Studying at the University of Verona

Here you can find information on the organisational aspects of the Programme, lecture timetables, learning activities and useful contact details for your time at the University, from enrolment to graduation.

This information is intended exclusively for students already enrolled in this course.
If you are a new student interested in enrolling, you can find information about the course of study on the course page:

Laurea in Scienze e tecnologie viticole ed enologiche - Enrollment from 2025/2026

The Study Plan includes all modules, teaching and learning activities that each student will need to undertake during their time at the University.
Please select your Study Plan based on your enrollment year.

2° Year  activated in the A.Y. 2010/2011

ModulesCreditsTAFSSD
12
B
AGR/15
12
B
AGR/03

3° Year  activated in the A.Y. 2011/2012

ModulesCreditsTAFSSD
9
B
AGR/11 ,AGR/12
12
B
AGR/15
Altre attivita' formative
6
F
-
Prova finale
3
E
-
activated in the A.Y. 2010/2011
ModulesCreditsTAFSSD
12
B
AGR/15
12
B
AGR/03
activated in the A.Y. 2011/2012
ModulesCreditsTAFSSD
9
B
AGR/11 ,AGR/12
12
B
AGR/15
Altre attivita' formative
6
F
-
Prova finale
3
E
-

Legend | Type of training activity (TTA)

TAF (Type of Educational Activity) All courses and activities are classified into different types of educational activities, indicated by a letter.




S Placements in companies, public or private institutions and professional associations

Teaching code

4S00136

Credits

9

Coordinator

Adolfo Speghini

Language

Italian

Location

San Pietro in Cariano

Scientific Disciplinary Sector (SSD)

CHIM/03 - GENERAL AND INORGANIC CHEMISTRY

The teaching is organized as follows:

Teoria

Credits

6

Period

1st Semester

Location

San Pietro in Cariano

Academic staff

Adolfo Speghini

Laboratorio

Credits

3

Period

1st Semester

Location

San Pietro in Cariano

Academic staff

Adolfo Speghini

Learning outcomes

Module: Theory
-------
The aim of the course is to acquire the main concepts of General Chemistry and some notions of Inorganic Chemistry. In particular:
- models and general concepts for the explanation and prediction of some physics and chemistry properties of systems of increasing complexity: single atoms, ions, molecules, pure substances, macroscopic systems of one or more components;
- concepts and methods to qualitatively and quantitatively predict the variations of the intensive and extensive properties of chemical systems in evolution.

Module: Laboratory
-------
Numerical exercises integrate the knowledge acquired by the student in the theoretical part of the Course, in order to to teach the student how to solve problems of chemical interest.
The experiments in the General Chemistry laboratory integrate the knowledge acquired by the student in the theoretical part of the Course. The student learns how to manage problems of chemical interest, obtains information about the common equipment present in a chemical laboratory and how to work in safe conditions.

Program

Module: Theory
-------
Introduction. Chemical and physical properties of matter and their measurements.
Elements, atoms and compounds.
Nomenclature of inorganic compounds. 
Types of chemical reactions. Reaction stoichiometry.
Ideal and real gases. 
Thermochemistry. Internal energy and enthalpy. Standard enthalpy of reaction and formation.
Atomic structure. Atomic orbitals. Electronic configuration, Aufbau principle. 
Periodic properties: atomic and ionic radii, ionization energy, electron affinity, electronegativity.
Elementary notions on the ionic bond. Ionic compounds.
Covalent bond. Lewis formula. Resonance. Molecular geometry and polarity. Orbital hybridisation. Single and multiple bonds.
Interparticle forces.
Properties of liquids. Solutions. Colligative properties. Binary liquid mixtures. Distillation. 
Properties of solids.
Chemical kinetics. Arrhenius equation. Reaction mechanisms. 
Chemical equilibrium. Equilibrium constant. 
Acid-base equilibrium. Acid, base and salt solutions. Acid-base titration. Buffer solutions.
Solubility equilibrium.
Entropy. Spontaneous processes. Gibbs free energy. Standard free energy of reaction and formation.
Electrochemical cells. Electrolysis.


Module: Laboratory
-------

Stoichiometry problems solving.


Laboratory experiments:
- determination of the hydrogen peroxide concentration in commercial samples for pharmaceutical use
- determination of drinking water hardness
- gravimetric determination of iron
- determination of the number of water molecules in hydrate copper sulphate
- weak base-strong acid titration
- strong base-strong acid titration
- determination of the properties of buffer solution

Examination Methods

The final examination consists of a written part, consisting of stoichiometry problems and general questions and of an oral part.

Students with disabilities or specific learning disorders (SLD), who intend to request the adaptation of the exam, must follow the instructions given HERE