GENERAL AND INORGANIC CHEMISTRY
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- Versione italiana
- Academic year
- 2022/2023
- Teacher
- ALESSANDRA BOSCHI
- Credits
- 9
- Didactic period
- Secondo Semestre
- SSD
- CHIM/03
Training objectives
- The course aims to present the theoretical and experimental foundations of the chemical sciences and provide an elementary introduction on the role of the molecular paradigm in the interpretation of biological phenomena.
The main knowledge acquired during the course is: fundamentals of atomic and molecular theory; elementary Introduction to quantum-mechanical description of atoms and molecules; phenomenological theory of ideal gases; elementary introduction to the description of solids, liquids and solutions; fundamentals of classical thermodynamics; elementary thermodynamic description of chemical reactions; elementary description of acid-base, redox and precipitation reactions; fundamentals of electrochemistry; periodic properties of the most important elements for biology; introduction to simple operations in the chemistry laboratory.
The main skills acquired during the course are: interpretation of fundamental properties of the elements; interpretation of structure and properties of molecules; stoichiometric calculations; calculation of properties of gases and solutions; calculation of equilibria in aqueous solution; calculation of thermodynamic potentials; ability to correctly describe and discuss experimental observations and results. Prerequisites
- Although no preparatory learning is required, Students are strongly encouraged to achieve the following background: basic mathematical concepts of elementary algebra and basic physical concepts.
Course programme
- Atomic and molecular theory (25 hours), Scientific method and fundamental concepts of classical physics, Chemical elements and compounds, Laws of chemical combination of elements, Daltons atomic theory, Relative atomic weights of elements. Atoms and molecules, Empirical formula, Molecular formula, Molecular weight (mass), Mole, Molar weight (mass). Rutherfords atomic model, Elementary particles, Proton, Neutron, Electron, Atomic number Mass number, Isotopes,Types of chemical compounds, Binary compounds with hydrogen, Oxides, Acid and basic oxides, Amphoteric oxides, Peroxides, Salts, Formula weight, Oxidation states (numbers). Chemical reactions, Acid-base reactions, Redox reactions, Law of mass conservation, Law of charge conservation, Balance of a chemical reaction, Stoichiometric calculations, Balance of a redox reaction. Black-body radiation, Plancks hypothesis, Energy quantization, Bohrs atomic model, Photoelectric effect. Elementary introduction to quantum mechanics, De Broglies hypothesis, Wavelike model of hydrogen atom, Quantum probability, Quantum numbers, Atomic orbitals, Electron spin, Paulis exclusion principle, Multi-electron-atom configurations. Periodic Table of Elements, Periods and groups, Metallic and non-metallic elements. Chemical bond, Valence, Lewis theory, Electronic pairs, Lewis structures and resonances, Formal charges, Exceptions to octet rules. Molecular geometry, Valence-shell electron pair repulsion (VSEPR) model, Electronegativity, Polar molecules. Fundamentals of valence bon theory, s e p bonds, Hybrid orbitals, Molecular geometries and hybridization.
States of matter (5 hours)
The gaseous state, The variables PVT, Ideal gases, Absolute temperature, Avogadros hypothesis, State equation of ideal gases, Real gases, Van der Waals equation. Solid state, Ionic and molecular solids, Covalent solids, Metallic solids, Structure of solid water, Hydrogen bond, Interpretations of the hydrogen bond. Liquid state, Polar and non-polar liquids, Solutions, Concentration of solutions, Evaporation, Vapor pressure, Ideal solutions, Raoults law, Real solutions. Phase transitions, Phase diagrams, Phase diagram of water and carbon dioxide, Critical temperature, Colligative properties of solutions.
Chemical reactions (20 hours)
Chemical reactions, Chemical equilibrium. Self-ionization of water, Ionic product of water, pH and pOH, Acids and bases, Broensted-Lowry definition, Acid and base dissociation constants, Buffer solutions. Solubility of salts, Solubility product, Calculations of the solubility of salts.
Thermodynamic and electrochemistry (14 hours)
Introduction to thermodynamic theory, Heat and temperature, Conservation of energy, First principle of thermodynamic, Internal energy, State functions, Reversible and irreversible transformations, Isothermal processes, Adiabatic processes, Isobaric processes, Internal energy of an ideal gas, Enthalpy, Hess Law, Conversion of heat into mechanical work, Entropy, Time-reversible and -irreversible processes, Spontaneous and irreversible processes, Second principle of thermodynamics, Interpretation of entropy, Clausius inequality, Thermodynamic interpretation of temperature, Molecular interpretation of entropy, Statistical thermodynamics, Boltzmanns equation, Third principle of thermodynamics. Gibbs free energy, Vant Hoff equation, Standard free energy.
Free energy and electrical work, Electrochemical cells, Electrochemical potential, Nernst equation, Standard hydrogen electrode, Electrolysis, Electrolytic cells.
Chemistry laboratory (8 hours)
Observation of the course of selected chemical reactions, Preparation of solutions, Measuring the pH of aqueous solutions, Titrations, Instrumental methods for pH determination. Didactic methods
- The course has the following organization (in the absence of limitations related to the health pandemic): theoretical lessons, deepening of theoretical issues in the classroom, resolution of numerical problems in the classroom, laboratory experiments carried out through the implementation of tours in laboratory tests. Students perform the proposed experimental test independently. Before the execution, the principles of the experiment are presented and discussed with the Students. During the course of the experiment, students can consult a written guide describing the various phases and operations of the experimental procedure.
Learning assessment procedures
- The purpose of the examination is to ascertain the level of understanding and deepening of the arguments developed during the course. It is also intended to evaluate Student's ability to follow a logical reasoning and to draw consistent conclusions from abstract principles underlying the chemical theory, and to employ correctly the scientific language.
The exam consists of a written test that requires the resolution of 10-13 theoretical and numerical problems. During the exam, the student will be able to consult the periodic table, a form (maximum 2 A4 pages) and the calculator. Each question will be clearly attributed a score. There will be 33 total points . A minimum score of 33 will be given praise. Reference texts
- Modern chemistry
David W. Oxtoby, H. P. Gillis, Alan Campion
(Thomson Brook/Cole)
Chemical principles - the quest for insights
di Peter Atkins, Loretta Jones
(W. H. Freeman and Co.)
General chemistry: principles and modern applications
Ralph H. Petrucci, F. Geoffrey Herring, Jeffry D. Madura, Carey Bissonnette
(Pearson Education Canada, Inc.)
Lecture notes distributed by the teacher.
