63708 - General and Inorganic Chemistry with Laboratory

Learning outcomes

Students will gain an understanding and a knowledge of the fundamental concepts of chemistry and stoichiometry. They will acquire the skills necessary to work in a chemical laboratory and be able to correlate their experimental data with chemical reactivity.

Course contents

1- Brief introduction to atomic structure- Atomic mass- Introduction to chemical forces and bonds- Molecules- Molecular, covalent, metallic and ionic solids- Molecular mass- Mol- Chemical reactions and conservation of mass- Elemental analysis- Nomenclature- Heat of reaction and conservation of energy 2- The gaseous state and deduction of its laws from experiments- The molecular kinetic theory and the inductive scientific methods- Interpretation of pressure and temperature of a gas- Mixtures of gases and Dalton law of partial pressures- Graham law of diffusion and applications- Real gases and Van der Waals equation. 3- Homogeneous chemical equilibrium- Definitions of concentration- Law of Guldberg-Waage- Equilibrium constants and their use- Heterogeneous equilibrium- The le Chatelier principle 4- Equilibria in solution- Ionic product of water- pH- Definitions of acids and bases- Solutions of strong acids and bases and their pH- Solutions of weak acids and bases and their pH- Polyprotic acids- Hydrolysis of salts and pH- Buffered solutions and titration. 5- Solubility- Ionic salts- Solubility product and effect of common ions and pH. 6- Thermochemistry- Introduction to chemical thermodynamic- Enthalpy and bond energy- Entropy and disorder- Free energy and spontaneity of chemical reactions- Free energy and equilibrium constants- Effect of temperature on equilibrium constants. 7- Introduction to kinetic: rate of reaction- reaction order and mechanism- Effect of temperature on reaction rate- Catalysis. 8- Electrochemistry: Chemical energy and electrical work- Electrochemical cells- Standard potentials- Latimer diagrams- Nernst equation- Electrolysis- Overtension- Corrosion. 9- Changes of state and state diagrams- Properties of solutions. Azeotropes- Distillation- Colligative properties and their effect in day life. 10- Earlier atomic models and their conflict with classical physical laws and experimental data- Waves and particles- Atomic model of Schroedinger and outlines for solving the electron wave equation- Quantic numbers- Orbitals- Electronic configuration of atoms- Derivation of periodic table- Atomic properties. 11- The chemical bond in molecules according to the lewis method- Resonance- Lewis acids and bases- Molecular geometry- VSEPR theory. 12- Molecular orbitals- Sigma and pi bonds- MO of diatomic homonuclear and heteronuclear molecules- Bond order- Electronegativity- Dipole moments- Polyatomic molecules according to MO and VB methods- Hybrid orbitals- Application of VB method to sigma bonds and MO method to pi bonds to interpret a series of inorganic and organic molecules with delocalized bonds. 13- Intermolecular forces and molecular solids- Covalent solids- Allotropy and relations structure-properties- Insulators, semiconductors and conductors- The metallic bond. 14- Properties and chemistry of element of groups 1 and 2. 15- Properties and chemistry of most important elements of groups 13-17.

Genaral and inorganic chemistry laboratory

Safety in the chemical laboratory. SI units of measurement. Uncertainty in measurements. Significant figures. Names and formulas of inorganic compounds. The mole. Percent composition of compounds. Empirical and molecular formulae. Chemical equations and their balance. Oxidation numbers. Stoichiometric calculations based on chemical equations. Yields from chemical reactions. The limiting reactant concept. Chemical equilibrium in gas phase. Properties of solutions and their concentrations. Molar fraction. Heterogeneous equilibrium: solubility product. Ionic equilibrium. Autoionization of water. Acid and base solutions. pH. Ionization constants for weak monoprotic acids and bases. Buffers. Acid-base titration curves. Electrochemistry: standard reduction potentials; voltaic and electrolytic cells; the Nernst equation.

 

Readings/Bibliography

• R. E. Dickerson, H. B. Gray, G. Haight, "Principi di Chimica", Zanichelli Editore, Bologna.
• D. W. Oxtoby, N. H. Nachtrieb, “Chimica Moderna”, EDISES, Napoli
• K. H. Whitten, R. E. Davis, M. L. Peck, G. G. Stanley, “Chimica Generale”, Piccin, Padova .
• Lucidi e appunti di lezione.
• I. Bertini, C. Luchinat, F. Mani: "Stechiometria",  Ambrosiana 5° ed.
• Michelin Lausarot, G. A. Vaglio: " Stechiometria per la Chimica Generale", Piccin

 

Teaching methods

Lectures integrated with numerical exercises. The course is divided in four phases. The first phase (ca. 6 hours) introduces the objectives of the course and gives a brief description of the nature of matter and its transformations with the aim to learn the chemical language and nomenclature. The second phase (ca. 30 hours) presents the phenomena and their quantitative handling with the help of introductory numerical exercises. The third phase (ca. 20 hours) is devoted to the comprehension and interpretation of behaviour and phenomena, object of the second phase. The fourth phase (ca. 10 hours) describes the most significant aspects of the chemistry of s and p elements, and interprets their behaviour with theories and models learned in the third phase. A tutor will be available two hours per week to help students in solving exercises and override encountered difficulties.

Assessment methods

The exam is integrated with that of the course of Laboratory of General and Inorganic Chemistry. It consists in a written test and an oral colloquium at the end of semester. Monthly written examinations during the semester can substitute the final written test.

Teaching tools

Blackboard, overhead and video projector.

The experimental parts will take place in the chemical laboratory.

Office hours

See the website of Giuliano Longoni

See the website of Cristina Femoni

See the website of Maria Carmela Iapalucci