00130 - General Inorganic Chemistry

Learning outcomes

At the end of the course the student will have an understanding of the fundamental concepts of General and Inorganic Chemistry. In particular, the student will be knowledgeable about atomic and molecular structures, the periodic table and chemistry of some elements, the different types of chemical bonding, elements of nomenclature of chemical compounds, the aggregation states of matter (gas, liquid and solid), the phase diagrams, the thermodynamics of chemical reactions and chemical equilibra, the properties of solutions, acid-base reactions, pH, buffer solutions, hydrolysis, solubility products, oxidoreduction reactions, electrochemistry, chemical kinetics. The student will also be able to solve all types of problems related to equilibria and stoichiometry. The student will be able to communicate orally and in writing on the main themes of the discipline, using appropriate scientific terminology, in order to possess the necessary tools to deal with the subsequent courses that involve chemical, biochemical and pharmaceutical topics.

Course contents

Atomic structure, energy, electromagnetic radiation, wave-particle dualism, quanta and photons, uncertainty principle, wave functions, energy levels, atomic models, quantum numbers, Bohr model of the hydrogen atom, electronic structure of multi-electron atoms, electronic configuration, periodic table and periodic properties. The nature of the chemical bond, valence bond theory, covalent bond, Lewis formalism, bonding and non-bonding electron pairs, resonance, formal charge, bond order, octet rule, radicals, molecular electric dipole, polar covalent bond, electronegativity, bond length and bond energy, polarizability, molecular structure, VSEPR model, hybridization of atomic orbitals. Ionic bond and crystal lattices. Intermolecular forces and their electrostatic nature, properties of solids and liquids, hydrogen bond and the structure of water. Properties of ideal and real gases. Thermochemistry, thermodynamic system, thermodynamic state, internal energy, work, heat, thermal capacity, temperature, reaction enthalpy, entropy, Gibbs free energy. The chemical equilibrium, equilibrium constant, state diagrams, solubility, colligative properties. Gas phase equilibria, Le Chatelier principle. Aqueous phase equilibria. Acids and bases, self-protolysis of water, acid/base conjugate pairs, pH, pOH, acidity scale, weak and strong acids and bases, solution pH, polyprotic acids, buffers, acid/base titrations. Heterogeneous equilibria and solubility. Redox reactions, galvanic cells, cell potential, Nernst equation. Chemical kinetics, reaction rate, kinetic law, order of reactions, activation energy, Arrhenius law, catalysis.

Readings/Bibliography

Atkins, Jones, Laverman "PRINCIPI DI CHIMICA" Casa Editrice Zanichelli

Bertini, Luchinat, Mani, Ravera "STECHIOMETRIA" (VI edizione) Casa Editrice Zanichelli

 

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.

Assessment methods

The final examination comprises either i) two partial tests or ii) a final test made of 10-15 multiple choice questions (1 point each) and 5-6 problems, with partial credit for partial answers, to ascertain the level of knowledge of the student, as well as a colloquium. Access to the colloquium is not prevented if the test is failed, but the test outcome will be considered to determine the final grade. No partial tests will be carried out through the teaching period. The final grade is the average of the written and the oral exam.

Teaching tools

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

Office hours

See the website of Stefano Luciano Ciurli