Ateneo - UPO

The course provides the basic concepts of general and inorganic chemistry: properties, composition and structure of the matter, thermodynamics, chemical kinetics, chemical equilibrium and electrochemistry.

Slides (pdf format) are available on the DIR platform. Suggested texts: Kotz, Treichel, Townsend, Treichel, Chimica, Edises, VII Ed., 2021 R.H. Petrucci, F.G. Herring, J.D. Madura, C. Bissonnette, General Chemistry Brown, Lemay, Bursten, Murphy, Woodward, Stoltzfus, Fondamenti di Chimica. Edises, IV Ed., 2018 Atkins, Jones, Laverman, Principi di Chimica, Zanichelli, 2018 Silberberg, Amateis, Licoccia, CHIMICA, Quarta Edizione, Mc Graw Hill, 2019.

Provide a solid foundation for understanding chemical events at the molecular level and relating them to the macroscopic world.
Skills: Introduce students to the use of the structure–property concept and to the molecular interpretation of chemical phenomena.
Promote the development of critical thinking that enables students to draw conclusions on issues related to the topics covered.
Communication skills: Students will be guided in the use of appropriate scientific vocabulary and in developing the ability to present the topics covered in the course clearly and effectively.

No particular prerequisites are expected, save for the basic competences required by the TCI test, with particular reference to basic mathematics.

Classroom lectures, slide shows and guided exercises with open discussion. Students will be encouraged to supplement in-class work with individual homework for a successful fruition of the course.

Students with physical disabilities, Learning Disabilities or Special Education Needs can request specific services and tools via the Staff Sviluppo e Coordinamento Carriere e Servizi alle Studentesse e agli Studenti, consulting the University webpage:
https://www.uniupo.it/en/services/services-students-physical-or-learning-disabilities

Students with disabilities, learning disabilities or special education needs, once they have contacted the University Staff, can refer to the tutor in charge of the course to define the examination modalities, concerning academic aspects.

The exam consists of a written test lasting a maximum of 3 hours and includes 12 open-ended, semi-open, or numerical (stoichiometry)/graphical (molecular structure) resolution questions, which are assigned a variable score (1-2 points) based on their complexity. At the same time, students must also answer 3 questions (each worth 1 point) regarding the Laboratory module, placed at the end of the 12 General Chemistry module questions.
The maximum total score (General Chemistry module and Laboratory module) is 20 points. Honors (laude) may be awarded if the content of the answers exceeds what is required or is of a quality worthy of distinction. The exam is passed with a score of 12/20. This score will be added to that of the stoichiometry and laboratory module to reach a final grade expressed on a 30-point scale.
To achieve a passing grade, students must demonstrate a basic understanding of the core topics of the course, with particular reference to chemical bonding, molecular geometry, intermolecular forces, chemical equilibrium, acids and bases, and electrochemistry. They must also demonstrate knowledge of the main elements and the most common simple chemical compounds, their distribution in nature, and their main properties.
The evaluation of the test and the corresponding score assignment will be primarily based on the students' ability to understand the question, identify the unknown variables of the problem, formulate a logical, rigorous, and relevant answer (for open and semi-open questions) or a rational and justified resolution strategy (for numerical/graphical questions), and use chemical language and symbology appropriately and rigorously. The entire course syllabus may be subject to examination.

The matter: homogeneous and inhomogeneous mixtures. Elements, compounds and chemical formulas. Nomenclature of chemical compounds. The laws of chemistry. The mole and the Avogadro number. The structure of the atom: subatomic particles, isotopes, radioactivity. The atomic theory. The periodic system and the periodic properties of the elements. Basic concepts of chemical bonding: Lewis theory and molecular geometry according to the VSEPR model. Covalent, ionic and metallic bonds. Molecular orbitals. Intermolecular forces. Aggregation states and their properties. Ionic, metal and molecular solids. Gases and their properties. Solutions and their properties: solubility, vapor tension osmotic pressure. Chemical reactions and chemical equations. Fundamentals of chemical kinetics. Thermochemistry: entalpy, entropy, free energy. The chemical equilibrium: the equilibrium constant, the Le Chatelier Principle and its application. Acids and bases: Arrhenius, Lewis and Brønsted-Lowry theories. Acid base equilibria and buffer solutions. Heterogeneous equilibria. Electrochemistry : oxidation states and redox reactions. Standard potentials and electrochemical series. Concepts of radiochemistry.

Knowledge and competences: achieving a solid solid background on the fundamental concepts of chemistry (chemical quantity, reactions, states of matter, chemical bonds, molecular structure, equilibrium, acids and bases, thermochemistry, electrochemistry). Capability to apply the acquired knowledge for the resolution of chemical problems. Ability tounderstand and interpret chemical and physico-chemical transformations at the macroscopic and microscopic level. Ability to recognize the main classes of inorganic compounds and name them. Master a critical approach in the design and resolution of chemical problems and experiments. Communication skills: the student is expected to acquire and properly use a suitable scientific vocabulary and be able to report on a chemical problem/experiment in a clear and concise manner.