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Second cycle
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School of Science
Course unit
SC01122479, A.A. 2017/18

Information concerning the students who enrolled in A.Y. 2017/18

Information on the course unit
Degree course First cycle degree in
IF0320, Degree course structure A.Y. 2017/18, A.Y. 2017/18
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Number of ECTS credits allocated 12.0
Type of assessment Mark
Website of the academic structure
Department of reference Department of Chemical Sciences
E-Learning website
Mandatory attendance
Language of instruction Italian
Single Course unit The Course unit can be attended under the option Single Course unit attendance
Optional Course unit The Course unit can be chosen as Optional Course unit

Teacher in charge DAVIDE BARRECA
Other lecturers CHIARA MACCATO CHIM/03

ECTS: details
Type Scientific-Disciplinary Sector Credits allocated
Basic courses CHIM/02 Physical Chemistry 4.0
Basic courses CHIM/03 General and Inorganic Chemistry 8.0

Course unit organization
Period First semester
Year 1st Year
Teaching method frontal

Type of hours Credits Teaching
Hours of
Individual study
Laboratory 2.0 32 18.0 2
Lecture 10.0 80 170.0 No turn

Start of activities 02/10/2017
End of activities 19/01/2018
Show course schedule 2019/20 Reg.2017 course timetable

Examination board
Examination board not defined

Prerequisites: Fundamental knowledge of mathematics and analysis, with particular regard to first- and second-degree equations, logarithms, powers, exponential notation.
Target skills and knowledge: Through theoretical lectures and practical exercises, students will acquire know-how on fundamental chemistry. The resolution of numerical exercises will also make the student familiar with a scientific approach towards various topics.
Laboratory experiences are aimed at providing practical knowledge regarding phenomena and chemico-physical processes related to some key arguments of the General and Inorganic Chemistry program.
Examination methods: Examination in three parts:
- written (general and inorganic chemistry and physical chemistry)
- laboratory evaluation (behavior and written reports)
- a brief oral on the laboratory part, for those who have passed the written examination
No intermediate examinations.
Assessment criteria: Student knowledge will be evaluated considering both specific concepts provided during the course, and also evaluating the capacity of using the acquired know-how in the solution of numerical problems.
Course unit contents: General and Inorganic Chemistry (D. Barreca)
Matter classification and fundamental properties. Atomic structure, isotopes and brief introduction to atomic models. Atomic orbitals and quantum numbers. Aufbau principle and electronic configurations. Atomic and molecular weight. Mole/Avogadro number. Compounds and empirical formulae. Nomenclature. Chemical reactions. Redox reactions; oxidizing and reducing agents. Balancing reactions and related calculations.
Building up the periodic table and periodic properties. Chemical bonding: ionic, metallic and covalent bonds. Valence bond theory and main hybridization patterns. Lewis formulae.
Matter aggregation states and related phase transitions. The gaseous state and related laws. Kinetic theory of gases: the basics. Real gases. Intermolecular forces. Hydrogen bonding. The solid and liquid states: classification and main characteristics. Vapor pressure and its dependence on temperature.
Solutions; Concentration and related units. Dilutions. Colligative properties (vapor pressure lowering and Raoult law; boiling point elevation; lowering of the melting point; osmotic pressure). Solute dissociation.
Chemical equilibria. The law of mass action and equilibrium constants. Homogeneous and heterogeneous equilibria. Le Chatelier principle and equilibrium perturbation.
Strong and weak acids and bases. Dissociation constants. pH and acidity scale. Introduction to polyprotic acids. Hydrolysis reactions. Acid and base mixtures. Buffer solutions. Acid-base titrations with indicators and pH-meter.
Precipitation equilibria of sparingly soluble salts and hydroxides. Common ion effect.
Electrochemistry: Galvanic cells and standard potentials. Nernst equation. Cell voltage. The Daniell Cell. Examples.
Electrolysis and electrolytic conduction. Application to molten salts and salt aqueous solutions. First Faraday law. Examples.

General and Inorganic Chemistry Laboratory (C. Maccato)
- Representative simple chemical reactions (salt formation; energetic variations; dehydrating power of sulfuric acid).
- Copper reaction cycle.
- Effect of concentration, temperature and common ions on reaction equilibria.
- Alum preparation from recycled aluminum.
- Acid-base titrations with indicators and pH-meter. Application to a commercial vinegar.
- Reactions of common domestic reactants and solubility tests in different solvents.
- Redox reactions and the Daniel cell.

Physical Chemistry (A. Toffoletti)
Physical states of matter and macroscopic properties of matter. Thermodynamic state and equations of state. Perfect gases and real gases. Energy conservation and the first law of thermodynamics: work and heat, internal energy and enthalpy. Entropy and the second law, absolute entropy and third law of thermodynamics. Spontaneous processes and Gibbs free energy. Thermochemical and standard properties. Phase equilibria and Clausius-Clapeyron equation. Thermodynamic description of mixtures: chemical potential, ideal solutions, real solutions and thermodynamic activity. Thermodynamic description of chemical equilibrium: free energy of reaction, Kp, and the van't Hoff law.
Rates of chemical reactions, reaction order; kinetic laws of the first and second order. Reaction mechanisms: elementary chemical reactions, steady state assumptions. Dependence on temperature, the Arrhenius equation. Catalysts and inhibitors; the enzyme catalysis mechanism (Michaelis-Menten).
Basic elements of molecular spectroscopy: the spectrum of electromagnetic radiation, Lambert-Beer law. UV-visible absorption spectroscopy, and emission spectroscopy.
Planned learning activities and teaching methods: Direct teaching activity, through informatics instruments and lectures/exercises on the blackboard, on the fundamental concepts of general and inorganic chemistry and physical chemistry. Lessons will start with the easiest topics, such as compound formula and names, up to Lewis structures, acid-base equilibria, electrochemistry, and thermodynamics and kinetics. Exercises will be performed with the aim of providing the course with practical contents and giving the students the chance to become technicians able to handle the fundamental chemistry elements needed in future career.
Additional notes about suggested reading: The presence of students during direct teaching activities and exercises are strictly recommended in order to acquire the presented material.
Textbooks (and optional supplementary readings)
  • R. Chang, K. Goldsby, Fondamenti di Chimica Generale (con eserciziario). --: Ed. Mc Graw-Hill Education, 2015. Cerca nel catalogo
  • R. H. Petrucci, W. S. Harwood, F. G. Herring, Ed. italiana a cura di L. Cattalini e G. Paolucci, Chimica generale. --: Piccin, 2013. Cerca nel catalogo
  • A. Paterno Parsi, A. Parsi, T. Pintauer, L. Gelmini, R. W. Hilts, Chimica generale - Esercizi svolti. --: Piccin, 2014. Cerca nel catalogo
  • P.W. Atkins, J. De Paula, “Elementi di Chimica Fisica”, terza edizione italiana. --: Zanichelli, 2007. Cerca nel catalogo