00130 - General Inorganic Chemistry

Learning outcomes

At the end of the course, students will have acquired a solid foundation in chemistry and will be prepared to undertake the study of more specialized areas of the discipline.

In particular, upon completion of the lectures, students will be familiar with the fundamental principles of General and Inorganic Chemistry, including: atomic structure, periodic properties of the elements, the formation and nature of chemical bonds, molecular geometry and properties, chemical reactions, and the states of matter and their properties. Students will also understand the principles of thermodynamics and ckinetics, as well as equilibria in liquid phase, with particular emphasis on acid–base and solubility equilibria. Finally, students will gain an understanding of the fundamentals of electrochemistry and redox reactions.

Upon completion of the practical sessions, students will be able to correctly draw Lewis structures of simple molecules, determine their molecular geometry and physicochemical properties, and solve quantitative problems involving stoichiometry, chemical equilibrium, pH and buffer solutions, thermodynamics and chemical kinetics, electrochemistry, and redox reactions.

Course contents

Introduction. Organization of lectures and assessment methods. Overview of the course contents. Introduction to chemistry, its tools, and its objectives.

Atomic structure and properties. Properties of matter. Physical and chemical changes. Pure substances and mixtures. Elements and compounds. Dalton’s atomic theory. Atoms and molecules. Electrical nature of matter: electrons, protons, and neutrons. Atomic number and mass number. Isotopes. Ions. Kinetic and potential energy in atomic systems. Electromagnetic radiation and the electromagnetic spectrum. Wave and particle nature of light: the photoelectric effect and the Planck–Einstein equation. Wave and particle nature of matter: electron diffraction and the de Broglie equation. Hydrogen emission and absorption spectra and energy quantization. Bohr atomic model. Emission and absorption spectra of multi-electron atoms. Heisenberg uncertainty principle. Quantum-mechanical description of the atom and the Schrödinger equation. Quantum numbers and atomic orbitals. Visualization of the wave function. Hydrogen-like atoms and orbital energies as a function of the principal quantum number. Multi-electron atoms: shielding effect and orbital energies as a function of the azimuthal quantum number. Dependence of orbital energies on quantum numbers. Electron configurations and the organization of the periodic table. Periodic properties of the elements: atomic radius, ionization energy, and electron affinity. Metals and non-metals.

Chemical bonding and states of matter. Chemical bonding: energy in a diatomic system. Valence bond theory. Sigma and pi bonds. Hybridization of atomic orbitals. Bonding and non-bonding electrons. Electron pair repulsion and molecular geometry. Lewis structures for the prediction of molecular structures. Electronegativity. Electric dipole moment. Molecular geometry and the VSEPR model. Formal charges and oxidation numbers. Resonance structures. Exercises on Lewis structures. Polar covalent bond. Ionic bond. Hard-sphere model and crystal packing. Atomic and ionic radii. Madelung constant. Properties of ionic solids. Intermolecular forces. Polarizability. Hydrogen bonding. Kinetic molecular theory of ideal gases. Ideal gas equation of state. Phase transitions. Phase diagrams. Vapor pressure. Surface tension. Capillarity. Viscosity.

Chemical transformations. Stoichiometry. Chemical equations. Mass relationships in chemical reactions. Atomic mass scale. Percent composition of compounds. The mole and molar mass. Limiting reagent. Reaction yield. Numerical exercises and problems in stoichiometry. Mixtures. Solutions and dispersions. Electrolytes. Concentration units. Colligative properties of solutions. Osmosis. Solubility of gases in water. Chemical reactions and equilibrium. Chemical thermodynamics. Thermodynamic systems. Work and heat. Internal energy and enthalpy. Gibbs free energy and reaction spontaneity. Numerical exercises and problem solving.

Chemical equilibria in aqueous solution. Reaction quotient. Equilibrium constant. Le Chatelier’s principle. Numerical exercises and problem solving. Equilibria in aqueous solutions. Autoionization of water. pH. Acids and bases according to Arrhenius, Brønsted–Lowry, and Lewis. Acid dissociation. Base hydrolysis. Strength of acids and bases. Numerical exercises and problem solving. Acid–base reactions. Buffer solutions. Effect of dilution. Numerical exercises and problem solving. Heterogeneous equilibria and solubility. Solubility product. Common-ion effect. Selective precipitation of metal ions. Numerical exercises and problem solving.

Electrochemistry. Oxidation–reduction reactions and electrochemistry. Electromotive force. Reduction potentials. Nernst equation. Numerical exercises and problem solving. Concentration cells. Standard electrodes. Spontaneity of redox reactions. Numerical exercises and problem solving. Balancing oxidation–reduction reactions. Numerical exercises and problem solving.

Chemical kinetics. Reaction rates. Rate laws. Reaction order. Rate constants. Reaction mechanisms. Collision theory. Activation energy. Arrhenius equation. Multistep reactions. Catalysis. Integrated rate laws for zero-, first-, and second-order reactions. Numerical exercises and problem solving.

Readings/Bibliography

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

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

Credi, Del Zotto, Gasparotto, Marchetti, Zuccaccia "VIAGGIO NELLA CHIMICA" Casa EditriceEdiSES

Marcì, Palmisano, Ruffo "STECHIOMETRIA" Casa EditriceEdiSES

Teaching methods

Teaching activities will consist of lectures supported by slides, videos, and computer-based animations for the visualization of molecules and materials. Classroom problem-solving sessions will be held throughout the course to develop students' skills in solving quantitative chemical problems and numerical exercises.

Assessment methods

Assessment is based on a written examination consisting of a series of multiple-choice questions and numerical exercises covering the topics addressed during the course. The examination is designed to assess students’ knowledge of the fundamental principles of General Chemistry, their ability to apply these principles to problem solving, and their correct use of scientific terminology. At the end of the written examination, the solutions to the exercises and questions will be presented and discussed.

Teaching tools

The multimedia materials used during the lectures will be made available to students for download from the instructor’s website.

Students with specific learning disorders (SLD) or temporary or permanent disabilities are encouraged to contact the relevant University Office in a timely manner (https://site.unibo.it/studenti-con-disabilita-e-dsa/it ). The Office will propose any necessary accommodations for the students concerned. Such accommodations must be submitted to the teacher for approval at least 15 days in advance. The teacher will assess their appropriateness in relation to the learning objectives of the course.

Office hours

See the website of Luca Mazzei