ITALIANO

Gli argomenti trattati nel corso riguarderanno:
LA STRUTTURA DELLA MATERIA
LEGAMI E STRUTTURE MOLECOLARI
STATI DELLA MATERIA ED EQUILIBRI FISICI
LE SOLUZIONI.
CENNI DI TERMOCHIMICA.
EQUILIBRI FISICI.
CINETICA CHIMICA
Durante le esercitazioni numeriche verranno trattati gli aspetti numerici e quantitativi associati alle reazioni chimiche.
Durante le esercitazioni di laboratorio verranno trattati gli aspetti applicativi e saranno effettuati esperimenti e dimostrazioni di reazioni trattate durante le lezioni.

Fondamenti di Chimica Generale- Raymond Chang, Kenneth Goldby. Mc Graw Hill Ed.

L’insegnamento si prefigge di fornire conoscenze di base sulla struttura atomica e di fornire gli strumenti per la comprensione a livello molecolare delle trasformazioni della materia

Il corso prevede lezioni ed esercitazioni di stechiometria in aula ed esercitazioni pratiche in laboratorio

Modalità di apprendimento: La verifica del livello di apprendimento consisterà in una prova scritta che sarà effettuata alla fine del corso o sarà eventualmente frazionata in tre prove di verifica scritte durante il semestre, e in un colloquio orale. Se l’esito delle prove di verifica scritte risulterà superiore o pari alla sufficienza (15/30), si accederà ad un colloquio orale che sarà tradotto in voto per l’esame di Chimica. Concorrerà al giudizio finale anche la valutazione delle relazioni di laboratorio.

LA STRUTTURA DELLA MATERIA:
- ATOMI E MOLECOLE.
- Leggi fondamentali della chimica e la teoria atomica
- Modelli atomici.
- Configurazione elettronica degli elementi e tavola periodica.

LEGAMI E STRUTTURE MOLECOLARI
- IL LEGAME CHIMICO.
- Strutture molecolari. Struttura elettronica e geometria di molecole semplici. Nomenclatura di composti inorganici
- Forze intermolecolari.
STATI DELLA MATERIA ED EQUILIBRI FISICI
- Stato gassoso
- Stato liquido.
- Stato solido, solidi ionici, covalenti, molecolari, metallici; Polimorfismo e allotropia
- SISTEMI A DUE O PIÙ COMPONENTI.
- soluzioni. Unità di Concentrazione. Proprietà colligative delle soluzioni
- Equilibri Fisici
- Termochimica : cenni
REATTIVITA’ ED EQUILIBRI CHIMICI
- Equilibri chimici gassosi.
- Equilibri acido-base.
- Equilibri di solubilità.
- CINETICA CHIMICA

Italian

The topics covered in the course will include:
- Structure of Matter
- Chemical Bonds and Molecular Structures
- States of Matter and Physical Equilibria
- Solutions
- Basics of Thermochemistry
- Physical Equilibria
- Chemical Kinetics

During numerical exercises, numerical and quantitative aspects associated with chemical reactions will be addressed.

During laboratory sessions, the practical applications will be covered, and experiments and demonstrations of reactions discussed in the lectures will be conducted.

Fondamenti di Chimica Generale- Raymond Chang, Kenneth Goldby. Mc Graw Hill Ed.

The teaching aims to provide basic knowledge of the atomic structure of matter and to equip students with the tools for understanding matter transformations at the molecular level.

The course includes classroom lectures and stoichiometry exercises, as well as practical laboratory sessions.

Learning assessment: The evaluation of learning level will consist of a written exam, which will be conducted either at the end of the course or may be divided into three written assessment tests throughout the semester, along with an oral examination. If the results of the written assessment tests are equal to or above the pass mark (15/30), the student will proceed to an oral examination, which will be translated into a final grade for the Chemistry exam. The evaluation of laboratory reports will also contribute to the final assessment.

THE STRUCTURE OF MATTER
Atoms and molecules. Atomic theory and fundamental laws of chemistry. Atomic weight, molecular weight, and isotopic mass. Moles and molar mass.
Atomic structure. Components of the atom. Mass defect and nuclear binding energy. Atomic models. The hydrogen atom: energy levels, quantum numbers, atomic orbitals. Poly-electronic atoms - Orbitals and energy levels of poly-electronic atoms.
Electronic configuration of elements. Ionization energy and electron affinity. Effective Nuclear Charge, Z*.
The periodic table. Periodicity of chemical properties of elements.
BONDS AND MOLECULAR STRUCTURES
Chemical bonds.Ionic, covalent, and coordination bond. Valence bond theory. Electronegativity of atoms and dipole moment. Hybrid orbitals and resonance. Molecular orbital theory. Molecular orbitals of homo-nuclear diatomic molecules. Diamagnetism and paramagnetism.
Molecular structures. Electronic structure and geometry of simple molecules. Valence Shell Electron Pair Repulsion (VSEPR) theory. Oxidation number. Systematic nomenclature of inorganic compounds (oxides, hydrides, hydroxides, oxyacids, salts).
Intermolecular forces. Van der Waals forces. Hydrogen bonding. Physical properties of compounds. Solubility and miscibility.
STATES OF MATTER AND PHYSICAL EQUILIBRIA
Gaseous state. The ideal gas. Temperature and velocity of gas molecules. Real gases.
Liquid state. Properties of liquids. Surface tension. Vapor pressure. Viscosity.
Solid state. Properties of solids. Elementary cell and lattice. Molecular, covalent, and ionic solids. Metals. Allotropy and polymorphism.
Solutions. Concentration units. Colligative properties of solutions. Electrolytic dissociation.
Chemical Equilibria. Reversibility of chemical reactions and chemical equilibrium. Law of chemical equilibrium. Homogeneous chemical equilibrium in the gas phase. Homogeneous chemical equilibrium in the liquid phase. Heterogeneous chemical equilibrium. Le Chatelier's principle. Solubility product. Common ion effect.
Acid-base equilibria. Definition of acids and bases according to Brønsted. Structure-acidity relationships. Autoionization of water. pH of strong acids and bases, *mono- and polyprotic acids and bases. pH of saline solutions. Buffer solutions. Ampholytes. Isoelectric point. Indicators. Acid-base titrations. Definition of acids and bases according to Lewis.
Solubility equilibria. The common Ion effect on the solubility
Coordination compounds. Metallic complexes as Lewis acid-base adducts. Nomenclature. Coordination number. Formation equilibria and stability of complexes in solution.
Electrochemistry. Brief overview
Chemical Kinetics. Reaction rate. Reaction order. Reaction mechanism. Activation energy. Catalysis