Code: | MA217 | Acronym: | QFI |
Keywords | |
---|---|
Classification | Keyword |
OFICIAL | Chemistry |
Active? | Yes |
Responsible unit: | Chemistry |
Course/CS Responsible: | Aquatic Sciences |
Acronym | No. of Students | Study Plan | Curricular Years | Credits UCN | Credits ECTS | Contact hours | Total Time |
---|---|---|---|---|---|---|---|
LCMA | 32 | Official Study Plan | 2 | - | 5 | 49 | 135 |
Teacher | Responsibility |
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Maria Antónia Santos Mendes Salgado |
Theoretical and practical : | 5,00 |
Laboratory Practice: | 2,00 |
Type | Teacher | Classes | Hour |
---|---|---|---|
Theoretical and practical | Totals | 2 | 10,00 |
Maria Antónia Santos Mendes Salgado | 10,00 | ||
Laboratory Practice | Totals | 2 | 4,00 |
Maria Antónia Santos Mendes Salgado | 4,00 |
The Fundamental Principles of Chemistry will be addressed and studied with special emphasis on the quantitative chemical description of natural as well as non-natural water systems. Among the main topics we emphasize the following: Chemistry and Transformations; stoichiometry and mass balances; Energy and transformation; Spontaneity, entropy and Gibbs energy; Phase Equilibria, Chemical Equilibrium; rates of chemical transformations. Acids and Bases and their equilibria; Equilibrium Processes involving the Precipitation and Dissolution of solid minerals, the processes of electron transfer and the formation of metalic complexes and coordination compounds. In addition, a set of laboratorial classes is offered in order to introduce students to the main analytic techniques used in the analytical chemistry and environmental chemistry laboratories.
After completing the course the student will be able to understand and correctly interpret relevant information and data relating to the specification of the qualitative and quantitative laboratorial chemical analysis of samples collected from natural water systems. The student should also be able to understand the main mechanisms describing the physico/chemical phenomena which control the composition and chemical speciation of natural water systems. The result from this learning process will be adequate for the student to proceed to more advanced and specialized studies in other related scientific areas.
- Fundamentals and Theory - Chemical Equilibrium. - Proton Exchange. Acid/Base Equilibria. Acid/Base Equilibria without algebra: Graphical Methods for the determination of equilibrium state and composition. - The calculation of Acid/Base equilibria. Neutralization Reactions. Acid/Base Titrations. The calculation of titration curves. Potenciometric titrations. - Reactions at Interfaces. Heterogeneous Equilibria. Phase Rule. Dissolution and Precipitation Equilibria. Accurate numerical calculations of dissolution/precipitation equilibria.
- Physical Equilibria. Vapour Pressure. Volatility and intermolecular forces. Variation of Vapour Pressure with Temperature. Melting and Boiling Temperatures. Solubility. Solubility of gases. Henry's Law.
- Properties of the gases. Avogadro's Law. Ideal Gases and Real Gases. The Equation of State of Ideal Gases. Mixtures of Gases. Dalton's Law.
Intermolecular Forces. Real Gases. van der Waals Equation. - Basic Principles of Chemical Energetics. - Work and Energy. Heat. First Law of Thermodynamics. State Functions. Enthalpy. Heat Capacity. Phase Change Enthalpy Variations. Heating Curves. - Reaction Enthalpy. Enthalpy and Internal Energy Changes. Reaction Standard Enthalpy. Hess's Law. Influence of Temperature on the heat of reaction. - Spontaneous and non-spontaneous Transformations. Entropy and molecular disorder. Entropy variations in physical changes. Standard Molar Entropy. Standard Reaction Molar Entropy. - Gibbs Energy. Gibbs Energy variations for reactions. Temperature dependence of reaction Gibbs Energy Variation. Chemical equilibrium and Gibbs energy change.
- Electron Exchange. The concepts of oxidation state and oxidation number. Balancing Redox Equations. Electrochemical Potential concept. Standard Half-Reaction. Standard Reaction Potential and Electromotive Force. Oxidation/Reduction Equilibria. Standard Reaction Potential and Equilibrium Constant. Peters and Nernst Equations. Quantitative Calculations of Redox Equilibria.
- Fundamentals of the rates of chemical reactions. - Chemical Kinetics. The rate of chemical reactions. Instantaneous reactions. - Reaction rate and collision theory. Rate equations and order of reaction. - Differential and Integrated rate laws. - Characteristic times and rate constants. Half-Life. Complex Reactions. Reaction Mechanisms. - The Chemistry of Complex Formation and Complexation Equilibrium. The Stability of Molecular Complexes. Metal Complexes. Complexation Reactions. The concepts of coordination state and of coordination number. Types of Complexes. Stability and Stability Constants. Complexation Equilibria.
- Tutorial Classes - Resolution of Selected Applied Numeric Problems evidencing the importance of the concepts already studied, as a means of providing a better understanding of the physico/chemical concepts involved.
two types of classes are offered:
- theoretical and tutorial lectures, where the lecturer presents to the students the chemical theoretical fundamentals of the several topics covered, including analytical chemistry, followed by examples of numerical problems resolution applied to the presented concepts.
Laboratory classes where the students do a group laboratory project following a guide provided and applying theoretical knowlege previously acquired. A report with the results obtained by the students is handed-in to be scored.
Designation | Weight (%) |
---|---|
Exame | 70,00 |
Trabalho laboratorial | 20,00 |
Trabalho prático ou de projeto | 10,00 |
Total: | 100,00 |
Designation | Time (hours) |
---|---|
Estudo autónomo | 76,00 |
Frequência das aulas | 49,00 |
Trabalho laboratorial | 10,00 |
Total: | 135,00 |
The final classification will be obtained according to the formula:
score in the exam * 0,70 + score in laboratory classes * 0,20 + score in problem solving worksheets *0,10
The score in the laboratory sessions is obtained by the average score of the reports done in the laboratory classes + the average score of the problem solving worksheets.