Applied Chemistry

The theoretical classes aim at the detailed presentation of the syllabus, using an expositive-active methodology. The contents are exposed calling for constant student intervention and analytical calculations will be made. In practical classes laboratory experimental procedures will be performed by the students, such as preparation of solutions, solubility equilibrium and titration.
Continuous assessment includes two assessment instruments: a written test regarding the evaluation of the theoretical component and a written test regarding the evaluation of the practical component.
The final grade is obtained by the weighted average of the two corresponding matrices: T matriz 75%; PL matrix 25%. The classification obtained in each matrix must be at least 9/20 values.
Students also have a normal exam time where the assessment takes on a global character (theoretical and theoretical¬practical component), also in the form of a written test, as well as a period of appeal and special time.

The student must acquire skills on:
Identification of the major inorganic and organic compounds.
Perform analytical calculation related to chemical equilibrium, as acid-base equilibrium.
Applied Chemistry, as an integrated discipline, allows the student to familiarize with the structures and common occurring chemical schemes within the general chemistry and organic chemistry. On the other hand, the analytical calculation concerning the content taught it is an important and extensive part. So, the conclusion of this course
should provide the student with a high degree of calculation capacity to perform mathematical operations that allow with some deftness the application of acquired knowledge. The main purpose of this syllabus it is the creation of an interface between the taught knowledge and chemical phenomena with the major aim of helping to assimilate them into
various disciplines that rely upon this same knowledge as far as theoretic levei and laboratory practical experiments.

Inorganic compounds (phosphates, sulfates, nitrates and nitrates, carbonates, oxygenated compounds).
Organic compounds (hydrocarbons, alcohols, ethers, aldehydes and ketones, carboxylic acids, amines, amides).
Structural isomerism and stereoisomerism. Chemical Bonding (ionic bonding and covalent bonding, hybridization). Molecular geometry. Intermolecular forces.
Concentration of solutions (weight, volume and mass/volume percentages, molarity, molality, mole fraction, normality, dilution factor). Properties of dilute solutions. Chemical equilibrium. Nature of chemical equilibrium. Equilibrium constants, Kp and Kc. Equilibrium constants interpretation. The ideal law of chemical equilibrium. The reaction
quotient. Analytical calculations. Acid-base equilibria. Theories. Strength of acids and bases. pH scale. pH indicators and changing colour moment. Titrations. Theory of the pH calculations on severa’ titrations. Buffer solutions. Buffer capacity and buffer effect. Analytical calculations.

NAO