43049 - General Inorganic Chemistry

Learning outcomes

At the end of the course, the students will know the fundamental principles of General and Inorganic Chemistry. In particular, they will understand the structure of the atom, the properties of the elements and their ability to form compounds, molecular structures, chemical reactions, energy exchanges, states of matter, chemical kinetics, solution equilibria, acid–base properties, and electrochemistry.

Course contents

Introduction:

Organization of lectures and examination methods. Introduction to the topics covered in the program. Presentation of chemistry, its tools, and its objectives.

Structure and properties of the atom:

Properties of matter. Physical and chemical transformations. Pure substances and mixtures. Elements and compounds. Dalton’s atomic theory. Atoms and molecules. Electrical nature of matter: electrons, protons, neutrons. Atomic number, mass number. Isotopes. Ions. Kinetic and potential energy in the atomic system. Electromagnetic radiation and the electromagnetic spectrum. Wave and particle nature of light: photoelectric effect and Planck–Einstein equation. Particle and wave nature of matter: electron interference and the De Broglie equation. Emission and absorption spectra of hydrogen and quantization of energy. Bohr’s atomic model. Emission and absorption spectra of multielectron atoms. Heisenberg’s uncertainty principle. Probabilistic theory of the atom and the Schrödinger equation. Quantum numbers and atomic orbitals. Radial and angular functions. Illustration of the wave function. Hydrogen-like atoms and orbital energies as a function of the principal quantum number. Multielectron atoms: shielding effect and orbital energies as a function of the secondary quantum number. Dependence of atomic orbital energies on quantum numbers. Electron configurations and the organization of the periodic table of the elements. Periodic properties of the elements: atomic radius, ionization energy, and electron affinity. Metals and nonmetals.

Chemical bonding and the states of matter:

Chemical bonding: energy in the diatomic system. Valence bond theory. Sigma and pi bonds. Hybridization of atomic orbitals. Bonding and nonbonding electrons. Electron pair repulsion and molecular geometry. Lewis formalism for predicting molecular structures. Electronegativity. Electric dipole moment. Molecular geometry and the VSEPR model. Formal charges and oxidation numbers. Resonance forms. Polar covalent bonding. Ionic bonding. Hard-sphere model and packing. Atomic and ionic radii. Properties of ionic solids. Intermolecular forces. Polarizability. Hydrogen bonding. Molecular kinetic theory of ideal gases. Ideal gas law. Phase transitions. Phase diagrams. Vapor pressure. Surface tension. Capillarity. Viscosity.

Chemical transformations:

Stoichiometry. The concept of a chemical equation. Mass relationships in chemical reactions. Atomic mass scale. Percent composition of a compound. The mole and molar mass. Limiting reagent. Reaction yield. Solving exercises and numerical problems in stoichiometry. Mixtures. Solutions and dispersions. Concept of electrolyte. 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. Solving exercises and numerical problems.

Chemical equilibria in the gas phase and in aqueous solution:

Reaction quotient. Equilibrium constant. Le Chatelier’s principle. Solving exercises and numerical problems. Equilibria in aqueous solution. Autoprotolysis of water. pH. Acids and bases according to Arrhenius, Brønsted–Lowry, and Lewis. Acid dissociation. Basic hydrolysis. Strength of acids and bases. Solving exercises and numerical problems. Acid–base reactions. Buffer solutions. Effect of dilution. Acid–base titrations. Colorimetric acid–base indicators. Solving exercises and numerical problems. Heterogeneous equilibria and solubility. Solubility product. Common-ion effect. Selective precipitation of metal ions. Solving exercises and numerical problems.

Electrochemistry:

Redox reactions and electrochemistry. Electromotive force. Reduction potentials. Nernst equation. Solving exercises and numerical problems. Concentration cells. Standard electrodes. Spontaneity of a redox reaction. Solving exercises and numerical problems. Balancing redox reactions. Solving exercises and numerical problems.

Chemical kinetics:

Reaction rate. Rate law. Reaction order. Rate constant. Reaction mechanism. In-depth work with software dedicated to visualizing reaction mechanisms. Collision theory. Activation energy. Arrhenius equation. Multistep reactions. Catalysis. Integration of rate laws for zero-, first-, and second-order reactions. Solving exercises and numerical problems.

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

Teaching methods

The lectures will be conducted using computer-guided projections of slides and videos, as well as animations from computational and visualization software for molecules and materials. Classroom exercises will be carried out to familiarize students with solving problems and numerical exercises.

Assessment methods

Assessment of learning is carried out through a final written exam consisting of a series of multiple-choice questions and several exercises. Students who pass the written test with a score between 18/30 and 30/30 may request that this result be recorded. Alternatively, the student may request to improve the written test result by taking an individual oral exam. The oral exam will build on the topics covered in the written test and will include all the subjects in the syllabus, consisting both of numerical exercises and discussion of theoretical topics.

Teaching tools

The material used during the lectures will be made available to students by downloading it from Virtuale.

Students with specific learning disorders (SLD) or temporary/permanent disabilities are advised to contact the University Office in charge in advance (https://site.unibo.it/studenti-con-disabilita-e-dsa/it ). The office will advise the students concerned on any possible accommodations, which must in any case be submitted to the teacher for approval at least 15 days in advance. The teacher will assess their suitability, also in relation to the learning objectives of the course.

Office hours

See the website of Luca Mazzei