Introduction to Physical Chemistry
Code
10690
Academic unit
Faculdade de Ciências e Tecnologia
Department
Departamento de Química
Credits
6.0
Teacher in charge
Ana Isabel Nobre Martins Aguiar de Oliveira Ricardo
Weekly hours
5
Total hours
74
Teaching language
Português
Objectives
The overall objective of Introduction to Physical-Chemistry is to provide the fundamental scientific background and practical training in Chemistry that are the basis for the understanding of the world around us. A key general objective is the development of qualitative and quantitative problem-solving skills. Of comparable importance is to learn proper laboratory practices, execute experiments, interpret experimental results and draw reasonable conclusions. Specific learning objectives for this course include the development of conceptual understanding of: bulk properties and models of gases, liquids and solids; thermodynamic laws and their relation with equilibrium - entropy and free energy concepts; physical and chemical equilibria; acqueous equilibria; electrochemistry and chemical kinetics.
Subject matter
1.1.Intermolecular forces.
1.1.1.Solids, liquids and gases.
1.1.2.Phase transitions.
1.1.3.Phase diagrams for pure substances
1.1.4.Ideal gases and real gases.
1.1.5.State equations.
1.2.Thermochemistry.
1.2.1.Revision of concepts: sistems, work, energie and heat.
1.2.2.Calorimetry. Specific heat and heat capacity.
1.2.3.1st Law of Thermodynamics.
1.2.4.Energy transfer in chemical reactions.
1.2.5.Enthalpy. Formation Enthalpy and reaction Enthalpy.
1.3.Entropy, Gibbs energy and equilibrium.
1.3.1.Spontaneous processes.
1.3.2.Entropy and the 2nd law of Thermodynamics.
1.3.3.Total entropy chnages.
1.3.4.Gibbs energy.
1.3.5.Gibbs energy and chemical equilibrium.
1.4. Physical equilibrium
1.4.1.Phase transitions and phase diagrams.
1.4.2.Solubility.
1.4.3.Colligative properties.
1.4.4. Binarymixtures. Ideal solutions. Raoult Law.
1.5. Chemical Equilibrium.
1.5.1.The concept of chemical equilibrium. Ways of expressing equilibrium constants.
1.5.2.Factors that affect chemical equilibrium. Le Châtelier Principle.
1.6. Acid-Base Equilibria.
1.6.1.Conjugate acid-base pair. The ion product of water and the pH scale.
1.6.2.pH of solutions.
1.6.3.Buffer solutions
1.7. Solubility.
1.7.1.Solubility equilibria and solubility product.
1.7.2.Common ion effect.
1.7.3.Applications.
1.8. Electrochemistry
1.8.1.Galvanic Cells. Schematic representation of galvanic cells.
1.8.2.Standard electrode potentials.
1.8.3.Nernst equation.
1.8.4.Electrolytic Cell.
1.8.5.Electrolysis.
1.9.Chemical kinetics.
1.9.1.The rate of reactions.
1.9.2.Rate laws. Experimental determination of rate law.
1.9.3.Arrhenius Law and activation energy.
1.9.4. Reaction mechanisms. Elementary steps. Molecularity.
1.9.5.Introduction to the collision theory and activated complex theory.
Bibliography
-“Chemical Principles. The Quest for Insight”, P.Atkins and L. Jones, Freeman 5th ed.(2010).
- Chemical Principles Student Solutions Manual, C. Hoeger, L. Lavelle and Y. Ma 6th ed. (2013), ISBN: 978-1-4641-0707-8.
-Química, R. Chang & K. A. Goldsby, McGraw-Hill 11th ed.
Teaching method
The course is organized into lectures (T 28h), problem-solving sessions (TP, 21h) and lab sessions that link the classroom, the lab and the real world (P, 15h, 6h and 9h laboratory in computer room). Concepts, approaches and techniques are explained during the lectures, using date show and challenging the students to think about and solve new problems. Prior to each TP class, problem-sheets are offered to students that must be solved before each TP session, and be demonstrated in class, while explaining to colleagues. The lab classes follow the method of directed study, students are organized in groups of three and the work done by the group is evaluated at the end of each lab session.
It provided access to a page in moodle, containing all course material and related information. This page provides files (pdf) of lecture notes, problems (questions and solutions), exams, and moodle-quizzes that are element of continuous assessment.
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Evaluation method
Lab mark: evaluation of experimental data achieved (all the lab sessions are compulsive).
Final mark: 0,20 lab mark + 0,20 moodle quizzes mark+0,60 theory mark.