|Curricular Unit (UC)||
Course category: B - Basic; C - Core Engineering; E - Specialization; P - Complementary.
|Year: 1st||Semester: 2nd||ECTS: 6||Total Hours: 165|
|Contact Hours||T: 30||TP: 15||PL:15||S:||OT:2|
|Professor in charge||
Alexandra Isabel Martins Paulo da Costa
T - Lectures; TP - Theory and practice; PL - Lab Work; S - Seminar; OT - Tutorial Guidance.
- Learning outcomes of the curricular unit
Upon completion General Chemistry course, the student should understand:
The basic structures of atoms and the theories of chemical bonding. Predict molecular geometry using VSEPR theory.
The intermolecular attractive forces that determine the properties of the states of matter and phase behaviour.
The concept of chemical equilibrium, and the energies that drive chemical reactions: an introduction to the field of thermodynamics.
The acid/base theory and the concepts of soft/hard acids/bases. Calculate and utilize solution concentration units such as molarity, % v/v and % m/m.
The construction and operation of galvanic and electrolytic electrochemical cells. Determine standard and non-standard cell potentials and balance oxidation-reduction reactions.
The preparation, structure, spectroscopic properties and applications of coordination compounds.
Atomic structure. Atomic models. Periodic properties of the elements. Isotopes. Electromagnetic radiation. Photoelectric effect.
Chemical bond. Lewis theory. Octet rule. Valence-bond Theory. Hybridization theory. Resonance hybrid. Molecular orbital theory. Polarity. Molecular geometry. Solutions and Intermolecular Forces. Hydrogen bonds. Concentration units.
Oxidation and reduction reactions. Oxidation state. Redox half-reactions. Reference electrodes and standard reduction potentials. Electrochemical series. Nernst equation. Half cells and galvanic cells. Batteries. Electrolysis.
Chemical equilibrium e reaction rates. Acid/base equilibrium. Ionic product of water. Determination of pH in solutions. Buffer solutions. Acid-base titrations. Titration of amino acids.
Coordination chemistry. Geometry. The 18-electron rule VE. Crystal field theory. Magnetic properties. Electronic spectra. Reactions of coordination compounds. The biological and medicinal roles of metal ions.
- Demonstration of the syllabus coherence with the curricular unit's objectives
General chemistry introduces students to the understanding of the fundamental theories of chemistry (within contents 1 and 2), and to issues of intermediate knowledge that provide sustainable development of essential subjects such as thermodynamics, acid base chemistry, chemical equilibria, redox properties and coordination chemistry (within contens 3-7), to provide the requirements to support a sustained development of the course as well as to develop skills of critical analysis and reflection and calculation required for those students wishing to pursue a career in the biomedical or biotechnology fields.
- Teaching methodologies
The themes covered in the UC program will be presented and developed in lectures, through slideshow (previously available to students through MOODLE platform).
The practical classes should be used for troubleshooting application.
The practical/laboratory classes consist in carrying out 4 laboratory sessions. Student presence is mandatory.
Course assessment: Continuous Assessment or Final Exame.
Evaluation will be done through:
- Demonstration of the coherence between the teaching methodologies and the learning outcomes
The fundamental concepts introduced and discussed in the lectures are applied and consolidated in the theoretical-practical classes through exercises resolution.
Concepts with practical (experimental) application are additionally consolidated through the laboratory work performed in Laboratory.
Learning outcomes 1-7 are individually assessed by two written tests during the semester, allowing monitoring of the learning progression of the student. The learning outcome 8 will be evaluated by conducting a survey (prepared in group) for each laboratory experiment.
- Main Bibliography
Chang, R., K. Goldsby, A., Chemistry, McGraw-Hill, 12th ed., 2016.
Romão Dias, A. Ligação Química, IST Press, 2007.
Housecroft, C.E.; Sharpe, A.G., Inorganic Chemistry, Prentice Hall, 2nd ed., 2005.
Shriver, D.F.; Atkins, P. W.; Logford, C. H. Inorganic Chemistry, 2nd ed., Oxford University Press, 1994.
Pombeiro, A.J.L. Técnicas e operações unitárias em química laboratorial, Fundação Calouste Gulbenkian, Lisboa, 1980.