CHIMICA A - C

The Chemistry course aims to provide Industrial Engineering students with the fundamental skills to understand how the microscopic structure of matter determines its macroscopic properties and technological behavior. The course is not conceived as a purely theoretical discipline, but rather as an essential practical tool for addressing real-world challenges in design, material selection, and energy management.

The curriculum consistently combines theory with numerical exercises, aiming to enable students to independently quantify chemical and energy transformations. Exam topics are selected based on their direct relevance to the work of an industrial engineer: thermodynamics for studying reactions and phase changes; solid-state chemistry for understanding the structural properties of materials; and electrochemistry for analyzing wet corrosion phenomena and the operation of energy storage systems.

By the end of the course, students will have acquired the methodological rigor and scientific terminology needed to interact with specialists in other fields and to approach the subsequent technological and applied courses in their study plan with the necessary preparation.

In accordance with the Degree Programme's Academic Regulations.

Nature of matter. Matter and states of aggregation. Homogeneous and heterogeneous systems. Phases and their separation. Chemical elements and compounds. Atoms and molecules. Laws of mass (Lavoisier, Proust, Dalton). Volumetric laws (Gay-Lussac, Avogadro). Determination of atomic weight (Cannizzaro's rule) and molecular weight (gas densities). Avogadro's number. The mole.

Structure of matter. Description of the atom. Protons, neutrons, and electrons. Atomic number and mass number. Atomic mass unit. Isotopes. Mass defect. Thomson's experiment. Thomson's atomic model. Millikan's experiment. Rutherford's experiment. Rutherford's atomic model. Electromagnetic radiation. Black-body emission spectrum. Photoelectric effect. Hydrogen atom emission spectrum. Bohr's theory. De Broglie relation. Heisenberg uncertainty principle. Wave mechanics. Schrödinger equation. Quantum numbers and energy levels. Orbitals. Polyelectronic atoms. Pauli exclusion principle. Hund's rule. Aufbau principle. Periodic table. Periodic properties (ionization energy, electron affinity, atomic radius, electronegativity, metallic character).

Chemical bond. Electron sharing. Covalent bond. Octet rule. Bond distance and bond energy. Homopolar and heteropolar bonds. Dative bond. Dipoles. Sigma and pi bonds. Hybridization. Bond angles. VSEPR. Molecular geometry. Resonance. Ionic bond. MO-LCAO theory. Molecular orbitals of second-period diatomic molecules. Metallic bond. Weak bonds. Hydrogen bond.

Chemical compounds and nomenclature. Valence and oxidation number. Oxidation and reduction. Hydrides. Binary acids (hydracids). Oxides. Peroxides. Hydroxides. Oxyacids. Salts. Chemical equations. Reactions. Redox reactions. Disproportionation reactions. Combustion reactions. Mass relationships. Limiting reactant rule. Calculation examples. Types of formulas (empirical, molecular, structural, and stereochemical). Elemental analysis. Calculation examples.

Thermodynamics. Thermodynamic system. Types of systems. Extensive and intensive variables. State functions. Work. Heat. Energy. Heat capacity. Work. First law of thermodynamics. Internal energy and enthalpy. Thermochemistry. Hess's law. Second law of thermodynamics. Conversion of heat into work. Entropy. Free energy. Spontaneity of chemical reactions. Third law of thermodynamics.

States of matter. The gaseous state. Ideal and perfect gases. Boyle's law. Gay-Lussac's law. Charles's law. Avogadro's law. Ideal gas equations of state. Determination of gas molecular weight. Gaseous diffusion. Partial pressures. Molar heat capacities of gases. Maxwell-Boltzmann velocity distribution. Real gases. Van der Waals equation. Gas liquefaction. Andrews diagram. Numerical exercises. The liquid state. Surface tension. Vapor pressure. Clausius-Clapeyron equation. The solid state. Crystalline and amorphous solids. Isotropy and anisotropy. Primitive cells. Bravais lattices. X-ray diffraction and Bragg's equation. Polymorphism. Ionic solids. Covalent solids. Molecular solids. Metallic solids.

Phase changes and heterogeneous equilibria. Phase changes: melting, evaporation, sublimation. Clausius-Clapeyron equation. Variance. Phase rule. Phase diagrams. One-component systems: water, sulfur, carbon dioxide. Systems with a eutectic point.

State of solution. Types of solutions. Solubility of a species. Concentration and methods of expressing it. Solute-solvent interactions: ideal and real solutions. Raoult's law. Relationships between the composition of a binary liquid mixture and its vapor. Systems exhibiting maximum- and minimum-boiling azeotropes. Dilute solutions of non-volatile solutes. Colligative properties. Vapor pressure lowering. Freezing-point depression. Boiling-point elevation. Osmotic pressure. Numerical exercises.

Electrolytic solutions. Electrolytic dissociation. Strong and weak electrolytes. Degree of dissociation. van't Hoff factor. Conductance. Equivalent conductance. Law of independent ion migration. Acids and bases. Arrhenius, Brønsted-Lowry, and Lewis theories. Strength of acids and bases. Ion product of water. Relationship between Ka and Kb. Definition of pH. pH calculation for acid, base, and salt solutions. Buffer solutions. pH indicators. Acid-base titrations. Ampholytes. Solubility equilibria. Solubility product. Common ion.

Elettrochimica. Reazioni di ossido-riduzione: metodo ionico elettronico. Potenziali elettrodici. Equazione di Nernst. Potenziale standard e sua misura. Pile galvaniche. Pile a concentrazione. Serie elettrochimica degli elementi. Pile chimiche. Previsioni di reazioni redox. Costante di equilibrio. Determinazione del pH, KPS e grado di dissociazione. Energia libera di reazione. Esercitazioni numeriche.

Electrochemistry. Redox reactions: ion-electron method. Electrode potentials. Nernst equation. Standard potential and its measurement. Galvanic cells. Concentration cells. Electrochemical series of elements. Chemical cells. Predicting redox reactions. Equilibrium constant. Determination of pH, Ksp, and degree of dissociation. Reaction free energy. Numerical exercises.

Electrolysis. Decomposition voltage. Overpotential. Faraday's laws and numerical exercises. Law of electrochemical equivalents. Electrolysis of molten salts. Electrolysis of water. Electrolysis of aqueous solutions. Industrial electrolytic processes. Accumulators. Corrosion. Passivation.

Chemical kinetics. Reaction rate. Rate law. Molecularity. Reaction order: first- and second-order reactions. Arrhenius equation. Effect of temperature. Activation energy. Catalysts. Kinetic derivation of the equilibrium constant. Chain reactions.

CONTRIBUTION OF THE COURSE TO THE 2030 AGENDA FOR SUSTAINABLE DEVELOPMENT GOALS

The course provides the molecular and thermodynamic foundations necessary to understand and manage the ecological transition of industrial processes and products. The integration of theoretical content with sustainability goals focuses on three specific pillars:

SDG 7 — Affordable and Clean Energy

The course covers the fundamentals of chemical thermodynamics, redox reactions, and electrochemistry (chemical power sources, electrolysis), providing the scientific tools to address two key targets:

Target 7.2 (Increase the share of renewable energy): Study of the chemistry of alternative energy carriers, with a particular focus on hydrogen and storage technologies.

Target 7.3 (Double the global rate of improvement in energy efficiency): Understanding the thermal balances of reactions and chemical kinetics to optimize the energy efficiency of industrial and thermal processes.

SDG 9 — Industry, Innovation and Infrastructure

The study of solid-state chemistry and the structure-property relationships of materials (metallic, polymeric, ceramic, and composite) aims to ensure structural safety and durability:

Target 9.4 (Upgrade infrastructure and make industries sustainable): Focus on the physicochemical mechanisms of material degradation, with particular attention to the thermodynamics and kinetics of metal corrosion and related chemical and galvanic protection techniques to extend the lifecycle of industrial plants.

SDG 12 — Responsible Consumption and Production

Principles of Green Chemistry applied to industrial design are introduced, moving beyond the linear production model:

Target 12.4 (Environmentally sound management of chemicals and all wastes): Study of catalytic reactions to minimize toxic by-products and maximize process atom economy.

Target 12.5 (Reduce waste generation through recycling and reuse): Physicochemical analysis of the degradation and recyclability of polymeric materials (plastics) and metallurgical recovery processes, which are fundamental to the transition toward a circular economy.

1. M. Tagliatesta: Chimica Generale e Inorganica; edi-ermes
2. Pimental-Spratley: Chimica Generale-Zanichelli-Bologna

Mid-term assessments are scheduled, which allow students to pass the exam.

The final exam consists of a written test and an oral test.

MID-TERM ASSESSMENTS

Two mid-term assessments (lasting 90 minutes each) are scheduled: one halfway through the course and one at the end. These assessments are written and consist of numerical exercises involving stoichiometric calculations; they may also include theoretical questions. Each question will be assigned a specific score, indicated next to the question itself. A mid-term assessment is considered passed if the score obtained is between 18 and 30 (out of 30); otherwise, the student must retake the entire assessment on one of the dates scheduled in the exam calendar. Passing both mid-term assessments grants exemption from the written exam. Before the assessment begins, the instructor will provide all necessary instructions for completing the exam successfully. Registration for the mid-term assessment is mandatory and must be completed exclusively via the Studium platform (http://studium.unict.it) by the indicated deadline.

END-OF-COURSE EXAMS

The exam consists of a written test followed by an oral test.

Registration for the written test is mandatory for each exam session and must be completed exclusively via the student portal (https://studenti.smartedu.unict.it/) by the indicated deadline. The written test is considered passed if the score obtained is at least 18/30; otherwise, the student must retake the entire test on one of the dates scheduled in the exam calendar. The oral test consists of presenting topics covered in the course syllabus. The final exam grade will be based on both the written and oral tests.

Assessment of learning outcomes may also be conducted online, should conditions require this method. In such cases, the duration of the written test may be subject to change. Assessment will be based on the accuracy and completeness of the content (as outlined in the "course syllabus"), the clarity and logical rigor of the presentation, and the ability to apply principles to practical cases.

To ensure equal opportunities and in compliance with current regulations, students registered with CInAP may arrange compensatory and/or dispensatory measures with the instructor, based on learning objectives and specific needs. Students may also contact the designated CInAP (Center for Active and Participatory Integration – Services for Disabilities and/or Specific Learning Disorders) representatives for the DIEEI department: Professors Antonella Di Stefano and Arturo Pagano (https://www.cinap.unict.it/content/referenti).

Atomic structure. Chemical bonding. Thermodynamics. Chemical reactions. Nomenclature. States of matter. Solutions. Chemical equilibrium. Ionic equilibria in solution. Acids and bases. Electrochemistry. Chemical kinetics.
Examples and models are available on the Studium portal (http://studium.unict.it).