Degree | Type | Year | Semester |
---|---|---|---|
2501922 Nanoscience and Nanotechnology | FB | 1 | 2 |
It is recommended that those students who have not studied Chemical subjects during the Bachelor attend the chemical courses, which the Faculty of Sciences organizes at the beginning of September.
The general objectives of the subject are to establish the fundamental concepts that allow understanding chemical reactions and to be able to relate them with other more specific subjects of the Degree of Nanoscience and Nanotechnology. These bases will allow the student to identify and apply the principles and their meaning to solve real world problems in a systematic and fast way and increase their critical and learning abilities.
The subject offers the students the fundamental principles of chemistry, their applications and qualitative and quantitative reasoning. Examples of the real world and more specifically of the field of Nanoscience will be given. The following areas will be emphasized: thermochemistry, homogeneous and heterogeneous equilibria, chemical kinetics, basic electrochemistry and organic chemistry.
BLOCK I. Homogeneous and heterogeneous equilibrium
1. Acids and Bases (I). Review of Arrhenius theory. Bronsted-Lowry theory. Self-ionization of water and pH scale. Strong acids and strong bases. Weak acids and weak bases. Polyprotic acids. Ions as acids and bases. Lewis’ acids and bases.
2. Acids and Bases (II). Common ion effect in acid-base equilibria. Buffer solutions. Indicators. Neutralization reactions and titration curves. Polyprotic acid solutions. Calculations.
3. Solubility and complexation. Solubility product and solubility. Common ion effect. Total and partial precipitation. Solubility and pH. Complexation equilibrium.
BLOCK II. Thermodynamics, kinetic and electrochemistry
4. Thermochemistry. Reaction heat and calorimetry. Work-energy. First law of thermodynamics. Heats of reaction: ΔU and ΔH. Hess’ Law. Standard enthalpies of formation. Calorimetric techniques.
5. Spontaneity and equilibrium. Spontaneity and Entropy. Second law of thermodynamics: Gibbs Energy. Relationship between Gibbs energy and equilibrium constant. Prediction of chemical change. ΔGo and Keq depending on the temperature.
6.Principles of chemical equilibrium. Concept of chemical equilibrium, expressions and relationships between the equilibrium constants. The reaction quotient Q. Modifications of the equilibrium conditions: Le Châtelier’s principle. Examples.
7. Introduction to chemical kinetics. Reaction rate and temperature. Rate measurement. Rate equations and order of reaction. Reaction rate and temperature. Catalysis.
8. Electrochemistry. Basic concepts: redox reactions. Electrode potential and standard electrode potential. Relationship between E, ΔGo and Keq. Energy variation with the concentration: Nernst equation. Batteries. Electrolysis. Corrosion.
DIRECTED ACTIVITIES |
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Theoretical Lessons |
2-3/week |
Theoretical lecturing |
Exercises lessons |
1/week |
Exercises discussion and solving 2 groups
|
Laboratory practices |
3 days 9-13h
Compulsory: laboratory attendance, reports delivery and test
|
Guided Laboratory practices 2 groups |
To be able to do the laboratory practices you must keep the security forms up to date (via moodle). It is also mandatory to wear a lab coat and safety glasses (normal glasses will not be accepted).
SUPERVISED ACTIVITIES |
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Tutorials |
once a week |
Tutorials to help to assimilate theoretical concepts and to do the exercises |
AUTONOMOUS ACTIVITIES |
||
Study |
|
Perform schemes and abstracts and assimilation of concepts |
Exercises solving |
|
Exercises approach and solving |
Practical reports reading |
|
Comprehensive reading of the laboratory reports |
Practical reports writing |
|
Laboratory reports writing in pairs |
Annotation: Within the schedule set by the centre or degree programme, 15 minutes of one class will be reserved for students to evaluate their lecturers and their courses or modules through questionnaires.
Title | Hours | ECTS | Learning Outcomes |
---|---|---|---|
Type: Directed | |||
Evaluation Activities | 8.75 | 0.35 | 1, 3, 25, 21, 23, 26 |
Exercises lessons | 17.5 | 0.7 | 18, 5, 15, 20, 25, 7, 21, 23, 26, 28, 9 |
Laboratory Practices | 12.25 | 0.49 | 1, 18, 10, 4, 22, 6, 2, 27, 20, 24, 25, 26, 8, 9 |
Theoretical lectures | 31.5 | 1.26 | 5, 3, 13, 12, 11, 14, 15, 17, 16, 2, 27, 25, 21, 23 |
Type: Supervised | |||
Tutorial meetings | 17.5 | 0.7 | 1, 10, 4, 19, 2, 25, 26, 9 |
Type: Autonomous | |||
Exercises solving | 29.75 | 1.19 | 1, 18, 5, 3, 15, 19, 20, 25, 7, 21, 23, 26, 9 |
Practical reports reading | 1.75 | 0.07 | 1, 10, 6, 24, 28, 8, 9 |
Practices Reports writing | 19.25 | 0.77 | 1, 10, 5, 4, 15, 20, 24, 25, 7, 21, 28, 9 |
Study | 36.75 | 1.47 | 18, 13, 12, 11, 14, 19, 17, 16, 20, 25 |
The final grade of the subject is obtained from the exam notes, the continuous work of the student (learning evidences) and of the practices.
Average of the exams of the subject = 0.50 x note exam block I + 0.50 x note exam block II
Final mark of the course = 0.85 x average mark of the exams of the subject + 0.15 x note continuous work + 0.20 x note practices
To pass the subject, the following three conditions must be fulfilled:
1) The average of the exams of the subject should be ≥ 5.0
2) The mark of the examination of each block must be ≥ 3.0
3) The note of the practices should be ≥ 4.0
Students who do not pass the subject for failing to meet any of the above three conditions, regardless of whether the final grade is greater or equal to 5.0, they will obtain a maximum final grade of 4.5 considering- if the subject is suspended.
Continued work (10%):
1) Evidence of each student will be collected in each of the two blocks throughout the semester (problems solved individually or in groups, self-assessments on the virtual campus, short tests in class, tests, etc ...).
2) The note of the continuous work will be the average of the notes of the evidences collected throughout the course. The fact of not appearing to evidence implies a zero in that evidence.
Exams (70%):
1) An examination will be carried out at the end of each block (examination of block I and examination of block II).
2) At the end of the semester will be offered examinations of recovery of the two blocks (exams of second option).
- To participate in the recovery, the students must have been previously evaluated in a series of activities whose weight equals to a minimum of two thirds of the total grade ofthe subject.
- There is the possibility that students who do not need it will be presented to second-choice exams to improve the qualification of the course.
For all students to submit to these second-choice exams (recovery) or improvement), the block exam will be the one they get in this second option exam.
For all students to submit to these second-choice exams (improvement), the block exam will be:
- equal to that of the second option exam, if the note of the second option exam> course examination note,
- equal to the average of the block exam and the second option exam, if the note of the second option of the option < course exam notes.
Practices (20%):
The final mark of the practices will be calculated from the laboratory reports (60%) and the test exam of the knowledge acquired in the laboratory (40%).
Use unauthorized methods during one of the examinations of the subject (copy or communicate with a colleague, use of cell phones, use of smart clocks, etc ...) will be penalized with a "suspense" rating in the global course of the current course.
To attend an examination of any block it is essential to bring an identification document (ID or university card) with a recent and good quality photograph.
The qualification of "NOT EVALUABLE" will be obtained in the following cases:
Title | Weighting | Hours | ECTS | Learning Outcomes |
---|---|---|---|---|
Block 1 (1st partial) exam | 35% | 0 | 0 | 1, 10, 3, 13, 11, 14, 15, 25, 23, 28 |
Block 2 (2nd partial) exam | 35% | 0 | 0 | 10, 5, 12, 17, 16, 7, 21, 28 |
Learning evidences | 10% | 0 | 0 | 1, 18, 10, 4, 19, 2, 27, 20, 25, 26 |
Practices | 20% | 0 | 0 | 1, 10, 4, 15, 22, 19, 6, 2, 20, 24, 25, 26, 8, 9 |
Textbook:
- “Química General”. Ralph Petrucci, Wiliam Harwood, Geoffrei Herring. Prentice-Hall (Pearson) 10a Edició, 2011. ISBN: 9788483226803
http://www.ingebook.com.are.uab.cat/ib/NPcd/IB_Escritorio_Visualizar?cod_primaria=1000193&libro=6751
Other support books:
- “Química”, Raymond Chang, Kenneth A. Goldsby. 11a Edició. Editor MacGraw Hill, 2013. ISBN 978-6071509284
- "Principios de Química", P. Atkins i L. Jones, Médica Panamericana, 3ª edició, 2006. ISBN 950-06-0080-3
- "Equilibrios iónicos y sus aplicaciones analíticas” Manuel Silva, José Barbosa. Ed. SINTESIS, 2002. ISBN: 9788497560252
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