Learning objectives
Knowledge and understanding.
The Course of General and Inorganic Chemistry intends to provide, on the basis of the interpretation and analysis of experimental data, the fundamental concepts needed to conduct the study of Biology. The theoretical treatment of many topics is followed by stoichiometric calculations that facilitate the understanding and deepening of chemical phenomena.
Applying knowledge and understanding.
The educational objective of the course is to come to acquire a simple language that can express clearly and with scientific rigor the development of a practical event and place in relation to the theoretical concept.
Knowledge and understanding (D1). The student will acquire the basic chemical knowledge needed to undertake studies at the molecular level of biological aspects proposed in more advanced courses. The student will know the basic concepts of: formulations and nomenclature of compounds, properties of elements and their compounds, relationship between stable electron configuration and the formation of bonds, intermolecular forces and their influence on macroscopic properties of matter. The student will learn to recognize the structural characteristics of simple compounds. The student will learn the theories used to describe the typical characteristics of the states of matter. The student will learn the fundamentals of thermodynamics, electrochemistry, chemical kinetics, and their applications. The student will learn to perform numerical calculations (solve stoichiometry problems) which are usually made in laboratories during the practical execution of a chemical analysis, in this way the student will be facilitated in the understanding and deepening of the fundamental aspects of basic chemistry.
Prerequisites
- - -
Course unit content
1) Matter and energy.
2) The law of periodicity.
3) The chemical bond.
4) States of matter.
5) The solutions and their properties.
6) Chemical equilibrium.
7) Oxidation-reduction.
8) The energy of the chemical transformations.
9) Chemical Kinetics.
10) Complements of inorganic chemistry and inorganic biochemistry.
Full programme
1) Matter and energy.
Description of matter. Chemical and physical phenomena. Energy. The atomic structure of matter. Introduction to atomic and molecular structure. Discovery and electron properties. Electromagnetic radiation. Dual nature of light. The atomic nucleus. Isotopes. The line spectrum of hydrogen atom. Bohr’s theory. Uncertainty principle.
2) The law of periodicity.
Distribution of electrons in atoms. Quantum theory. Interpretation of atomic spectra. Quantum mechanics theory. Atomic orbitals. The periodic table of the elements. Periodic properties.
3) The chemical bond.
Ionic bond. Covalent bond. Homonuclear diatomic molecules. Multiple bonds. Localized molecular orbitals. Hybrid orbitals. Dipole moments. The method of Lewis and VSEPR theory. The valence bond method. The molecular orbital method. Resonance and delocalization of charge. The metallic bond. The hydrogen bond. Van der Waals interactions.
4) States of matter.
General remarks on the structure of matter. Perfect gas equation of state. Absolute zero and absolute temperature scale. Law of partial pressures. The Kinetic theory of gases. Law of gaseous diffusion. Changes of state. Evaporation and saturated vapour pressure. Boiling. State or phase diagrams. Phase rule. Binary systems formed by liquids miscible in all relationships. Fractional distillation. General remarks on the structure of crystals. Symmetry elements. Use of X-ray analysis of crystal structures. X-ray diffraction by crystals. Ionic crystals, covalent crystals and molecular crystals. Metallic crystals and metallic bond. Lattice energy.
5) The solutions and their properties.
Solubility. Dependence of solubility from pressure and temperature. Ideal and real solutions. Raoult’s law. Vapour pressure of solutions. Concentration of a solution. Colligative properties of solutions. Osmosis.
6) Chemical equilibrium.
Gas phase equilibria. Kinetics and equilibrium. Heterogeneous chemical equilibrium. Phase rule. Equilibrium in solution. Water ionization and ionic product. Acidity and basicity in terms of pH and pOH. The concept of acid and base according to Bronsted-Lowry. Relative strengths of acids and bases. Dissociation equilibrium of weak acids and weak bases. Polyprotic acids. Hydrolysis. Buffer solutions. Experimental determination of pH. Indicators. Titration. Solubility product. Lewis theory of acid and bases.
7) Oxidation-reduction.
Electrolyte solutions and their properties. Quantitative laws of electrolysis (Faraday’s law). Specific conductivity and molar conductivity. Mobility of ions. Galvanic cells. Concentration cells. Electrochemical series. Acidic storage batteries. Fuel cells. Overvoltage.
8) The energy of the chemical transformations.
Equilibrium states of a system. The first law of thermodynamics. Work and heat. Enthalpy. Thermochemistry. Heats of formation. Entropy. Free energy and equilibrium constant. Thermodynamics and biochemistry.
9) Chemical Kinetics.
Order of a reaction. Speed of reaction and concentration. Speed of reaction and temperature. Collision theory. Theory of the activated complex. Reaction mechanism. Catalysis and catalysts.
10) Complements of inorganic chemistry and inorganic biochemistry.
Main elements of the I, II, III, IV, V, VI, VII group and of transition.
Written exercises on the following topics: stoichiometry.
Chemical reactions. Equivalent weight. Normality. Ways to express the concentration of a solution. Redox reactions. Principles of volumetric analysis. Equilibria in solutions. pH. Buffer solutions. Titration curves. Choice of the indicator.
Bibliography
J. C. Kotz, P. M. Treichel, J. R. Townsend. Chemistry&chemical reactivity. VII Ed., 2009. Thomson Brooks/Cole.
P. Michelin Lausarot, G. A. Vaglio. Stechiometria per la chimica generale, 2005. PICCIN (PD).
I. Bertini, C. Luchinat, F. Mani. Stechiometria un avvio allo studio della chimica. 5° edizione, 2009. C. E. A. (MI).
Teaching methods
Class lectures and exercises.
Assessment methods and criteria
Written (problems) and oral exam.
The exam consists of a written test and an oral test. During the exam written the student will have to solve six problems similar to those carried out during the course. The duration of each written test is three hours. Starting from the day after the trial, in the presence of the student, each individual written paper will be correct and commented on. The student, at the time of delivery, chosen freely twenty minutes by affixing his signature on the “correction calendar” prepared by the teacher, in which the task will be correct. If the outcome reported is positive (sufficient, discreet, good, excellent) the student will be able to take the oral test, otherwise will have to be redone the written proof. Within one year of the date of passing the written test, the student must agree with the teacher on the date of the oral. After the oral examination, the overall vote (final vote) will be proposede, considering both the results of the written and oral tests. If the student accepts the final grade, it will be recorded.
Other information
- - -
