27711 - Laboratory of General and Inorganic Chemistry L

Learning outcomes

Fundamental concepts concerning the atomic structure, the Periodic Table and the principal chemical properties of the elements, the chemical bond, the formation of molecules and ions, the intermolecular forces and condensed states of matter. The comprehension of matter and energy balances associated to a chemical reaction. The chemical equilibrium and the spontaneity of a reaction. Rate and mechanisms of chemical reactions.

Course contents

The contents are closely related with those of the General and Inorganic Chemistry course.

1) Historical view of the atomic theory, atomic and molecular weights, the mole and the Avogadro's number, molecular and empirical formulas, elemental analysis, balancing chemical equations, nomenclature of compounds. 2) The properties of gases, the ideal gas law, gas mixtures and Dalton's law of partial pressures, the kinetic molecular theory of ideal gases, Graham's law, deviations from ideal behaviour and the Van der Waals equation for non ideal gases. 3) Thermochemistry: energy, heat and work, the first law of thermodynamic, enthalpy and Hess's law, heat of a reaction, standard heats of formation. 4) The chemical equilibrium, equilibrium constants, le Chatelier's principle, heterogeneous equilibrium. 5) Acids and bases, Brönsted-Lowry acid base concept, pH, relative strengths of acid and bases, pKa and pKb, hydrolysis, polyprotic acids and bases, buffer solutions, acid base indicators, acid base titrations. 6) Solubility, equilibrium constants for slightly soluble salts, the common ion effect, solubility and pH. 7) The electronic structure of atoms: the nature of light, Planck equation and the photoelectric effect, origin of spectral lines, the hydrogen spectrum and the Rydbergh equation, Bohr's theory of hydrogen atom, many electron atoms, waves and particles dualism, De Broglie equation, the uncertainty principle, quantum numbers and the distribution of electrons in atoms, the Periodic Table, ionisation energy and electron affinity, atomic radius, ionic radius, chemical properties of oxides. 8) The chemical bond, Lewis theory of bonding, the octet rule, Lewis acid base concept, shapes of molecules and VSEPR theory. 9) The molecular orbital concept, the hydrogen molecule, sigma and pigreco bond, OM of diatomic molecules, bond order, bond polarity, electronegativity, polyatomic molecules, hybrid atomic orbitals, bond energies. 10)Intermolecular forces, dipole moments, molecular solids, ionic bond, Van der Waals forces, hydrogen bond, enthalpy of hydration. 11)Chemical Kinetics, determining reactions orders and rate constants, mechanism of a reaction, catalysis. 12)The spontaneity of a reaction, the second and third laws of thermodynamics, entropy enthalpy and free energy, relationships between free energy and equilibrium constant. 13)Electrochemistry, spontaneous oxidation-reduction reactions, galvanic cells, reversible electromotive force, the Nernst's equation, the scale of half-cell potentials, electromotive force and equilibrium constant, electrolysis. 14)The condensed states of matter, vapour pressure, changes of states, the phase diagram, solutions, Raoult's law, colligative properties, boiling point elevation and freezing point lowering, osmotic pressure. 15)The chemistry of Group I and II elements. Periodic properties in boron, carbon, nitrogen, oxygen and fluorine groups. Numerous practical experiences will be carried out in laboratory concerning the topics previously described

Readings/Bibliography

Stechiometria, un avvio allo studio della Chimica, I. Bertini, F. Mani, Casa Editrice Ambrosiana.

Exercises and lessons notes will be soon available at http://amscampus.cib.unibo.it/

Teaching methods

Lessons in classroom accompanied by suitable exercises and practical experiences in laboratory and by tutorial activities

Assessment methods

The examination is made up of a written test, with numerical applications, followed by an oral exam. It is possible to make written tests "in itinere" during the lessons. The course of "General and Inorganic Chemistry" and the correspondent Laboratory course are carried out through an joint examination that assignes one mark.

Teaching tools

Lessons in classroom accompanied by suitable exercises and practical experiences in laboratory.

Office hours

See the website of Stefano Stagni