ID:
510656
Duration (hours):
72
CFU:
9
SSD:
CHIMICA GENERALE E INORGANICA
Year:
2025
Overview
Date/time interval
Primo Semestre (29/09/2025 - 23/01/2026)
Syllabus
Course Objectives
The course aims to provide the fundamental principles of Chemistry which constitute the essential cultural background for understanding the teachings for which General Chemistry is preparatory, introducing the language and methodology of Chemical Sciences.
The topics of Inorganic Chemistry are contextualized with those of General Chemistry with the aim of making students confident with both the deductive and inductive methods.
The course will also provide the student with the main calculation methods to solve stoichiometry problems.
At the end of the course, the expected learning outcomes are:
- knowing, understanding and explaining with an appropriate language theoretical principles and basic concepts;
- understanding and applying the basic concepts (mole, pH, equilibrium in solution, etc.);
- comprehending the basic structure of atoms and molecules;
- knowing how to assign names to molecules and correctly write chemical formulas starting from the chemical name;
- knowing how to draw the structural formulas of molecules;
- writing correctly chemical reactions and understanding their thermodynamics and kinetics bases;
- knowing the chemistry of the elements and their main compounds, interpreting and foreseeing their behavior applying the fundamental principles;
- understanding and solving stoichiometry problems.
The topics of Inorganic Chemistry are contextualized with those of General Chemistry with the aim of making students confident with both the deductive and inductive methods.
The course will also provide the student with the main calculation methods to solve stoichiometry problems.
At the end of the course, the expected learning outcomes are:
- knowing, understanding and explaining with an appropriate language theoretical principles and basic concepts;
- understanding and applying the basic concepts (mole, pH, equilibrium in solution, etc.);
- comprehending the basic structure of atoms and molecules;
- knowing how to assign names to molecules and correctly write chemical formulas starting from the chemical name;
- knowing how to draw the structural formulas of molecules;
- writing correctly chemical reactions and understanding their thermodynamics and kinetics bases;
- knowing the chemistry of the elements and their main compounds, interpreting and foreseeing their behavior applying the fundamental principles;
- understanding and solving stoichiometry problems.
Course Prerequisites
To follow the course profitably, basic knowledge of both mathematics (e.g. solving linear systems and quadratic equations, knowing and being able to apply the properties of powers and logarithms, knowing the concepts of function, derivative and integral, knowing plane and solid geometry) and physics (classical mechanics and electromagnetism) provided by secondary school are useful.
Teaching Methods
Traditional through frontal lessons at the blackboard.
Stoichiometry based exercises will be part of the course.
Students will also be supported by tutors both in classroom and through Kiro platform.
For students with specific needs, who cannot attend in person the teaching activities and who have applied for Inclusive Teaching Methods, adequate teaching material will be available for a profitable independent study. If requested, self-learning can be supported by tutoring or supplementary teaching activities, and by dedicated meetings, also online, with flexible hours depending on the needs.
Stoichiometry based exercises will be part of the course.
Students will also be supported by tutors both in classroom and through Kiro platform.
For students with specific needs, who cannot attend in person the teaching activities and who have applied for Inclusive Teaching Methods, adequate teaching material will be available for a profitable independent study. If requested, self-learning can be supported by tutoring or supplementary teaching activities, and by dedicated meetings, also online, with flexible hours depending on the needs.
Assessment Methods
The final examination consists in a two-hour written test containing five exercises of stoichiometry and general chemistry, and a subsequent oral test in order to verify the degree of learning of the theoretical principles and the inorganic chemistry part. The marks average of the two tests, if both positive, leads to the final evaluation.
For first-year students there are also three in-itinere tests, which - if all passed with marks greater than or equal to 18 - replace the written part of the exam for the first exam session.
Appropriate examination methods are provided for students who fall into the categories of Specific Learning Disorders (SLD) and Special Educational Needs (SEN).
For first-year students there are also three in-itinere tests, which - if all passed with marks greater than or equal to 18 - replace the written part of the exam for the first exam session.
Appropriate examination methods are provided for students who fall into the categories of Specific Learning Disorders (SLD) and Special Educational Needs (SEN).
Texts
Lecture notes, detailed program provided by the teacher on Kiro platform, exercises carried out in class.
Any textbook of General Chemistry at a specialist university level can be useful, while a workbook containing numerous examples for the stoichiometry part is strongly recommended.
Here are some suggestions:
- P. Atkins. L. Jones, L. Laverman, Principi di chimica, Zanichelli.
eBook available @Zanichelli/CEA LockLizard.
- T. L. Brown, H. E. LeMay, B. E. Bursten, [et.al.], Fondamenti di Chimica, EDiSES.
- K. Whitten, R. Davis, M. L. Peck, G. Stanley, Chimica, Piccin.
- J. C. Kotz, P. M. Treichel, J. R. Townsend, D. A. Treichel, Chimica, EDiSES.
- I. Bertini, C. Luchinat, F. Mani, E. Ravera, Stechiometria un avvio allo studio della chimica, Casa Editrice Ambrosiana.
eBook available @Zanichelli/CEA LockLizard.
- A. Caselli, S. Rizzato, F. Tessore, Stechiometria, EDiSES.
Any textbook of General Chemistry at a specialist university level can be useful, while a workbook containing numerous examples for the stoichiometry part is strongly recommended.
Here are some suggestions:
- P. Atkins. L. Jones, L. Laverman, Principi di chimica, Zanichelli.
eBook available @Zanichelli/CEA LockLizard.
- T. L. Brown, H. E. LeMay, B. E. Bursten, [et.al.], Fondamenti di Chimica, EDiSES.
- K. Whitten, R. Davis, M. L. Peck, G. Stanley, Chimica, Piccin.
- J. C. Kotz, P. M. Treichel, J. R. Townsend, D. A. Treichel, Chimica, EDiSES.
- I. Bertini, C. Luchinat, F. Mani, E. Ravera, Stechiometria un avvio allo studio della chimica, Casa Editrice Ambrosiana.
eBook available @Zanichelli/CEA LockLizard.
- A. Caselli, S. Rizzato, F. Tessore, Stechiometria, EDiSES.
Contents
The course program is divided into three parts.
I) Structure and properties of matter:
Physical quantities and units.
Atoms and atomic structure, atomic number, mass number and isotopes; atomic mass unit, Avogadro's number and the concept of mole, stoichiometry; classification of elements and compounds, chemical formula, molecules; solutions and concentration measurement, dilution of solutions; chemical reactions and equations, limiting agent, reaction yield; oxidation number; systematic and traditional nomenclature of inorganic compounds; redox reactions and solving methods; atomic models; matter, light and energy; hydrogen atom, atomic spectroscopy, uncertainty principle, quantum mechanics, wave function and Schrödinger equation; atomic orbitals, quantum numbers, electron spin; polyelectronic atoms, Aufbau principle, electronic configuration of the elements, periodic table of the elements, periodic properties; electronegativity and dipole moment.
Interactions between molecules, metallic bond; ionic bond, geometry of ionic compounds and energy aspects; covalent bond, Lewis theory, octet rule, resonance and formal charge; geometry of molecules and VSEPR theory, prediction of the polarity of molecules; valence bond theory, hybridization and hybrid orbitals; molecular orbitals.
States of aggregation; Van der Waals forces, London forces, hydrogen bond, ion-dipole forces; solid state, ionic solids, molecular solids, covalent solids, metals; liquid state, surface tension, viscosity, capillary action, changes of state, critical temperature, water phase diagram; solutions, dissolution, strong electrolytes and non-electrolytes, solubility ionic compounds; gas, gas laws, general equation of state of ideal gases, gas mixtures and partial pressures, Dalton's law; molecular kinetic theory; real gases, Van der Waals equation.
II) The reactions:
Chemical kinetics, reaction rate and concentration, reaction order, Arrhenius equation, catalysis, photochemistry. Chemical equilibrium, equilibrium constant, heterogeneous equilibria, reaction quotient, Le Châtelier's principle.
Acid-base reactions, Arrhenius acids and bases, Brønsted-Lowry theory; strength of acids and bases, acid base dissociation constant, ionic product of water, polyprotic acids, acidity of metal aquo complexes, reactions between acids and bases; measurement of acidity, calculation of pH; acidity and basicity of salts; Lewis acids and bases; buffer solutions; quantitative volumetric methods, chemical equivalent, types of titration; acid-base titrations; acid-base indicators.
Coordination compounds, nomenclature, structure and stereochemistry; crystal field theory, color of metal complexes; metal complexes in solution, thermodynamic and kinetic stability; multidentate ligands, chelate effect, macrocyclic effect.
Solubility of salts and precipitation reactions, dissolution equilibrium, solubility product, common-ion effect, precipitation reactions, solubilization of ionic precipitates, fractional precipitation.
Thermodynamics, enthalpy, spontaneous and non-spontaneous processes, entropy, Gibbs free-energy, variations of free energy for non-standard states.
Electrochemistry, voltaic cell and electrode potentials; disproportionation and comproportionation reactions; cell potential, free-energy and equilibrium constant; cell potential as a function of pH, solubility equilibrium and complex formation constant; concentration batteries, determination of redox active species from the measurement of the potential; batteries as energy generators; corrosion; electrolysis.
III) Inorganic Chemistry:
Hydrogen; elements of the p-block; metals of s- and d-block; notes on lanthanides.
I) Structure and properties of matter:
Physical quantities and units.
Atoms and atomic structure, atomic number, mass number and isotopes; atomic mass unit, Avogadro's number and the concept of mole, stoichiometry; classification of elements and compounds, chemical formula, molecules; solutions and concentration measurement, dilution of solutions; chemical reactions and equations, limiting agent, reaction yield; oxidation number; systematic and traditional nomenclature of inorganic compounds; redox reactions and solving methods; atomic models; matter, light and energy; hydrogen atom, atomic spectroscopy, uncertainty principle, quantum mechanics, wave function and Schrödinger equation; atomic orbitals, quantum numbers, electron spin; polyelectronic atoms, Aufbau principle, electronic configuration of the elements, periodic table of the elements, periodic properties; electronegativity and dipole moment.
Interactions between molecules, metallic bond; ionic bond, geometry of ionic compounds and energy aspects; covalent bond, Lewis theory, octet rule, resonance and formal charge; geometry of molecules and VSEPR theory, prediction of the polarity of molecules; valence bond theory, hybridization and hybrid orbitals; molecular orbitals.
States of aggregation; Van der Waals forces, London forces, hydrogen bond, ion-dipole forces; solid state, ionic solids, molecular solids, covalent solids, metals; liquid state, surface tension, viscosity, capillary action, changes of state, critical temperature, water phase diagram; solutions, dissolution, strong electrolytes and non-electrolytes, solubility ionic compounds; gas, gas laws, general equation of state of ideal gases, gas mixtures and partial pressures, Dalton's law; molecular kinetic theory; real gases, Van der Waals equation.
II) The reactions:
Chemical kinetics, reaction rate and concentration, reaction order, Arrhenius equation, catalysis, photochemistry. Chemical equilibrium, equilibrium constant, heterogeneous equilibria, reaction quotient, Le Châtelier's principle.
Acid-base reactions, Arrhenius acids and bases, Brønsted-Lowry theory; strength of acids and bases, acid base dissociation constant, ionic product of water, polyprotic acids, acidity of metal aquo complexes, reactions between acids and bases; measurement of acidity, calculation of pH; acidity and basicity of salts; Lewis acids and bases; buffer solutions; quantitative volumetric methods, chemical equivalent, types of titration; acid-base titrations; acid-base indicators.
Coordination compounds, nomenclature, structure and stereochemistry; crystal field theory, color of metal complexes; metal complexes in solution, thermodynamic and kinetic stability; multidentate ligands, chelate effect, macrocyclic effect.
Solubility of salts and precipitation reactions, dissolution equilibrium, solubility product, common-ion effect, precipitation reactions, solubilization of ionic precipitates, fractional precipitation.
Thermodynamics, enthalpy, spontaneous and non-spontaneous processes, entropy, Gibbs free-energy, variations of free energy for non-standard states.
Electrochemistry, voltaic cell and electrode potentials; disproportionation and comproportionation reactions; cell potential, free-energy and equilibrium constant; cell potential as a function of pH, solubility equilibrium and complex formation constant; concentration batteries, determination of redox active species from the measurement of the potential; batteries as energy generators; corrosion; electrolysis.
III) Inorganic Chemistry:
Hydrogen; elements of the p-block; metals of s- and d-block; notes on lanthanides.
Course Language
Italian
Degrees
Degrees
MEDICINAL CHEMISTRY AND PHARMACEUTICAL TECHNOLOGY
Single-cycle Master’s Degree
5 years
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