Base Knowledge
Not applicable
Teaching Methodologies
Theoretical contents are presented in theoretical classes. These contents are applied to practical exercises carried out in theoretical-practical classes.
Learning Results
It is intended that students learn the basic concepts of Chemistry, in order to be able to apply them in solving problems. At the end of the semester, it is important that students have developed personal skills that will allow them to learn independently in the future.
Program
1. Electronic Structure of Atoms and Periodic Table
Electromagnetic radiation and interaction with matter. Planck’s quantum theory.
Photoelectric effect. Bohr’s theory of the hydrogen atom. Duality of the nature of electrons – De Broglie’s principle. Heisenberg Uncertainty Principle. Quantum Mechanics. Quantum numbers. Atomic Orbitals.
Electronic configuration – Aufbau’s principle, Pauli’s exclusion principle and Hund’s rule.
Development 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 chemical properties of 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 forces, ion-dipole forces, London dispersion, hydrogen bonding
Liquid properties – surface tension, viscosity.
Phase changes – vapor-liquid equilibria; liquid-solid and solid-vapor.
4. Chemical Reactions
Chemical equations: writing and correcting.
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 temperature on solubility.
Effect of pressure on the solubility of gases. Colligative properties.
5. Properties of Gases
Pressure of a gas.
Gas Law – Boyle’s 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 behavior.
6. Chemical Balance
Equilibrium constant.
Expressions of equilibrium constants – homogeneous and heterogeneous equilibria.
Factors that affect chemical equilibrium – Le Châtelier’s principle, variations in concentration, volume and pressure.
Equilibrium involving poorly soluble salts – solubility product, 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 enthalpy of formation 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 standard reduction potentials.
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.
Curricular Unit Teachers
Internship(s)
NAO
Bibliography
– CHANG, R. – Química Geral – Conceitos Essenciais, McGraw-Hill, 4ª edição, Lisboa 2007. ISBN: 85-86804-98-3
– ATKINS, P.; JONES, L. – Chemical Principles: The Quest for Insight, W.F. Freeman and Company, 3ª edição New York 2005. ISBN: 0-7167-5701-X
– KOTZ, J.C. ; TREICHEL, P. Jr. – Chemistry and Chemical Reactivity ; Saunders College Publishing, 1999. ISBN 0-03- 023762-9
– ATKINS, P.; JONES, L. – Chemistry – Molecules, Matter and Change Principles: The Quest for Insight, W.F. Freeman and Company, 3ª edição New York 1997. ISBN: 0-7167-2832-X
– KOTZ, J.C. ; PURCEL, P. Jr. – Chemistry and Chemical Reactivity ; Saunders College Publishing, 1991 ISBN 0-03- 047562-7
– ATKINS, P.; – The Elements of Physical Chemistry, Oxford University Press, 3ª edição UK 2001. ISBN: 019 879290 5