thermochemical equations (Hess Law). - 2nd law of thermodynamics: entropy function. The entropy at zero absolute (3rd principle of thermodynamics). - The free energy function (or Gibbs function). - Criteria of spontaneity and equilibrium in chemical reactions and phase transformations. - The chemical potential. - free energy of the system change in the progressive advancement of a reaction until equilibrium. - chemical equilibrium Law: standard constant (equilibrium) of a reaction. Dependence of the equilibrium constant on the temperature: equation Van t'Hoff. The yield of a reaction. BALANCE BETWEEN DIFFERENT LEVELS OF SUBSTANCES NOT CHEMICALLY REAGENTS Systems with a single component. - equilibria between different phases of the same substance: Clausius - Clapeyron. Diagram of state of water. Systems with two completely miscible components. - The vapor-liquid equilibrium: Raoult's law. isothermal Diagrams "vapor pressure - composition of the liquid phase and the vapor phase in equilibrium". isobars Diagrams "boiling temperature - composition of the liquid phase and the vapor phase in equilibrium". Distillation. completely immiscible or partially miscible two-component systems. - immiscibility Concept and chemical aspect of the phenomenon. distribution constant of a substance in two immiscible liquids. - Partial Miscibility and miscibility gap for liquids and solids. - colligative properties: Lowering of the solvent vapor pressure,passing from pure solvent to solution; lowering the freezing temperature and increasing the boiling temperature of a solution. - Cooling curves, eutectic and peritectic diagrams of solutions and alloys. - The electrical conductivity of electrolytic solutions: conductivity, equivalent conductivity and limit equivalent conductivity. IONIC EQUILIBRIUM IN SOLUTION The chemical equilibrium law for reactions in solution (Kc). The reaction of auto-ionization of water and its constant (Kw). Definition of acid and base according to Arrhenius. Acid-base reaction according to Bronsted and Lewis. Neutral solutions, acids and bases: pH. Calculation of pH of solutions of acids, bases and salts. Calculation of the pH of mixtures of acids, bases and strong acid with a strong base: neutralization. Electrolytes slightly soluble: solubility and solubility product (Kso) Electrochemistry - Semi redox reactions and their balancing with ionic-electronic method. - - The Nernst equation. - Electromotive force of a galvanic element. - potential electrode and the standard electrode potential of the semi elements. - standard hydrogen semi-element. - Table of standard reduction potentials, oxidizing power. Mention on CHEMICAL KINETICS

basic knowledge of math

Chimica generale e inorganica authors: Tagliatesta - Failla - Paolesse - Pasini - Pasquali - Valli Ed. Edi Ermes Fondamenti di chimica authors: Paolo Silvestroni Ed. Zanichelli Problemi di chimica authors: Mauro Pasquali Alessandro Dell'Era Ed. Esculapio

classroom lessons and training by periodic exercises in which students can perform exercises collaborating with each other and they can ask the teacher.

not required

written test and subsequent oral test. The written test will consist of 3-4 exercises and will last 2.5-3 hours. The oral test will be a question lasting about 30-40 minutes. The examinations will fall on the dates established by the university but there would be a kind of pre-test. To pass the exam it is necessary to obtain a mark not less than 18/30. The student must demonstrate to have acquired sufficient knowledge of the subjects.To achieve a score of 30/30 cum laude, the student must instead demonstrate that he has acquired excellent knowledge of all the topics of the course, being able to connect them in a logical and coherent way.

since the expected results are exclusively related to the acquisition of knowledge, lectures and periodic exercises will be carried out in which students are called to carry out exercises, collaborating with each other and asking the teacher.