To provide introdutory knowledge in chemistry to students with different backgrounds.
The student should learn the contents of General Chemistry included in the program, to know how to do the experimental work and solve the proposed problems.
On successful completion of the module, students will be able to
a) apply fundamental Chemistry concepts in Engineering subjects.
b) understand simple chemical phenomena with impact in society.
b) solve simple problems in thermochemistry, chemical thermodynamics, ideal gases, chemical kinetics, acids and bases, solubility, electrochemistry and organic chemistry.
c) perform calculations related to chemical phenomena and the corresponding physical measurements.
d) perform simple lab tasks – weighting, transfer of liquids and solids, titrations, measurement of absorvances and determination of concentrations.
e) critically assess results.
On successful completion of the module, students will have improved interpersonal skills and the ability to study alone.
João Montargil Aires de Sousa
Weekly - 4
Total - 68
"Chemistry", R. Chang, McGraw Hill, 8th Edition 2004
Química (Portuguese translation of Chemistry ), R.Chang, McGraw Hill, 11 Edition, 2012.
"Chemical Principles, The quest for insight", P. Atkins, L. Jones, Freeman, 2001
This course uses Team-Based Learning, TBL, http://www.teambasedlearning.org .
The unit is organised in 5 modules. Before each module, students are provided with the learning material and a list of specific objectives. Before the first class of each module, each student must answer an individual test (Readiness Assurance Test). The same test is answer by teams in class, followed by a mini-lecture to solve the test, discuss doubts and reinforce the most difficult points.
In the other classes of the module, teams are challenged with application activities, including lab works.
Class evaluation: 50%, Final exam (or 2 written tests): 50%
Minimum mark in exam (or tests): 9,5.
Mark for class activities=average of individual tests (25%) and team results (20% labs, 80% team works). Mark corrected by peer evaluation (team mark x points received by colleagues/100).
Periodic properties and chemical bonding
Chemical Reactions. Stoichiometry: Aqueous solutions and concentration units.
Vapor- Liquid Equilibrium. Ideal solutions. The Raoult´s Law. Distillation. Colligative properties.Chemical Equilibrium . The first Law of Termodinamics. Enthalpy. Standard Entalphy of formation and reaction. le Châteliers Principle.
Spontaneous proceses. Entropy. The second low. Gibbs Free Energy and Chemical equilibrium.
The ideal gas equation. Dalton´s law of partial pressure.
Activation Energy. Arrhenius Law. Catalysis.
Acids and Bases.Autoionization of water. pH. Strength of acids and bases. Buffers. Acid-base Indicators.
Precipitation Reactions. Solubility equilibria. The common ion effect. Separation of ions.
Redox Reactions. Standard Reduction Potencial. The effect of concentration on Cells. The Nerst Equation. Corrosion.
Chemical kinetics. Rate of reaction. Rate laws. Determination of reaction orders, rate laws, and rate constant by method of initial rate. Determination of rate laws by graphical or integration method. Determination of half-lives. Arrhenius equation. Catalysis.
1st session - Chemical Reaction stoichiometry and Purity of an Unknown Sample
2nd session - Acid-Base Titrations
Session 3 - Determination of the rate constant fo a chemical reaction
Programs where the course is taught: