Catalogo dei Corsi di studio

The main objectives are the knowledge of the fundamental concepts of general chemistry and the skill to address numerical exercises relevant to the application of these concepts.
More specific objectives are the knowledge and application of fundamental concepts concerning the atomic structure, the chemical bond, the geometry and structure of molecules, the states of matter and their properties, the transitions phase, the main laws of thermodynamics and kinetics, the equilibria in solution and in the gas phase, the acids, bases and titration, the solubility equilibria, the electrochemistry and its application.
Further objectives are the ability to connect the acquired knowledge, the ability to communicate what the student has learnt, the ability to understand the contents of the following chemistry courses.

Programme

1-Matter and transformations; atoms: elements, nuclides, isotopes; molecules: formulas, elemental composition; mixtures, substances. Atomic structure; electronic structure of atoms: the atomic spectra, orbitals and their energy; electron configuration of the elements (aufbau); periodic table and properties of the elements. Electronic configuration. (8 h)

2-Chemical bond and theories. Different types of bonds, energy and length. Molecular orbitals and hybrid orbitals. Resonance. (8 h)

3-Geometry and structure of typical molecules. Intermolecular bonding. (5 h)

4-States of matter. Gas, liquid and solid state. The gas laws. Kinetic theory. Volatility of liquids and their properties. (5 h)

5-Elements of thermochemistry. Principles of thermodynamics. Thermochemistry. The Hess Law. The Equilibrium. The thermodynamic criteria for spontaneous or equilibrium processes. The Clausius Clapeyron law. (10 h)

6-Solutions and their properties. Phase transitions. Phase equilibria. (6 h)

7-Chemical equilibrium and Le Chatelier's principle. Electrolites and their properties. (8 h)

8-Acids and bases. Acid-base equilibria theories. Titrations. pH calculations. Solubility and equilibria. (16 h)

9-Basics of electrochemistry: conductivity, voltaic and electrolytic cells. Redox ractions. Nernst equation. (4 h)

10-Chemical kinetics, kinetic constants, dependence of the rate constant on the temperature. The Arrehnius equation. Catalysis. (4 h)
Inorganic chemistry.


Stoichiometry

1-Calculations methods. Figures. Atomic weigth. Isotopic abundance and molecular weigth. The mole concept. (2 h)

2-Chemical equations. Oxidation number and redox reactions. Oxidation number. Equivalent weigth. (4 h)

3-Solutions and concentration units. Dilution and mixing of solutions. Density. (3 h)

4-Gas phase: volume, pressure and temperature.The laws of Boyle, Charles and Gay-Lussac, the Avogadro's principle.The ideal gases equation. Partial pressures and the Dalton's law. (3 h)

5-Electrolites. Vapor pressure, the Raoult's law, the osmostic pressure. Electrolytic dissociation. Strong and weak electrolytes. Dissociation degree. (4 h)

6-Chemical equilibrium and Le Chatelier's principle. Gaseous dissocaition. Equilibrium constants. (6 h)

7-Acid-base equilibria. pH. Strong and weak acids and bases. pH calculations. Poliprotic acids. Buffer solutions. Salts. Titration. (10 h)

8-Solubility equilibria. The effect of pH on the solubility. (2 h)

9-Electrolysis and Faraday's laws.The Nernst equation. (2 h)

Adopted texts

F. Cacace, U. Croatto - Istituzioni di Chimica

F. Cacace, Schiavello - Stechiometria



The recommended texts are sufficient to provide the necessary knowledge of the topics covered in the course.
The students are strongly encouraged to enrich their knowledge utilizing any other text at their disposal, even if not present in the suggested bibliography, in order to make comparisons of different texts and make the best personal synthesis.

Bibliography

Kotz, Treichel, Weaver: Chimica P. Silvestroni: Fondamenti di Chimica Nivaldo J. Tro: CHIMICA P. Atkins, L. Jones: FONDAMENTI DI CHIMICA GENERALE

Prerequisites

Basic knowledge of mathematics: elementary calculations, powers and logarithms, first and second degree equations, exponentials, limits, derivatives, integrals and functions.

Exam modes

The assessment takes place at the end of the course by a written test (lasting three hours) and an oral one, aimed at verifying the ability to apply the acquired knowledge to practical problems of stoichiometry and also verifying the general knowledge acquired.

Since there are no limits to the number of sustainable tests during the year, the written tests have the twofold function of examination and self-assessment of the degree of knowledge acquired, in case the student does not want the test is validated.

Exams are held during the exam periods provided for in the university teaching regulations, while intermediate tests are not in progress so as not to interfere with the regular attendance of the semester lessons, as established by the study program board.

Other elements such as the language, the critical capacity, the reasoning skills, the ability to summarize the arguments and make connections concur to determine the final vote in its graduality.

Exam reservation date start	Exam reservation date end	Exam date
03/02/2020	17/02/2020	20/02/2020
09/06/2020	21/06/2020	23/06/2020
01/07/2020	12/07/2020	14/07/2020
03/09/2020	15/09/2020	17/09/2020
15/11/2020	01/12/2020	03/12/2020
10/01/2021	24/01/2021	26/01/2021

Programme

Accounting Methods. Experimental and Significant Measures. Unit of measure. Weight ratios in chemical combinations. Atomic weight, isotopic abundance, molecular weight, formal weight. Mole concept. Chemical formulas. Chemical equations and their quantitative significance. Balancing chemical equations. Oxidation number. Oxidation Reduction - Balancing Reactions. Equivalent weight. Quantitative relationships between substances involved in a reaction. Solutions. Concentration and its units: molarity, normality, molarity, molar fraction, percent by weight, percent by volume. Dilution and mixing of solutions. Density. The gaseous state: units relative to volume, pressure and temperature. The laws of the ideal gas: the ideal gas state equation. Avogadro's Principle. Gas mixtures. Partial pressures. Dalton Law. Colligative properties. Colligative Properties of Non-Electrolyte Solutions. Electrolytic dissociation. Weak and strong electrolits. Degree of dissociation. Effect of electrolytic dissociation on colligative properties (van't Hoff). Thermal dissociation. Degree of dissociation. Indirect analysis. Mass action law. Different forms of equilibrium constant and their relationships. Equilibria in a homogeneous and heterogeneous phase. Application of the Le Chatelier principle Mass Action law of Electrolyte. Ostwald Law. Acid-base reaction. Ionic water product. Definition of pH and pOH. Acid solutions and strong bases; Of weak monoprotic acids and bases. Dissolution of polyprotic acids. Buffer solutions. Acid-base equilibria in saline solutions: salts strong acid and weak base and weak acid and strong base. Salts of polyprotic acids and ampholytes. Titrations. Solubility equilibria. Solubility. Solubility and solubility product. Common ion effect. Condition of formation of precipitates. Fractioned Precipitation. Galvanic cell. Normal potential. Nernst's equation. Various types of electrodes and their applications.

Adopted texts

- F. Cacace, M. Schiavello “Stechiometria” Bulzoni Publisher

Bibliography

R. H. Petrucci, F. G. Herring, J. D. Madura, C. Bissonnette “Chimica generale” Piccin

Prerequisites

It is important to master the following preliminary knowledge: • Fundamental concepts of elementary algebra, use of powers and logarithms, methods for the resolution of first and second degree equations and systems of linear equations. Elements of mathematical analysis (limits, derivatives, integrals, functions) • Elements of physics (mechanics, thermodynamics, electromagnetism).

Exam modes

The purpose of the exam consists in verifying the level of understanding and deepening on the subject exposed during the course. It also intends to evaluate the student's reasoning skills and the ability to summarize the arguments carried out in the vision of an organic framework of the subject.
The exam consists of a written test for the resolution of numerical exercises after which, a few days later, there is the oral exam. The student also has the possibility to defer the oral exam up to two appeals after the one in which he/she passed the written exam.
Exams are held during the exam periods provided for in the university teaching regulations, while intermediate tests are not in progress so as not to interfere with the regular attendance of the semester lessons, as established by the study program board.

Programme

Introductory notions. Subject of chemical research. Chemical phenomena. Basic laws of chemistry. Elementary particles, Proton, Neutron, Electron, Atomic number, Mass number, Symbols and chemical notation. Mole. Atomic theory. Atoms and their properties. Atomic mass. Avogadro number. Molecules and molecular weight. Types of chemical compounds and their nomenclature. Chemical reactions, acid-base reactions, oxidation-reduction reactions, conservation of mass and charge, balancing of a chemical reaction, stoichiometric calculations, balance of oxidation-reduction reactions. Numerical applications. 18 hours
Atomic structure. Photoelectric effect. Plank hypothesis. Atomic spectra. Bohr model. De Broglie hypothesis, Wave model of the hydrogen atom. Quantum numbers and atomic orbitals, Electronic spin, Pauli exclusion principle, Electronic configuration of polyelectronic atoms. Periodic table. Metals and non-metals. Chemical bond: concept of valence. The different types of bonds and their properties: order, energy, bond distance, dipolar moment. Valence bond theory and molecular orbitals. σ and π bonds. Hybrid orbitals, resonance. Molecular geometry, Valence shell electronic pair repulsion (VSEPR) theory, Electronegativity, Polar molecules. Intermolecular bonds. 26 hours

Aggregation states and phase transitions. Aeriform, liquid and solid state. State diagrams. Solutions and their colligative properties. Equilibrium between phases and phase rules. Le Chatelier's principle. Overview of thermodynamics. The concept of chemical equilibrium. Principles of thermodynamics. Some thermodynamic functions. Termochemistry. Reactions and chemical equilibria. Thermodynamic criteria for spontaneity and equilibrium in chemical transformations. Equilibrium constant and Van’t Hoff laws. Factors that influence the position of equilibrium. Numerical applications. 32 hours
Electrolytic dissociation. Electrolytes and their properties in solution. Acids and bases. Definition and theories on acid-base equilibria. Relations between molecular structure and acid-base properties. Acid-base equilibria in aqueous solutions. Titrations. Indicators. Solubility. Solubility equilibria and factors that influence them. Electrochemistry. Redox reactions. Galvanic cells and semielements. Normal potentials, electromotive force, Nernst equation. Electrolysis and Faraday laws. Chemical kinetics. Rate, order, molecularity of a reaction, kinetic constant and its dependence on temperature. Arrhenius equation, activation energy. Notes on the theory of collisions. Catalysis. Overview of inorganic chemistry. Systematic nomenclature. Elements of the main groups and their compounds. Numerical applications. 40 hours
The teacher makes available on the course website the teaching material displayed during the lessons so as to allow students to have a precise idea on the subject matter and degree of detail.

Adopted texts

M. Schiavello, L. Palmisano “Fondamenti di Chimica” EdiSES
J. Burge, J. Overby "Chimica Generale" edra
J. C. Kotz, P. M. Treichel, J. R. Townsend “Chimica” EdiSES
R. H. Petrucci, F. G. Herring, J. D. Madura, C. Bissonnette "Chimica Generale" Piccin
F. Cacace, U. Croatto “Istituzioni di Chimica” La Sapienza Editrice
M. Speranza “Chimica Generale e Inorganica” EdiErmes
Whitten, Davis, Peck, Stanley “Chimica” Piccin
F. Cacace, M. Schiavello “Stechiometria” Bulzoni Editore
Educational files on elearning2

Exam reservation date start	Exam reservation date end	Exam date
20/01/2020	14/02/2020	17/02/2020
20/05/2020	21/06/2020	23/06/2020
20/06/2020	12/07/2020	14/07/2020
20/08/2020	15/09/2020	17/09/2020
05/11/2020	02/12/2020	03/12/2020
02/01/2021	24/01/2021	25/01/2021

Programme

Experimental Measures. Unit of measure. Weight ratios in chemical combinations. Atomic weight, isotopic abundance, molecular weight, formal weight. Mole concept. Chemical formulas. Chemical equations and their quantitative significance. Balancing chemical equations. Oxidation number. Oxidation-Reduction and Balancing Reactions. Quantitative relationships between substances involved in a reaction. Solutions. Concentration and its units: molarity, molarity, molar fraction, percent by weight, percent by volume. Dilution and mixing of solutions. Density. The gaseous state: units relative to volume, pressure and temperature. The laws of the ideal gas: the ideal gas state equation. Avogadro's Principle. Gas mixtures. Partial pressures. Dalton Law. Colligative properties. Colligative Properties of Non-Electrolyte Solutions. Electrolytic dissociation. Weak and strong electrolits. Degree of dissociation. Effect of electrolytic dissociation on colligative properties. (van't Hoff). Thermal dissociation. Degree of dissociation. Indirect analysis. Mass action law. Different forms of equilibrium constant and their relationships. Equilibria in a homogeneous and heterogeneous phase. Application of the Le Chatelier principle. Mass Action law on Electrolyte. Ostwald Law. Acid-base reactions. Ionic water product. Definition of pH and pOH. Acid solutions and strong bases; of weak monoprotic acids and bases. Dissolution of polyprotic acids. Buffer solutions. Acid-base equilibria in saline solutions: salts of strong acid and weak base and of weak acid and strong base. Salts of polyprotic acids and anfolites. Solubility equilibria. Solubility and solubility product. Common ion effect. Condition of formation of precipitates. Galvanic cell. Normal potential. Nernst's equation. Various types of electrodes and their applications.

Tests of past exams are carried out during the lessons.

Adopted texts

F. Cacace, M. Schiavello “Stechiometria” Bulzoni Editore

Bibliography

R. H. Petrucci, F. G. Herring, J. D. Madura, C. Bissonnette “Chimica generale” Piccin

Prerequisites

It is important to master the following preliminary knowledge: • Fundamental concepts of elementary algebra, use of powers and logarithms, methods for the resolution of first and second degree equations and systems of linear equations. Elements of mathematical analysis (limits, derivatives, integrals, functions) • Elements of physics (mechanics, thermodynamics, electromagnetism).

Exam modes

The purpose of the exam consists in verifying the level of understanding and deepening on the subject exposed during the course. It also intends to evaluate the student's reasoning skills and the ability to summarize the arguments carried out in the vision of an organic framework of the subject.
The exam consists of a written test for the resolution of numerical exercises after which, a few days later, there is the oral exam. The student also has the possibility to defer the oral exam up to two appeals after the one in which he/she passed the written exam.
Exams are held during the exam periods provided for in the university teaching regulations, while intermediate tests are not in progress so as not to interfere with the regular attendance of the semester lessons, as established by the study program board.

Programme

Experimental Measures. Unit of measure. Weight ratios in chemical combinations. Atomic weight, isotopic abundance, molecular weight, formal weight. Mole concept. Chemical formulas. Chemical equations and their quantitative significance. Balancing chemical equations. Oxidation number. Oxidation-Reduction and Balancing Reactions. Quantitative relationships between substances involved in a reaction. Solutions. Concentration and its units: molarity, molarity, molar fraction, percent by weight, percent by volume. Dilution and mixing of solutions. Density. The gaseous state: units relative to volume, pressure and temperature. The laws of the ideal gas: the ideal gas state equation. Avogadro's Principle. Gas mixtures. Partial pressures. Dalton Law. Colligative properties. Colligative Properties of Non-Electrolyte Solutions. Electrolytic dissociation. Weak and strong electrolits. Degree of dissociation. Effect of electrolytic dissociation on colligative properties. (van't Hoff). Thermal dissociation. Degree of dissociation. Indirect analysis. Mass action law. Different forms of equilibrium constant and their relationships. Equilibria in a homogeneous and heterogeneous phase. Application of the Le Chatelier principle. Mass Action law on Electrolyte. Ostwald Law. Acid-base reactions. Ionic water product. Definition of pH and pOH. Acid solutions and strong bases; of weak monoprotic acids and bases. Dissolution of polyprotic acids. Buffer solutions. Acid-base equilibria in saline solutions: salts of strong acid and weak base and of weak acid and strong base. Salts of polyprotic acids and anfolites. Solubility equilibria. Solubility and solubility product. Common ion effect. Condition of formation of precipitates. Galvanic cell. Normal potential. Nernst's equation. Various types of electrodes and their applications.

Tests of past exams are carried out during the lessons.

Adopted texts

F. Cacace, M. Schiavello “Stechiometria” Bulzoni Editore

Bibliography

R. H. Petrucci, F. G. Herring, J. D. Madura, C. Bissonnette “Chimica generale” Piccin

Prerequisites

It is important to master the following preliminary knowledge: • Fundamental concepts of elementary algebra, use of powers and logarithms, methods for the resolution of first and second degree equations and systems of linear equations. Elements of mathematical analysis (limits, derivatives, integrals, functions) • Elements of physics (mechanics, thermodynamics, electromagnetism).

Frequency modes

Attendance aims to improve the quality of learning and to give a track record for the exam. Students who cannot attend the lessons can download the detailed program and receive assistance from the teacher.

Exam modes

The purpose of the exam consists in verifying the level of understanding and deepening on the subject exposed during the course. It also intends to evaluate the student's reasoning skills and the ability to summarize the arguments carried out in the vision of an organic framework of the subject.
The exam consists of a written test for the resolution of numerical exercises after which, a few days later, there is the oral exam. The student also has the possibility to defer the oral exam up to two appeals after the one in which he/she passed the written exam.
Exams are held during the exam periods provided for in the university teaching regulations, while intermediate tests are not in progress so as not to interfere with the regular attendance of the semester lessons, as established by the study program board.

Programme

Introduction: the scientific method; experimental measurements and units; properties of matter and chemical and physical transformations; states of matter; mixtures, substances, compounds and elements; atoms, molecules, formulas; the mole and Avogadro's number; nuclides, isotopes, elements; formulas and elemental composition; chemistry and the environment. Measurement of the atomic masses: the mass spectrometer;
Atomic structure: fundamental particles and their discovery; the nucleus and mass defect; electromagnetic radiation-matter interactions; waves and particles; photoelectric effect; electronic structure of the atom: atomic spectra, Bohr model, quantum model of the atom; orbitals and their energy; polyelectronic atoms and electronic configuration of the elements (aufbau); periodic table and periodic properties of the elements nuclear decay fission and fusion;
Chemical bonds and molecular geometry: valence electrons and Lewis structures; ionic , covalent and dative bonding; bond properties: electronegativity, resonance, hybridization; the shape of molecules; metals, dielectrics and semiconductors; intermolecular forces; isomerism. valence bond and molecular orbitals;
States of matter: gas: ideal gas equation of state; gas mixtures; Measurement of the molecular weight; Boltzmann equation; diffusion and effusion; real gases; liquids and their properties; Solid: crystals, crystal lattice and unit cell; phase transitions. Kinetic theory of gases: distribution of molecular velocities and their measure, the emissions of pollutants and greenhouse gases; industrial emissions and water pollution;
Fundamentals of thermodynamics: laws of thermodynamics; state functions, their meaning and dependence on state variables and composition; spontaneity and equilibrium in physical and chemical changes; activities and standard state; Gibbs-Helmholtz equation; Clausius-Clapeyron; chemical equilibrium; isothermal and isochoric van t'Hoff equations; solubility and solubility product; colligative properties of solutions; laws of Raoult and Henry; phase rule. Energy production and air pollution; phase diagrams;
Acids and bases: definitions; autoionization of water; acid-base equilibria in solution; pH calculation; ampholytes; isoelectric point; buffer solutions; pH indicators; acid-base titrations; influence of pH on solubility.Structure and strength of acids and bases;
Electrochemistry: strong and weak electrolytes; conductivity; ionic strength and activity coefficients; conductometric titrations; batteries; electrodes; standard potential; voltaic series of the elements; electrolysis; potentiometry and its applications; redox reactions in the environment.
Chemical kinetics: reaction rate; order and molecularity; Arrhenius equation; catalysts; collision theory and transition state; evolution of pollutants in the atmosphere.

Adopted texts

F. Cacace, U. Croatto: Istituzioni di Chimica
F. Cacace, M. Schiavello: Stechiometria
or one of the following:
Kotz, Treichel, Weaver: Chimica
P. Silvestroni: Fondamenti di Chimica
Nivaldo J. Tro: CHIMICA
M. Speranza: CHIMICA GENERALE ED INORGANICA
P. Atkins, L. Jones: FONDAMENTI DI CHIMICA GENERALE

Exam modes

In the written test the student will solve 3 stoichiometry problems, using the concepts learned in the course and proving to know how to apply them.
The oral examination will focus on the topics of the programme and will assess the student's ability to make logical connections between them.

Exam reservation date start	Exam reservation date end	Exam date
01/02/2020	15/02/2020	17/02/2020
08/06/2020	23/06/2020	25/06/2020
01/07/2020	14/07/2020	16/07/2020
07/09/2020	19/09/2020	21/09/2020
07/01/2021	26/01/2021	28/01/2021