The course aims to provide the basic knowledge necessary for the interpretation of chemical phenomena, for the understanding of the structure and properties of crystalline solids and for the understanding and calculation of energy phenomena related to chemical and electrochemical systems. It intends to provide the student with a solid scientific preparation, aimed at the knowledge, understanding and description of the structure and properties of matter, contributing, together with the other courses of the first year, to the consolidation of the technical-scientific cultural foundations typical of each engineer. The teaching of Chemistry therefore constitutes an effective tool for increasing both the capacity for critical reasoning and the appropriate use of scientific language.

To make profit of the course it is required to master the basic notions of general chemistry, the symbols of elements and compounds, the simplest nomenclature both organic and inorganic, the balancing of elementary stoichiometric reactions.

ATOM Constitution of the nucleus, structure of the hydrogen atom and atomic models (Bohr and quantum-mechanical) Quantum numbers, exclusion principle and Hundt rule Spatial form of s,p and d orbitals CLASSIFICATION OF THE ELEMENTS AND PERIODIC TABLE Electronic configuration of the elements and periodicity in the chemical and physical properties Atomic radius, ionization energy and electron affinity Subdivision into metals, non-metals and semimetals. Basics on the main groups of the periodic table and some transition metals. THE CHEMICAL BOND Bond: ionic, covalent, metallic. Intermolecular interactions. Covalent bond: single, double and triple. Molecular geometry, hybridisation and resonance. Notes on the theory of molecular orbitals. NOMENCLATURE, FORMULAS AND STOICHIOMETRY Atomic and molecular mass, the mole, Avogadro's constant. Acid-base reactions and formation of salts. Oxidation state and balancing of redox reactions. Mass relationships in a chemical reaction, limiting reagent. Combustion reactions GASEOUS STATE Ideal gas laws. State equation of ideal gases. Equilibrium distribution of kinetic energies in an ideal gas (Boltzmann). Liquefaction of a gas. LIQUID STATE Vapour pressure of pure liquids. Solutions: ways to express concentration. Dissociation and ionization degree. Colligate properties of solutions, both electrolytic and non. Definition of acid and base according to Arrhenius, Brønsted and Lewis. Ostwald dilution law. Ionic product of water, pH and pOH. SOLID STATE Unit cell and structure of simplestcrystalline solids. Crystal lattices. Classification of solids. CHEMICAL KINETICS AND CATALYSIS Reaction rate and order. Arrhenius equation. Activation energy. Catalysis and catalysts. CHEMICAL EQUILIBRIUM Mass action law. Equilibrium constant. Homogeneous and heterogeneous chemical equilibria. Le Chatelier principle and influence of the temperature on the equilibrium. CHEMICAL THERMODYNAMICS First, second and third Principle. Reaction enthalpy and Hess law. Change in entropy and free energy of a reaction. Spontaneity criterion. ELECTROCHEMISTRY Normal and effective potential of an electrode. Electrochemical cells and Nernst equation. Electrochemical force of a cell. Reactivity of metals with ocids, oxidizing or not. Electrolysis and Faraday laws. ORGANIC CHEMISTRY Nomenclature and properties of the main organic compounds. Most common functional groups and their main reactions. Isomerism: structural, geometric, conformational.

The teaching is structured in: - 58.5 hours of classroom theory lessons aimed at developing knowledge of the structure and properties of matter. After introducing the atomic structure, the teaching will deal with the different types of chemical bonds, the properties of the different states of aggregation, the kinetic and thermodynamic aspects of chemical and physical transformations, the fundamentals of electrochemistry. - 18 hours of EXERCISES in the classroom (students divided into two teams). During the exercises, no new topics are explained, but the numerical and computational aspects of some of them are treated, in particular: ' Review of inorganic nomenclature. ' Mole, molecular mass and molar mass. ' Weight relationships in chemical reactions. ' Redox reactions and their balancing. ' Ideal gas laws. ' Colligative properties of solutions. ' Homogeneous and heterogeneous chemical equilibria. ' Thermochemistry ' pH and equilibria in aqueous solution ' Nernst equation relating to an electrode or a cell. ' Faraday's laws. - 3 hours of didactic LAB, in which the students, divided into teams of 3-4 people, carry out some simple didactic experiments under the guidance of tutors which favor the understanding and assimilation of the theoretical notions covered during the course ' Reaction kinetics ' Precipitation reactions ' Acid-base titration ' Redox reactions ' pH measurement ' Daniell Cell TUTORING MODULE. In parallel with the theory lessons and exercises, a TUTORING module is foreseen, aimed at consolidating basic knowledge and skills, as well as encouraging the active participation of the student during the semester, and gradual preparation for the final exam. To this end, four computer tests are also planned, on a monthly basis (remotely) useful for the student to become familiar with the exam method based on multiple-choice tests. MID-TERM TESTS. The Mid-term tests consist of two computer tests with scoreing (in the middle and at the end of the course, at the Laib), reserved for students in their first year of attendance (neo-matricole); passing both tests (which have a similar structure and scores to those of the exam test) gives direct access to the written exam (see the exam method section). The methods and deadlines of these tests will be announced at the beginning of the course and published on the course web page.

PRINCIPLES OF GENERAL CHEMISTRY (International Edition). Author: Martin Silberberg. Publisher: MgGraw-Hill

Lecture slides; Text book; Practice book; Multimedia materials;

You can take this exam before attending the course

Exam: Computer lab-based test; Written test; Optional oral exam;

For each round (appello), the exam consists of a computer test (at the Laib) with multiple-choice questions, followed by a mandatory written test. To access the written test, students must necessarily pass the computer test that precedes it (i.e. within the same round). Students who pass the written test may request to take an oral test. Mid-term tests at the Laib: first-year students (neo-matricole) have the opportunity to take part in a series of mid-term tests, proposed during the course. Passing the first test (in November) allows access to the second one (in January). Passing the second test allows direct access (i.e. without taking the computer test of the session exams) to the one of the written tests (only one) of the 4 rounds (appelli) within the current academic year. The computer test, as well as the two mid-term tests, aims to assess the basic knowledge required to attend the written exam. The written and oral tests aim to assess the knowledge of inorganic and organic general chemistry acquired by the student during the course and the student's ability to solve stoichiometric calculations on chemical and electrochemical reactions, thermochemical equations, gas and liquid solutions. No teaching material is allowed in any test. The duration of each mid-term test, consisting of 15 multiple choice questions, is 25 minutes. The maximum score achievable at each test is 9. If the score achieved at the test is less than 6, the test is failed. To access the second test, students must necessarily pass the first one. Those who pass both tests can directly access the written test of one of the 4 exam rounds of the current academic year. Those who do not pass the mid-term tests can register for the exam to be taken during the sessions. The duration of the computer test, consisting of 15 multiple choice questions, is 25 minutes. The maximum score achievable at the computer test is 9. If the score achieved at the test is less than 6, the examination is registered as failed. If the score is in the range 6-9 the student must attend the written test, consisting of both exercises and theoretical questions. The duration of the written test is 70 min. The written test allows achieving a maximum score of 22. If the score obtained in the written test is less than 12, the examination is registered as failed. The final mark is the sum of the marks obtained at the computer test (or the average of the two mid-term tests, both of which must be passed) and the written test. If the final grade is equal to or greater than 18/30, the student has the opportunity to request and sit for an additional oral examination on the whole program developed during the course. In this case, the final vote will also take into account the oral test. In addition, the teacher reserves the right to call a student for an oral test, to verify the written exam.

In addition to the message sent by the online system, students with disabilities or Specific Learning Disorders (SLD) are invited to directly inform the professor in charge of the course about the special arrangements for the exam that have been agreed with the Special Needs Unit. The professor has to be informed at least one week before the beginning of the examination session in order to provide students with the most suitable arrangements for each specific type of exam.