General and Inorganic Chemistry

It is recommended to have some knowledge in chemistry related to the programs taught in secondary grade, which include the subjects described here, namely, chemical bonding, concentration of solutions and chemical equilibrium. The topics will be deepened taking into account the needs of the Pharmacy Degree. In addition, students will also be heard in order to establish the perception of their knowledge. A basic knowledge in mathematics is also recommended.

The theoretical classes aim at the detailed presentation of the program, using an expositive-active methodology. Theoretical classes allow the students to acquire in-depth knowledge in the addressed aspects of Chemistry, establishing bridges between different topics.

Theoretical-practical component allow to consolidate the knowledge obtained in the theoretical component, thus increasing the skills and abilities of the students. The contents are exposed calling for constant students’ intervention. Standard analytical calculations are performed by the teacher; also, the students will be encouraged to solve the exercises by themselves, with monitoring and validation by the teacher.

Practical component allow to implement, at an experimental level, the themes studied in the various theoretical aspects of the discipline through laboratory work of an appropriate level.

Students should acquire the following knowledge and skills:

– Identify main inorganic compounds: understand structure and nomenclature.

– Understand the notion of chemical bonding.

– Understand and identify the concept of concentration of aqueous solutions expressed in different physical and chemical units.

– Understand the notion of dilution and dilution factor: presenting analytical calculations.

– Understand stoichiometry concepts: stoichiometric calculations; yield definition: excess reactant, limiting reactant.

– Identify chemical equilibrium situations: understand equilibrium constants, Kp, Kc e Kps, analytical calculations.

– Identify acid-base equilibrium situations. Understand the concepts concerning pH scale, titrations, pH indicators, buffer solutions.

– Identify redox reactions.

General and Inorganic Chemistry is an integrated discipline that aims the familiarization of the student with the most common chemical structures and schemes within the general and inorganic chemistry. On the other hand, the analytical calculations concerning the contents taught constitute an important and extensive part, so, the conclusion of this discipline should provide the student with a high degree of calculation capacity. The main purpose of this discipline is the creation of an interface between the knowledge and the chemical phenomena taught and other disciplines that may rely on them, theoretically or practically.

Rules for presentation, discussion and treatment of results: random and systematic errors, accuracy and precision, significant figures.

Solutions: solution definition, solute, solvent, concentration. Dilution: properties of diluted solutions, preparation of diluted solutions, dilution factor. Different ways to express concentrations: molarity, molality, percentage (w/w), percentage (w/v), percentage (v/v), normality, molar fraction; conversion between concentration units.

Stoichiometry: chemical equations, stoichiometric coefficients. Chemical yield: theoretical yield, limiting reactant, excess reactant, real yield, purity grade.

Inorganic chemistry nomenclature: ionic compounds, molecular compounds, acids and bases, hydrates. Rules for nomenclature. Compounds’ identification.

Chemical equilibrium: concentration equilibrium constant, Kc, pressure equilibrium constant, Kp. Relation between Kc and Kp. Interpretation of equilibrium constants. Reaction quociente. Le Chateliêr Principle.

Solubility equilibrium: solubility product constant, Kps, precipitate formation, common ion effect.

Acid-base equilibrium: acid and basic species – Arrhenius and Bronsted and Lowry definitions, ionization extension, acidity constant, Ka, basicity constant, Kb. Water acid-base behaviour. Logarithmic notation: pH, pOH, pKw, pH and pOH scales. Titrations: titration curves, titration endpoints, indicators, buffer solutions, buffer zone and effect. Calculations of pH in different types of titrations.

Redox reactions: reduction reaction, oxidation reaction, reducing agent, oxidizing agent, reduced substance, oxidized substance, oxidation state. Redox reactions balancing. Electrochemical cell, cell potential, Nernst Equation.

NAO

Primary bibliography (existing on the library)

Alexéev V. Quantitative Analysis. 3^rd ed. Lopes da Silva Editora, Porto, 1983.

Skoog DA, West DM. Fundamentals of Analytical chemistry. 7^th ed. Saunders College Publishing, New York, 1996.

Goldsby A, Chang R. Chemistry. 10^th ed., McGraw Hill. New York, 2010.

Secondary bibliography (other recommended bibliography)

Vogel RI. Quantitative Chemical Analysis. 15^th ed. Longman Scientific & Technical, New York, 1989.

Guernet M, Guernet E, Herrenknecht-Trottmann C. Équilibres en solution aqueuse. 1^st ed. Masson, Paris, 1996.