First cycle
degree courses
Second cycle
degree courses
Single cycle
degree courses
School of Science
Course unit
SCN1035672, 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
SC1163, Degree course structure A.Y. 2008/09, A.Y. 2019/20
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Number of ECTS credits allocated 13.0
Type of assessment Mark
Course unit English denomination GENERAL AND INORGANIC CHEMISTRY
Department of reference Department of Chemical Sciences
E-Learning website
Mandatory attendance No
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 GIAN-ANDREA RIZZI CHIM/03
Other lecturers FRANCESCO SEDONA CHIM/03

ECTS: details
Type Scientific-Disciplinary Sector Credits allocated
Basic courses CHIM/03 General and Inorganic Chemistry 10.0
Core courses CHIM/03 General and Inorganic Chemistry 3.0

Course unit organization
Period Annual
Year 1st Year
Teaching method frontal

Type of hours Credits Teaching
Hours of
Individual study
Practice 3.0 30 45.0 No turn
Laboratory 2.0 24 26.0 No turn
Lecture 8.0 64 136.0 No turn

Start of activities 30/09/2019
End of activities 20/06/2020
Show course schedule 2019/20 Reg.2008 course timetable

Examination board
Examination board not defined

Prerequisites: Concept of measuring units, resolution of equation of first and second degree , systems of equations, use of powers and logarithms.
Target skills and knowledge: The lectures are designed to provide an initial chemical rigorous literacy to students who are going to study the discipline. The part of exercises and laboratory provides acquisition of the basic elements of stoichiometry, i.e., the numerical aspects of the simplest chemical concepts and the acquisition of knowledge concerning rules of prevention and safety.
Examination methods: Laboratory reports, written and oral exam.
Assessment criteria: The acquisition of the contents of the laboratory experience is evaluated on the basis of written reports compiled respecting a grid of predetermined questions. Will be considered as criteria for evaluation, the accuracy, completeness, conciseness and ownership of expression in preparing the reports. The delivery of lab reports gives access to the written test. The correctness of the numerical results, the clarification of the processes used to obtain them, the internal consistency between the results and rigor in the use of the correct unit of measurement associated with the physical quantities used are elements of evaluation of the written test. This gives access to the oral exam, where we evaluate the skills acquired by the student in the theoretical part of the course. Criteria for assessing the oral test are rigorous quantitative demonstrations, the degree of detail of this, the ability to establish links between different aspects of a chemical phenomenon.
Course unit contents: LESSONS IN CLASSROOM: Atomistic Theory - Structure of the atom, atomic number, mass number and isotopes, molecules, ions, chemical formulas, nomenclature of compounds. Stoichiometry - atomic mass, Avogadro number, molar mass of elements and compounds, composition and percentage, determination of chemical formula from elemental analysis, chemical reactions and chemical equations, reagents, products and limiting reagent. Reactions in aqueous solution - precipitation reactions, acid-base reactions, redox reactions, concentration of the solutions. Gases - the gas pressure, ideal gas laws, partial pressures, kinetic molecular theory, real gases. Energy in chemical reactions - types of energy, energy changes in chemical reactions, introduction to thermodynamics, internal energy and enthalpy. Electronic structure of atoms - quantum theory, photoelectric effect and black body, Bohr atom, quantum mechanics, atomic orbitals and quantum numbers, electronic configuration. The periodic table - the periodic system of the elements, periodic variations of the physical properties, chemical properties of the elements of groups ns-np. The chemical bond - representation of Lewis, ionic bond, lattice energy, covalent bond and electronegativity, Lewis structures and formal charges, exceptions to the octet rule, enthalpy in chemical bonds. Molecular geometry and hybrid orbitals - VSEPR theory, dipole moment, valence bond theory, hybridization of atomic orbitals, hybridization in molecules containing double and triple bonds, molecular orbital theory, metallic bond. Intermolecular forces - liquids and solids - kinetic molecular theory of liquids and solids, intermolecular forces, liquid properties, crystal structure, bonding in solids, state transitions, state diagrams and distillation. Physical properties of solutions - types of solution, concentration measurement, colligative properties. Chemical equilibrium – concept of chemical equilibrium, ways of expressing the equilibrium constants, factors that influence the chemical equilibrium. Acids and Bases - definition of Broensted and Lewis, acid-base properties of water, pH, strength of acids and bases, strong acids and bases, weak acids and bases, conjugate acids and bases, acid-base properties of the salts and oxides , buffer solutions, acid-base titrations, indicators, solubility equilibria, common ion effect. Thermodynamics - The three principles of thermodynamics, spontaneous processes, entropy, the second law of thermodynamics, the Gibbs free energy and chemical equilibrium. Electrochemistry and redox reactions – balancing redox reactions, galvanic cells, table of standard potentials, thermodynamics of redox reactions, Nernst equation, batteries, corrosion and electrolysis.
1) Properties of some cations and inorganic anions: soluble and insoluble salts, pH of the metal cations.
2) The chemical equilibrium: effect of temperature and concentration of reactants / products.
3) Experiments in electrochemistry: Daniel galvanic cell, Cu electroplating, electrolysis of water.
4) Acid-base titrations: titration strong-strong and strong-weak with indicator and pH meter.
5) distillation of an aqueous solution of hydrochloric acid.
6) The cycle of copper: oxidation of metallic Cu, precipitation of copper, preparation of copper oxides and dismutation.
Planned learning activities and teaching methods: Lessons in the classroom, laboratory experiments and guided solutions of exercise.
Additional notes about suggested reading: Notes and powerpoint slides.
Textbooks (and optional supplementary readings)
  • Raymond Chang, Kenneth Goldsby, Fondamenti di Chimica Generale. --: Mc Graw Hill Education (Italy), 2015. Cerca nel catalogo