COMPETENCES



SPECIFIC COMPETENCES



FB4. Ability to understand and apply the basic knowledge of principles of general chemistry, organic and inorganic chemistry, and their applications in engineering.



FB7. Ability to apply strategies of scientific method: analyze a problematic situation qualitatively and quantitatively, propose hypotheses and solutions using appropriate models.



FB8. Ability to communicate effectively the knowledge, procedures, results, skills and issues relating to basic engineering subjects, using appropriate vocabulary, terminology and means.



TRANSVERSAL COMPETENCES



FB10. Adoption of a responsible and ordered attitude at work, prepared to a lifelong learning experience.



LEARNING OUTCOMES



1. Know and apply models of the structure of the matter to understand the properties and behavior of substances and materials (FB4).



2. Know and understand the basic principles and theories about the physical and chemical processes that chemical substances can undergo under certain conditions in order to determine, in each case, the effects produced (FB4).



3. Resolve problems and/or laboratory experiences reasonably, including writing accurate lab-reports (FB7).



4. Communicate and transfer knowledge, procedures and results by using the specific terminology of chemical engineering (FB8).



5. Adopt a responsible and ordered attitude and a positive learning readiness (FB10).



6. Acquire knowledge and learning strategies that enable to progress in subsequent studies (FB10).

To achieve the objectives defined in the subject, the following selection of contents has been made:



UNIT 1. BASIC PRINCIPLES

- Nomenclature of inorganic chemistry.

- States of matter.

- Basic concepts (atomic mass, mole concept, molar mass, etc.).

- Determination of chemical formulas (empirical and molecular formulas).

- Symbolic representation of chemical reactions through chemical equations.

- Basic concepts related with chemical equations (stoichiometry, limiting reagent, yield and purity).



UNIT 2. ATOMIC AND MOLECULAR STRUCTURE

- Quantum-mechanical model of the atom.

- Electronic structure.

- Periodic table. Periodic properties.

- Chemical bonding.

- Structure and properties of molecular compounds.



UNIT 3. AGREGATE STATES OF MATTER. PHASE EQUILIBRIA

- Solid state (types of crystalline solids and their characteristic properties (thermal conductivity, electrical conductivity in solid state, liquid or in solution, melting point and solubility, among others).

- Gaseous state (properties of the gases, ideal gaseous systems, kinetic theory of gases).

- Liquid state (surface tension, viscosity, vapour pressure).

- Equilibrium phase diagram.



UNIT 4. THERMOCHEMISTRY

- First principle of thermodynamics.

- Calculation of the change of internal energy (∆U) and enthalpy (∆H) in a substance. Energy exchange processes with and without phase change.

- Calculation of the change of internal energy (∆U) and enthalpy (∆H) in a chemical reaction.



UNIT 5. SOLUTIONS. COLLIGATIVE PROPERTIES

- Solutions and calculation of the concentration.

- Solubility and Henry’s Law.

- Colligative properties.

- Volatile solute solutions. Ideal behaviour (Raoult’s Law) and real behaviour (Pxy/Txy diagrams).

-Simple distillation process.



UNIT 6. BASIC PRINCIPLES OF ORGANIC CHEMISTRY

- Nomenclature of organic compounds. Functional groups.



UNIT 7. KINETICS OF CHEMICAL REACTIONS

- Basic concepts of chemical kinetics: reaction rate, reaction order and reaction law.

- Simple kinetics models: zero, first and second order reactions.

- Effect of temperature. Arrhenius equation.

- Introduction to catalysis.



UNIT 8. CHEMICAL EQUILIBRIUM

- Thermodynamic principles of chemical equilibrium.

- Le Chatelier’s principle.



UNIT 9. EQUILIBRIUM IN AQUEOUS SOLUTIONS

- Basic concepts (acid, base, conjugated species, amphoteric species).

- Acid (Ka) and basic (Kb) dissociation constant.

- pH scale.

- Reaction of hydrolysis.

- Acid-base titration (equivalence point, titration error and acid-base indicators).



UNIT 10. HETEROGENEOUS IONIC EQUILIBRIUM

- Precipitation reactions.

- Constant solubility product (Kps).

- The common-ion effect.

- The pH variation effect.

- Fractional precipitation.



UNIT 11. ELECTROCHEMISTRY

- Redox reactions.

- Voltaic or galvanic cell.

- Electrolytic cell.

PRESENTIAL ACTIVITIES



THEORETICAL CLASSES (45 h)



During the 30 weeks of the academic year, concepts and theoretical developments will be taught in a weekly session (1.5 h). Explanations will be complemented with standard exercises and activities that will allow the acquisition of stablished skills.



CLASSROOM PRACTICES (30 h)



During the 30 weeks of the academic year, resolution of exercises and practical activities will be carried out in a weekly session (1.0 h).



LABORATORY PRACTICES (15 h)



Students must complete 5 laboratory practices of 3 hours each. Lab sessions will be taught in the Laboratory practices will allow students to experiment and put into practice the knowledge acquired through lectures, classroom practices and personal work. Moreover, they will make it possible to learn about the basic experimental techniques used in a chemical laboratory and to acquire skills typical of laboratory work.



Students must complete 5 different laboratory practices of 3 h each. Lab sessions will be taught in the Basic Chemistry laboratory of the Faculty of Engineering Vitoria-Gasteiz, according to the calendar and schedule proposed for each group.



The practices will be carried out individually, as long as the available material allows it. Otherwise, the practices will be carried out in pairs, which will allow, additionally, to promote other skills, such as teamwork.



Each student must deliver a questionnaire before the beginning of each practical session, in which several questions related to the practice must be answered. This report must be answered and delivered individually at the time of entering the laboratory. At the end of the practical session, the students must take a test related to the content of the practice. Finally, the students will have one week to deliver a final report containing the results obtained and the main conclusions of the practice.



TUTORSHIP SESSIONS



In general, it is a voluntary activity (individual or collective) conducted in response to students’ request. However, throughout the course a series of voluntary group deliverables will be proposed that will require attendance at tutorials.



NON-PRESENTIAL ACTIVITIES (135 h)



Continued work of student is essential to develop the competences of the subject. In addition to preparing the written exams, students should devote the hours of non-presential teaching to:



o Complete notes, consult bibliography and solve questions and/or problems, including voluntary deliverable tasks (a time commitment of approximately 3-4 h per week).



o Prepare the laboratory sessions (a time commitment of 1.5-2.0 h to prepare the laboratory practice and answer a set of preliminary questions per practice) and complete the corresponding report (2.0-3.0 h commitment per practice).



If the extraordinary circumstances derived from the current public health emergency situation caused by the outbreak of COVID-19 oblige to develop online teaching, all media available in the UPV/EHU (BlackBoard Collaborate, eGela, etc.) will be used.

EVALUATION SYSTEM



WRITTEN TEST/EXAM (70 % of the final mark)



The written test will comprise two partial tests:



- The first test corresponds to the contents of the first four-month period and will be carried out during the month of January, coinciding with the period established by the Center to carry out the exams of the first four-month period.



-The second test will be carried out in May, coinciding with the period established by the Center to perform the exams of the Ordinary Call. In this case:



If the student has obtained a mark ≥5 in the first test, he/she will be evaluated on the contents of the second four-month period.



The final grade corresponding to the written test will be calculated as the simple average of the marks of the two tests, as long as a mark ≥4 has been obtained in the second test.



If the student has obtained a mark <5 in the first test, he/she will be evaluated on the contents of the whole subject. Moreover, the exam will be formed by two differentiated parts, belonging each one to the contents of each four-month period.



The final grade corresponding to the written test will be calculated as the simple average of the grades obtained in the 2 parts that make up the exam of the Ordinary Call, being necessary that both grades are ≥4 out of 10.





PRACTICAL ACTIVITIES (10 % of the final mark)



Practical activities will be undertaken throughout the course, such as problem solving and cases, written tests or questionnaires, amongst others.



LABORATORY PRACTICES (20 % of the final mark)



- Laboratory work: 25 %

- Presentation and evaluation of the previous deliverables: 15 %

- Evaluation test (after each lab-session): 25 %

- Presentation and evaluation of the final deliverables: 35 %



REQUIREMENTS to pass the subject:



- Complete all the laboratory practices and deliver all the previous questionnaires, post-practice evaluation tests and the final report within the deadline.



- Obtain a mark ≥5 in the final grade (obtained as a weighted average of the marks corresponding to the written test, practical activities and laboratory practices). Moreover, it is compulsory to:



o Obtain a mark ≥5 out of 10 in the written test (70 %).



o Obtain a mark ≥4 out of 10 in the laboratory practices (20 %).



o It is not necessary to obtain a minimum mark in the practical activities (10 %).



Those students who do not meet any of these requirements will be marked with a 4.0 (maximum) in the Ordinary Call regardless of the final grade obtained.



*If the extraordinary circumstances derived from the current public health emergency situation caused by the outbreak of COVID-19 oblige to develop an online evaluation, all media available in the UPV/EHU (Webex, eGela, etc.) will be used. The characteristics of this new evaluation mode will be published in eGela.



CALL RESIGNATION



Those students who do not appear for the written test will be recorded as "Not Presented" in the Ordinary call.



FINAL TEST



Students who meet the conditions established in the UPV/EHU regulations and request to take a final test within the deadline set for that purpose (Chapter II, Article 8 of the Agreement of December 15, 2016, of the Governing Council of the University of the Basque Country/Euskal Herriko Unibertsitatea, which approves the Regulations governing the students’ Evaluation in official Bachelor's degrees), they need to implement the following activities:



- A written test related to the theoretical-practical contents of the subject (80 % of the final grade).



- A practical laboratory exam (20 % of the final exam).



REQUIREMENTS to pass the subject (FINAL TEST)



Obtain a mark equal to or greater than 5 in the final grade (obtained as the weighted average of the marks corresponding to the written test and the practical exam).



*If the extraordinary circumstances derived from the current public health emergency situation caused by the outbreak of COVID-19 oblige to develop an online evaluation, all media available in the UPV/EHU (BlackBoard Collaborate, eGela, etc.) will be used. The characteristics of this new evaluation mode will be published in eGela.



CALL RESIGNATION



Those students who do not appear for the final test will be recorded as "Not Presented" in the Ordinary call.

Collections of problems and specific questions related to the subject.

Basic bibliography

NOMENCLATURE OF INORGANIC CHEMISTRY



o Beobide, G. (2019). Formulazioa eta nomenklatura kimikoa. IUPACen arauak eta ariketak. Ed. UPV/EHU.



o Quiñoá, E.; Riguera, R.; Vila, J. M. (2010). Nomenclatura y formulación de los compuestos inorgánicos. Ed. McGraw-Hill.



o Quiñoá, E.; Riguera, R. (2010). Nomenclatura y representación de los compuestos orgánicos. Ed. McGraw-Hill.





GENERAL CHEMISTRY



o Brown, T. D.; Lemay, H. E.; Bruce, J. R.; Bursten, E.; Burdge, J. (2003). Química. La Ciencia Central. Ed. Pearson Prentice Hall.



o Casabó, J. (2009). Egitura atomikoa eta lotura kimikoa. Ed. UPV/EHU.



o Chang, R. (2010). Química. Ed. McGraw-Hill, 10º edición.



o Quiñoá, E.; Riguera, R. (2004). Cuestiones y ejercicios de química orgánica. Ed. McGraw-Hill, 2º edición.



o McMurry, J.E.; Fay, R.C. (2009). Química General. Ed. Pearson Education, 5º edición.



o Reboiras, M.D. (2008). Química: la ciencia básica. Ed. Thomsom, 2º edición.



o Urretxa, I.; Iturbe, J. (1999). Kimikako problemak. Ed. Udako Euskal Unibertsitaea.



o Vollhardt, K.P.C.; Schorbe, N.E. (2008). Kimika organikoa egitura eta funtzioa. Ed. UPV/EHU.





LABORATORY PRACTICES



o Beran, J.A. (2014). Laboratory Manual for Principles of General Chemistry. Ed. Wiley.



o Chemical Education Material Study (1987). Química. Una ciencia experimental. Ed. Reverté.



o Martínez, J.; Narros, A.; de la Fuente, Mª del Mar; Pozas, F.; Díaz, V. M. (2009). Experimentación en química general. Ed. Paraninfo.



o Navarro, A.; Gonzalez, F. (1986). Prácticas y técnicas de laboratorio. Ed. Universidad Politécnica de Catalunya.

In-depth bibliography

o Casabó, J. (2007). Estructura atómica y enlace químico. Editorial Reverté.

o Ghasem, N.; Henda, R. (2009). Principles of Chemical Engineering Processes. Editorial Taylor & Francis Group.

o Primo-Yúfera, E. (2007). Química Orgánica básica y aplicada: de la molécula a la industria. Tomo II. Editorial Reverté.

o Rodgers, G. E.; Cabañas, M. V.; Regi, M. V. (1995). Química inorgánica: introducción a la química de coordinación, del estado sólido y descriptiva. Editorial McGraw-Hill Interamericana de España.