Chemistry

Scholar Year: 2020/2021 - 1S

Courses

Head Teacher Responsability António Pedro dos Santos Lopes Castela Head

Weekly workload Hours/week T TP P PL L TC THE EL OT OT/PL TPL S Type of classes 4 Lectures Type Teacher Classes Hours Theorethical and Practical classes Totals 2 8,00 António Castela   8,00

Teaching language

Portuguese

Intended learning outcomes (Knowledges, skills and competencies to be developed by the students)

Know and understand the basic foundations of Chemistry, within the basic scientific training of the student, with a view to understanding the structure of matter and its transformations and its impact on the study of Mechanical Engineering, namely on the behavior of materials and on the applications of combustion and oxidation-reduction reactions.

Syllabus

1. Atomic Structure: Atomic orbitals and quantum numbers. Electron configurations: Aufbau principle, Pauli exclusion principle and Hund’s rule. Electron distributions in polyelectronic atoms.

2. Periodicity: Evolution of the periodic representation of elements. Periodic Table. Periodic variation of atomic properties: atomic radius, ionization energy and electron affinity. Electronegativity.

3. Chemical Bond: Lewis Dot Symbol. Octet rule. Types of chemical bond: Metallic, Ionic and Covalent (polar nonpolar). VSEPR and molecular geometry. Dipole moments. Polarity of a molecule. Resonance structure.

4. Intermolecular Forces: Van der Waals Forces (Keeson, Debye and London) and hydrogen bonds. Qualitative prediction of physical properties based on the type of intermolecular forces of organic and inorganic substances: melting points, boiling points, viscosity and solubility.

5. Concentration Units and Stoichiometric Calculations: Atomic mass and relative atomic mass. mol concept. Molar mass. Irreversible chemical reactions. Lavoisier's law and correctness of chemical equations. Stoichiometric calculations. Limiting reagent and reaction yield. Reagents/Gaseous products: Perfect gas law and molar volume. Solutions and concentration units: Molarity and mass percentage.

6. Chemical Equilibrium - Reversible Reactions: Chemical Equilibrium. Equilibrium constants. Reaction ratios. Equilibrium disturbances and Le Chatelier's Principle.

7. Chemical Thermodynamics: 1st Law of Thermodynamics. Enthalpy. Endothermic and exothermic reactions. Hess's Law. Entropy. 2nd Law of Thermodynamics. Gibbs energy and reaction spontaneity. 3rd Law of Thermodynamics. Gibbs energy and chemical equilibrium.

8. Acid-base equilibrium: Arrhenius, Brønsted e Lewis definition of acid and bases. Conjugate acid-base pairs. Water as an amphoteric species. Kw, ion-product constant for water. Strength of acids and bases. Ka e Kb, base and acid ionization constants. Ionization percentage. Relationship between Ka and Kb of a conjugate acid-base pair. Polyprotic species. Acidity scale and pH concept. pH calculations of acid and base solutions (strong and weak).

9. Electrochemistry: Oxidation and reduction. Oxidation numbers. Balancing redox reactions. Galvanic cells. Electromotive force. Reference electrode and standard reduction potentials. Reaction potentials calculations under standard and real conditions: Nernst equation.

Demonstration of the syllabus coherence with the UC intended learning outcomes

This is an introductory chemistry course, new concepts are reminded and taught regarding the understanding of the structure of matter and its transformations and its impact on the study of Mechanical Engineering, essential tools in subsequent curricular units.
Thus, in chapters 1 to 4, the evolution of the concept of atom is transmitted to the student, as well as its periodic properties, the concept of molecule and its structure, as well as the interactions between molecules that allow explaining the macroscopic behavior of matter.
At the end of these chapters, the student must acquire the necessary knowledge to know and distinguish the different groups of elements and their periodic properties, as well as the ability to interpret the geometries of the molecules adopted considering different models of chemical bonding. The student will be able to understand the concept of intramolecular and intermolecular bonding and the influence of different types of intermolecular bonds on the physical state and properties of matter.
Within the scope of the course, students must acquire solid knowledge regarding calculus in chemistry, such as the concept of moles, molar concentrations, stoichiometric calculations, whether in irreversible as well as reversible reactions, and also in chemical equilibrium calculus (chapters 5 and 6).
Finally, within this course there must be a special focus on acid-base reactions (chapter 8), oxidation-reduction reactions (chapter 9), as well as all fundamental concepts relating to the energy of reactions and spontaneity (chapter 7).

Teaching methodologies

theoretical-practical classes, the fundamental concepts will be taught by exposition, using audio-visuals means, resorting, whenever possible, to the rediscovery method and the use of models that make the concepts more real. These contents are interspersed with practical examples of the application of theoretical concepts, to be solved by students within the classroom.

Demonstration of the teaching methodologies coherence with the curricular unit's intended learning outcomes

The student can choose from a continuous evaluation and/or an exam.
1. Evaluation by exam: If student want to be evaluated by exam, will take the test in the normal season or in the appeal season, obtaining approval with a grade equal or greater than 9.5 val in any of the exams.
2. Continuous Evaluation: Only students who attend 70% of classes can opt for continuous evaluation. If student miss this appointment, it must do an evaluation by exam.
If the student intent to do continuous evaluation (at least active in 70% of the classes), the student will do two tests and homework. The final grade corresponds to 100% of the weighted average of the grades obtained in the 2 tests (50% in each, minimum grade of 8.0 val). If this grade is higher than 9.5 val, the student is approved. Otherwise, student must do an evaluation by exam.
“Active attendance of classes” corresponds to being in class and participating in the activities that are being proposed. If the teacher understands that the student is not in this situation, he/she should alert the student and, if the situation does not change, he/she should invite the student to leave the room, which will count as a fault.

Assessment methodologies and evidences

1. Evaluation by exam: final grade = exam grade
2. Continuous Evaluation: final grade = (T1 + T2)/2
In which T1 and T2 are the evaluations of the 1st and 2nd tests to be carried out during the class period, with the 1st test having a grade higher than 8.0 values.

Attendance system

Students with the status of working students, high competition athlete, association leader or students under the law of religious freedom must send an email to the teacher responsible for the discipline by the second week of the semester, to present their pertinent specificities, under the terms provided for in the respective diplomas.

Assement and Attendance registers

Primary Bibliography

Secondary Bibliography

Observations

- It is absolutely forbidden to use mobile phones or other means of communication during classes and evaluation tests.
- For classes, it is mandatory to bring problem statements (available in moodle), calculating machine and periodic table.

Opening hours: Friday from 15.30-16.30h