00130 - General Inorganic Chemistry

Learning outcomes

At the end of the course the student:
- possesses basic knowledge of atomic structure, chemical bonding, solution properties, the main chemical reactions and the thermodynamic and kinetic elements that characterize them;
- is able to trace the geometric structure and nomenclature of inorganic compounds;
- knows how to balance chemical reactions from reactants, predicting their spontaneity;
- is able to apply the acquired knowledge to the solution of problems peculiar to the profession.

Course contents

Introduction: Lectures organization and exams. Introduction to the topics discussed during the course. Presentation of the subject of Chemistry, its tools and its goals.

Structure and proprerties of the atom: The properties of matter. Physical and chemical changes. Elements, compounds and mixtures. Dalton’s atomic theory. Atoms and molecules. Electric nature of matter: electrons, protons and neutrons. Atomic number, mass number. Isotopes. Ions. Kinetic and potential energy in the atom. Electromagnetic radiation and spectra. Wave-particle dualism: photoelectric effect and Plank-Einstein equation. Corpuscular and undulatory nature of matter: electron interference and De Broglie equation. Emission and absorption spectra of hydrogen and energy quantization. Bohr model of the hydrogen atom. Emission and absorption spectra of polyelectronic atoms. Heisenberg's uncertainty principle. Probabilistic theory of the atom and Schroedinger's equation. Quantum numbers and atomic orbitals. Wave function. Hydrogenidal atoms and orbital energy as a function of the main quantum number. Polyelectronic atoms: screen effect and energy of the orbitals as a function of the secondary quantum number. Energy dependence of atomic orbitals as a function of the quantum number. Electronic configurations and organization of the periodic table of elements. Periodic properties of elements: atomic radius, ionization energy and electronic affinity. Metals and not metals.

The chemical bond and the aggregation states of matter: The chemical bond: energy in the diatomic system. Valence bond theory. Sigma and Pi bonds. Hybridization of atomic orbitals. Bonding and non-bonding electrons. Repulsion of electronic pairs and molecular geometry. Lewis formalism for the prediction of molecular structures. Electronegativity. Moment of electric dipole. Molecular geometry and VSEPR model. Formal charges and oxidation number. Resonance forms. Resolution of exercises on Lewis formulas. Molecular orbital theory. Paramagnetism and diamagnetism. HOMO, LUMO. Schemes of molecular orbitals of homo- and hetero-nuclear molecules. Polar covalent bond and molecular orbitals. Ionic bond. Theory of rigid spheres and packing. Atomic radius and ionic ray. Madelung constant. Metallico bond. Properties of ionic solids. Intermolecular forces. Polarizability. Hydrogen bonds. Molecular kinetic theory of ideal gases. Equation of state of ideal gases. State transitions. State diagrams. Vapor pressure. Surface tension. Capillarity. Viscosity.

Chemical transformations: Stoichiometry. Concept of chemical equation. Mass relationships in chemical reactions. The relative atomic mass. Percent composition of a compound. The mole and the molar mass. Limiting reagent. Yield of a reaction. Resolution of exercises and numerical problems on stoichiometry. Chemical reactions and equilibria. Thermodynamics. Work and heat. Internal energy and enthalpy. Enthropy. Gibbs free energy and spontaneity of a reaction. Reaction quotient. Equilibrium constant. Gas-phase equilibria. K_p and K_c. Le Chatelier's principle. Resolution of exercises and numerical problems.

Chemical equlibria in aqueous solution: Solutions and dispersions. Electrolyte concept. Unit of concentration. Van't Hoff coefficient. Colligative properties of solutions. Osmosis. Solubility of gases in water. Equilibria in aqueous solution. Self-ionization of water. pH. Acids and bases according to Arrhenius, Brønsted-Lowry and Lewis. Aqueous solutions of acids and bases. Dissolution of weak acids and bases. Strength of acids and bases. Acid-base reactions. Buffer solutions. Effect of dilution. Polyprotic acids and bases. Acid-base titrations. Acid-base colorimetric indicators. Complex ions and instability constant. Heterogeneous equilibria and solubility. Solubility product. Effect of the ion in common. Selective precipitation of metal ions. Resolution of exercises and numerical problems.

Electrochemistry: Electrochemical reactions. Electromotive force. Reduction potentials. Nernst's equation. Galvanic cella. Standard electrodes. Spontaneity of a redox reaction. Resolution of exercises and numerical problems. Balancing redox reactions.

Chemical kinetics: Reaction rate. Kinetic law. Reaction order. Rate constant. Reaction mechanism. Collision theory. Activation energy. Arrhenius equation. Multistage reactions. Catalysis. Integration of the kinetic rate laws of order zero, one and two. Resolution of exercises and numerical problems.

Readings/Bibliography

Bertini, Luchinat, Mani, Ravera "Chimica" Casa Editrice CEA

Credi, Del Zotto, Gasperotto, Marchetti, Zuccaccia "Viaggio nella Chimica" Casa Editrice EdiSES

Arnesano, Bandoli, Bisceglie, Dolmella, Maggioni, Musiani, Natile, Natile, Tesauro "Chimica di Base" Casa Editrice EdiSES

Bertini, Luchinat, Mani, Ravera "Stechiometria" Casa Editrice CEA

Del Zotto "Esercizi di Chimica Generale" Casa Editrice EdiSES

Pacifico, Margiotta "Esercizi risolti (e non) di Stechiometria" Casa Editrice EdiSES

Teaching methods

The lectures will involve the use of presentations through a beamer driven by a PC. Multimedial material will be presented, such as slides, movies, animations and three-dimensional visualization of atoms, molecules and materials. Problem solving sessions will be carried out in order for the student to gain acquaintance with the numeric treatment of chemical problems.

Please note that it is necessary to attend at least 60 percent of the lectures to be eligible for the exam. Attendance will be collected via QRcode generated using the University's "Presenza Studenti" application.

Assessment methods

The assessment of learning occurs through a final examination, in which the acquisition of the expected knowledge and skills is ascertained through the performance of a preliminary written test lasting one hour, the performance of a written test lasting 2 hours, followed by an interview. The examinations will be conducted without the aid of notes or books.

The preliminary written test consists of 15 multiple-choice questions worth 2 points each. Achieving a sufficiency in the preliminary written test (i.e. correctly answering at least 9 out of 15 questions) is necessary to gain access to the written test. The written test consists of 4-8 problems (the scoring of which depends on the difficulty of the individual problem and which award partial points for partial answers). The mark for the written test is calculated as the arithmetic average of the preliminary written test and the written test.

A minimum score of 18 points in the written test is not required to be admitted to the oral test, but is strongly recommended. The final grade is calculated as the arithmetic average of the written test and the oral test.

Please note that, in order to be admitted to the examination, it is mandatory to attend at least 60% of the lesson hours. Attendance is verified at each lesson by means of a QRcode.

Teaching tools

The multimedial material utilized during the lectures will be made available for download from the teacher's web site.

Students are asked to report any needs to the teacher via private mail. This will allow the teacher to evaluate which teaching support tools are most adequate to make the course accessible to all students.

Office hours

See the website of Francesco Musiani