00088 - Chemistry

Learning outcomes

At the end of the course, the student knows the basic principles of general chemistry and the chemical properties of elements and compounds, which are necessary for the study of geological processes and materials. The student can : - utilize the IUPAC nomenclature, SI units, concentration expressions; - describe the atomic structure of the elements and classify compounds on the basis of the different kinds of chemical bond; - perform stoichiometric calculations using mole, concentration, pH, solubility; - apply the principles of chemical equilibrium to homogeneous and heterogeneous systems, and illustrate the properties of the different aggregation states; - use the Periodic Table to identify the characteristics of the main elements and of their inorganic compounds.

Course contents

Prerequisites. Basic mathematical functions: roots, power of and logarithms. Solutions of algebraic equations, Knowledge of the principal physical tenets, their correlation with each other and their measure units.

Introduction. Chemical and physical properties of matter. States of aggregation and phases.

Atoms. The fundamental laws of chemistry. Subatomic particles. Atomic number and mass number. Isotopes. Mole. Wave-particle dualism and quantum-mechanical model of atom; quantum numbers and their meaning, orbital shells and sub-shells, electronic configurations.

The Periodic Table. Periodic properties. Dimensions of atoms and ions, ionization energy, electronic affinity and interpretation of their periodic behavior.

Name of inorganic compounds. Chemical compounds. Oxidation numbers. Name of inorganic compounds.

Stoichiometry. Chemical reactions, chemical equations and their balancing. Reactions in solution. Concentration in solution and dilution. Redox reactions and their balancing. Combustion reactions. Titrations. Limiting reagent and reaction yield.

Chemical bond. Electronegativity. Compounds characteristics as a function of chemical bonds. Ionic bond: reticular energy, Born-Haber cycle. Covalent bond: octet rule, Lewis structures, multiple bonds, resonance, partial and formal charges, molecules geometry, valence bond model, hybrid orbitals. Metallic bond. Intermolecular bonds and hydrogen bond.

Gases. Properties of gases, laws of gases, ideal gas law, Dalton law on partial pressures. Ideal and real gases.

Chemical equilibrium. Haber process. Law of mass action. Relation between Kp and Kc. Principle of Le Chatelier. Homogeneous and eterogeneous equilibria.

Equilibria in solution. Dissociation of water and pH. Properties and strength of acids and bases. pH calculations for strong and weak acids and bases, salts and pH of their solutions. Buffer solutions. Solubility and solubility product. The common ion effect. Titration curves; pH indicators.

Phase diagrams. Phase diagrams of pure substances: equilibrium curves, triple point, critic point.

Liquids and solutions. Vapor pressure and liquid properties. Colligative properties. Osmotic pressure.

The solid state. Physical properties of solids. Crystal structures. Ionic, covalent, molecular and metallic solids. Polymorphism and isomorphism. 

Fundamentals of Inorganic Chemistry. Overview on the chemical properties of the principal elements as a function of their position in the Periodic Table. Elements and compounds of high geological relevance.

Readings/Bibliography

The topic treated in this course can be found in any recent university textbook of general chemistry.

See, for exemple: L. Palmisano G. Marci, A. Costantini, G. Luciani, M. Schiavello, Elementi di Chimica EdiSES.

For numerical exercises: Anfuso, Palmisano, Guida per la Risoluzione di Esercizi di Chimica, EdiSES.

Teaching material is provided, available through username and password at VIRTUALE - Online teaching support - University of Bologna.

Teaching methods

Lectures with the use of PowerPoint presentations. Exercises aimed to solve stoichiometry problems. Laboratory experiments.

Numerical exercises and laboratory activity are focused to acquire practical skills.

In consideration of the types of activities and teaching methods adopted, the attendance of this training activity requires the performance of modules 1 and 2 in e-learning mode and participation in module 3 of specific training on safety and health in places of study. Information on dates and methods of attendance of module 3 can be consulted in the specific section of the degree program website.

Assessment methods

Written and oral tests.

Written test presents numerical problems. The minimum mark requested to proceed to the oral exam is 18/30. Oral test is aimed at verifying the acquired knowledge and skills.

On written tests only pen, scientific calculator and periodic table of elements are admitted.

Teaching tools

Blackboard, PC, video projector, powerpoint presentations, laboratory instruments and tools.

The slides used in the lectures can be downloaded as PDF files from the Virtuale platform. Texts of problems and exercises will be available in the same platform.

Office hours

See the website of Elisa Boanini