Academic Year 2023/2024 - Teacher: Giuseppe Marcello LOMBARDO

Expected Learning Outcomes

The aim of the course is to provide the student with the general basics of chemistry as well as the understanding of topics related to it and developed in other courses.

Course Structure

Classrom lectures and tutorials.

Should teaching be carried out in mixed mode or remotely, it may be necessary to introduce changes with respect to previous statements, in line with the programme planned and outlined in the syllabus.

Information for students with disabilities and/or DSA

To guarantee equal opportunities and in compliance with current laws, interested students can request a personal interview in order to plan any compensatory and/or dispensatory measures, based on the educational objectives and specific needs.

It is also possible to contact the CInAP (Centre for Active and Participated Inclusion - Services for Disabilities and/or DSA) professor of our Department, prof. Anna De Angelis.

Required Prerequisites

knowledge of basic mathematics, such as operations with rational (real) numbers and solution of 1st and 2nd degree equations.

Attendance of Lessons

NOT Mandatory as required by the teaching regulations

Detailed Course Content

The matter and the periodic system of the elements

Chemical and physical properties of the elements

The chemical bond

Nomenclature and chemical reactions

Oxidation numbers.

Balancing chemical equations

Classification of inorganic compounds

Acid-base, exchange and oxidation-reduction reactions.

States of aggregation.


Chemical equilibrium.


Chemical Kinetics.

Inorganic Chemistry

Textbook Information

1. A. M. Manotti Lanfredi & A. Tiripicchio, FONDAMENTI DI CHIMICA, CEA

2. Fusi et al., -CHIMICA GENERALE ED INORGANICA - Idelson-Gnocchi

3. Petrucci et al., -CHIMICA GENERALE- Piccin

4. Speranza et al. -CHIMICA GENERALE ED INORGANICA- Edi-Ermes

5. M. Schiavello, L. Palmisano - FONDAMENTI DI CHIMICA - EdiSES

6. J.C. Kotz et al. - CHIMICA - EdiSES

7. P.W. Atkins, L. Jones - CHIMICA GENERALE - Zanichelli


9. Nivaldo J. Tro - CHIMICA – EdiSES Chimica Inorganica

10. D.H. Bandinelli - CHIMICA INORGANICA – Piccin

11. I. Bertini,C. Luchinat, F. Mani - CHIMICA INORGANICA - Ambrosiana, (distribuzione Zanichelli)


13. P. Giannoccaro, S. Doronzo -ELEMENTI DI STECHIOMETRIA- Edises

Learning Assesment

Written with multiple choice quizzes.

Learning assessment may also be carried out on line in oral mode, if the conditions require it.

Information for students with disabilities and/or DSA.
As a guarantee of equal opportunities and in compliance with current laws, interested students can ask for a personal interview in order to plan any compensatory and/or dispensatory measures, based on their specific needs and on teaching objectives of the discipline. It is also possible to ask the departmental contacts of CInAP (Center for Active and Participatory Integration - Services for Disabilities and/or DSAs), in the persons of professors Giovanna Tropea Garzia and Anna De Angelis.

Course Planning

 SubjectsText References
1Presentation of the course. - Scientific notation of numbers. - Units of measurement and international system*. - Properties and classification of matter*. - Laws of chemical combination*. - Chemical Equations*Testo 1: Cap. 1
2Dalton's Atomic Theory. - Avogadro's principle. - Cannizzaro rule. - Constitution of atoms. – Notes on electromagnetic radiation. - Rutherford atom model.Testo 1: Caps. 1 e 2
3Introduction to the periodic tables. - Bohr* model of the hydrogen atom. - Quantum mechanics. - Schrodinger equation. - ExercisesTesto 1: Cap. 2
4Electronic structure of the elements. - Periodic properties: - atomic radii; - ionization potential; - electron affinityTesto 1: Cap. 2
5Octet rule. - Lewis symbols. - Metallic bond and ionic bond. - Covalent bond: Homeopolar, heteropolar and dative. - ExercisesTesto 1: Cap. 3
6Exceptions to the octet rule; - Energy in the covalent bond; - Covalent-polar bond; - ElectronegativityTesto 1: Cap. 3
7VSEPR Molecular Geometry; - Introduction to the valence bond (VB). - Description of N2, H2O; CH4, C2H2 and C2H4 with VB theory; Limits of VB theory; - Molecular Orbital Theory (MO).Testo 1: Cap. 3
8Correlation diagrams of homonuclear diatomic molecules. - Dipole-dipole and induced dipole bond. - Hydrogen bond. - Oxidation number (n.o.), - calculation n.o. from the structural formulaTesto 1: Cap. 3
9Rules for determining the no. in various compounds. - Nomenclature of binary compounds (IUPAC and otherwise). –Nomenclature of ternary compounds - hydroxides and acids. Nomenclature of salts and ionsTesto 1: Cap. 4
10Structural formulas of various inorganic compounds. - Chemical reactions without variation of the n.o. - Acidobase; Acid-oxide; Base-oxide; - Salt-salt - Chemical reactions with variation of the n.o. (redox). - Balancing of redox reactions: - Direct methodTesto 1: Cap. 4
11Balancing of redox reactions: Half-reaction method in an acidic environment; - Semi-reaction method in a basic environment; - exercisesTesto 1: Cap. 4
12States of aggregation of matter - Solid State: Amorphous and crystals and properties. - Crystal lattices and unit cells. - Gaseous state: properties; - Equation of state of ideal gases*. - Gaseous mixturesTesto 1: Caps. 5 - 6 - 7
13Real gases; van der Waals equation; Application of the ideal gas law; - Liquid State: Properties, evaporation and vapor pressure. Boiling, - sublimation, fusion and solidification. - State diagrams* of H2O and CO2Testo 1: Caps. 5 - 6 - 7
14Solutions - Nature, enthalpy of solution. -Concentration definitions*: mole fraction, molarity, molality and NormalityTesto 1: Cap. 8
15Vapor pressure of solutions: - solutions with ideal behavior - Raoult's law. - Colligative properties: - Lowering of vapor pressure; Ebulloscopic elevation; - Cryoscopic lowering; - Osmotic pressure. - AnomaliesTesto 1: Cap. 8
16Thermodynamics: State variables, state functions, Spontaneous and reversible processes, Principles of thermodynamics. - Hess' law - Gibbs free energyTesto 1: Cap. 9
17Chemical Equilibrium: Homogeneous and heterogeneous. - Equilibrium constant. - Principle of mobile equilibrium. - Dependence of the equilibrium constant on temperature. - Solubility equilibria of poorly soluble salts.Testo 1: Cap. 10 e Testo 3 Cap. 15
18Autoprotolysis of water. - Hydrogen concentration - Acidity and basicity of the solutions. - Definition of Arrhenius acid and base. - Exercises.Testo 1: Cap. 12
19Solubility equilibria of poorly soluble salts. - Bronsted-Lowry definitions of acid and base. - Strength of Acids and Bases. - Polyprotic acids and basesTesto 1: Cap. 12
20Strength - structure correlation of acids and bases. - Lewis acids and bases. - Saline hydrolysis. - ExercisesTesto 1: Cap. 12
21Amphoteric compounds. - Buffer Solutions: Definition and operating mechanisms. Constitution, limits and capabilities. Examples.Testo 1: Cap. 12
22Heterogeneous Equilibria: One and two component systems: Fractional distillation; Azeotropic mixtureTesto 1: Cap. 11
23Electrochemistry: Faraday's laws, hydrogen electrode, normal reduction potentials, Nerst equation.Testo 1: Cap. 13
24Introduction Chemical Kinetics. -Reaction speed: Influence of the concentration of the reactants; First and second order reactions.Testo 1: Cap. 14

Learning Assessment

Learning Assessment Procedures

Written quiz with multiple suggested answers.

  Voting follows the following scheme:

Below 18:

Knowledge and understanding of the topic: Important deficiencies. Significant inaccuracies

Analysis and synthesis skills: Irrelevant. Frequent generalizations. Inability to synthesize

Use of references: Completely inappropriate


Knowledge and understanding of the topic: At threshold level. Obvious imperfections

Analysis and synthesis skills: Just sufficient skills

Use of references: As appropriate


Knowledge and understanding of the topic: Routine knowledge Analysis and synthesis skills: Able to correctly analyze and summarize. Argue logically and coherently

Using references: Use standard references


Knowledge and understanding of the topic: Good knowledge

Analysis and synthesis skills: Has good analysis and synthesis skills. The arguments are expressed coherently

Using references: Use standard references


Knowledge and understanding of the topic: More than good knowledge

Analysis and synthesis skills: Has considerable analysis and synthesis skills

Use of references: He explored the topics in depth


Knowledge and understanding of the topic: Excellent knowledge

Analysis and synthesis skills: Has considerable analysis and synthesis skills.

Using references: Important insights.

Examples of frequently asked questions and / or exercises

For the reactionSO3 (g) = SO2 (g) + ½O2 (g), 1.00 mole of sulfur trioxide is reacted in a volume of 2.00 litres. At equilibrium, 0.100 moles of oxygen are measured. determine the equilibrium constant Kc.

Simple and structural formula of calcium carbonate;

  Calculate the osmotic pressure of an aqueous solution of KCl obtained by dissolving 2.50 g of this salt in 250.0 ml of water at 25 °C, assuming that the change in volume is negligible. (R=0.0821 atm·l·K-1·mol-1).

Determine the pH of a buffer solution consisting of 0.1 M acetic acid and 0.05 M sodium acetate.