Physical and Inorganic Chemistry

Code:

MA217

Acronym:

QFI

Keywords
Classification	Keyword
OFICIAL	Chemistry

Instance: 2022/2023 - 1T (of 12-09-2022 to 28-10-2022)

Active?	Yes
Responsible unit:	Chemistry
Course/CS Responsible:	Aquatic Sciences

Cycles of Study/Courses

Acronym	No. of Students	Study Plan	Curricular Years	Credits UCN	Credits ECTS	Contact hours	Total Time
LCMA	34	Official Study Plan	2	-	5	49	135

Teaching language

Portuguese

Objectives

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. Quantitative accurate treatments of the equilibrium processes studied earlier will be studied and conducted, as a means of quantitatively describing the composition of aquatic systems and its evolution, in order that speciation of the substances can be adequately described and characterized. 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.

Learning outcomes and competences

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.

Working method

Presencial

Program

- 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. - 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 of State. Pressure and Fugacity. - 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. Giggs 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. Standard Half-Reaction or Electrode Potentials. Standard Reaction Potential and Electromotive Force. Oxidation/Reduction Equilibria. Standard Reaction Potential and Equilibrium Constant. Nernst Equation and Peters Equation. Quantitative Calculations of Redox Equilibria. Potentiometric Titrations.
- Fundamentals of the rates of chemical reactions. - Chemical Kinetics. The rate of a chemical reaction. 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. 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.

Mandatory literature

Raymond Chang; Química. ISBN: 978-989-97172-7-5
Raymond Chang; Chemistry. ISBN: 978-1-259-25458-1

Complementary Bibliography

Jones Loretta; Chemistry. ISBN: 0-7167-3595-4
Chang Raymond; Physical chemistry for the chemical and biological sciences. ISBN: 1-891389-06-8

Teaching methods and learning activities

two types of classes are offered: 

 - theoretical and tutorial lectures, where the lecturer begins by presenting the students to the chemical theoretical fundamentals of the several topics covered, including analytical chemistry, followed by examples of numerical problem resolution applied to the presented concepts.

 

 Laboratory classes where the students participate in group doing a laboratory project following a provided guide and applying theoretical knowlege previously acquired. A report with the results obtained is handed-in for classification. 

Evaluation Type

Distributed evaluation with final exam

Assessment Components

Designation	Weight (%)
Exame	70,00
Trabalho laboratorial	20,00
Trabalho prático ou de projeto	10,00
Total:	100,00

Amount of time allocated to each course unit

Designation	Time (hours)
Estudo autónomo	76,00
Frequência das aulas	49,00
Trabalho laboratorial	10,00
Total:	135,00

Eligibility for exams

Students must attend at least 25% of all tutorials and laboratory classes.

The students without approval, but who had attended the minimum required classes, can keep the practical componente of the classification for 3 consecutive years, being dismissed of pratical classes for that period of time.

Calculation formula of final grade

The final classification will be obtained according to the formula:

score in the exam * 0,75 + 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.

Classification improvement

Taking further exams.