Code: | Q102 | Acronym: | Q102 |
Keywords | |
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Classification | Keyword |
OFICIAL | Chemistry |
Active? | Yes |
Web Page: | http://moodle.up.pt/course/view.php?id=1879 |
Responsible unit: | Department of Chemistry and Biochemistry |
Course/CS Responsible: | Bachelor in Environmental Sciences and Technology |
Acronym | No. of Students | Study Plan | Curricular Years | Credits UCN | Credits ECTS | Contact hours | Total Time |
---|---|---|---|---|---|---|---|
L:AST | 9 | Plano de Estudos a partir de 2008 | 1 | - | 7,5 | 60 | 202,5 |
3 | |||||||
L:B | 198 | Plano de estudos a partir de 2008 | 1 | - | 7,5 | 60 | 202,5 |
L:CC | 0 | Plano de estudos de 2008 até 2013/14 | 2 | - | 7,5 | 60 | 202,5 |
L:CTA | 78 | Plano de estudos de 2008 até 2015/16 | 1 | - | 7,5 | 60 | 202,5 |
L:F | 41 | Plano de estudos a partir de 2008 | 1 | - | 7,5 | 60 | 202,5 |
L:G | 68 | P.E - estudantes com 1ª matricula anterior a 09/10 | 1 | - | 7,5 | 60 | 202,5 |
3 | |||||||
P.E - estudantes com 1ª matricula em 09/10 | 1 | - | 7,5 | 60 | 202,5 | ||
3 | |||||||
L:M | 0 | Plano de estudos a partir de 2009 | 3 | - | 7,5 | 60 | 202,5 |
MI:EF | 39 | Plano de Estudos a partir de 2007 | 1 | - | 7,5 | 60 | 202,5 |
The course "Fundamentos de Química (1st year, 2nd semester) is the first,and in some cases the only, chemistry course in the different B.Sc. of Science Faculty. The main objective is thus to provide a solid understanding of the essential chemistry concepts necessary for further applications in other more specialized courses and multidisciplinary courses.
The students should achieve the following general goals:
Be able to apply the concepts learned to real situations. Be able to analyze simple chemical problems and to select the theoretical tools necessary to obtain further chemical information for those systems.
Chemistry : the Study of Change: matter, energy, scientific method
Atoms, Molecules, Ions and Chemical reactions:the structure of atoms, the periodic table; molecules and ions, inorganic nomenclature; mass relatioships in chemical reactions, limiting reactants, reaction yield.
Chemical bonding: Lewis theory: covalent bond, ionic bond; valence bond theory;hybridization of atomic orbitals, molecular geometry. Organic compounds.
Gases: ideal gas equation, Dalton´s law of partial pressures, real gas equation of van der Walls; Intermolecular interactions and liquids and solids
Chemical Thermodynamics: inernal energy and the 1st law; enthalpy and thermochemistry; entropy and spontaneity, 2nd and 3rd laws.; gibbs energy and equilibrium; facrtos affectinga equilibrium.
Physical equilibria: phase diagrams of pure substances; liquid crystals, colligative properties of solutions
Chemical equilibrium; acids and bases, pH; strength of acids and bases;buffe solutions; acid-base titrations. Solubility equilibria: the common ion effect
Eletrochemistry :Redox reactions; Galvanic cells; standard reduction potentials;spontaneitiny of redox reactions; Corrosion; Batteries; Electrolysis
Kinetics: reaction rate, mechanism and rate laws for zer, first and second order reactions
Teorethical classes: presentation/discussion.
Theorethical-practical: Problem solving
designation | Weight (%) |
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Participação presencial | 0,00 |
Teste | 100,00 |
Total: | 100,00 |
The students must have no more absences then that 1/4 of the ttal number of he theorethical-practical classes.
The final classification is the average of the grade obtained in three tests. T1 and T2 during the semester and T3 in exam. In the exam the student can do two of the three possible tests. The best classification will be considered for the calculation of the mean value
Students with special status can choose global exam
BIBLIOGRAPHY
Chang, Chemistry, 9th ed., McGraw-Hill, 2007
P. W. Atkins, Loretta Jones, Chemical Principles; the Quest for Insight, 4th edition, W.H. Freeman and Company: New York 2008.