First cycle
degree courses
Second cycle
degree courses
Single cycle
degree courses
School of Science
Course unit
SCN1035672, 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
SC1157, Degree course structure A.Y. 2014/15, A.Y. 2016/17
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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
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 MAURO SAMBI CHIM/03
Other lecturers FRANCESCO SEDONA CHIM/03

Course unit code Course unit name Teacher in charge Degree course code

ECTS: details
Type Scientific-Disciplinary Sector Credits allocated
Basic courses CHIM/03 General and Inorganic Chemistry 11.0
Core courses CHIM/03 General and Inorganic Chemistry 2.0

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 01/10/2016
End of activities 16/06/2017
Show course schedule 2019/20 Reg.2014 course timetable

Examination board
Examination board not defined

Prerequisites: None
Target skills and knowledge: Classroom lectures are meant to provide basic, yet rigorous foundations in chemical knowledge to undergraduate beginners. Exercises provide basic elements of stoichiometric calculations. Fundamental prevention and safety issues regarding chemical substances, workplace behavior and first aid norms, the correct use of chemical glassware and simple instrumentation, as well as and the most common experimental procedures are provided through several laboratory experiences.
Examination methods: Laboratory reports, written examination on stoichiometry, oral examination.
Assessment criteria: The criteria for assessing the written test are the correctness of the numerical results, the traceability of procedures used to obtain them, the internal consistency between logically interdependent results and the rigorous usage of the correct units of measurement associated with the physical quantities. A successful outcome of the written test 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 in the answers, the ability to establish links between different aspects of a chemical phenomenon. The acquisition of the contents of the laboratory experiences is evaluated on the basis of written reports based on a grid of predetermined questions. The accuracy, completeness, conciseness and language quality in preparing the reports are the criteria for their evaluation.
Course unit contents: CLASSROOM LECTURES: The scientific method. States of matter. Mixtures (homogeneous, heterogeneous) and pure substances. Elements and compounds; atoms and molecules. Atomistic theory. The atomic number and the mass number. Isotopes. Atomic mass units. Relative atomic mass. Mole. Percentages in mass, minimal formula, molecular formula. Oxidation numbers and their determination. Balancing chemical equations in molecular / ionic form. Mass and charge balance. Balancing non-redox reactions. Oxidation numbers method and half-reactions method of balancing redox reaction equations.
The chemical bond I: covalent, ionic and metallic bonds. Lewis structures. VSEPR method.
Atomic structure according to quantum mechanics. Bohr's atom and its limits. Uncertainty principle. Wave-particle duality. Wave function. Schrödinger equation and its solutions for the one-electron atom. Atomic orbitals. Electron spin. Introduction to polyelectronic atoms. Shell model of the atom. Aufbau principle. Pauli exclusion principle. Hund's rule.
Periodic properties: atomic and ionic radius, ionization energy, electron affinity, electronegativity. Stoichiometry of binary hydrides and oxides. Acid / base properties of oxides.
The chemical bond II. LCAO-MO theory for diatomic homonuclear and heteronuclear molecules.
Brief comparison of VB and the MO theories. Carbon hybrid orbitals.
Perfect gas law. Dalton's law. Kinetic theory of gases. Maxwell-Boltzmann distribution of molecular speeds. Effusion. Real gases. Van der Waals equation. Intermolecular interactions. Structure of solids.
Chemical equilibrium. Law of mass action. Le Chatelier's principle. Chemical thermodynamics. First and second laws of thermodynamics. Hess's law. Gibbs free energy. Criteria of spontaneity of a chemical reaction. Relationship between equilibrium constant and ΔG°.
Equilibria in solution. Strong and weak electrolytes. Acids and bases according to Aarhenius, Brønsted-Lowry, Lewis. Hydrolysis of salts. Buffer solutions. Slightly soluble salts.
Introduction to p, T phase diagrams for a single component. Phase rule. Phase diagrams for mixtures of two volatile components. Raoult's law. Distillation. Azeotropic mixtures. Colligative properties.
Electrochemistry. Standard reduction potentials. Nernst equation. Batteries. Corrosion and corrosion protection. Electrolysis. Faraday's laws. Overpotential.
Chemical kinetics. The speed and the order of reaction. Half-life. Activation energy. Arrhenius equation. Reaction mechanisms. Elementary processes. Rate-determining step. Catalysts.
NUMERICAL EXERCISES: exercises and demonstrations on topics covered in classroom lectures, with which they are closely matched.
LABORATORY: (1) Properties of some physical and chemical processes (acid / base reactions, salt formation, endo / exothermic processes); (2) Experiments in electrochemistry (redox reactions, Daniell cell, electrolysis of water); (3) Chemical equilibrium (effects of concentration, temperature and common ion) (4) acid-base titrations (strong / strong and weak / strong acid-base titrations); (5) Distillation of an aqueous solution of hydrochloric acid; (6) the cycle of copper (redox reactions, acid / base equilibria and precipitation applied to the chemistry copper in aqueous solution).
Planned learning activities and teaching methods: Classroom lectures, classroom numerical exercises, laboratory experiences.
Additional notes about suggested reading: Lecture notes, lecture slides available on the lecturer's website:
Textbooks (and optional supplementary readings)
  • D. W. Oxtoby, H. P. Gillis, A. Campion, Principles of Modern Chemistry. --: Ed. Brooks/Cole, Cengage Learning, --. Cerca nel catalogo
  • S. S. Zumdahl, Chemical Principles. --: Ed. Brooks/Cole, Cengage Learning, --. Cerca nel catalogo
  • P. Michelin Lausarot , G. A. Vaglio, Fondamenti di stechiometria. --: Piccin, --. Cerca nel catalogo
  • P. Ferri, Calcoli stechiometrici. --: ETS, --. Cerca nel catalogo