CHEMISTRY

The course aims to provide the fundamental principles of Chemistry as an essential cultural and scientific foundation for understanding the subjects for which Chemistry serves as a prerequisite. The course also aims to provide students with an understanding of the role of chemistry in society and in everyday life, with particular reference to topics of relevance to the natural and environmental sciences.

Students will be introduced to chemical nomenclature, structural formulae of the main inorganic compounds, chemical stoichiometry, chemical bonding, the fundamental principles of chemical thermodynamics, the properties of solutions and related chemical equilibria, with particular emphasis on acid-base and precipitation equilibria, the basic concepts of chemical kinetics and electrochemistry, and the rational understanding of the chemical properties of the different families of organic compounds in relation to those of more complex molecules of biological interest.

Through the study of chemistry, students will become aware not only of the fundamental role played by this discipline in several scientific, technological, naturalistic and environmental fields, but will also become familiar with the basic principles underlying the scientific method.

In particular, the course is structured to provide a sound knowledge of basic chemistry, including inorganic chemistry and stoichiometry, using the scientific method and appropriate scientific terminology. The course consists of a theoretical component and a practical component based on exercises aimed at solving chemistry problems (knowledge and understanding). Furthermore, the course aims to develop the reasoning skills required to approach the study of chemical phenomena using analytical and numerical methods (applying knowledge and understanding).

According to the Dublin Descriptors (DD), this course contributes to the acquisition of the following transversal skills:

Knowledge and understanding of chemical and biochemical aspects:

• acquire basic knowledge of the composition of matter, chemical elements, the periodic system, and the main inorganic compounds;
• acquire basic knowledge of chemical bonding and the states of matter;
• acquire basic knowledge of the main classes of organic compounds;
• acquire the knowledge and ability to represent a chemical reaction or equilibrium in both qualitative and quantitative terms;
• acquire the knowledge and ability to formulate a chemical problem by using appropriate relationships between chemical and physical quantities and to solve it through analytical methods;
• acquire inductive and deductive reasoning skills.

Applying knowledge and understanding:

• ability to apply the acquired knowledge to the description of chemical phenomena through the rigorous use of the scientific method;
• ability to perform quantitative calculations involving chemical reactions and chemical equilibria;
• ability to describe the chemical behaviour of elements and their inorganic compounds;
• ability to distinguish between inorganic and organic compounds.

Making judgements:

• ability to contextualise the scientific knowledge and skills acquired;
• development of independent and critical reasoning regarding chemical phenomena, including scientific and ethical reflection on environmental and naturalistic issues;
• ability to identify the predictions derived from a theory or model;
• ability to identify the most appropriate methods for critically analysing, interpreting and solving chemical problems.

Communication skills:

• ability to describe chemical phenomena clearly and rigorously, both in written and oral form, to both specialist and non-specialist audiences;
• effective use of Italian and/or English, with appropriate language and terminological accuracy, to present a scientific topic and clearly explain its rationale and results.

Learning skills:

• possess the basic cognitive tools required for the continuous updating of one's knowledge;
• acquire the ability to independently read, understand and critically analyse scientific texts and topics, with particular reference to the chemical sciences;
• develop the ability to independently learn new scientific topics required for further study with a high degree of autonomy.

The course is delivered through in-person lectures (56 hours), according to the timetable and in the classrooms indicated on the Degree Programme website. Additional hours (12) are devoted to exercises aimed at solving problems related to the topics covered during the lectures. These exercise sessions will also provide an opportunity to further explore and clarify any doubts concerning the theoretical aspects of the entire course programme.

For the exercise sessions, the lecturer may be assisted by a qualified tutor, if such a figure is made available by the Degree Programme.

The lecturer will make available, through the Studium platform, all teaching materials and exercises used during the course.

It should be noted that the material provided by the lecturer is intended as support for individual study and cannot be considered a substitute for one of the recommended textbooks.

If the course is delivered in blended or remote mode, appropriate adjustments may be made to the above, in order to ensure consistency with the syllabus.

The course does not require any formal prerequisites from other courses within the degree programme. 

However, a basic knowledge of mathematical analysis and general physics is considered important.

Attendance at course lectures is mandatory. In accordance with the regulations of the degree programme, attendance requirements are considered to be fulfilled if the student has attended at least 60% of the scheduled curricular hours for the course. The teacher will verify attendance by taking attendance at the beginning of each in-person classroom lecture.

For working students, student athletes, and students experiencing particular difficulties (Regolamento Didattico di Ateneo, art. 30), whose status is duly certified, the Degree Programme provides for:

• a reduction in the attendance requirement of up to 20%;
• the possibility of taking examinations during extraordinary examination sessions reserved for repeating students and students who are beyond the standard duration of their degree programme;
• specific academic support activities to be agreed upon with the teacher.

COURSE SYLLABUS:

1 - INTRODUCTION TO THE COURSE, COMPOSITION OF MATTER AND ATOMIC STRUCTURE
Brief overview of the history of Chemistry - Scientific method - Lavoisier’s principle - Composition of matter: pure substances, compounds, mixtures - Dalton’s atomic theory - States of matter - Physical and chemical transformations of matter - Subatomic particles: electron, proton, neutron - Atomic number, mass number - Chemical symbols - Isotopes - Ions: cations and anions - Atomic mass unit - Early atomic models: Thomson’s atomic model, Rutherford’s atomic model, Bohr’s atomic model - Brief overview of wave-particle duality - Heisenberg uncertainty principle - Modern atomic model: introduction to the quantum-mechanical description of the atom - Atomic orbitals - Quantum numbers - Electron configuration of atoms and ions - Pauli exclusion principle - Hund’s rule of maximum multiplicity. Exercises on the topics covered in the module.

2 - PERIODIC TABLE OF THE ELEMENTS
Periodic table: periods and groups - Periodic classification of the elements and periodic law - Metals, non-metals and metalloids - General properties of the main elements of the periodic table - General characteristics of each group of the periodic table - Electron configuration of the elements - Relationship between the electron configuration of an element and its position in the periodic table - Periodic properties: atomic and ionic radii, ionisation energy, electron affinity and electronegativity. Exercises on the topics covered in the module.

3 - CHEMICAL BONDING
Definition of chemical bonding - Ionic bonding - Covalent bonding - Lewis model and Lewis symbols - Octet rule - Structural formulae of the most common inorganic compounds - Brief overview of the magnetism of matter - Electronegativity of atoms and bond polarity - Resonance - Valence bond theory - VSEPR theory and molecular geometries - Hybrid orbitals and hybridisation theory - Metallic bonding. Exercises on the topics covered in the module.

4 - INTERMOLECULAR FORCES
Dipoles and induced dipoles - Ion-dipole interactions - Van der Waals forces: dipole-dipole, dipole-induced dipole, and induced dipole-induced dipole interactions - Hydrogen bonding. Exercises on the topics covered in the module.

5 - NOMENCLATURE AND STOICHIOMETRY
Composition of matter - Atomic mass unit - Relative atomic mass - Atomic weight - Molecular masses and molecular weights - The mole concept and the laws of stoichiometry - Avogadro’s number - Chemical formula of a compound: meaning and determination - Empirical and molecular formulae - Oxidation number - Nomenclature of the main classes of inorganic compounds - Chemical equations and balancing - Identification of oxidation-reduction reactions - Balancing of oxidation-reduction reactions - Stoichiometric calculations: quantitative relationships in chemical reactions - Limiting reagent - Reaction yield - Exercises on the topics covered in the module.

6 - GASEOUS STATE
General characteristics of the gaseous state - Ideal gases - Ideal gas laws - Ideal gas equation of state - Law of partial pressures and partial volumes - Brief overview of real gases - Difference between gas and vapour - Exercises on the topics covered in the module.

7 - CONDENSED STATES AND PHASE TRANSITIONS
Brief overview of the characteristics of condensed states in relation to chemical bonding and intermolecular forces - Characteristics of the liquid state - Vapour pressure - Surface tension - Viscosity - Phase changes - Characteristics of the solid state - Crystalline and amorphous solids - Phase transitions - Phase diagram of water. Exercises on the topics covered in the module.

8 - FUNDAMENTALS OF CHEMICAL THERMODYNAMICS AND CHEMICAL KINETICS
Definition of thermodynamics - System, surroundings and universe - State functions - Internal energy - First law of thermodynamics - Enthalpy - Hess’s law - Spontaneity of processes - Entropy - Second law of thermodynamics - Gibbs free energy - Role of temperature in the spontaneity of chemical reactions - Definition of reaction rate - Factors affecting reaction rate - Reaction mechanism and rate-determining step - Brief overview of collision theory, activation energy and catalysts. Exercises on the topics covered in the module.

9 - AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES
Types of solutions - Concentration units - Solubility, with particular reference to the solubility of ionic compounds - Gas solubility and Henry’s law - Ideal solutions and Raoult’s law - Colligative properties of solutions: vapour-pressure lowering, freezing-point depression, boiling-point elevation, osmosis and osmotic pressure - Electrolyte solutions and van ’t Hoff factor - Concept of dilution - Exercises on the topics covered in the module.

10 - CHEMICAL EQUILIBRIUM
Forward and reverse chemical reactions - Reversible reactions - Chemical equilibrium - Law of mass action and equilibrium constant - Thermodynamic interpretation of chemical equilibrium - Principle of mobile equilibrium, or Le Chatelier’s principle, and factors affecting chemical equilibrium - Dissociation of electrolytes - Ionic equilibria in aqueous solution - Acid-base theories: Arrhenius acids and bases and Brønsted-Lowry theory - Strength of acids and bases - Dissociation of water (autoprotolysis) and pH scale - pH of aqueous solutions of strong and weak acids and bases - pH of aqueous salt solutions (hydrolysis) - Buffer solutions - Exercises on the topics covered in the module.

11 - FUNDAMENTALS OF ELECTROCHEMISTRY
Galvanic cells and the Daniell cell - Cell potentials - Standard reduction potential series and its significance - Nernst equation - Corrosion of metals - Electrolytic cells - Electrolysis of water - Brief overview of rechargeable batteries. Exercises on the topics covered in the module.

12 - FUNDAMENTALS OF ORGANIC CHEMISTRY
Introduction to Organic Chemistry - Carbon hybridisation - Structural formulae, nomenclature, properties and reactivity of the main classes of organic compounds: alkanes, alkenes, alkynes, aromatic hydrocarbons, alcohols, phenols, ethers, amines, aldehydes, ketones, carboxylic acids and their derivatives, with particular reference to esters and amides - Brief overview of stereoisomerism and chirality - Exercises on the nomenclature of organic compounds and questions and answers on the topics covered in Organic Chemistry.

The recommended textbooks for General and Inorganic Chemistry topics are:

1. A. Credi, A. Del Zotto, A. Gasparotto, F. Marchetti, D. Zuccaccia - VAGGIO NELLA CHIMICA - EdiSES, Napoli

2. Kotz, Treichel, Townsend (ed edizioni precedenti) - CHIMICA - EdiSES, Napoli

3. Petrucci - CHIMICA GENERALE - PICCIN

The recommended textbook for Organic Chemistry topics is:

4. W. H. Brown, M. K. Campbell, S. O. Farrell - ELEMENTI DI CHIMICA ORGANICA - EdiSES, Napoli

The recommended textbooks for exercises and numerical applications related to the course topics are:

5. Lausarot, Vaglio - STECHIOMETRIA PER LA CHIMICA GENERALE - Piccin

6. Marcì, Palmisano, Ruffo - STECHIOMETRIA - EdiSES, Napoli

7. I Bertini, C. Luchinat, F. Mani - STECHIOMETRIA - CEA

Other textbooks already owned by the students may also be used, subject to approval by the lecturer.

Final exam

The final assessment for the course consists of a written examination, including open-ended questions, multiple-choice questions and problem-solving exercises, aimed at assessing the student’s knowledge of all the topics covered during the course. The written examination is followed by an oral examination, focused on the discussion of the written test and on further assessment of the topics included in the course programme. Access to the oral examination is permitted only after successful completion of the written examination.

Mid-term assessments

Two mid-term assessments are scheduled during the course.

Each mid-term assessment consists of a written examination including open-ended questions, multiple-choice questions and problem-solving exercises.

All students, including repeating students and students who are beyond the standard duration of the degree programme, may take part in the mid-term assessments, provided that they have attended at least 60% of the curricular teaching hours scheduled for the relevant academic year, as recorded by the lecturer up to the date of the assessment. Students who successfully pass the first mid-term assessment, scheduled after approximately 50% of the course has been completed, will be allowed to take the second mid-term assessment, scheduled immediately after the end of the course.

Only students who successfully pass both mid-term assessments will be exempted from the written component of the final examination and will be allowed to proceed directly to the oral examination. Students who fail either the first or the second mid-term assessment, or who do not take part in them, will be required to take the complete final examination.

Learning assessment may also be carried out on-line, should the conditions require it.

To ensure equal opportunities and in compliance with current laws, interested students may request a personal interview in order to plan any compensatory and/or dispensatory measures based on educational objectives and specific needs. Students can also contact the CInAP (Centro per l’integrazione Attiva e Partecipata — Servizi per le Disabilità e/o i DSA) referring teacher within their department (https://www.cinap.unict.it/content/referenti).

The following criteria will be taken into account when assigning the final grade:

Grade 29–30 with honours: the student demonstrates thorough knowledge of the course topics and is able to promptly and correctly integrate and critically analyse the situations presented, independently solving even highly complex problems. The student has excellent communication skills and uses appropriate and precise terminology.

Grade 26–28: the student demonstrates good knowledge of the course topics and is able to integrate and critically analyse the situations presented in a clear and coherent manner. The student is able to solve complex problems with a good degree of independence and presents the topics clearly using appropriate terminology.

Grade 22–25: the student demonstrates a satisfactory knowledge of the course topics, although mainly limited to the core subjects. The student is able to integrate and critically analyse the situations presented, although not always in a fully coherent manner, and presents the topics with reasonable clarity and generally appropriate terminology.

Grade 18–21: the student demonstrates the minimum required knowledge of the course topics, has limited ability to integrate and critically analyse the situations presented, and presents the topics with sufficient clarity, although with limited command of the appropriate terminology.

Fail: the student does not demonstrate the minimum required knowledge of the main course contents. The ability to use subject-specific terminology is very limited or absent, and the student is unable to independently apply the acquired knowledge.

• Nomenclature of the main inorganic and organic compounds;

• Structural formulae of the main inorganic and organic compounds, molecular geometry according to VSEPR theory, and hybridisation of the central atom;

• Stoichiometric calculations;

• Exercises on colligative properties;

• pH calculations for acid-base mixtures, salt solutions, and buffer solutions;

• Balancing of redox reactions;

• Chemical equilibrium;

• Reaction rates and the factors affecting them;

• Solutions and colligative properties;

• The periodic table and periodic properties of the elements;

• Electron configurations of the elements;

• Enthalpy, entropy, and Gibbs free energy;

• Nomenclature, properties, and reactivity of the main classes of organic molecules.