Study-unit GENERAL CHEMISTRY
Course name | Biological sciences |
---|---|
Study-unit Code | GP004014 |
Curriculum | Comune a tutti i curricula |
Lecturer | Enrico Ronca |
Lecturers |
|
Hours |
|
CFU | 7 |
Course Regulation | Coorte 2023 |
Supplied | 2023/24 |
Supplied other course regulation | |
Learning activities | Base |
Area | Discipline chimiche |
Sector | CHIM/03 |
Type of study-unit | Obbligatorio (Required) |
Type of learning activities | Attività formativa monodisciplinare |
Language of instruction | Italian |
Contents | Concepts of matter and energy. Units of measure. the structure of the atom and molecules. Responsiveness of the elements and periodic table. Chemical nomenclature and chemical reactions. chemical bond. The states of matter (liquid, solid, gaseous). The chemical kinetics and the speed of reactions. The solutions. The chemical balance. The balances of solubility in watery solution and acid-base balances. Redox reactions. |
Reference texts | -Schiavello, Palmisano. Fondamenti di Chimica Edises VI Edizione -Nivaldo J. Tro Chimica Un approccio molecolare. Edises, III edizione. -Chimica J. C. Kotz, P. M. Treichel, J. R. Townsend e D. A. Treichel Edises, VII edizione. |
Educational objectives | The course of chemistry aims to provide, as main training objective, an appropriate basic knowledge of the following contents: -Knowing how to balance chemical reactions and adequately use of mole concept. -Understanding the properties and responsivenes of the elements of the periodic table. -Having a basic knowledge of the atomic structure, the electronic properties and the main characteristics of the chemical bond. -Knowing how to do stoichiometric calculations on solutions. -Knowing how to calculate the pH of acidic and basic solutions. -Understanding the behaviour of chemical species in oxidation-reduction reactions. |
Prerequisites | The general chemistry course is one of the fundamental subjects of the first year of the course of study. The prerequisites for satisfactorily addressing the study of chemistry are: -An appropriate knowledge of arithmetic, algebraic rules and logarithmic calculations. -Appropriate knowledge of the use of physical quantities and conversion factors. -Adequate capacity of analysis and synthesis of the contents provided by the teacher. -Autonomy in the personal deepening of the formative contents. |
Teaching methods | Theoretical lectures with the help of slides and numerical exercises on the blackboard. |
Other information | The course is held at Porcellati Room in Via del Giochetto. Slides of the course will be available on-line. |
Learning verification modality | The exam consists in passing a final written test at the end course. Subsequently, for those who have passed the written tests with a grade equal or higher than 16/30 there will be oral test on the topics of the course apt to to confirm or improve the grade of the written test. In case of need due to the pandemic, the exam will take place remotely through the LibreEOL platform. For those who pass this test with a grade equal or higher than 16/30 there will be an oral integration on the Teams platform in order to confirm or improve the grade of the written test. For information on support services for students with disabilities and/or DSA visit the page http://www.unipg.it/disabilita-e-dsa |
Extended program | Introduction to matter and energy: homogeneous and heterogeneous systems. Solutions, simple substances and compound substances. Constitution Of the atom, atomic number, mass number, nuclei, isotopes, elements. Atomic masses. Atomic weights Scale. Isotopic abundance. Defect in mass. Average atomic weight. Avogadro's constant and mole concept. Chemical formulas: Minimal formulas and molecular formulas. Reports of Combination. Percent composition by weight. Analysis overview Elementary. Chemical reactions. Balance. Preservation principle Atoms. Complete reactions and with limiting reagent. Energy, Heat and work. Isolated, closed and open systems. The electromagnetic spectrum. Internal energy. The first principle of thermodynamics. Enthalpy and Standard enthalpy. Warmth and enthalpy. Exothermic and Endotermal processes. Status functions. Energy of physical water transformations. Fundamentals on Atomic theory: Atomic spectra. The hydrogen atom According to Bohr. Quantum mechanics. Wave Nature of the electron. The wavefunction. The quantum numbers and the spin. Orbitals and Energy levels. The principle of Aufbau, the Hund rule, the principle of Pauli exclusion. Electronic structure of the elements. Configurations Electronic. The periodic table. Periodic properties. Effect of Shielding and effective nuclear charge. Radius and atomic volume and Ionic. Ionization energy. Electronic affinity. Valencia Electronegativity and oxidation number. Simple Methods for Determine the oxidation number. Average oxidation number. Basic reactivity of elements. Metallic, Semimetallic and Non-metallic. Hydrides and oxides. Basic oxides and hydroxides. Acid oxides (anhydrides), Oxyacids and Oxianions. Nomenclature. Formation of salts. Overview To the acid and basic behaviour of the substances. Classification of Chemical reactions. Redox and non-redox reactions. Training reactions, decomposition, combustion, displacement, exchange. Balance Of redox reactions with ionic-electronic method in aqueous environment Acid and Basic. Ionic and molecular reaction. Disproportions. Molecular structure and chemical bonds: hints on the ionic bond. Description of the covalent bond with the valence bond method. Sigma ties and more Greek ties. Octet rule. Simple Bond, Double and triple. Dative bond. Electron-deficient molecules. expansion Of the valence sphere and violation of the octet rule. Method V.S.E.P.R. and molecular geometry. Hybridization. Formulas of structure of Common molecules and the most common molecular ions. Resonance. Polarity of Covalent bonds. Dipole moment. Definition and unit of measure. Covalent polar and homeolar bond. Intermolecular interactions: Ioneione, Ion-dipole (dissociation and solvatation of ionic solids), dipole Permanent-permanent dipole, permanent dipole-induced dipole, dipole Instantaneous-induced dipole (Van der Waals forces and dispersal forces of London). Hydrogen Bridge bond. Molecular examples of binding a Intermolecular and intramolecular hydrogen bridge. The bridge link Hydrogen in the water and its chemical-physical effects. The bridge link Hydrogen in proteins and nucleic acids. The states of matter: solids. General information about the types of solids classified According to the nature of the chemical bond: Metallic Solids (properties Fundamentals, model of the Sea of electrons), Ionic (property Fundamental, dissociation, solvatation), covalent (property Fundamental, dimensionality of covalent solids according to the directions Propagation in the space of covalent bonds), molecular (properties Fundamental, intermolecular interactions). Gases: Nature and pressure definition. Unit of measure. The pressure Atmospheric. The perfect gas model. Perfect gas energy. Law of Maxwell-Boltzmann on the distribution of molecular energies. Dependence on the temperature of the energy distribution curves According to Maxwell-Boltzmann law. Laws of perfect gases. Perfect gas state equation. Perfect gas blends. Pressure Partial. Dalton's law. Molar fraction. Partial Volume. Liquids. Vapor pressure of a liquid. Liquid-vapor equilibrium. Definition of State of equilibrium. Dependence of the vapour pressure on the Temperature. Clausius-Clapeyron equation. Solid-vapor balance. Phase balances for systems to a component. Phase diagrams. Point Triple. Normal melting and boiling temperatures. The diagram of Phase of water and carbon dioxide. Variance concept. Perturbations of the equilibrium. Principle of the mobile balance of Le Chatelier. Applications to phase balances. Solutions. Concentration. Unit of measure:% by weight,% by volume, Molar fraction, molarity, molality. Ideal solutions. Definition of Ideal solution. Enthalpy of Intermination. Deviations from ideality. Dissociation of solutes. Types of solutes: strong electrolytes, weak electrolytes, Electrolytes. Degree of dissociation. Binomial of Van T'hoff. Property Colligative: Raoult's Law on the vapour tensions of the solutions; Case of Two components both volatile and case of two components of which one is Non-volatile: reduction of the solvent vapour pressure. Cryoscopic lowering of the melting and raising temperature Ebullioscopic of the solvent's boiling temperature. Pressure Osmotic. Operational definition. Semipermeable membranes. Solutions Isotonic. Osmosis. Chemical equilibrium. Characteristics of chemical equilibrium. Constant of Balance and its properties. Prediction of reactivity based on the principle Of the mobile balance of Le Chatelier. Effects of perturbations On balance: variation in concentration, pressure, volume and Temperature. Equilibrium constant and reaction quotient. Predictions of Reactivity. Reversible reactions and spontaneous reactions. Entropy. Definition. Second principle of thermodynamics. Variation of entropy for the System and the environment. Criterion of spontaneity and reversibility based On the variation of entropy. Entropy and order-disorder concept. Microscopic interpretation of entropy. Boltzmann equation. Microstate concept. Qualitative evaluation of the variation of Entropy for some chemical reactions. Third principle of Thermodynamics and scale of absolute entropies of substances. Energy Free G. Definition. Criterion of spontaneity and reversibility based on the variation of free energy at constant temperature and pressure. Energies Standard education free and standard training entalpies. Tables Thermodynamics and their use. Relationship between standard free energy variation and constant equilibrium. Van T'hoff's equation. Dependence of the equilibrium constant on the temperature. Chemical Kinetics. Kinetic equation. Constant speed. Order of reactions. Solubility balances in aqueous solution. Concept of solubility. product of solubility. Calculation of ionic equilibrium concentrations. Effect of Salt stoichiometry. Effect of the ion in common. Acid-base balances. Definition of acid and base according to Lowry-Bronsted. Acid-base reactions. Ampholytes. Reactions of autoprotolysis. Base acid headstocks. Saline hydrolysis. pH calculation of strong, weak and polyprotic acids. Property of the buffer solutions and mechanism of the effect of Tamponade. Calculations for the determination of concentrations of Balance in Buffer solutions Electrochemical. Galvanic and Electrolyic cells. Daniell stack. Closed and open circuit batteries. First and second species electrodes. Redox potentials. Nernst equation. |