Unit CHEMISTRY
- Course
- Economics and culture of human nutrition
- Study-unit Code
- GP000457
- Curriculum
- In all curricula
- Teacher
- Anna Donnadio
- Teachers
-
- Anna Donnadio
- Hours
- 81 ore - Anna Donnadio
- CFU
- 9
- Course Regulation
- Coorte 2022
- Offered
- 2022/23
- Learning activities
- Base
- Area
- Discipline chimiche
- Academic discipline
- CHIM/03
- Type of study-unit
- Obbligatorio (Required)
- Type of learning activities
- Attività formativa monodisciplinare
- Language of instruction
- Italian
- Contents
- Introduction to the general chemistry. Atomic theory and electronic structure of the atoms. Molecular geometries. Ionic and covalent bond theories. Intermolecular forces. Chemical reactions. State of matter: solid, liquid, gas. Equilibrium. Acids, Bases, and Salts-Ionic Equilibria. Electrochemistry. Thermodinamic and Kinetic principles. General characteristics and reactivity of the main organic chemical groups.
- Reference texts
- L. Palmisano, G. Marcì, A. Costantini, G. Luciani, M. Schiavello
Elementi di Chimica - II Edizione
EdiSES
W.H. Brown, M.K. Campbell, S.O. Farrell
Elementi di Chimica Organica - II Edizione
EdiSES
lecture notes - Educational objectives
- This teaching is the first rigorous approach to the general and organic chemistry. The main objective of the course is provide to the students the basic concepts of general and organic chemistry 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:
- Atomic theory and electronic structure of atoms.
- Chemical bond and molecular geometries.
- Intermolecular forces.
- Chemical reactions.
- Chemical equilibrium in the gas phase and in aqueous solution.
- Criteria to establish the spontaneity of chemical reactions.
- Main functional groups of organic compounds and their reactivity
The main skills (ability to apply the knowledge acquired):
- Identify and be able to write formulas of inorganic compounds;
- Represent inorganic and organic molecules or molecular ions highlighting the orientation of the atoms and the bonds between them;
- Predict the reactivity of inorganic and organic compounds;
- Write and describe the qualitative aspects of a chemical reaction. - 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 to 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:
- Lectures on all the topics of the course. The lessons will be conducted with the help of the blackboard and by the projection of slides.
- Numerical exercitations in classroom for the guided solution of numerical exercises with the aid of the blackboard.
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 of 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. 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 of the atom, atomic number, mass number, nuclei, isotopes, elements. Atomic mass. Scale of atomic masses. Isotopic abundancy. Average atomic mass. Avogadro constant and the mol. Molar scale of atomic masses. Minimal and molecular chemical formula. Combination ratios. Weight percent composition. Outline on elemental analysis. Chemical reactions. Principle of atom conservation. Complete reactions.
Fundamentals of Quantum Mechanics. The wave function. 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. Electronic configurations. The periodic table. Periodic properties. Atomic and ionic radius. Ionization energy. Electron affinity. Valence, electronegativity and oxidation number. Simple methods to determine the number of oxidation.
Metallic, semimetallic and metallic character. Hydrides and oxides. Basic oxides and hydroxides. Acid oxides (anhydrides), and oxoacids (oxoanions). Nomenclature. Formation of salts. Classification of chemical reactions. Redox and non-redox reactions. Formation , decomposition, 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. Octet rule. Simple, double and triple bond. Dative bond. Electrondeficient molecules. Expansion of valence sphere and the octet rule violation. V.S.E.P.R. method and molecular geometry. Hybridization. Structural formula of common molecules and molecular ions. Polarity of bonds, polarity of molecules. . Hybridization of atomic orbitals. sp, sp2 and sp3 hybrids. Pi bonds. Polarity of bonds. Dipole moment. 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.ion-ion, ion-dipole (dissociation and solvation of ionic solids), permanent dipole-permanent dipole, permanent dipole-induced dipole, instantaneous dipole-induced dipole (van der Waals forces and London dispersion forces). Concept of polarizability. Examples of typical systems. Hydrogen bond. Examples of intermolecular / intramolecular hydrogen bonds. 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.
Gases: the nature and definition of pressure. Units of measurement. The model of perfect gases. State equation of perfect gases. Mixtures of perfect gases. Partial pressure. Dalton's law.
Liquids. Vapor pressure of a liquid. Liquid-vapor equilibrium. Definition of equilibrium state. Dependence of vapor pressure on temperature. Clausius-Clapeyron. Solid-vapor equilibrium. Phase equilibria for systems with a component. Phase diagrams. Triple point. Normal melting and boiling temperatures. The phase diagram of water and carbon dioxide. Concept of variance. Perturbations of equilibria. Le Chatelier's principle of mobile equilibrium. Applications to phase equilibria.
Solutions. Concentration. Measure unit:% by weight,% by volume, mole fraction, molarity, molality Dissociation of solutes. Types of solutes: strong electrolytes, weak electrolytes, non-electrolytes. Degree of dissociation. Van t'Hoff Binomial.
Colligative properties: vapor pressure of solutions Raoult's law , both volatile two components and the case of two components, one of which is non-volatile. Lowering the vapor pressure of the solvent. Cryoscopic lowering of melting temperature and ebullioscopic increase of boiling temperature of the solvent. Osmotic pressure. Operational definition. Semipermeable membranes. Isotonicity.
Chemical equilibrium. 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: variation of concentration, pressure, volume and temperature. Equilibrium constant and reaction quotient. Dependence of equilibrium constant on temperature. Van t'Hoff Equation.
Equilibrium solubility in aqueous solution. Concept of solubility. Solubility product. Effect of an ion in common.
Acid-base equilibria. Definition of acid and base according to Bronsted-Lowry. Acid-base reactions. Ampholytes. Autoprotolysis reactions. Water autoprotolysis Equilibrium. Kw. Strong and weak acids and bases. Relative strength of acids and bases. Dissociation constants Ka and Kb and Kw and their relationship. Polyprotic acids. pH and the pH scale. Calculations of equilibrium concentration of typical aqueous acid-base systems: strong and weak acid solutions and bases. Neutralization reaction. 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. Henderson-Hasselbach equation. Lewis acid-base theory. 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.
Thermodynamics. Concept of energy, heat and work. The egocentric convention. Isolated, closed and open systems. Internal energy. The first principle of Thermodynamics. Enthalpy and standard enthalpy. Heat and enthalpy. Exothermic and endothermic processes. Status functions. Second and third principle of thermodynamics. Gibbs Free Energy.
Organic chemistry
functional group concept. Resonance. Alkanes. Isomerism of organic molecules. Atomic conformation. Basic principles on the reactivity, Introduction to organic reactivity. Alkenes: structure and reactivity. The reaction of electrophilic addition. Aromatic compounds: aromaticity concept, structure and reactivity of aromatic compounds. The electrophilic aromatic substitution reaction
Elements of organic stereochemistry: stereoisomery, enantiomers and diastereoisomers.
Functional groups: amines, alcohols, aldehydes and ketones, carboxylic acids.
Derivatives of carboxylic acids: acid halides, anhydrides, esters and amides.