GENERAL AND INORGANIC CHEMISTRY AND ELEMENTS OF ORGANIC CHEMISTRY

Academic Year 2025/2026 - Teacher: GIUSEPPE MARCELLO LOMBARDO

Expected Learning Outcomes

The course aims to provide the fundamentals of General and Inorganic Chemistry as an essential cultural foundation for understanding the physical, analytical, and organic chemistry courses, for which it is a prerequisite. Through the study of chemistry, students will not only gain an understanding of the fundamental role this discipline plays in various scientific and technological fields, but will also familiarize themselves with the fundamental principles underlying the scientific method. The General Chemistry course will provide students with initial examples of chemical reactivity, particularly with processes in the gaseous phase and in aqueous solution. The concept of chemical equilibrium applied to chemical reactions in aqueous solution, and basic notions of atomic theory and chemical bond theory, with particular emphasis on molecular geometry

Course Structure

Classroom lessons and exercises

Required Prerequisites

Basic knowledge of arithmetic and algebra, such as operations with rational and real numbers, and solving first- and second-degree equations. Basic physics.

Attendance of Lessons

Attendance is required

Detailed Course Content

• The composition of matter: molecules and molecular compounds, ions and chemical compounds, chemical nomenclature, constitution of the atom, atomic weight and molecular weight, periodic table of elements, groups and periods, periodic properties of the elements, diagonal relationships.

• Fundamental laws of chemistry: Dalton's atomic theory, Avogadro's principle, combination laws, discovery of electrons, protons and neutrons.

• Chemical reactions: the concept of mole, chemical equations, balancing simple reactions, definition of oxidant and reducing agent, oxidation number and redox reactions, definition of acid and base, acid-base reactions, quantitative meaning of chemical reactions, at equilibrium and irreversible.

• Structure of the atom: Electromagnetic radiation, hints of quantum mechanics: Planck, photoelectric effect, atomic spectra, Bohr, de Broglie, Heisenberg model, Schrödinger equation, monoelectronic atoms, polyelectronic atoms: spin and quantum number of spin, orbital energies of polyelectronic atoms, Pauli, Aufbau's exclusion principle and Hund's rule.

• The chemical bond: covalent bond according to Lewis, Molecular geometry and VSEPR theory, Valence bond theory, Molecular geometry and hybridization, Multiple bonds, Outline of molecular orbital theory, electronic configuration of homopolar diatomic molecules of the second period, non- covalent, ionic bond, hydrogen bond, metal bond.

• The gaseous state: laws of gases, equation of state for ideal gases, molar volume, density of gases, diffusion law of gases, real gases, van der Waals equation for real gases, molecular meaning of pressure and temperature, hints of kinetic theory of gases.

• State transitions: Gas-Vapor-Liquid, critical pressure and temperature, state diagrams, equilibria between phases.

• Notes on the solid state: metallic and ionic solids, molecular solids and covalent lattice solids, lattice energy, Born-Haber cycle.

• The liquid state and solutions: role of non-covalent interactions, vapor pressure of liquids and boiling temperature, solvation of solutes, concentration of solutions, Raoult's law, deviations from Raoult's law, notes on the distillation of liquids, properties colligative, cryoscopy and ebullioscopy, osmotic pressure, strong and weak electrolytes, degree of dissociation, solubility of gases in liquids.

• Kinetics and chemical equilibrium: equilibrium reactions, speed of a chemical reaction, order of a reaction, activation energy and Arrhenius equation, kinetic deduction of the chemical equilibrium, equilibrium constant, influence of concentration, pressure and temperature on chemical equilibria, catalysis, homogeneous and heterogeneous catalysts.

• Hints of thermodynamics and thermochemistry: definitions and system-environment relations, state functions, I principle of Thermodynamics, molar thermal capacities, measurement of heat, Hess's law and reaction enthalpies, II principle of Thermodynamics, III principle of Thermodynamics and entropies of reaction, free energy, relationship between free energy and the equilibrium constant.

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

8. R. Chang - FONDAMENTI DI CHIMICA GENERALE - Mc Graw Hill

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)

Stechiometria

12. P. M. Lausarot, G.A. Vaglio - STECHIOMETRIA PER LA CHIMICA GENERALE- Piccin

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

Please note: Although lessons are based on one or two texts for each section, all the texts listed above are equally valid, and students are free to choose the one they feel is best suited to their learning. Any texts not listed may be reviewed by the instructor.

Course Planning

	Subjects	Text References
1	Course Presentation. - Scientific Notation of Numbers. - Units of Measurement and the International System. - Properties and Classification of Matter. - Laws of Chemical Combination. - Chemical Equations	Text 1: Chapter 1
2	Dalton's Atomic Theory. - Avogadro's Principle. - Cannizzaro's Rule. - Constitution of Atoms. - Notes on Electromagnetic Radiation. - Rutherford's Atomic Model.	Text 1: Chapters 1 and 2
3	Introduction to the periodic table. - Bohr's model of the hydrogen atom*. - Overview of quantum mechanics and the Schrödinger equation. - Exercises	Text 1: Chapter 2
4	Electronic structure of the elements. - Periodic properties: - atomic radii; - ionization potential; - electron affinity	Text 1: Chapter 2
5	Octet Rule. - Lewis Symbols. - Metallic Bonds and Ionic Bonds. - Covalent Bonds: Homeopolar, Heteropolar, and Dative. - Exercises	Text 1: Chapter 3
6	Exceptions to the octet rule; - Energy in the covalent bond; - Polar covalent bond; - Electronegativity	Text 1: Chapter 3
7	VSEPR molecular geometry; - Introduction to valence bonding (VB). - Description of N2, H2O; CH4, C2H2, and C2H4 with VB theory; Limitations of VB theory; - Molecular Orbital Theory (MO).	Text 1: Chapter 3
8	Correlation diagrams for homonuclear diatomic molecules. - Dipole-dipole and induced dipole bonds. - Hydrogen bonds. - Oxidation number (OR), - Calculating the OR from the structural formula.	Text 1: Chapter 3
9	Rules for determining the ion number of various compounds. - Nomenclature of binary compounds (IUPAC and non-IUPAC). - Nomenclature of ternary compounds - hydroxides and acids. Nomenclature of salts and ions. Chemical Systematics	Text 1: Chapter 4
10	Structural formulas of various inorganic compounds. - Chemical reactions without change in r.u. - Acid-base; Acid-oxide; Base-oxide; - Salt-salt - Chemical reactions with change in r.u. (redox). - Balancing redox reactions: - Direct method	Text 1: Chapter 4
11	Balancing redox reactions: Half-reaction method in an acidic environment; Half-reaction method in a basic environment; Exercises	Text 1: Chapter 4
12	States of Matter - Solid State: Amorphous and Crystalline Forms and Properties. - Crystal Lattices and Elementary Cells. - Gaseous State: Properties; - Equation of State for Ideal Gases*. - Gaseous Mixtures	Text 1: Chapters 5, 6 and 7.
13	Real gases; van der Waals equation; Application of the ideal gas law; Liquid state: Properties, evaporation, and vapor pressure. Boiling, sublimation, melting, and solidification. Phase diagrams* of H2O and CO2	Text 1: Chapters 5, 6 and 7.
14	Solutions - Nature, enthalpy of solution. - Definitions of concentrations*: mole fraction, molarity, molality, and normality.	Text 1: Chapter 8
15	Vapor pressure of solutions: - ideally behaved solutions - Raoult's law. - Colligative properties: - Vapor pressure decrease; - Bulloscopic rise; - Cryoscopic depression; - Osmotic pressure. - Anomalies	Text 1: Chapter 8
16	Thermodynamics: State variables, state functions, spontaneous and reversible processes, principles of thermodynamics. - Hess's law - Gibbs free energy	Text 1: Chapter 9
17	Introduction to Chemical Kinetics. - Reaction Rate: Influence of Reactant Concentration; First- and Second-Order Reactions.	Text 1: Chapter 14
18	Chemical Equilibrium: Homogeneous and Heterogeneous. - Equilibrium Constant. - Principle of Mobile Equilibrium. - Dependence of the Equilibrium Constant on Temperature. - Solubility Equilibria of Sparsely Soluble Salts.	Text 1: Chapter 10 and Text 3 Chapter 15
19	Autoprotolysis of water. - Hydrogen ion concentration - Acidity and basicity of solutions. - Definition of Arrhenius acid and base. - Exercises.	Text 1: Chapter 12
20	Solubility equilibria of sparingly soluble salts. - Bronsted-Lowry definitions of acid and base. - Strength of acids and bases. - Polyprotic acids and bases.	Text 1: Chapter 12
21	Strength-structure correlation of acids and bases. - Lewis acids and bases. - Salt hydrolysis. - Exercises	Text 1: Chapter 12
22	Amphoteric Compounds. - Buffer Solutions: Definition and mechanisms of action. Constitution, limits, and capacities. Examples.	Text 1: Chapter 12

Learning Assessment

Learning Assessment Procedures

The final exam consists of a written exam (the day of the exam is the one indicated on the official calendar), based on exercises similar to those faced in the classroom during the course, and in an oral interview (date and place will be indicated by the teacher) based on on all topics of the program and on laboratory experiences.

The exam tends to ascertain the level of overall knowledge acquired by the candidate, his ability to critically address the topics studied and to relate the various parts of the program. The exam consists of a written test and an oral exam.

The written exam consists in solving simple stoichiometry problems related to nomenclature, chemical reactions, gas transformations and the study of chemical phenomena in aqueous solution, thermochemistry. This test tends to verify the possession of the basic notions of the discipline. The written test will be considered passed if the student has solved exactly more than half of the assigned exercises. During the written exam, students will be able to use the periodic table and calculator, but not cell phones.

Passing the written exam is a necessary but not sufficient condition to pass the final exam.

The oral exam will consist of questions relating to the various parts of the program to ascertain the overall level of knowledge acquired by the candidate.

Criteria for awarding the final grade:

The mastery shown in the qualitative and quantitative arguments, the critical vision of the topics addressed during the course and the ability to correlate the various parts of the program will contribute in equal measure to the formulation of the final grade.

Examples of frequently asked questions and / or exercises

The course will address a variety of problems that will be covered in the written exam. Exercises and exam assignments (previous years) will be published on Studium. All course topics are eligible for exam questions (e.g., nomenclature, Lewis structures of molecules and VSEPR molecular geometry, hybridization of the central atom and energy diagrams, stoichiometric calculations, colligative properties, chemical equilibria, acid-base reactivity, balancing redox reactions, the periodic table, electronic configurations of the elements, chemical bonding, hybrid orbitals, thermodynamics and kinetics).

VERSIONE IN ITALIANO

Degree Course in

Geological Sciences