CHIMICA
Academic Year 2026/2027 - Teacher: VALENTINA SIRACUSAExpected Learning Outcomes
The student will know the main phenomena of basic chemistry and will be able to understand their applications in the engineering field. The student will also learn the ability to understand a scientific text, to rework, even in an original way, what has been studied and to transform and reflect on the knowledge learned.
The student will be able to apply the knowledge acquired to recognize the laws that govern chemical and chemical-physical phenomena, to independently solve complex problems and exercises, even in fields other than chemistry.
The student, using the knowledge of chemical and chemical-physical phenomena acquired during the course, will be able to independently judge the importance of the results obtained, as well as the meaning of the units of measurement and the order of magnitude of the variables that describe the phenomena .
The student who has successfully passed the course will be able to present the knowledge acquired clearly and accurately.
The student who has successfully passed the course will have acquired the ability to study independently and to delve deeper into the concepts studied in full independence.
Course Structure
If the teaching is taught in mixed or remote mode, the necessary variations may be introduced with respect to what was previously declared, in order to respect the planned program and reported in the syllabus.
Required Prerequisites
Attendance of Lessons
Detailed Course Content
1. * Nature of the subject. The matter and the states of aggregation. Homogeneous and heterogeneous systems. Stages and their separations. Elements and chemical compounds. Atoms and molecules. Ponderal laws (Lavoisier, Proust, Dalton). Volumetric laws (Gay-Lussac, Avogadro). Determination of atomic weight (Cannizzaro rule) and molecular weight (gaseous density). Avogadro number. 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. Atomic model of Thomson. Millikan experiment. Rutherford experiment. Atomic model of Rutherford. Electromagnetic radiation. Emission spectrum of the black body. Photoelectric effect. Emission spectrum of the hydrogen atom. Bohr theory. Report by De Broglie. Uncertainty principle of Heisenberg. Wave mechanics. Schrödinger equation. Quantum numbers and energy levels. Orbital. Polyelectronic atoms. Principle of Pauli. Hund rule. Principle of Aufbau. Periodic table. Periodic properties (ionization energy, electronic affinity, atomic radius, electronegativity, metallic character).
3. * Chemical bond. Electron sharing. Covalent bond. Octet rule. Distance and bonding energy. Homeopolar and heteropolar link. Dative tie. Dipoles. Bonds π and s. Hybridization. Bonding angles. VSEPR. Molecular geometry. Resonance. Ionic bond. MO-LCAO theory. Molecular orbitals of diatomic molecules of the second period. Metal tie. Orbitals of Bloch. Weak links. Hydrogen bond.
4. * Chemical compounds and nomenclature. Valence and oxidation number. Oxidation and reduction. Hydrides. Hydrogen acids. Oxides. Peroxides. Hydroxides. Oxyacids. Salts. Chemical equation. Reactions. Redox reactions. Disruption reactions. Combustion reactions. Ponderal relationships. Limiting reagent rule. Calculation examples. Types of formulas (minimum, brute, structure and steric formula). Elementary analysis. Calculation examples.
5. * Thermodynamics. Thermodynamic system. Types of systems. Extensive and intensive variables. Status functions. Work. Heat. Power. Thermal capacity. Work. First principle of thermodynamics. Internal energy and enthalpy. Termochimica. Law of Hess. Second principle of thermodynamics. Heat conversion in work. Entropy. Free energy. Spontaneity of chemical reactions. Third principle of thermodynamics.
6. * States of aggregation of the matter. The gaseous state. Ideal gas and perfect gas. Boyle's law. Law of Gay Lussac. Law of Charles. Avogadro's law. Equations of state of ideal gases. Determination of the molecular weight of a gas. Gaseous diffusion. Partial pressures. Molar heat of gases. Maxwell-Boltzmann speed distribution. Real gases. Van der Waals equation. Liquefaction of gases. 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 equation. Polymorphism. Ionic solids. Covalent solids. Molecular solid. Metallic solids.
7. * State steps and heterogeneous equilibria. State steps: fusion, evaporation, sublimation. Clausius-Clapeyron equation. Variance. Phase rule. State diagrams. One-component systems: water, sulfur, carbon dioxide. Systems with eutectic point.
8. * Status of solution. Types of solution. Solubility of a species. Concentration and way of expressing it. Solute-solvent interaction: ideal and real solutions. Rault law. Relationships between the composition of a mixture of two liquids and that of its vapor. Systems with maximum and minimum azeotrope. Dilute solutions of non-volatile solutes. Colligative properties. Lowering the vapor pressure. Cryoscopic lowering. Ebullioscopic elevation. Osmotic pressure. Numerical exercises.
9. * Chemical equilibria. Law of chemical equilibrium. Le Chatelier's principle. Relationship between free energy and equilibrium constant. Balance constant (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. Coefficient of Van't Hoff. Conductance. Equivalent conductance. Law of independent ion migration. Acids and bases. Theories of Arrhenius, Bronsted-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 solution of acids, bases and salts. Buffer solutions. PH indicators. Acid-base titrations. Ampholytic. Solubility equilibria. Solubility product. Ion to common.
11. * Electrochemistry. Oxidation-reduction reactions: electronic ion method. Electrode potentials. Nernst's equation. Standard potential and its measure. Galvanic batteries. Concentration batteries. Electrochemical series of elements. Chemical stacks. Forecasts of redox reactions. Balance constant. Determination of pH, KPS and degree of dissociation. Free reaction energy. Numerical exercises.
12. * Electrolysis. Decomposition voltage. Overvoltage. Faraday laws and numerical exercises. Law of electrochemical equivalents. Electrolysis of molten salts. Water electrolysis. Electrolysis of aqueous solutions. Industrial electrolytic processes. Accumulators. Corrosion. Passivation.
13. * Chemical kinetics. Reaction speed. Kinetic law. Molecularity. Reaction order: reactions of the 1st and 2nd order. Arrhenius equation. Influence of temperature. Activation energy. Catalysts. Kinetic derivation of the equilibrium constant. Chain reactions.
* obligatory skills
- Goal 4: Ensure inclusive and equitable quality education and promote lifelong learning opportunities for all
- Goal 5: Achieve gender equality and empower all women and girls
Textbook Information
1) T.L. Brown, H.E. LeMay, B.E. Bursten, : Fundamentals of Chemistry, fourth Italian edition, EdiSES (or english edition) (new edition)
2) R. Chang – K. Goldsby: “Fundamentals of General Chemistry”, McGrawHill Education - (both new and old editions)
3) P. Atkins – L. Jones: “Fundamentals of General Chemistry”, Zanichelli - (both new and old editions)
Course Planning
| Subjects | Text References | |
|---|---|---|
| 1 | Nature of matter (6 hours) | book 1 (chapters 1, 2); 2, 3 |
| 2 | Structure of the subject and exercises (8 hours) | book 1 (chapters 2, 3, 4, 6, 7); 2, 3 |
| 3 | Chemical bond (9 hours) | book 1 (chapters 8, 9); 2, 3 |
| 4 | Chemical compounds and nomenclature (4 hours) | book 1 (chapters 2, 3), 2, 3 |
| 5 | Thermodynamics and numerical exercises (5 hours) | book 1 (chapters 5, 18); 2, 3 |
| 6 | States of aggregation of matter (10 hours) | book 1 (chapters 10, 11, 12); 2, 3 |
| 7 | State transitions and heterogeneous equilibria (5 hours) | book 1 (chapter 11) ; 2, 3 |
| 8 | Solution state (4 hours) | book 1 (chapter 13); 2, 3 |
| 9 | Chemical equilibria (3 hours) | book 1 (chapter 15); 2, 3 |
| 10 | Electrolyte solutions (5 hours) | book 1 (chapter 16); 2, 3 |
| 11 | book 1 (chapter 16); 2, 3 | book 1 (chapter 19); 2, 3 |
| 12 | Electrolysis (5 hours) | Electrolysis (5 hours) |
| 13 | Chemical kinetics (6 hours) | book 1 (chapter 14); 2, 3 |
Learning Assessment
Learning Assessment Procedures
Two written mid-term tests are scheduled, one halfway through the course and one at the end of the course, consisting of theoretical questions and numerical exercises, including stoichiometric calculations. A specific score will be assigned to each question and indicated next to it.
The examination will be considered passed if both mid-term tests are successfully completed with a score of at least 18/30. The final grade will be calculated as the arithmetic mean of the grades obtained in the two tests and must be at least 18/30.
Additional questions will also be included to allow students to be awarded honours (30/30 cum laude) if their overall score exceeds 30/30.
Students who choose not to take the mid-term tests, or who fail either of the two tests, will be required to take the final examination, which consists exclusively of a written test. Each mid-term test and the final examination have a duration of 90 minutes. The final examination is considered passed with a minimum score of 18/30. Additional questions will be included to allow students to achieve honours (30/30 cum laude) if their overall score exceeds 30/30.
The assessment may also be conducted online, should circumstances require it. In such cases, the duration of the written examination may be subject to change.
To ensure equal opportunities and in compliance with current legislation, students concerned may request an individual meeting in order to arrange any appropriate compensatory and/or dispensatory measures, in accordance with the learning objectives of the course and their specific needs. Students may also contact the CInAP representative (Centre for Active and Participatory Integration – Services for Students with Disabilities and/or Specific Learning Disorders) of their Department.
MID-TERM TESTS
Two mid-term tests, each lasting 90 minutes, are scheduled and will take place respectively halfway through and at the end of the course.
Each test consists of a written examination including theoretical questions and numerical exercises, including stoichiometric calculations. A specific score will be assigned to each question and indicated next to it.
Each mid-term test is considered passed with a score of 18/30 or higher. If the student fails even one of the two tests, they will be required to take the entire examination on one of the officially scheduled examination dates.
Students who successfully pass both mid-term tests and achieve a final grade of at least 18/30, calculated as the arithmetic mean of the grades obtained in the two tests, will be exempted from taking the final examination.
Before the beginning of each test, the instructor will provide all the necessary information regarding the examination procedures. These instructions will apply both to the mid-term tests and to examinations taken on the officially scheduled examination dates.
Registration for the mid-term tests is mandatory and must be completed by the deadline communicated by the teacher and explained in class during the course.
The mid-term tests will be conducted using the Exam.net platform. Students are therefore required to bring a computer to the classroom on the scheduled test date. Students who do not have access to a computer or whose computer is accidentally damaged or unavailable will be allowed to take the test on paper provided by the teacher.
FINAL EXAMINATION
The final examination, lasting 90 minutes, consists of a written test including theoretical questions and numerical exercises, including stoichiometric calculations. A specific score will be assigned to each question and indicated next to it.
The examination is considered passed if the student obtains a grade between 18/30 and 30/30. Otherwise, the student will be required to retake the entire examination on one of the officially scheduled examination dates.
Before the beginning of the examination, the instructor will provide all the necessary instructions to enable students to complete the examination correctly.
Registration for each examination session is mandatory and must be completed exclusively through the student portal (https://studenti.smartedu.unict.it/) by the specified deadline. Students are free to take part in any of the examination sessions scheduled during the Academic Year 2026-2027.
The final examination will be conducted using the Exam.net platform. Students are therefore required to bring a computer to the classroom on the scheduled examination date. Students who do not have access to a computer or whose computer is accidentally damaged or unavailable will be allowed to take the examination on paper provided by the teacher.
Examples of frequently asked questions and / or exercises
For simplicity's sake, here are some examples of questions:
1. 130 g of Cu are reacted with 530 grams of HNO3 through the following chemical reaction, which must be balanced completely (score = 3):
Cu + HNO3 = Cu(NO3)2 + NO + H2O
Which reagent is in excess?
Calculate the volume in liters of NO, measured at 0°C and 2 atm, that is released from the reaction between Cu and HNO3. Assume ideal gas behavior.
2. The electric charge of an electron is equal to (Score = 1):
☐ -1.602 10-19C ☐ 1.602 10-19C ☐ -1.602 10-24C ☐ -1.602 1023C
3. Isobars are nuclides characterized by the same (Score = 1):
☐ atomic number ☐ type of radioactive decay ☐ mass number ☐ number of neutrons
4. The correct form of Einstein's mass-energy relationship is (Score = 1):
☐ m=Ec2 ☐ E=mc ☐ E2=mc2 ☐ E=mc2
5. The number of protons and electrons in the O- ion is respectively (Score = 1):
☐ 8, 8 ☐ 16, 8 ☐ 16, 16 ☐ 8, 10
6. Balance the following oxidation-reduction reactions (Score = 2)
Zn (s) + HCl (aq) = ZnCl2(aq) + H2 (g)
Al(s) + Cu(NO3)2 (aq) = Cu ( s) + Al(NO3)3 (aq)
7. Balance the following acid-base chemical reactions (Score = 2):
Hg2(NO3)2 + KI Hg2I2 + KNO3
Cl2 + NaOH NaCl + NaClO + H2O