Chemistry

Undefined

The contents of theoretical matter are presented in theory lessons, being then applied to practical exercises done in practical lessons.

The objectives defined for the Curricular Unit of Chemistry relate to its fundamental, generalist and pedagogical support role. The approach and development is based on the students’ specific level of knowledge, in view of their applicability to the study of chemical applications. It is intended to provide students with an understanding of the fundamentals of chemistry that it is underlie the transformation and characterization of the matter and the structures that it forms.

With this curricular unit it is intended that the students develop the skills, attitudes, behaviours, methodologies and the best practices, scientific reasoning and that they be able to:
●understand the basic concepts of chemistry, chemical bonds and mass relationships in chemical reactions, state of matter, chemical and thermochemistry equilibrium;
● identify the precipitation, complex formation, acid-base and redox reactions and understand the mechanism underlying to the respective titrations.

1. Basic concepts. Electronic configuration of atoms and ions. Periodic table. Quantic numbers and atomic orbitals. Energy of atomic orbitals.

2. Chemical bonds and nomenclature. Ionic bond. Covalent polar bonds, nonpolar and dative. Inorganic molecular compounds. Lewis structures.

3. Mass relationships in chemical reactions. Atomic masses. Avogadro number and molecular weight. Percent composition of the compounds and mixtures. Chemical reactions and chemical equations. Settlement of chemical equations. Stoichiometry. Limiting reagent. Reagent with impurities. Yield of the reaction.

4. States of matter: gases, liquids and solids. Characteristics and properties of gaseous state, liquid state, solid state.

5. Reactions in aqueous solution. Solution settings, solute and solvent. Electrolytic properties. Composition of solutions: Molarity, molality, normality and others. Dilution and ratio solution / diluent (solvent). Precipitation reactions (molecular equations and Ionic Equations), precipitation and complexation equilibria and their titrations. Acid-base reactions (acids and bases, their definitions and properties) and acid-base titrations. Oxidation-reduction reactions (settlement the redox reactions) and oxidation-reduction titrations.

6. Chemical and physical changes of the reactions: energy, kinetic and equilibrium. Thermochemical. Endothermic and exothermic reactions. Enthalpy and thermochemical reactions. Stoichiometry and thermochemical equivalences. Kinetics of chemical reaction. Chemical balance. Chemical equilibrium concepts and equilibrium constant. Prediction the direction of a reaction. Calculation of the equilibrium concentrations. Factors affecting the chemical equilibrium. Le Chatelier’s principle. Equilibrium solubility.

NAO

Chang, R. (1994). Química. (5ª edição). Lisboa : McGraw-Hill. (Disponível na Biblioteca do ISEC: 6-1-114 )

Atkins, P., Jones L. (1997). Chemistry : molecules, matter and change.(3th Ed.). New York : Freeman and Company (Disponível na Biblioteca: 6-1-123 (ISEC) – 08684 )

Atkins, P.W. (1998). Physical Chemistry. (6th ed.) Oxford University Press, Oxford. (Disponível na Biblioteca do ISEC: 6-5-47 (ISEC) – 09344 )