Chemistry

Undefined

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

With this curricular unit it is intended that the student is able to: i) understand the basic concepts of chemistry, chemical bonds and mass relations in chemical reactions, state of matter, thermochemistry and chemical equilibrium; ii) identify precipitation, complexation, acid-base, oxidation-reduction reactions and understand the mechanism underlying the respective titrations; iii) identify the functional groups of organic compounds and their properties; iv) determine the structure of an organic compound from its name and vice versa

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.

7. Nomenclature of organic compounds.

1) In addition to the final exams there is a continuous assessment, written, with the following components:
1.1) Two written mini-tests, marked up to the 2nd week of classes, to which a minimum of 75% attendance is required in all theoretical and theoretical-practical classes, which were taught until the date of each test;

1.2) The Final Classification of the Curricular Unit will result from the following equation: CFinal = 0,5 × T1 + 0,5 × T2, where T1 is the classification obtained in the 1st test, T2 the classification obtained in the 2nd test.

2) If the student chooses not to carry out a continuous evaluation or opting out, he/she may take the full exam at any of the times provided for in the ISEC school calendar.
2.1) The final grade will be the best of the marks between the continuous evalutation Tests or the total exam.

NAO