First cycle
degree courses
Second cycle
degree courses
Single cycle
degree courses
School of Science
Course unit
SC10101298, A.A. 2019/20

Information concerning the students who enrolled in A.Y. 2019/20

Information on the course unit
Degree course First cycle degree in
SC1161, Degree course structure A.Y. 2008/09, A.Y. 2019/20
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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 30/09/2019
End of activities 18/01/2020
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)

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 knownledge on logarithms and exponential notation. Moreover, the student should be able to solve equations of first and second degree.
Target skills and knowledge: The student should 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 test and laboratory report.
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.(0.5 CFU)
ATOMIC THEORY. Notes on 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.(1CFU)
FORMULAS AND CHEMICAL EQUATIONS *. Minimum and molecular formulas. Binary and ternary compounds. Nomenclature. Chemical reactions and their balance.(0.25 CFU)
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.(1 CFU)
STATES OF AGGREGATION OF MATTER. The ideal gas. Liquids and solids. Phase equilibria. State diagrams of a pure substance.(0.25 CFU)
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. (1 CFU)
CHEMICAL BALANCE*. Law of mass action. Chatelier's principle. Equilibrium constant and its expressions. Thermodynamic of chemical balance.
EQUILIBRIA IN WATER SOLUTION*. Definitions (Arrhenius, Brønsted-Lowry and Lewis). Ionic product of water. The pH scale. Acid base balance in the water. Strength of acids. Buffer solutions. Hydrolysis in Acid-Base Reactions. Solubility equilibrium. Common ion effect. Coordination compounds. Definition of coordination compounds, Lewis acids and bases, characteristics of coordination compounds. (1 CFU)
Planned learning activities and teaching methods: Frontal lessons with exercises of stoichiometric calculations.
Additional notes about suggested reading: Track of the lessons and handouts of laboratory.
Textbooks (and optional supplementary readings)

Innovative teaching methods: Teaching and learning strategies
  • Laboratory
  • Working in group
  • Questioning
  • Loading of files and pages (web pages, Moodle, ...)

Innovative teaching methods: Software or applications used
  • Moodle (files, quizzes, workshops, ...)

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