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School of Science
Course unit
SCN1036943, 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
IF1839, Degree course structure A.Y. 2011/12, A.Y. 2019/20
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Number of ECTS credits allocated 10.0
Type of assessment Mark
Website of the academic structure
Department of reference Department of Biology
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 LAURA ORIAN CHIM/02
Other lecturers ROBERTINO PILOT

ECTS: details
Type Scientific-Disciplinary Sector Credits allocated
Basic courses CHIM/02 Physical Chemistry 4.0
Basic courses CHIM/03 General and Inorganic Chemistry 6.0

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

Type of hours Credits Teaching
Hours of
Individual study
Practice 1.0 16 9.0 No turn
Laboratory 1.0 16 9.0 2
Lecture 8.0 64 136.0 No turn

Start of activities 30/09/2019
End of activities 18/01/2020
Show course schedule 2019/20 Reg.2011 course timetable

Examination board
Board From To Members of the board
11 M-Z CHIMICA 1 2018-2019 01/10/2018 30/11/2019 ZOLEO ALFONSO (Presidente)
RUZZI MARCO (Membro Effettivo)
10 A-L CHIMICA 1 2018-2019 01/10/2018 30/11/2019 ORIAN LAURA (Presidente)
PILOT ROBERTINO (Membro Effettivo)

Prerequisites: No prerequisite
Target skills and knowledge: The course is based on a part of general chemistry, which includes stoichiometry and lab exercises, and a part of physical chemistry.


The aim of the course is to provide a basic but rigorous knowledge of chemistry. The goal of the exercises is the acquisition of the fundamentals of stoichiometry. During the lab sessions the student will become familiar with simple chemical equipments and common lab practices.
It wants to offer basic knowledge on the general chemistry, described in five points:

1) Basic chemistry laws (mass conservation, specie conservation, charge conservation, periodic table relationships, etc.)
2) Chemical names (symbols, isotopes, hot to name a compound, etc.)
3) Matter structure (atom, molecule, solid, liquid, chemical bond, etc.)
4) Matter transformations (physical and chemical process, reactions, equilibria, etc.)
5) Stoichiometry, i.e. mass measurements in chemistry: pH measurement, concentrations, titrations, etc.

At the end of this part, the student shoud be able to:

1) Describe and comment the main chemical laws
2) Manage the terminology and names in chemistry
3) Have specific knowledge about matter microscopic structure (atoms, molecules, ions, electrons, electron configuration, orbitals, etc.)
4) Write a generic reaction, balance it, indicating the various parts
5) Carry out stoichiometric calculations (preparation of solutions, concentration calculations, pH determinations, solubility determination, calculations of REDOX potentials of electrodes in electrochemical cells, etc.)


This part provide basic knowledge on chemical equilibrium thermodynamics and kinetics, according to the following list:

1) The concepts (heat, work, temperature, pressure, volume, reaction velocity, reaction order, etc.)
2) The models (close, open, isolated systems, phases, perfect gas, etc.)
3) The transformations (physical, chemical, adiabatic, isochore, isothermal, expansion, compression, reversible, irreversible)
4) The laws (gas laws, Thermodynamics first law, second law, third law, Hess' law, Arrhenius' law, etc.)
5) Thermodynamics quantities (enthalpy, entropy, free energy, kinetics constant)
6) Applications to chemical reactions (spontaneity, reaction direction, heat, decay velocity, etc.)
7) The equilibrium constant and its dependency on temperature and pressure.

At the end of this part the student should be able to:

1) Have clear in mind the basic concepts (heat, work, temperature, etc.), and the suitable definitions
2) Connect the type of transformation with the type of variables at stake
3) Carry out physical chemical calculations of the variables at stake (pressure, partial pressure, volume calculations; volume, enthalpy, entropy, free energy, variations
4) Know the factors which allow to control the direction of a process and the effects of heat, pressure and temperature on the equilibrium and kinetic constants.

The aim of the course is to provide a basic but rigorous knowledge of chemistry. The goal of the exercises is the acquisition of the fundamentals of stoichiometry. During the lab sessions the student will become familiar with simple chemical equipments and common lab practices.
Examination methods: Written exam. Lab reports.
Assessment criteria: Evaluation criteria of lab reports: correctness, completeness and conciseness of the reports. Evaluation criteria of the written exam: the student must prove the acquisition of the fundamental concepts of chemistry through the solution of problems and answering to open questions. Evaluation criteria: correctness of the numerical results, explanation of the whole procedure, coherence among interdependent results and rigorous use of units of measurement
Course unit contents: GENERAL CHEMISTRY

Atoms, atomic number and mass number; isotopes; ions. Molecules and compounds. Atomic and molecular weight. Mole. Nomenclature of inorganic compounds.
Chemical reactions and their balancing.
Stoichiometry of chemical reactions. Ways of expressing concentration.
Quantum-mechanical model of atom: quantum numbers; orbitals; electronic configurations (Hund’s rule and Pauli’s principle); periodic properties of elements.
The chemical bond: 1) ionic bond. 2) covalent bond: Lewis’s structure; molecular geometry and VSEPR method; valence bond theory; molecular orbitals theory. 3) hydrogen bond.
Chemical equilibrium: homogeneous and heterogeneous equilibria; Mass action law and equilibrium constant;
Le Chatelier’s principle.
Acid-base equilibria: properties and definitions of acids and bases; water autoprotolysis reaction; pH; hydrolysis; buffer solutions; acid-base titration.
Solubility equilibria: Solubiltity product; molar solubility; factors affecting the solubility (common ion, pH and complexation).
Electrochemistry: voltaic cells; standard reduction potential; Nerst equation; electrochemical cells in non-standard conditions; batteries; electrolytic cells.
The problem solving activities aim to practical application of the theoretical tools provided during the lectures.
Laboratory experiments are relative to General and Inorganic Chemistry program


Thermodynamics: physical and chemical systems. Aggregation states of matter. Extensive and intensive state variables. State functions and equations. Perfect and real gases. Zeroth law. First law: work, heat and internal energy. Enthalpy. Standard phase transition, reaction and formation enthalpy, Hess law. Kirchoff law. Reversible and irreversible transformations. Second law: entropy and spontaneous processes in adiabatic conditions. Third law; Debye law and absolute entropy. Gibbs free energy and spontaneous processes. Chemical potential. Spontaneous chemical reactions and reaction equilibrium. Reaction free energy and equilibrium constant. Phase transitions and equilibria. Clapeyron and Clausius-Clapeyron equations. Ideal and real solutions. Colligative properties and osmotic pressure. Chemical kinetics: reaction rate; kinetic laws and constants. Half-life. Reaction mechanisms. Arrhenius law. Elements of catalysis.
Planned learning activities and teaching methods: The course consists of classroom lectures, problem solving activities and laboratory experiments.
Additional notes about suggested reading: lesson's notes, downloads of complementary material.
Textbooks (and optional supplementary readings)
  • Petrucci, Ralph H.; Herring, F. Geoffrey; Madura, Jeffrey D.; Bissonette, Carey, Chimica generale. Principi ed applicazioni moderne. Padova: Piccin, 2013. Decima Edizione Cerca nel catalogo
  • Paterno Parsi, A.; Parsi, A.; Pintauer, T.; Gelmini, L.; Hilts, R.W., Esercizi Svolti - Chimica Generale. Principi ed applicazioni moderne di Petrucci-Herring-Madura-Bissonette. Padova: Piccin, 2015. Decima Edizione Cerca nel catalogo
  • Paterson Parsi, A.; Parsi, A.; Pintauer, T.; Gelmini, L. Hilts, R.W., Soluzione degli esercizi - Chimica Generale. Principi ed applicazioni moderne di Petrucci-Herring-Madura-Bissonette. Padova: Piccin, 2014. Decima Edizione Cerca nel catalogo
  • Atkins, Peter; de Paula, Julio, Elementi di chimica fisica. Bologna: Zanichelli, 2018. Quarta edizione italiana condotta sulla settima edizione inglese Cerca nel catalogo