Ateneo - UPO

1. Review of the International System of Units. The atom: atomic particles (protons, neutrons, electrons); mass number and atomic number. Atomic dimensions: the angstrom, relative atomic mass, and the atomic mass unit. The mole and Avogadro’s number. Isotopes: definition, properties, and atomic mass. Ions.
2. Overview of atomic models: Thomson’s model, Rutherford’s model, Bohr’s model, and the current atomic model.
3. Quantum numbers, electron configuration, and Lewis structures.
4. The periodic table of the elements: history and characteristics. Periodicity of the properties of the elements and determination of oxidation numbers.
5. Review of matter, mass, and weight. Pure substances (elements and compounds) and allotropes. Classification of the elements (metals, nonmetals, metalloids, noble gases). 6. Molecular compounds and the representation of molecules; ionic compounds (empirical formulas, nomenclature of cations, anions, and polyatomic ions). Mixtures (homogeneous and heterogeneous).
6. Solutions: characteristics and units of concentration. Theory and exercises on molarity, molality, mass percentage (weight %), volume percentage, mass-volume percentage, parts per million, and dilutions.
7. Chemical reactions: characteristics and the Law of Definite Proportions (Proust’s Law). Stoichiometry and balancing of chemical equations. Oxidation-reduction (redox) reactions: characteristics and balancing.
8. Acids and bases: Arrhenius theory, Brønsted–Lowry theory, the concept of conjugate acids and bases, and amphoteric electrolytes. Ka: acid and base strength and ionization constants. The ionic product of water. pH and pOH. Calculation of pH for monoprotic acids and strong bases.
9. Buffer solutions: pH of a buffer solution and the Henderson–Hasselbalch equilibrium/equation. The blood buffer system.
10. Systematic and traditional formulas and nomenclature of chemical compounds.

The teaching materials required for studying will be provided during the lectures and will also be available on the course page on the DIR platform.

The course aims to provide students with the fundamental knowledge of general chemistry and laboratory chemistry, with particular attention to the basic concepts of the structure of matter, the properties of elements and compounds, chemical reactions, and stoichiometric principles. The goal is to develop the ability to interpret chemical phenomena, solve simple quantitative problems, and correctly use chemical terminology, preparing students for both basic and applied scientific disciplines.

To successfully follow the course, it is useful to have basic knowledge of mathematics and physics at the high school level, in particular: elementary notions of algebra and proportions; concept of physical quantities and units of measurement; notions of mass, weight, and density.

Lectures supported by multimedia presentations. Guided classroom exercises on topics including stoichiometry, concentration calculations, balancing reactions, and pH.

PDF copies of the lecture slides, supplementary learning materials, and all information concerning the course and examination procedures will be made available on the DIR platform (https://www.dir.uniupo.it/).
Students with disabilities, Specific Learning Disorders (SLD), or Special Educational Needs (SEN) may request specific services and support tools dedicated to them by contacting the University’s Student Careers Development and Coordination Staff and Student Services Office, and by consulting the dedicated page on the University website: https://uniupo.it/it/servizi/servizi-studentesse-e-studenti-condizione-di-disabilità-e-dsa.
Students with disabilities, SLD, or SEN, once they have contacted the University’s relevant staff, may contact the course instructor regarding the arrangements for examination procedures and any aspects related to teaching and learning activities.

Written exam with numerical exercises (stoichiometry, solutions, pH, reaction balancing) and completion and open-ended questions on theoretical concepts.

1. Review of the International System of Units. The atom: atomic particles (protons, neutrons, electrons); mass number and atomic number. Atomic dimensions: the angstrom, relative atomic mass, and the atomic mass unit. The mole and Avogadro’s number. Isotopes: definition, properties, and atomic mass. Ions.
2. Overview of atomic models: Thomson’s model, Rutherford’s model, Bohr’s model, and the current atomic model.
3. Quantum numbers, electron configuration, and Lewis structures.
4. The periodic table of the elements: history and characteristics. Periodicity of the properties of the elements and determination of oxidation numbers.
5. Review of matter, mass, and weight. Pure substances (elements and compounds) and allotropes. Classification of the elements (metals, nonmetals, metalloids, noble gases). 6. Molecular compounds and the representation of molecules; ionic compounds (empirical formulas, nomenclature of cations, anions, and polyatomic ions). Mixtures (homogeneous and heterogeneous).
6. Solutions: characteristics and units of concentration. Theory and exercises on molarity, molality, mass percentage (weight %), volume percentage, mass-volume percentage, parts per million, and dilutions.
7. Chemical reactions: characteristics and the Law of Definite Proportions (Proust’s Law). Stoichiometry and balancing of chemical equations. Oxidation-reduction (redox) reactions: characteristics and balancing.
8. Acids and bases: Arrhenius theory, Brønsted–Lowry theory, the concept of conjugate acids and bases, and amphoteric electrolytes. Ka: acid and base strength and ionization constants. The ionic product of water. pH and pOH. Calculation of pH for monoprotic acids and strong bases.
9. Buffer solutions: pH of a buffer solution and the Henderson–Hasselbalch equilibrium/equation. The blood buffer system.
10. Systematic and traditional formulas and nomenclature of chemical compounds.

At the end of the course, students will be able to: describe the atomic and molecular structure of matter; interpret atomic models and explain the periodicity of element properties; correctly apply the concepts of mole, molar mass, concentration, and stoichiometry; recognize and classify chemical reactions, balance them, and calculate quantitative relationships; understand the concepts of acidity, basicity, and buffers, including pH calculations in different contexts; use systematic and traditional chemical nomenclature; communicate chemical concepts clearly and rigorously, both orally and in writing.