CHIMICA D - L

Expected learning outcomes

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 behaviour. The Chemistry course is not intended as a purely theoretical discipline, but as an essential practical tool for tackling real-world problems in design, materials selection and energy management.

The teaching programme consistently combines theory with numerical exercises, with the aim of enabling students to independently quantify chemical and energy transformations. The examination topics are selected on the basis of their direct relevance to the work of an industrial engineer: thermodynamics for the study of reactions and phase transitions, solid-state chemistry for understanding the structural properties of materials, and electrochemistry for the analysis of wet corrosion phenomena and the operation of energy storage systems.

By the end of the course, students will have acquired the methodological rigour and scientific language necessary to interact with specialists from other fields and to approach the subsequent technological and applied modules of the curriculum with the appropriate preparation.

Dublin Descriptors

Knowledge and understanding

The subjects in this area aim to equip graduates in Industrial Engineering with the ability to understand and solve problems of a chemical and chemical-physical nature. By the end of the programme, students must demonstrate that they have acquired the fundamental theoretical knowledge of chemistry and understand its role within the context of engineering. In particular:

Solid-state and materials chemistry: Understanding of chemical bonds (ionic, covalent, metallic, intermolecular) and their influence on the macroscopic properties (mechanical, electrical, thermal) of materials of engineering interest (metals, ceramics, polymers).

Chemistry of solutions: Understanding of the laws governing the behaviour of solutions in terms of solute-solvent interactions and their influence on macroscopic properties, with particular emphasis on electrochemistry.

Crystal structure and defects: Knowledge of the main crystal lattices, lattice defects and how these influence the plasticity and reactivity of metals.

Chemical thermodynamics and equilibria: A quantitative understanding of the principles of thermodynamics, the criteria for the spontaneity of reactions (DH, DS, DG), chemical equilibria (homogeneous and heterogeneous) and single- and multi-component phase diagrams.

Industrial Kinetics and Electrochemistry: An in-depth understanding of the factors influencing reaction rates (transition state theory, catalysis) and the laws governing electrochemical processes (galvanic cells, electrolysis, Faraday’s laws).

Applying knowledge and understanding

Graduates in Industrial Engineering should be able to:

understand and analyse engineering problems using appropriate terminology and formulations from a mathematical, chemical and physico-chemical perspective; share and apply their knowledge within multidisciplinary working groups.

The ability to apply knowledge and understanding will be acquired through the completion of exercises, including those of a multidisciplinary nature, relating to the topics covered during the courses, supplemented by individual and group study.

The assessment of the knowledge acquired and the resulting evaluation will be based primarily on written examinations and oral interviews.

Students will be able to use the mathematical and conceptual tools of chemistry to solve complex problems in the field of industrial engineering:

Stoichiometry: Ability to perform quantitative calculations on gas-phase reactions, equilibria in aqueous solution (acid-base reactions, buffer solutions, solubility equilibria) and yield calculations.

Analysis of phase diagrams: Ability to interpret phase diagrams (including simple binary systems and basic chemical aspects) and to apply Gibbs’ phase rule and the lever rule.

Corrosion prevention and control: Ability to calculate the electromotive force of cells (Nernst equation) and apply this knowledge to assess the risks of wet corrosion and define protection methods (cathodic protection, anodic protection, coatings).

Compulsory attendance for at least 70 per cent of teaching hours.

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

2. *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. Emission spectrum of the hydrogen atom. Bohr’s theory. De Broglie’s relation. Heisenberg’s uncertainty principle. Wave mechanics. Schrödinger’s equation. Quantum numbers and energy levels. Orbitals. Multi-electron atoms. Pauli exclusion principle. Hund’s rule. Aufbau principle. Periodic table. Periodic properties (ionisation energy, electron affinity, atomic, electronegativity, metallic character).

3. *Chemical bonding. Electron sharing. Covalent bonding. The octet rule. Bond length and bond energy. Homopolar and heteropolar bonding. Dative bonding. Dipoles. s- and p-bonds. Hybridisation. Bond angles. VSEPR. Molecular geometry. Resonance. Ionic bond. MO-LCAO theory. Molecular orbitals of diatomic molecules in the second period. Metallic bond. Weak bonds. Hydrogen bond.

4. *Chemical compounds and nomenclature. Valence and oxidation number. Oxidation and reduction. Hydrides. Hydracids. Oxides. Peroxides. Hydroxides. Oxoacids. Salts. Chemical equation. Reactions. Oxidation-reduction reactions. Dismutation reactions. Combustion reactions. Stoichiometric relationships. Rule of the limiting reactant. Calculation examples. Types of formulae (minimal, empirical, structural and steric). Elemental analysis. Calculation examples.

5. *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.

6. *States of matter. The gaseous state. Ideal gases and perfect gases. Boyle’s law. Gay-Lussac’s law. Charles’s law. Avogadro’s law. Equations of state for ideal gases. Determination of the molecular weight of a gas. Gas diffusion. Partial pressures. Molar heats of gases. Maxwell–Boltzmann velocity distribution. Real gases. Van der Waals equation. Liquefaction of gases. Andrews diagram. Numerical exercises. The liquid state. Surface tension. Vapour pressure. Clausius–Clapeyron equation. The solid state. Crystalline and amorphous solids. Isotropy and anisotropy. Unit cells. Bravais lattices. X-ray diffraction and Bragg’s law. Polymorphism. Ionic solids. Covalent solids. Molecular solids. Metallic solids.

7. *Phase transitions and heterogeneous equilibria. Phase transitions: melting, evaporation, sublimation. The Clausius–Clapeyron equation. Variance. The phase rule. Phase diagrams. Single-component systems: water, sulphur, carbon dioxide. Systems with a eutectic point.

8. *State of solution. Types of solution. Solubility of a species. Concentration and how it is expressed. Solute-solvent interaction: ideal and real solutions. Raoult’s law. Relationships between the composition of a mixture of two liquids and that of its vapour. Systems with maximum and minimum azeotropes. Dilute solutions of non-volatile solutes. Colligative properties. Vapour pressure lowering. Cryoscopic depression. Ebullioscopic elevation. Osmotic pressure. Numerical exercises.

9. *Chemical equilibria. The law of chemical equilibrium. Le Chatelier’s principle. Relationship between free energy and the equilibrium constant. Equilibrium constants (Kp and Kc). Relationships between equilibrium constants. Homogeneous and heterogeneous equilibria. Gaseous equilibria. Influence of pressure, temperature and concentration on equilibrium conditions.

10. *Electrolyte solutions. Electrolytic dissociation. Strong and weak electrolytes. Degree of dissociation. Van’t Hoff’s coefficient. Conductance. Equivalent conductance. Law of independent ion migration. Acids and bases. Theories of Arrhenius, Brønsted–Lowry and Lewis. Strength of acids and bases. Ionic product of water. Relationship between Ka and Kb. Definition of pH. Calculation of the pH of solutions of acids, bases and salts. Buffer solutions. pH indicators. Acid-base titrations. Ampholytes. Solubility equilibria. Solubility product. Common ion effect.

11. *Electrochemistry. Oxidation-reduction reactions: the ion-electron method. Electrode potentials. The Nernst equation. Standard potential and its measurement. Galvanic cells. Concentration cells. Electrochemical series of the elements. Chemical cells. Prediction of redox reactions. Equilibrium constant. Determination of pH, KPS and degree of dissociation. Free energy of reaction. Numerical exercises.

12. *Electrolysis. Decomposition voltage. Overvoltage. Faraday’s laws and numerical exercises. Law of electrochemical equivalents. Electrolysis of molten salts. Electrolysis of water. Electrolysis of aqueous solutions. Industrial electrolytic processes. Batteries. Corrosion. Passivation.

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

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

This 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 current generators, 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 heat balances of reactions and chemical kinetics to optimise 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 (metals, polymers, ceramics and composites) is aimed at structural safety and durability:

Target 9.4 (Modernise infrastructure and make industries sustainable): Focus on the chemical and physical mechanisms of material degradation, with particular attention to the thermodynamics and kinetics of metal corrosion and the related chemical and galvanic protection techniques to extend the life cycle of plant and equipment.

SDG 12 — Responsible consumption and production

The principles of Green Chemistry applied to industrial design are introduced, moving beyond the linear approach to production:

Target 12.4 (Environmentally sound management of chemicals and all types of waste): Study of catalytic reactions to minimise toxic by-products and maximise the atomic economy of processes.

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

Theory and exercises

B.B.Laird, Chemistry, McGraw-Hill

There will be ongoing assessments which must be passed in order to pass the course.

The final examination consists of a written and an oral component.

FORMATIVE ASSESSMENTS

There will be two formative assessments (each lasting 90 minutes) halfway through and at the end of the course. The formative assessments are written, consisting of numerical exercises involving stoichiometric calculations, and may also include theoretical questions. Each question will be awarded a mark, which will be indicated next to it. A mid-term assessment is considered passed if the mark obtained is between 18 and 30 (out of 30); otherwise, the student must retake the entire assessment on one of the dates specified in the examination timetable. Passing both mid-term assessments entitles the student to exemption from the written examination. Before the start of the assessment, the lecturer will provide all the necessary instructions to help students perform to the best of their ability. Registration for the mid-term assessment is compulsory and must be completed exclusively via the Studium platform (http://studium.unict.it) by the specified deadline.

END-OF-COURSE EXAMS

The examination consists of a written paper followed by an oral examination. Registration for the written paper, for each examination session, is compulsory and must be completed exclusively via the student portal (https://studenti.smartedu.unict.it/) by the specified deadline. The written examination is considered passed if a mark of at least 18/30 is achieved; otherwise, the student must retake the entire examination on one of the dates set out in the examination timetable. The oral examination consists of a presentation on topics covered in the course syllabus. The final examination mark will take into account both the written and oral components.

The assessment may also be conducted online should circumstances require the use of this method. In such cases, the duration of the written examination may be subject to change.

The assessment will take into account the accuracy and completeness of the content (listed in the ‘course syllabus’ section), the clarity and logical rigour of the presentation, and the ability to apply principles to practical cases. To ensure equal opportunities and in accordance with current legislation, students enrolled at CInAP may agree with their lecturer on any compensatory and/or adaptive measures, based on the learning objectives and their specific needs. You may also contact the CInAP (Centre for Active and Participatory Integration – Services for Disabilities and/or Specific Learning Difficulties) liaison lecturers at the DIEEI, Prof. Antonella Di Stefano and Prof. 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.