CHEMISTRY

Acquisition of important concepts of general chemistry, inorganic chemistry, stoichiometry and notes on organic matter. The course is organized so as to provide a good knowledge of basic chemistry (inorganic and stoichiometry) and is divided into a theoretical part and a part consisting of exercises aimed at solving chemistry problems (knowledge and understanding). The aim of the course is to acquire reasoning skills to deal with the study of chemical phenomena with analytical and numerical methods (applying knowledge and understanding). At the end of the course students should have their own judgment: ability to propose their own numerical exercises (making judgments) on specific topics.

In particular:

This course is specifically theoretical and contains many numerical exercises.

The specific training objectives of this course are:

Understanding the atomic structure;

understanding the mechanisms of chemical bond formation;

to know the chemical interactions in solids, liquids and understanding the gas state equations;

to know the main thermodynamic and kinetic quantities involved in chemical reactions;

To assess the conditions of chemical equilibrium;

to quantitatively determine the gaseous equilibria, in aqueous solutions and in electrochemical systems;

to discuss all proposed activities with scientific method and appropriate language.

To acquire the ability to set and correctly perform exercises on the various types of chemical reactions

Furthermore, in reference to the so-called Dublin Descriptors,

this course helps to acquire the following transversal skills:

Knowledge and understanding:

Capacity of inductive and deductive reasoning.

Ability to outline a chemical reaction in qualitative and quantitative terms.

Ability to set a problem using appropriate relationships between chemical and physical quantities and solve it with analytical methods.

Ability to apply knowledge:

Ability to apply the acquired knowledge for the description of chemical phenomena using the scientific method with rigor.

Capacity for quantitative calculation of reagents and products in chemical reactions.

Quantitative calculations on homogeneous solutions, of their colligative properties, of pH, and of electro-chemical phenomena.

Autonomy of judgment:

Ability to critical reasoning.

Ability to identify the most appropriate solutions to solve chemical problems.

Ability to identify the predictions of a theory or a model.

Ability to assess the accuracy required for stoichiometric calculations.

Communication skills:

Ability to describe a scientific topic in oral form, with properties of language and terminological rigor, illustrating the reasons and results.

Theoretical lessons will be alternate with numerous numerical exercises in the classroom. Students will be actively involved in numerical exercises on the board. If possible, as in the last 3-4 years, the teacher will experimentally perform simple and harmless chemical reactions in the classroom such as the preparation of cupric oxide, cuprous oxide, acid-base titrations with pH indicators, a redox titration (KMnO₄ - H₂C₂O₄) and the preparation of a chemical pile.

Should the circumstances require online or blended teaching, appropriate modifications to what is hereby stated may be introduced, in order to achieve the main objectives of the course.

Starting course on the nomenclature.

1 - STRUCTURE OF THE ATOM
Subatomic particles: Electron, proton, neutron - atomic number, mass number - isotopes - atomic mass unit - Bohr / Rutherford atomic model. Wave Mechanical atom model. - Atomic orbitals - quantum numbers - Principle of exclusion of Pauli - principle of maximum multiplicity - the principle of aufbau.

2 - PERIODIC SYSTEM OF ELEMENTS
Periodical classification and electronic configuration of the elements - Periodic properties: atomic and ionic radii, ionization energy, electron affinity, and electronegativity.

3 - STECHIOMETRY

The concept of mass and fundamental laws that govern the course of chemical reactions. The chemical equation. Classification of the main chemical reactions. Quantitative relationships in chemical reactions. Ionic compounds and molecular compounds; electrolytic dissociation; oxidation numbers, concepts of oxidant and reducing agent. Redox reactions and their balance. Determination of the formula of any compound. Numerical applications.

4 - CHEMICAL BOND

Concepts on ionic, covalent and dative bonds. Lewis formalism and valence bond theory. Structural formulas of the most common compounds: N2, O2, CO, NO, NO +, HCl, CO2, NO2, O3, NO2-, HCN, CH2O, CO3--, NO3-, CH4, C2H6, C2H4, C2H2, NH3, N2H4, NH4 +, NH2-, H2O, H2O2, H3O +, OH-, HF, CNO-, F2O; expanded valence shells: XeF2, PCl5, SO2, SO3, H2SO4, SO4--, SiF5-, SiF6--, PF5, PF6-, SF4, SF6, ClF3, BrF5, XeF4; common oxyacids and their anions; common isoelectronic molecules and ions; resonance concept. Electronegativity of atoms and polarity of bonds. Dipole moments of HF, HCl, HBr, HI, H2, NH3, NF3, BF3, H2O, H2S, SO2, CO2, CH4, CH3Cl, CH2Cl2, CHCl3, CCl4. Molecular geometries: state of carbon promotion, hybridization theory, sp3, sp2, sp, methane, ethane, ethylene, acetylene, benzene hybrid orbitals.

Molecular geometry and V.S.E.P.R theory: H2O, NH3, CH4, BF3, BeCl2, PCl5, TeCl4, ClF3, I3-, SF4, SF6, IF5, ICl4-, PF5, XeF2, BrF5, XeF4. Variation of potential energy during the formation of H2. Lattice energy and ionic bond. LiF molecule. Born-Haber cycle. Physical properties of ionic compounds. Chemical bond and theory of molecular orbitals, sigma and pi orbitals; diatomic molecules H2 +, H2, He2 +, Li2, B2, C2, N2, O2, F2, N2 +, N2-, O2 +, O2-. Order, length, force constant and binding energy. Dative bond. Metallic bond and hints of band theory. Heteronuclear diatomic molecules: HF, CN, CO, NO, O3, Benzene. Physical properties of covalent compounds. Metallic bond and hints of band theory.

5 - INTERMOLECULAR FORCES

Intermolecular forces: ion - ion, ion - dipole, dipole - dipole, Van der Waals and London forces. Hydrogen bond and boiling points of H2O, H2S, H2Se. Surface tension.

6 - ELEMENTS OF THERMODYNAMICS.

7 - GAS LAWS.
General characteristics of the gaseous state. Ideal gas. Ideal gas laws. State law of the ideal gas. Law of partial pressures and volumes. Gas diffusion. Real gases. Numerical applications.

8 - CONDENSED STATES AND STATE CHANGES

Characteristics of the solid state as a function of the chemical bond - Characteristics of the liquid state, vapor pressure and boiling temperature of pure liquids. Phase changes. Phase diagrams of water and carbon dioxide - Principle of mobile equilibrium.

9 - WATER SOLUTIONS

Solvent, solute, gaseous, liquid and solid solutions, interactions between solute and solvent, hydrogen bond, unit of measurement of concentration: % by mass and volume, equivalent weight and normality, molarity, molality, molar fractions. Colligative properties of electrolytes in solution: Vapor pressure of ideal and real solutions, Raoult's law, distillation, azeotropes. Solutions of non-volatile solutes. Degree and factor of dissociation. Relative lowering of solvent vapor pressure, ebullioscopy and cryoscopy. Phase diagrams of granita and brine. Osmosis and osmotic pressure. Electrolyte solutions and degree of dissociation. Solubility and Henry's law. Numerical applications

10 - CHEMICAL EQUILIBRIUM

Elements of chemical thermodynamics. Equilibrium in homogeneous chemical systems - Mass action law and equilibrium constants: Kp, Kc, Kx. Factors affecting equilibrium: temperature and pressure. Ionic equilibria in aqueous solution. Theories of acids and bases. Arrhenius, Bronsted and Lewis acids and bases. Ampholytes. Complex ions in aqueous solution, polyprotic acids and bases. Acid-base reactions and stoichiometry of solutions. Strength of acids and bases. Strong and weak acids and bases. Self-dissociation of water and definitions of pH and pOH and pKw. HCl-NaOH titration. pH of strong and weak acids and bases: definitions of pKa, pKb. Hydrolysis of salts and pH calculations. Acid, basic buffer solutions. PH indicators. Heterogeneous equilibria - Solubility product. Numerical applications.

11 - ELECTROCHEMISTRY

Metal electrodes, measurements of d.d.p., galvanic cells, Nerst equation. Second species electrodes (Ag / AgCl / KCl). Third type electrodes: Pt / Fe2 + - Fe3 +; Pt / Mn2 + and MnO4-, Pt / Quinhydrone. Normal standard hydrogen electrode. Saturated calomel electrode. Standard potential series of semi-elements, predictions of red-ox reactions.

Reactions of disproportion. Stacks of concentration. Electrochemical determination of pH. Electrolysis and Faraday's laws. Overvoltage, electrolysis of water, of NaCl solutions, of ZnSO4; lead-acid accumulator. Numerical applications.

12 - CHEMICAL KINETICS

Reaction rate, reaction order, half-life, reaction molecularity, collision theory, Arrhenius equation and activation energy, factors affecting the reaction rate, catalysts.

13 - INORGANIC CHEMISTRY

Metals and non-metals: general information on chemical and physical properties. General characteristics of each group of the periodic system. Alkaline and alkaline earth metals. Main oxidation states and compounds of Hydrogen, Oxygen, Carbon, Nitrogen, Phosphorus, Sulfur and Chlorine. Transition elements: generalities. Coordination compounds. Binders. Coordination number and geometry. Nomenclature. Notes on the theories of the chemical bond in coordination compounds.

Texts 1-4 are equivalent and the student is free to choose others not listed.
Texts of exercises 5-7 are equivalent and the student is free to choose others not listed.

1. KOTZ, TREICHEL, TOWNSEND Chimica V edizione - EdiSES
2. ATKINS, JONES, Principi di Chimica – Zanichelli
3. PETRUCCI, HERRING, MADURA, BISSONNETTE, Chimica Generale - Piccin
4. EBBING, Chimica Generale - Editoriale Grasso
5. NOBILE, MASTRORILLI, Vol.1 e 2, Esercizi di Chimica - Ambrosiana
6. GIOMINI, BALESTRIERI, GIUSTINI, Fondamenti di Stechiometria – EdiSES
7. P.MICHELIN LAUSAROT, G.A. VAGLIO, Fondamenti di Stechiometria - Piccin