CHIMICA E PROPEDEUTICA BIOCHIMICA BETTELHEIM PDF
Chimica E Propedeutica Biochimica Bettelheim Pdf Download by Nbulugero, released 26 October Chimica E Propedeutica Biochimica. libro chimica e propedeutica biochimica. EDISES autori: Bettelheim brown campbell e farrel. 5 years agoPalermo, Italia. martinapoli Come sono le condizioni. CHIMICA E BIOCHIMICA BIOLOGIA E GENETICA – channel 1 PICCIN. 2. Chimica e Propedeutica Biochimica – Bettelheim, Brown, Campbell, Farrel – EdiSES.
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Skip to main content. People search Search with a name Search with a name. Text size Normal Large. Atomic theory and electronic structure of the atoms. Ionic and covalent bond theories. Acids, Bases, and Salts-Ionic Equilibria. Thermodinamic and Kinetic principles.
General characteristics and reactivity of the main organic chemical groups. Torres EdiSES lecture notes Educational objectives This teaching is the first rigorous approach to the general and chi,ica chemistry.
The main objective of the course is provide to the students the basic concepts of general chiica organic bettepheim as a description of nature, an appropriate scientific language and the ability to study in a critical and reasoned way. The main knowledge gained will be: Prerequisites In order to understand and achieve the expected learning targets the student should possess skills of mathematics and physics.
In particular, the student should know and be able bettelhei, use some basic mathematical tools equivalence, linear and quadratic equations, logarithm, exponential function and notions of fundamental physics unit of measurement, force, energy. Teaching methods The course is organized as follows: The lessons will be conducted with the help of the blackboard and by the projection of slides.
The teaching material slides, exercises proposed during numerical exercitations are made available to students on the platform unistudium after registration. Learning verification modality The evaluation bettellheim the actual acquisition by students of the learning outcomes will be done through an oral exam.
The oral exam consists of questions on theoretical aspects related to the issues addressed in teaching and reported in the detailed program of the course.
Università degli Studi di Perugia
The purpose of the oral exam is to assess the knowledge, the understanding and the discipline language acquisition. Moreover, the ability of the student to explain the theoretical aspects and to apply the skills acquired in more complex systems, correlated to the program of teaching, is verified.
Extended program General Chemistry Homogeneous and heterogeneous systems. Solutions, simple and compound systems. Constitution chimmica the atom, atomic number, mass number, nuclei, isotopes, elements.
Scale of atomic masses. Avogadro constant and the mol.
Molar scale of atomic masses. Minimal and molecular chemical formula. Outline on elemental analysis. Principle of atom conservation. Fundamentals of Quantum Mechanics.
The quantum numbers and spin.
Orbital and energy levels. The principle of Aufbau, the Hund rule, the Pauli exclusion principle. Electronic structure of the elements. Atomic and ionic radius. Valence, electronegativity and oxidation number. Simple methods to determine the number of oxidation.
Metallic, semimetallic and metallic character.
Basic oxides and hydroxides. Acid oxides anhydrides proppedeutica, and oxoacids oxoanions. Classification betteheim chemical reactions. Redox and non-redox reactions. Formationdecomposition, combustion, displacement, and exchange reactions. Balancing of redox reactions with the ionic-electronic method in acid and basic aqueous solutions. Notes on ionic bonding. Description of the covalent bond with the valence bond method. Sigma and pi bonds. Simple, double and propedeutca bond. Expansion of valence sphere and the octet rule violation.
Structural formula of common molecules and molecular ions. Polarity of bonds, polarity of molecules. Hybridization of atomic orbitals. Homopolar and polar covalent bond. Molecular dipole moment as a vector sum of dipole moments of individual bonds. Study of the polarity of molecules. Polarity and molecular symmetry. Examples of typical systems. The hydrogen bond in water and its chemical and physical effects.
The hydrogen bond in proteins and in nucleic acids. General types of solids, classified by the nature of chemical bonding. The model of perfect gases.
State equation of perfect gases. Mixtures of perfect gases. Vapor pressure chmiica a liquid. Definition of equilibrium state. Dependence of vapor pressure on temperature.
Phase equilibria for gettelheim with a component. Normal melting and boiling temperatures. The bettelheij diagram of water and carbon dioxide. Le Chatelier’s principle of mobile equilibrium. Applications to phase equilibria.
Lowering the vapor pressure of the solvent. Cryoscopic lowering of melting temperature and ebullioscopic increase of cuimica temperature of the solvent. Characteristics of chemical equilibrium. Equilibrium constant and its properties. Prediction of reactivity based on the principle of Le Chatelier mobile equilibrium. Effects of perturbation of equilibrium: Equilibrium constant and reaction quotient. Dependence of equilibrium constant on temperature.
Equilibrium solubility in aqueous solution. Effect of an ion in common. Definition of acid and base according to Bronsted-Lowry. Strong and weak acids and bases. Relative strength of acids and bases. Dissociation constants Ka and Kb and Kw and their relationship. Calculations of equilibrium concentration of typical aqueous acid-base systems: Determination of equilibrium constant of the reaction of neutralization.
Buffer solutions and mechanism of the buffering. Calculations for the determination of the equilibrium concentration in the buffers. Definition of Lewis acids and bases. Comparison with Bronsted theory. Typical Lewis acids and bases. Outline of complexation reactions and the formation of coordination compounds according to the acid-base Lewis theory.
Concept of energy, heat and work. Isolated, closed bkochimica open systems. The first principle of Thermodynamics. Enthalpy chimicz standard enthalpy. Exothermic and endothermic processes. Second and third principle of thermodynamics.