ID:
500172
Duration (hours):
56
CFU:
7
SSD:
CHIMICA GENERALE E INORGANICA
Year:
2025
Overview
Date/time interval
Primo Semestre (29/09/2025 - 23/01/2026)
Syllabus
Course Objectives
Learning the constitutive concepts of General Chemistry necessary to full understanding the chemistry courses that will
be attended in the next semesters and deeper learining of the chemistry of the elements and of the inorganic
compounds. Nomenclature, reactivity, properties of substances are illustrated in the frame of periodic properties of
elements, with the aim of assuring a clear and systematic learining, that allow the student to independently deduce and
elaborated concepts.The accurate teaching of stoichiometry (how to calculate concentrations, weight relations in
reactions, pH calculation, colligative properties) is intended to make the student capable of solving the daily problems of
a chemistry laboratory.
be attended in the next semesters and deeper learining of the chemistry of the elements and of the inorganic
compounds. Nomenclature, reactivity, properties of substances are illustrated in the frame of periodic properties of
elements, with the aim of assuring a clear and systematic learining, that allow the student to independently deduce and
elaborated concepts.The accurate teaching of stoichiometry (how to calculate concentrations, weight relations in
reactions, pH calculation, colligative properties) is intended to make the student capable of solving the daily problems of
a chemistry laboratory.
Course Prerequisites
The student is requestd to have introductory and basic knowldege of general chemistry, mathematics and phisics which are usaually given during secondary school
Teaching Methods
The course is based on powerpoint presentation of lessons, with problems and exercizes which will be solved in the class. No practical (laboratory) experiences.
Assessment Methods
Two intermediate written examinations containing: i) open questions on theory ii) questions regarding stoichiometry calculations.
Final examination:
Average positive result (18/30 or higher) on the 2 intermediate examinations. In the case of an average negative result: written examination in occasion of regular examination sessions, with stoichiometry problems and open questions on theory
Final examination:
Average positive result (18/30 or higher) on the 2 intermediate examinations. In the case of an average negative result: written examination in occasion of regular examination sessions, with stoichiometry problems and open questions on theory
Texts
One among: 1) Whitten Davis Peck Stanley – Chimica (Piccin); 2)Kotz Treichel Townsend – Chimica (EdiSES): 3) Peter
Atkins, Loretta Jones, Chimica Generale (Zanichelli); 4) Bertani, Clemente, Depaoli e altri , Chimica Generale e
Inorganica, 2° edizione (Casa Editrice Ambrosiana)
Moreover, for stoichiometry, one among: 1) Bertini, C. Luchinat, F. Mani, Stechiometria – un avvio
allo studio della chimica (Casa Editrice Ambrosiana); 2) Michelin Lausarot, Vaglio – Stechiometria per la Chimica
Generale (Piccin); 3) Giannocaro Doronzo – Elementi di Stechiometria (EdiSES).
Atkins, Loretta Jones, Chimica Generale (Zanichelli); 4) Bertani, Clemente, Depaoli e altri , Chimica Generale e
Inorganica, 2° edizione (Casa Editrice Ambrosiana)
Moreover, for stoichiometry, one among: 1) Bertini, C. Luchinat, F. Mani, Stechiometria – un avvio
allo studio della chimica (Casa Editrice Ambrosiana); 2) Michelin Lausarot, Vaglio – Stechiometria per la Chimica
Generale (Piccin); 3) Giannocaro Doronzo – Elementi di Stechiometria (EdiSES).
Contents
Fundaments: matter and substances, physical and chemical properties, elements, atoms, compounds, molecules,
mixtures. Measurements and their units. Derivative units, significant figures, errors. Elements, atoms: atoms masses,
isotopes.
Mole, molar mass. Molecular and ionic compounds. Molecular weight and formula weight. Nomencalture of inorganic
compounds. Chemical reactions: precipitation (strong and weak electrolytes) and acid-base. Balancing. Concept and
calculation of oxidation state. Redox reactions and their balancement. Calculating the mass relations in reactions.
Limiting reagent, reactions yields.
The atomic structure and the periodic table: H atom, ondulatory model, quantum numbers.
Aufbau. Periodic table and periodic properties: ionization energy, electronic affinity, electronegativity. Reactivity and
periodic table: properties of s, p, d-block elements. Noble gases. Ionic bonding. The Born-Haber cycle and the stability of
ionic compounds. Covalent bonding: molecules, Lewis structures for biatomic and polyatomic molecules, resonance.
Bond strength, bond length, dipolar moments. The shape of the molecules and their polarity. VSEPR theory. The
valence bond and molecular orbital model, hybridizaton, σ and π bonds.
The aggregation states of the matter: ideal gas and ideal gas law. Ideal gas mixtures and partial parameters.
Calculations on gas connected to P, T, V and mol variations. Real gas, Van der Waals equation of state for them. Solids
and liquids: the forces that allow substances to aggregate. Solutions: concentration, vapour pressure, colligative
properties.
The chemical equilibrium: the equilibrium constant and the LeChatelier principle. Caids, bases, Bronsted/Lowry theory.
Introduction to Lewis theory. pH and pOH. Calculation of pH of strong and weak acidsa and bases. Buffer solutions. A
concise introduction to electrochemistry The standard reduction potential
mixtures. Measurements and their units. Derivative units, significant figures, errors. Elements, atoms: atoms masses,
isotopes.
Mole, molar mass. Molecular and ionic compounds. Molecular weight and formula weight. Nomencalture of inorganic
compounds. Chemical reactions: precipitation (strong and weak electrolytes) and acid-base. Balancing. Concept and
calculation of oxidation state. Redox reactions and their balancement. Calculating the mass relations in reactions.
Limiting reagent, reactions yields.
The atomic structure and the periodic table: H atom, ondulatory model, quantum numbers.
Aufbau. Periodic table and periodic properties: ionization energy, electronic affinity, electronegativity. Reactivity and
periodic table: properties of s, p, d-block elements. Noble gases. Ionic bonding. The Born-Haber cycle and the stability of
ionic compounds. Covalent bonding: molecules, Lewis structures for biatomic and polyatomic molecules, resonance.
Bond strength, bond length, dipolar moments. The shape of the molecules and their polarity. VSEPR theory. The
valence bond and molecular orbital model, hybridizaton, σ and π bonds.
The aggregation states of the matter: ideal gas and ideal gas law. Ideal gas mixtures and partial parameters.
Calculations on gas connected to P, T, V and mol variations. Real gas, Van der Waals equation of state for them. Solids
and liquids: the forces that allow substances to aggregate. Solutions: concentration, vapour pressure, colligative
properties.
The chemical equilibrium: the equilibrium constant and the LeChatelier principle. Caids, bases, Bronsted/Lowry theory.
Introduction to Lewis theory. pH and pOH. Calculation of pH of strong and weak acidsa and bases. Buffer solutions. A
concise introduction to electrochemistry The standard reduction potential
Course Language
Italian
Degrees
Degrees
PHARMACY
Single-cycle Master’s Degree
5 years
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People
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