CHEMISTRY A - E

The course aims to provide the knowledge of Chemistry necessary to understand the behavior of the most common substances in order to deal with the interpretation of chemical and chemical physical phenomena and to establish the appropriate property-structure correlations of materials of engineering use.

Lectures and exercises.

If the teaching is taught in mixed mode or remotely, it may be necessary to introduce changes with respect to previous statements, in line with the programme planned and outlined in the syllabus

Information for students with disabilities and/or DSA

To guarantee equal opportunities and in compliance with current laws, interested students can request a personal interview in order to plan any compensatory and/or dispensatory measures, based on the educational objectives and specific needs.

It is also possible to contact the CInAP (Centre for Active and Participatory Integration - Services for Disabilities and/or DSA) professor of our Department, prof. A. Pagano. 

 (Elements, compounds and mixtures; physical and chemical properties; atoms and molecules; atomic number and mass number, isotopes, atomic mass units, atomic weight and molecular weight; the mole, laws of chemistry, notes of  nomenclature). 

STRUCTURE OF MATTER: Thomson's model; Rutherford's model; atomic number and mass number; atomic mass unit; atomic spectra; quantum theory, Bohr's theory, the Pauli principle, the uncertainty principle, wave-particle duality, wave mechanics, the equation of Schroedinger; quantum numbers and energy levels; ideal construction of the atoms, the periodic system: potential ionization, electronegativity and electronic affinity.
CHEMICAL BOND: Valence Bond Theory; covalent, metallic and ionic bonds, p and s covalent; hybridization; resonance; relationships between structure and bonding; intermolecular bonds; Molecular Orbital theory.

TYPE OF MATERIAL: Aggregation states; chemical elements and compounds, atoms and molecules, atomic and molecular weight, gram atom, gram-mole; Avogadro's number.
NOMENCLATURAL OF CHEMICAL COMPOUNDS: Brute and structural formulas; chemical equations and stoichiometry with exercises, oxidation, reduction, dismutation; equivalent weight and gram equivalent.
 GASEOUS STATE: Ideal gas, the laws of Boyle, Gay Lussac, Charles, Avogadro; ideal gas equation of state and numerical exercises; Avogadro's law; partial pressures, Dalton's law, equation of Van der Waals; critical state of real gases; Andrew diagram.
CHEMICAL THERMODYNAMICS: General concepts of thermodynamics, internal energy, the first law of thermodynamics, enthalpy, Hess's law, entropy and second law of thermodynamics, III law of thermodynamics, free energy and spontaneous processes.
CONDENSED STATES: Solid state, covalent solids, ionic, molecular, metallic; point, line and surface defects ; vapor pressure, boiling and solidification temperature.
STATE OF SOLUTION: Types of solution; solubility of a species; concentration units; solute-solvent interactions; ideal and real solutions; Raoult's law: the relationship between the composition of a mixture of two liquids and that of its vapor; systems with azeotrope of maximum and minimum; industrial applications, dilute solutions of non-volatile solutes, colligative properties, freezing point depression; boiling point elevation; osmotic pressure; numerical exercises.
CHEMICAL EQUILIBRIUM: Law of mass action, Le Chatelier's principle; derivation of thermodynamic equilibrium constant (Kp, Kc, Kx), the relationship between the equilibrium constants, homogeneous and heterogeneous equilibria, influence of pressure, temperature and concentration on the conditions of equilibrium, free energy and equilibrium constant.
HETEROGENEOUS EQUILIBRIA: Change of state; melting, evaporation, sublimation, Clausius-Clapeyron variance; phase diagrams, one-component systems: water, sulfur, carbon dioxide; systems with eutectic point.

CHEMICAL KINETICS: Rates of reaction, activation energy, rate constants, molecularity and order reaction; influence of temperature; homogeneous and heterogeneous catalysis.
ELECTROLYTE SOLUTIONS: Electrolytic dissociation, strong and weak electrolytes, degree of dissociation; Van't Hoff coefficient, specific and equivalent conductivity; Arrhenius, Bronsted and Lewis theories; ionic product of water ; definition of pH; calculating the pH of solutions of strong acids and bases; calculating the pH of solutions of weak acids and bases.
MULTIPLE EQUILIBRIA IN SOLUTION OF ELECTROLYTES: Salt hydrolysis, buffer solution,  solubility product and common ion effect; numerical exercises.
ELECTROCHEMISTRY: Oxidation-reduction reactions, electrode potentials, Nernst equation and numerical exercises, galvanic batteries; electrochemical series of the elements, electrolysis; Faraday's laws and numerical exercises; electrolysis of molten sodium chloride, electrolysis of an aqueous sodium chloride solution; the electrolysis of water; corrosion.
INORGANIC CHEMISTRY

Theory and exercises

B.B.Laird, Chemistry, McGraw-Hill

The exam includes a test with exercises and a test relating to the theory part of the program.

 During the period of the lessons, ongoing tests will be scheduled which have a double value: the first of a self-assessment type to allow students to verify their level of learning along the way; the second of an evaluative type to directly access the oral exam.

 The 1st ongoing test will take place on 18 December 2023 and will concern the topics (theory and exercises) relating to the material provided by the teacher in the collections between 1 and 8 (simulations will be available on Studium).

 The 2nd ongoing test will only concern exercises related to the material provided by the teacher in collections 10, 12 and 14 (simulations will be available on Studium) and the test can be taken on any of the exam dates established by the academic calendar.

Passing both ongoing tests will allow you to directly take an exam on theory, only on the topics related to the material provided by the teacher in the collections between 9 and 14. The exam can be taken either in the form of an oral interview ( the date is agreed by contacting the teacher via e-mail) or as a written test.

 The ongoing tests will remain valid until September 2024

In the event that the ongoing tests are not taken or passed, 6 (ordinary) exam sessions are set during the academic year, plus 4 sessions reserved for repeating and out-of-course students. These appeals consist of a written test in which the students are asked to carry out exercises (on the whole program) similar to those carried out in the classroom during the exercises. The exam relating to the theory part, on all the topics covered during the course, can be taken in the form of an oral interview or as a written test.

 The verification of learning can also be carried out electronically, should the conditions require it.

Ammonia molecule: present bonds, synthesis, properties.

Water molecule: bonds, ionic product of water, state diagram, electrolysis.

Ideal gases and real gases.

Chemical equilibrium and Le Chatelier's principle.

Chemical kinetics

Electrochemistry: batteries and electrolysis cells