1007777 - CHIMICA GENERALE ED INORGANICA A - L
Expected Learning Outcomes
The aim of the course is to provide the student with the knowledge of the basics of chemistry and with the understanding of related subjects developed in other courses of the Degree Program.
The student acquires the disciplinary and methodological know-how necessary to the basic technical and practical problem solving which he/she will use in the laboratory and in the subsequent courses.
The student acquires the ability to know and understand the General and Inorganic Chemistry in order to correctly write the most common chemical compounds, balance chemical reactions, calculate the concentration of solutions, describe the concept of chemical equilibrium and the pH of a solution.
The student develops critical ability in exercises solving, ability to communicate what was learnt, ability to continue the study in an autonomous way and critical abilities.
Course Structure
Lectures and exercises of stoichiometry.
Required Prerequisites
School knowledge of arithmetic and algebra, such as operations with rational numbers (real numbers). Solving of linear and quadratic equations, school knowledge of physics, such as vectors, speed and energy.
Attendance of Lessons
Detailed Course Content
1) Introduction - The 4 fundamental strenghts, matter and energy, states of matter*, homogeneous and heterogeneous systems, elements*, compounds* and mixtures*.
2) Fundamental Chemical Laws - Lavoisier's law of conservation of the mass, Proust's Law of definite proportions*, Daltom atomic theory, Dalton's Law of multiple proportions, Avogadro's Law, general knowledge on the atom, the atomic number* and the mass number*, isotopes*, a.m.u.*, atomic mass*, molecular mass*, mole*, weight percent composition.
3) Structure of matter – Rutherford, Bohr and Sommerfeld's atomic models. Theory of atomic orbitals*, Quantum numbers*, interpretation of the atom as a wave, atomic orbitals, Pauli's principle*, Hund's rule*, Heisenberg's uncertainty principle.
4) Periodic System - Periodicity and electron configuration*, ionization potential*, electron affinity*, electronegativity*.
5) Chemical bond* - ionic bond, covalent bond, dative bond, Lewis structures, valence, valence bond theory, orbital hybridization. Intermolecular bonds: hydrogen bond and Van der Waals forces.
6) Chemical nomenclature* - Chemical compounds, valence and oxidation number, chemical reactions and their balancing, redox reactions.
7) Gas phase - Partial pressures*, Dalton's Law*, Ideal gas law*, real gases.
8) Liquid phase - Properties, viscosity, surface tension, vapor pressure*.
9) Phase change - Phase Diagram for H2O* and CO2.
10) Solutions* - Molarity, normality, mole fraction, molality, mass percentage, density, vapor pressure, Raoult's law, colligative properties, electrolytes, degree of dissociation, Van’t Hoff coefficient.
11) Chemical equilibrium* - Law of mass action, equilibrium constant, relation between Kp and Kc, temperature dependence of the equilibrium constant, factors which influence the chemical equilibrium. Definition of exothermic, endothermic reaction and enthalpy change (H), spontaneity of a chemical equilibrium and free energy change (G).
12) Acids and bases* - Definition according to Arrhenius, Bronsted and Lowry, Lewis, acids and bases strenght, dissociation constant, amphoteric electrolytes, ion product of water, acidity, alkalinity and pH calculations, pH indicators.
13) Hydrolysis of salts - Hydrolysis constant, hydrolysis pH*, buffer solutions*, titrations strong-acid strong-base*, titrations weak-acid strong-base*, solubility and solubility product*.
14) Inorganic Chemistry - Chemistry of the main elements from I° to VII° group*, general properties of groups and periods*, chemical-physical properties of the main elements and of their most important compounds.
* fundamental topics to pass the exam.
Textbook Information
General and Inorganic Chemistry
1. P. Silvestroni - Fondamenti di chimica - undicesima edizione - CEA
2. P.W. Atkins, L. Jones, L. Laverman - Fondamenti di chimica generale – Seconda edizione - Zanichelli
3. J.C. Kotz, P.M. Treichel, J.R. Townsed - Chimica - quinta edizione - Edises
4. I. Bertini, C. Luchinat, F. Mani, E. Ravera - Chimica, struttura, proprietà e trasformazioni della materia- CEA
5. P. M. Lausarot, G.A. Vaglio - Stechiometria Guida alla soluzione di problemi di chimica- Piccin Esercitazioni a lezione
6. Slide projected at the lectures.
Course Planning
| Subjects | Text References | |
|---|---|---|
| 1 | Introduction to Chemistry, Matter and its properties, Compounds and Elements*, Fundamental Chemical Laws*, Avogadro's Law*. | T.3 I fondamenti , T.4: C.1 |
| 2 | Isotopes, a.m.u.*, Mole*, Chemical Formulae*, Atomic Theory, Rutherford's Model. | T.1: C.1 and 3, T2: Part 1, T.3 I fondamenti, T.4: C.1 and 2 |
| 3 | Exercises | T.5 |
| 4 | Bohr-Sommerfeld Model, Pauli's Principle*, Hund's Principle*, Quantum numbers*. | T.1: C.1, T.2: Part 1, T.3 C.1, T.4: C.2 |
| 5 | Heisenberg uncertainty principle, Periodic Table* (electron affinity, ionization potential, atomic radius, electronegativity). | T.1: C.1, T.2 Part 1, T.3 C.1, T.4: C.2 |
| 6 | Exercises | T.5 |
| 7 | Introduction to chemical bonds, ionic bond*, covalent bond | T.1: C.2, T.2: C.2 and C.3, T.3 Part 2, T.4: C. 3, 4 and 5 |
| 8 | Dative bond*, orbital hybridization and examples*, Valence and oxidation number*. | T.1: C.2, T.2: C.3, T.3 Part 2, T.4: C.3, 4 and 5 |
| 9 | Intermolecular bonds: hydrogen bond* and Van der Waals forces, Nomenclature and chemical reactions*. | T.1: C.2 and C.3, T.2: C.3, T.4: C.6 |
| 10 | Gas phase, Ideal gas*, Boltzmann distribution, Dalton's Law*, Gases Law*, Liquid phase*, viscosity, surface tension, vapor pressure*, Solutions and calculation of the concentration*. | T.1: C.5 and 6, T.2: C.3, T.3: Part 3, T.4: C.7 |
| 11 | Phase change, phase diagrams*, Raoult's Law, Colligative properties*, Dissociation degree*, Van't Hoff coefficient. | T.1: C.7 and C.8, T.2: C.3 e 5, T.3: Part 3, T.4: C.10 |
| 12 | Exercises | T.5 |
| 13 | Chemical Equilibrium*, Law of mass action*, equilibrium constant*, dependence of K from T, factors which influence the chemical equilibrium. Heterogeneous Equilibria (Clapeyron's Law), Exothermic, endothermic reactions and enthalpy change (H), Spontaneity of a chemical equilibrium and free energy change (G) | T.1: C.10 and 11, T.2: C.4 e 5, T.3: Part 4, T.4: C.11 |
| 14 | Ionic equilibria in solution*, Acid and base definition according to Arrhenius*, Bronsted Lowry* and Lewis*, pH of acids and bases*. | T.1: C.14, T.2:C.6, T.3: Part 4, T.4: C.12 |
| 15 | Exercises | T.5 |
| 16 | Hydrolysis of salts*, Hydrolysis constant, Buffer solutions*, titrations acid base* | T.1: C.15 e 16, T.2: C.6, T.4: C. 12 |
| 17 | Solubility and solubility product | T.1: C.15 e 16, T.2: C.6, T.4: C13 |
| 18 | Inorganic Chemistry - Chemistry of the main elements from I° to VII° group*, general properties of groups and periods*, chemical-physical properties of the main elements and of their most important compounds. | T.2: C.8 |
| 19 | Exercises | T.5 |
Learning Assessment
Learning Assessment Procedures
Separate written and oral exam.
Students will have to take a written test and will have 2 hours to complete 7 exercises. Passing the written test (mark greater than or equal to 18/30) is binding for access to the oral exam. The result of the written test will be averaged with the oral mark in order to determine the final mark.
The dates of the exams can be checked at the following link: http://www.dsf.unict.it/corsi/l-29_sfa/calendario-esami.
For the written and oral tests, students must bring a valid identity document. The use of mobile phones is absolutely NOT allowed during the tests, not even in calculation mode.
"Information for students with disabilities and/or SLD: To guarantee equal opportunities and in compliance with the laws in force, interested students can ask for a personal interview in order to plan any compensatory and/or dispensatory measures, based on the teaching objectives and specific needs. It is also possible to contact the referent teacher CInAP (Center for Active and Participated Integration - Services for Disabilities and/or SLD) of our Department, Prof. Teresa Musumeci.
Examples of frequently asked questions and / or exercises
Written exam:
Calculation of the pH of a solution of acids and bases.
Balancing of a redox reaction.
Calculation of colligative properties.
Calculation of the concentration of the solute in a solution.
Type of chemical bond in compounds.
Electron configuration of atoms and ions.
Molecular formula and Lewis structure of chemical compounds.
Oral exam:
Theory of acids and bases.
Equilibrium in solution (acid, base, hydrolysis).
Definition of buffer solutions, buffering capacity.
Redox reactions.
Chemical equilibrium and equilibrium constant.
Factors affecting the chemical equilibrium.
Metallic and non-metallic character of the elements.
Atomic orbitals.
Quantum numbers.
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