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Second cycle
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Single cycle
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School of Medicine
Course unit
FA13101298, A.A. 2019/20

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

Information on the course unit
Degree course 5 years single cycle degree in
PHARMACY (Ord. 2018)
FA1732, Degree course structure A.Y. 2018/19, A.Y. 2019/20
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Number of ECTS credits allocated 10.0
Type of assessment Mark
Course unit English denomination GENERAL AND INORGANIC CHEMISTRY
Department of reference Department of Pharmaceutical and Pharmacological 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 is available ONLY for students enrolled in PHARMACY (Ord. 2018)

Teacher in charge MAURIZIO CASARIN CHIM/03
Other lecturers MARZIO RANCAN 000000000000

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

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

Type of hours Credits Teaching
Hours of
Individual study
Practice 2.0 24 26.0 No turn
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.2018 course timetable

Examination board
Board From To Members of the board
13 Commissione a.a. 2019/20 02/12/2019 30/09/2020 DOLMELLA ALESSANDRO (Presidente)
CASARIN MAURIZIO (Membro Effettivo)
GANDIN VALENTINA (Membro Effettivo)

Prerequisites: The class of "General and Inorganic Chemistry" can be fruitfully attended also by those who have no prior knowledge of chemistry. However, because of the kind of the explanations that will be given during lectures, it is important that the Students already master some basic skills about the numerical calculus, in particular: the execution and the properties of operations with exponential numbers and logarithms, the solution of equations of first and second degree.
Target skills and knowledge: The class of "General and Inorganic Chemistry" aims to provide the Student basic chemistry concepts needed to pave the basis for all further teachings of the curriculum having chemical content and to grant a fruitful learning of the same.In particular, the chemistry of aqueous solutions will be emphasized, to enable a quicker grasp of specialized knowledge on the behavior of drugs.
At the end of the lectures the Student:
1) will have gained basic chemistry knowledge about the composition, structure, properties and modifications of matter;
2) will have acquired fundamental concepts about the atomic nature of the matter, the chemical bonding, the properties of gases and of solutions;
3) will be able to balance a chemical equation and assess the quantitative ratios in a reaction;
4) will be able to correctly represent the formula and molecular geometry of some simple chemical compounds;
5) will be able to understand the behavior of a system in condition of chemical equilibrium in an aqueous solution and foresee the evolution of a system outside equilibrium;
6) will have gained the knowledge to evaluate the concentration and the dilution of aqueous solutions;
7) will be able to evaluate acidity (pH) of aqueous solutions and conditions leading to the separation of poorly soluble compounds;
8) he can foresee the result of reactions on the basis of standard red-ox potentials.
Examination methods: The assessment consists of a written test integrated with an oral examination.
The aim of the written test is to verify that the Candidate has gained the knowledge described along the objectives of the course and the ability of the Candidate of translating into quantitative terms the theoretical knowledge gained.

The written test is passed only when the elaborate of the Candidate gets a positive rating.
Assessment criteria: The final examination is designed to assess the degree of achievement of the main teaching objectives:
(a) the knowledge of theoretical bases of General Chemistry;
(b) the knowledge of the methods to address the solution of problems concerning the various facets of General Chemistry;
(c) the knowledge of the chemistry of aqueous solutions;
(d) the knowledge of the chemical behavior of the elements of the main groups of the Periodic Table and of some of thir most notable compounds.
Course unit contents: Note on the "Objectives Agenda 2030" (see below). Chemistry has a pervasive impact on our life. The Teacher holds that the topics of the course, placed in the context of real life, are relevant to all the themes of the Agenda noted below.

Matter and energy. Elements and substances. Atomic nature of matter. Atom and subatomic particles. Atomic number, mass number, isotopes. U.m.a.. Atomic and molecular weights. Mole. The wave-mechanical atom. Quantum number. Electronic configurations. The Periodic Table and periodic properties. Metals and non-metals. Chemical symbols. Oxidation number. Systematic nomenclature. Chemical Formulas. Percentage composition. Percent purity. Chemical equations. Oxidation and reduction. Ionic dissociation and ionic form of a chemical equation. Balance of chemical reactions in aqueous solution. Quantitative ratios. Limiting reagent and reaction percentage yield. Theory of chemical bonding according to Lewis. Covalent and ionic bond. Simple and multiple bonds. Binding order. Energy of chemical bonds. Bond enthalpy. Molecular geometry (VSEPR) of compounds with steric no.s 2, 3, 4, 5, 6. VB theory and hybridization. Polar bonds. Bond dipoles and molecular dipoles. Dative bond. Coordination compounds and relevant nomenclature (outline). Isomers. Intermolecular forces:ion-ion and ion-dipole forces, dipole interactions, van der Waals forces, London forces. Hydrogen bond. Gaseous state. Pressure and measurement of pressure. Laws by Boyle, Charles, Avogadro. Equation PV =nRT for ideal gases. Dalton's law. Real gases. Van der Waals equation. Condensed phases and phase transitions. Evaporation, fusion, sublimation. Normal melting and boiling points. Condensation / liquefaction of gases. Critical phenomena. Critical temperature. Phase diagrams. Water phase diagram. Homogeneous mixtures. Solutions. Solubility. Methods for measuring solution concentration. Molarity, molality. Dilution. Raoult's laws for the non-volatile and volatile solute. Solubility of gases; Henry's law. Solubility dependence upon the nature of solute, solvent and temperature. Colligative properties of solutions. Osmosis and osmotic pressure. Fractional distillation. Thermochemistry. Hess'law. Thermodynamics applied to chemistry. Spontaneous reactions. Entropy. Free energy. Foundations of the chemical equilibrium. Law of mass action. Equilibrium constant: Kc, Kp and reaction quotient. Le Chatelier's principle. Factors influencing chemical equilibrium (temperature, pressure and concentration). Chemical equilibria in solution. Autoprotolysis of water and Kw. Acid-base equilibrium in aqueous solution. Arrhenius, Bronsted and Lewis' acids. Acid-base conjugated couples. pH, pOH, pKw. pH of solutions of acids and bases having different force. pH of salts and hydrolysis. pH of ampholytes. pH of buffer solutions. Solubility/precipitation equilibria. Solubility product, Kps, precipitation. Factors affecting solubility. Kps and solubility. Common ion effect. Solubility and pH. Solubility and complexation. Solubility of hydroxides, amphoteric hydroxides, sulfides. Electrochemistry. Redox conjugate couples. Electrochemical course of a reaction. Galvanic cells, half-cells, salt bridge, cathode, anode. Normal hydrogen electrode and standard reduction potentials. EMF of a cell. Table of standard potentials. Forecast of the course of redox reactions. Nernst's equation. Inorganic chemistry. Properties of the elements of the Periodic Table.
Planned learning activities and teaching methods: The course consists of classroom lectures (scheduled 64 hours) and stoichiometry tutorials (scheduled 24 hours).
Teaching is mainly conventional, with oral presentation, supported by writing on the board/electronic board. The Teacher explains the relevance of the topics by giving practical examples of their application in the Students' future professional milieu. The aim of the lectures is to transfer the theoretical bases pertinent to the discussed topics.
Stoichiometry tutorials.
The tutorials are hold in parallele to lectures, at the end of a series of lectures giving coherent informations. The goals of the tutorials are:
(a) the practical application of the proposed theory (acquisition of practical skills)
(b) stimulate analytical skills and the ability to identify a problem-solving oriented strategy (acquisition of processing abilities).
Additional notes about suggested reading: The teacher recommends frequent attendance and participation to lectures. The Teacher also recommends re-elaboration of the lecture notes, individually and in groups.
Textbooks (and optional supplementary readings)
  • Petrucci, Herring, Madura, Bissonnette, Chimica Generale - Principi ed Applicazioni Moderne. --: Piccin, --. Cerca nel catalogo
  • o, --. --: --, --.

Innovative teaching methods: Teaching and learning strategies
  • Working in group
  • Problem solving
  • Use of online videos
  • Loading of files and pages (web pages, Moodle, ...)

Sustainable Development Goals (SDGs)
Quality Education Gender Equality Reduced Inequalities