Chemistry

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The teaching/learning methodology focuses on three main components, being two in presencial format (theoretical and theoretical-practical) and the other are autonomous (guided study).
In-person component:
• Theoretical – the syllabus is presented in the form of projections, to which students have access and, whenever appropriate, the classroom framework. During the classes and as concepts, deductions and principles are presented, students are asked to participate, through questions raised by the teacher to the student, or vice versa, to check whether they are following the material.
• Theoretical-Practical – worksheets are solved individually and in groups on the different programmatic contents.

1. It is intended that students learn the basic knowledge of Chemistry, in order to be able to apply it in solving problems. At the end of the semester, it is important that students have developed personal skills that will allow them to learn autonomously.

1. Electronic Structure of Atoms and Periodic Table

Electromagnetic radiation and interaction with matter. Planck’s quantum theory.

Photoelectric effect. Bohr theory of the hydrogen atom. Duality of the nature of electrons –  The De Broglie principle. Heisenberg’s Uncertainty Principle. Quantum Mechanics. Quantum numbers. Atomic orbitals.

Electronic configuration – Aufbau principle, Pauli exclusion principle and Hund rule.

Struture of the Periodic Table. Periodic classification of elements.

Periodic variation of physical properties – nuclear charge, atomic radius, ionic radius.

Ionization energy, Electronic affinity. Variation of the chemical properties of the elements.

2. Chemical Bonds and Molecular Structure

Chemical bonds – ionic, metallic and covalent.

Lewis structure. Resonance concept. Exceptions to the octet rule.

Molecular geometry.

Dipole moments. Valence bond theory.

3. Intermolecular forces

Molecular Kinetic Theory of Liquids and Solids.

Intermolecular forces – dipole-dipole, ion-dipole forces, London dispersion, hydrogen bonding

Liquid properties – surface tension, viscosity.

Phase changes – liquid-vapor; liquid-solid and solid-vapor equilibrium.

4. Chemical reactions

Chemical equations: writing and balancing.

Stoichiometric calculations. Limiting reagents and reaction yield.

Properties of aqueous solutions – electrolytes versus non-electrolytes.

Three main types of reactions – precipitation, acid-base and oxidation-reduction.

Physical properties of solutions. Effect of the temperature on solubility.

Effect of the pressure on gas solubility. Colligative properties.

5. Properties of Gases

Pressure of a gas.

Gas law – Boyle law, Charles and Gay-Lussac’s law, Avogadro’s law.

Ideal gas equation.

Dalton’s law of partial pressures.

Kinetic theory of gases.

Deviation from ideal behaviour of the gases.

6. Chemical equilibrium

Equilibrium constant.

Expressions of equilibrium constants – homogeneous and heterogeneous equilibria.

Factors that affects chemical equilibrium – Le Châtelier’s principle, variations in concentration, volume and pressure.

Equilibrium involving poorly soluble salts – product of solubility, prediction of precipitate formation.

Common ion effect and solubility.

7. Thermochemistry

Endothermic and exothermic reactions.

Enthalpy of chemical reactions – enthalpy of reactions and thermochemical equations.

Standard formation enthalpy and standard reaction enthalpy

Hess’s law.

Specific heat and heat capacity.

Gibbs energy of reaction and chemical equilibrium.

8. Electrochemistry

Extension of oxidation-reduction reactions.

Galvanic Cells. Reference electrode and the standard potential reduction.

Spontaneity of oxidation-reduction reactions.

Effect of concentration on the electromotive force of the cell – Nernst equation.

Batteries. Corrosion. Electrolysis.

9. Organic chemistry

Classes of Organic Compounds.

Aliphatic hydrocarbons – alkanes, cycloalkanes, alkenes and alkynes.

Aromatic hydrocarbons.

Chemistry of Functional Groups – alcohols, ethers, aldehydes, ketones, carboxylic acids, esters and amines.

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 )

– KOTZ, J.C. ; TREICHEL, P. Jr. – Chemistry and Chemical Reactivity ; Saunders College Publishing, 1999. ISBN 0-03- 023762-9

– Campos, L.S. e Mourato, M. (1999). Nomenclatura dos Compostos Orgânicos (2ª edi.). Lisboa : Escolar Editora (Disponível na Biblioteca: 6-2-65 (ISEC) – 10570 )