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School of Science
Course unit
SC10101298, A.A. 2016/17

Information concerning the students who enrolled in A.Y. 2016/17

Information on the course unit
Degree course First cycle degree in
SC1161, Degree course structure A.Y. 2008/09, A.Y. 2016/17
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Number of ECTS credits allocated 8.0
Type of assessment Mark
Course unit English denomination GENERAL AND INORGANIC CHEMISTRY
Website of the academic structure
Department of reference Department of Biology
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 LUCA NODARI

ECTS: details
Type Scientific-Disciplinary Sector Credits allocated
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
Practice 1.5 18 19.5 No turn
Laboratory 0.75 12 6.75 No turn
Lecture 5.75 46 97.75 No turn

Start of activities 01/10/2016
End of activities 20/01/2017
Show course schedule 2019/20 Reg.2008 course timetable

Examination board
Board From To Members of the board
8 CHIMICA GENERALE E INORGANICA 2019-2020 01/10/2019 27/11/2020 NODARI LUCA (Presidente)
ZANONATO PIER LUIGI (Membro Effettivo)
7 CHIMICA GENERALE E INORGANICA 2018-2019 01/10/2018 30/11/2019 NODARI LUCA (Presidente)
CAUSIN VALERIO (Membro Effettivo)
6 CHIMICA GENERALE E INORGANICA 2017/2018 01/10/2017 25/11/2018 NODARI LUCA (Presidente)
ZANONATO PIER LUIGI (Membro Effettivo)
5 CHIMICA GENERALE E INORGANICA 2016-2017 01/10/2016 30/11/2017 NODARI LUCA (Presidente)
ZANONATO PIER LUIGI (Membro Effettivo)

Prerequisites: The student should master the unit of mass (mg, g, kg) and volume (mL, L, m3, dm3, cm3). Also, the student must have basic knowledge on logarithms and exponential notation.Moreover, he should be able to solve equations of first and second degree.
Target skills and knowledge: To know and be able to understand reference concepts and propaedeutic arguments regarding:
• the atomic nature of matter;
• the chemical bond;
• the properties of gases and solutions;
• the behavior of systems in chemical equilibrium, with particular reference to those in aqueous solution (acid-base and heterogeneous equilibria);
• the periodic table of elements, and the chemistry of selected elements.
Examination methods: Written and oral. Students must pass a written test with questions covering the whole activity. The student must also submit a report on the results of the short laboratory practice.
The oral part of the examination is optional.
Assessment criteria: A maximum of 27 points are awarded to written test.
A maximum of 3 points are assigned to the laboratory report.
Course unit contents: (Numerical applications are required for the topics marked with an asterisk)
CONSTITUENTS OF MATTER*. Homogeneous and heterogeneous systems. Chemical elements and compounds. Atoms and subatomic particles.
Isotopes and atomic masses. Molecules and molecular mass. Avogadro's number, mole concept.
ATOMIC THEORY. Notice about the first atomic theory and quantum theory. Description of the hydrogen atom: quantum numbers and orbitals. Multi-electronic atoms: Pauli exclusion principle, Hund's rule, the distribution of the electrons. Electronic structures and the periodic table of the elements.
FORMULAS AND CHEMICAL EQUATIONS *. Minimum and molecular formulas. Binary and ternary compounds. Nomenclature. Chemical reactions and their balance.
CHEMICAL BOND. Ionic and covalent bonding. Polarity of the bond. Electronegativity. Valence bond theory. Octect rule. Lewis structures. Resonance formulas. Molecular geometry by VSEPR method.
STATES OF AGGREGATION OF MATTER. The ideal gas. Liquids and solids. Phase equilibria. State diagrams of a pure substance.
SOLUTIONS*. Process of dissolution and solvation. Aqueous solutions. Concentration of a solution. Colligative properties of solutions: osmotic pressure. lowering of vapor pressure, raising and lowering of ebullioscopic and crioscopic points.
Chemical Kinetics. Definition of reaction rate. Parameters that affect the rate of reaction. Kinetic laws. Introduction to the theory of collisions. Activation energy Catalysis and catalysts.
CHEMICAL BALANCE*. Law of mass action. Chatelier's principle. Equilibrium constant and its expressions. Thermodynamics of 'chemical balance.
ACIDS AND BASES*. Definitions (Arrhenius, Brønsted-Lowry and Lewis). Ionic product of water. The pH scale. Acid base balance in the water. Strength of acids. Buffer solutions. Titrations of monoprotic acids and bases.
REACTIONS OF OXIDATION-REDUCTION*. Oxidation and reduction. Oxidation number. Rules for calculating the number of oxidation.
Balancing redox reactions.
ELECTROCHEMISTRY. Red-ox reactions and voltaic pile: Semi-elements; electromotive force; standard potential; standard electrodes. Nernst equation.
ELEMENTS AND COMPOUNDS. Introductory inorganic chemistry of the elements of the 1st, 2nd and 13th-18th groups.

- There will also be two laboratory exercises: Preparation of an inorganic chemical compound;
Reactivity of some metal cations representative of the periodic table with hydroxide ion and other inorganic anions.
Planned learning activities and teaching methods: Frontal lessons with exercises of stoichiometric calculations.
Additional notes about suggested reading: A CD with track of the lessons and handouts of laboratory. Photocopies. Exercises and solutions (sent by mail)
Textbooks (and optional supplementary readings)
  • R. H. Petrucci, F. G. Herring, J. D. Madura, C. Bissonnette, Chimica generale. Principi ed Applicazioni Moderne. Padova: Piccin, 2013. Si può comperare anche il libro con le soluzioni agli esercizi che si trovano nel testo
  • I. Bertini, C. Luchinat, F. Mani, Stechiometria Un avvio allo studio della chimica. MILANO: Ambrosiana, --. per i calcoli stechiometrici / in commercio ci sono molti libri equivalenti Cerca nel catalogo