The objective of the course is to understand and use the proper language of Chemistry and its nomeclature, in order to be able to communicate effectively with chemists and with companies dealing with chemicals, once the student, at the end of the engineering studies, will start the professional activity.
Moreover, the student will come to understand the fundamentals of the matter structure, from the atoms to the molecules, in al phases: Gas, liquid and solid.
D1- Knowledge and understanding.
At the end of the course the studnet will have to know the basic principles of chemistry and its nomenclature.
D2 - Applied knowledge and understanding
The student will have to write simple chemical formulas and structures. Moreover he will have to intrepret simple chemical phenomena on the bases of the learned theories.
D3 - Making judgements
The student will have to be able to evaluate the principal chemical/physical aspects of substances and reactin among substances.
D4 Communication skills
The student will have to be able to communicate effectively with the language of basic chemistry. Moreover he will have to explain the matter of structure in the different aggregation states, with the pertinent laws, mathematically expressed.
D-5 Learning skills
To be able to read, consult and comprehend a document or tscientific texts with contents of chemistry.

Basic notion of mathematics (functions, derivative, Integrals) and Physics (force, energy and work, power) Basic notion of metrology; the International System.

1. General introduction and basic concepts
2. Atomic structure
3. Chemical bond and molecular structure
4. Aggregation states of matter and phase transitions
5. Properties of solutions
6. Chemical thermodynamics
7. Chemical equilibrium in homogeneous and heterogeneous systems
8. Acid-base reactions
9. Electrochemistry
10. Chemical Kinetics
Contents are in agreement with the teaching objectives of the course of studies.

CHIMICA by Kotz et al. EDISES Publishing House


CHIMICA GENERALE by Petrucci et al. PICCIN Publishing House

MODERN CHEMISTRY, by Oxtoby et al.

FONDAMENTI DI CHIMICA by Chiorboli, UTET Publishing House (possibly not in reprint anymore).

For foreign students, any standard textbook, at University level, on Chemistry will be adequate for preparing the final exam.

Nomeclature and notation.
Chemical elements.
Definition and meaning of Atomic Mass Unit.
Atomic number and atomic mass.
Notation of a chemical reaction.
The periodic table.
Metals, non-metals and semimetals.
reactvity of elements with oxygen and water.
Structure of matter.
Thompson Experiment and model.
Rutherford experiment and model.
Planck quantum theory.
Photoelectric explanation and the Einstein interpretation.
Electromagnetic spectrum.
Atomic spectroscopy: hydrogen bands.
Bohr atomic theory and its success in interpreting atomic spectra.
Wave particle dualism.
De broglie relation.
Heisenberg indetermination principle.
Schoedinger equation.
Physical meaning of the wave function.
Physical meaning of the atomic numbers.
Aufbau and electronic configuration.
Ionization energy and electron affinity.
Pauling electronegativity.
Chemical bond and molecular geometry. The concept of valency.
Covalent bond: omopolar and heteropolar.
Ionic bond.
Metallic bond.
Van der Waals interaction.
Lewis rules.
Resonance.
VSEPR theory.
Valency Bond theory.
Molecular Orbital theory (MO -LCAO).
Paramagnetism and diamagnetism explained by MO theory.
States of matter.
Gaseous states: Boyle law, Charles Gay Lussac law.
Absolute tempetarure.
Equation of ideals gases.
Dalton law.
Kinetic theory of gases.
Gas liquefation; critical pressure and temperature.
Real gases and Van der Waals equation.
Solid state; bravais lattices.
notation for crystallographic planes and directions.
Bragg law and its geometrical derivation.
Crystalline structures of some materials with electronic properties: Zno, Zro2, SnO2, BaTiO3.
Liquid state: surface tension andf contact angle.
Solutions: units and Raoult's law.
Colligative properties: crioscopy, ebullioscopy and osmotic pressure.
Mixture of liquids: ideal behavior and positive and negative deviations.
Distillation diagram.
I and II thermodymamics principles.
definition of Enthalpy. Definition of Gibbs free energy. Spontaneity of chemical reactions.
Chemical equilibrium.
Le chatelier principle.
Reaction quotient and equilibrium constant.
Relation between Kc and Kp.
Solubility product.
Arrhenius acid-base theory.
Lowry bronsted Theory.
Water self-ionization.
Ph concept; pH of strong and weak acids and bases.
Salt hydrolysis.
Acid-base Indicators
Titrations.
Buffer solutions.
Electrochemistry; Galvanic cells.
Reduction potentials.
Nernst law for a cell.
Concentration cells.
Daniell cell.
Lead battery and Leclanchè battery.
Lithium ion cell.
Faraday laws.
Chemical kinetics.
Reaction rates, Reaction order. Arrhenius equation.
Reaction mechanism.
Industrial processes
Bayer process.
Solvay process.
Hall process.
Fritz-Haber process.
Preparation of NaOH on Hg cathode.
Industrial preparation af aluminium (hall process).
Industrial processes.
Organic nomenclature (hydrocarbons and most common plastics).

Class lectures with the help of multimedia tools (images and movies in Power Point).

Any changes to the formats described here, should they become necessary to ensure the application of the safety protocols related to the COVID19 emergency, will be communicated on the websites of the Department, of the Course of Study Program and of the individual course.

The power point images presented by the teacher are freely available in the MOODLE web page of the university. The images presented by the teacher are a graphical help for the student, but they alone are not sufficient to pass the exam.

The exam consists of a written test and an oral test. A passing score (18 or higher) on the written test grants access to the oral test. Students who pass the written test will therefore be required to take the oral test. The written test will be conducted digitally on MOODLE and will consist of a multiple-choice quiz with 15 questions covering the entire syllabus. Each correct answer is worth 2 points, unanswered questions are worth 0 (zero) points, and incorrect answers will be penalized with -0.5 points. A minimum score of 18 points is required to pass the written test. Students who pass the written test must take the oral test during the same exam session. The score from the written test is used solely to determine eligibility for the oral exam; the final grade will be determined based on the oral performance. Therefore, a passing score on the written test does not in itself guarantee passing the oral exam. For the oral exam, the grade will be assigned based on the following criteria: Excellent (30 - 30 cum laude): Outstanding knowledge of general chemistry, excellent command of terminology and chemical nomenclature, excellent analytical skills; the student is able to apply theoretical knowledge brilliantly to practical chemistry problems. Very Good (27 - 29): Good knowledge of general chemistry, strong command of chemical terminology, good analytical skills; the student is able to correctly apply theoretical knowledge to practical chemistry problems. Good (24 - 26): Good knowledge of general chemistry, fair command of terminology; the student demonstrates an adequate ability to apply theoretical knowledge to practical chemistry problems. Satisfactory (21 - 23): The student does not demonstrate full mastery of the general chemistry topics, though they possess fundamental knowledge; they nonetheless show satisfactory use of terminology and a sufficient ability to apply theoretical knowledge to practical chemistry problems. Sufficient (18 - 20): Minimal knowledge of the main topics and technical terminology, limited ability to adequately apply theoretical knowledge to practical chemistry problems. Insufficient (<18): The student does not demonstrate an acceptable understanding of the contents of the various topics covered in the general chemistry syllabus.

This course concurs to the realization of the UN 2030 Agenda for Sustainable Development