This course complements the content covered in General Chemistry I, which is taught in the first semester. Specifically, it focuses on introductory aspects related to Physical Chemistry and Analytical Chemistry.

Topics covered include descriptions of pure substances and various possible mixtures or solutions. Basic aspects of Thermochemistry and Chemical Kinetics are developed, followed by an introduction to general concepts of chemical equilibrium. These concepts are subsequently applied to equilibrium in ionic solutions, specifically addressing acid-base equilibria, redox equilibria, and complex ion equilibria. The course also covers concepts related to substance solubility.

The theoretical content of “General Chemistry II” is put into practice in the first-year course “Experimental Methodology in Chemistry.” Additionally, “General Chemistry II” serves as a foundation for other upper-level courses. Specifically, it is a prerequisite for three basic module courses in the second year: “Physical Chemistry I,” “Experimental Chemistry,” and “Analytical Chemistry I.”

To succeed in the “General Chemistry II” course, students need a solid understanding of chemistry and mathematics acquired during their high school education (“bachiller”) and the knowledge gained in “General Chemistry I.”

This course belongs to the Basic Module of the Chemistry Degree program. As such, it aims to develop the following competencies:



1.M01CM02: Understanding and handling the fundamental principles and theory of chemical reactions involving different types of substances.

2.M01CM10: Knowledge and use of referencing styles from scientific literature in oral and written communication.

3.M01CM11: Familiarity with common information sources and documentation methods in Experimental Sciences.



By taking this course, students achieve the following learning outcomes related to the competencies mentioned above:



1.RA1: Understands the concepts, principles, and fundamental theories related to chemical reactions in various types of substances. Applies this knowledge to solve quantitative or qualitative problems in the field of Chemistry.

2.RA2: Formulates the thermodynamic equilibrium constant and predicts reactions (neutralization, titration, masking, coprecipitation, etc.) that occur when different substances are mixed in solution. Deduces the major species present in equilibrium.

3.RA3: Familiar with referencing styles used in scientific literature. Cites and references sources in oral and written communication within the field of Chemistry.

4.RA4: Acquainted with common information sources and documentation methods in Experimental Sciences. Knows how to search, evaluate, and utilize relevant information in the field of Chemistry.



The translation of the given text to English is: "The coordination of this subject with the others in the Module and the Degree corresponds to the Degree Coordination Committee.

- Chemical Thermodynamics. Heat and work. First Law. Enthalpy. Enthalpies of reaction and formation. Hess’s Law. Temperature effect: Kirchhoff’s law. Standard enthalpies of formation. Heat of dissolution and dilution. Bond energies. Entropy and the Second Law. Free energy, spontaneity, and equilibrium.

- Phase Equilibria in Pure Substances. Liquid-vapor equilibrium. Vapor pressure. Solid-liquid equilibrium. Solid-vapor equilibrium. Phase diagrams.

- Mixtures and Solutions. Types of solutions. Concentration units. Partial molar quantities. Solubility and saturation. Ideal solutions: Colligative properties. Real solutions. Activity.

- Chemical Kinetics. Reaction rate. Rate equations and order of reaction. Factors influencing reaction rate. Reaction mechanisms. Catalysis.

- Chemical Equilibrium. Concept of equilibrium. Equilibrium involving gases. Equilibrium constants. Heterogeneous equilibria. Le Chatelier’s principle.

- Chemical Equilibrium in Ionic Solutions. Ionic strength. Concentration and activity. Debye-Hückel law. High ionic strength. Thermodynamic equilibrium constant.

- Acid-Base Equilibria. Equilibria in pure water. pH scale. Acid-base systems. Buffer solutions. Acid and base mixtures.

- Solubility. Solubility and solubility product. Common ion effect. Factors affecting solubility. Physical aspects of precipitation.

- Complex Ion Equilibria. Labile and inert complexes. Stable and unstable complexes. Chelates. Side reactions and conditional constants. Masking.

- Redox Equilibria. Electrochemical cells. Nernst equation. Relationship between E₀ and equilibrium constant. Factors affecting electrode potential.

The course consists of approximately two weekly lecture hours, during which theoretical content will be covered. In classroom practices, students will work on various problems and exercises. The class will be divided into smaller groups for these activities. Seminars will focus on teamwork and may involve computer-based tasks, oral presentations, and in-depth problem-solving.

• Continuous Assessment System
• Final Assessment System
• Tools and qualification percentages:
  • Written test to be taken (%): 70
  • Realization of Practical Work (exercises, cases or problems) (%): 20
  • Exhibition of works, readings ... (%): 10

The preferred evaluation system for this course is continuous assessment. All evaluative tasks required during the course are mandatory and consist on:



- Completion of both group exercises and individual questionnaires proposed on the eGela virtual platform within specific time frames. These contribute 20% to the final grade.

- Completion and public presentation of a project related to a thematic topic or problem within the course. The presentation can take the form of a poster or an oral presentation in class. This contributes 10% to the final grade.

- A theoretical-practical exam covering the entire course content. This exam constitutes 70% of the final grade.

- Active attendance in face-to-face classes and participation in required tasks are also considered.





To pass the course, students must complete all proposed activities and achieve a minimum score of 5 out of 10 in the overall subject. Additionally, they must obtain at least 4 points out of 10 in each of the two parts of the final exam.



Students can choose the final evaluation system independently of their participation in continuous assessment. To do so, they must submit a written request to the responsible faculty during the first 9 weeks of the teaching period (second semester). If students opt for the final evaluation system, it includes: a written theoretical-practical exam; a multiple-choice test similar to the questionnaires proposed on the eGela platform; and a brief oral presentation on one of the course topics.



Not taking the final exam will result in a final grade of “not presented.”

The extraordinary examination consists of a written exam, and students must obtain a minimum of 5 points out of 10. If students achieved positive results in continuous assessment activities during the course, those results will be retained. The final grade will then be calculated as 70% of the extraordinary exam, 20% from tasks, and 10% from the presentation. If continuous assessment results were not positive, they will not be considered for the extraordinary examination, and the final grade will be based solely on the 100% score from the final exam. In either case, obtaining at least 4 points out of 10 in each part of the final written exam is necessary.



Activities performed throughout the course, whether on the eGela platform or through oral presentations or posters, will be kept for one academic year in case a student does not pass the course.

Beharrezkoak diren irakas materialak ikasleek eskuragarri izango dituzte eGela plataforman.

Basic bibliography

R.H. Petrucci, W.S. Harwood y F.G. Herring. Química General, (8ª Ed.). Prentice Hall, 2003.

R. Chang. Química (9ª Ed.). McGraw-Hill, 2007.

M.S. Silberberg. Química General. McGraw-Hill, 2002.

P.W. Atkins. Química Física, 6ª edición. Omega, 1999.

J.M.Elortza. Termodinamika Makroskopikoa. U.E.U.-ko Kimika Saila, 1.991.

D.C. Harris. Análisis Química Cuantitativo 3ª ed. (6ª ed. Original). Editorial Reverté, 2007.

M. Silva, J. Barbosa. Equilibrios iónicos y sus aplicaciones analíticas. Editorial Síntesis, 2004.

L. Jones y P.W. Atkins. Principios de Química, 3rd edition. Editorial Médica Panamericana, 2003.

Problemas resueltos de Termodinámica. M. Del Barrio y otros. Thomson, Madrid 2005.

UEUko Kimika Saila Kimika Orokorra. Udako Euskal Unibertsitatea, 1996.

I. Urretxa y J. Iturbe. Kimikako Problemak. Udako Euskal Unibertsitatea, 1999.

In-depth bibliography

K.W. Whitten, K.D. Gailey y R.E. Davis. Química General, 3rd ed. McGraw Hill, 1992.
J. A. Rodríguez Renuncio, J.J. Ruiz Sánchez y J.F. Urieta Navarro. Termodinámica Química. Síntesis,1998.
I.N. Levine. Problemas de Fisicoquímica. McGraw Hill, 2005.
G. D. Christian. Analytical Chemistry 6th ed. John Wiley & Sons, 2004.

Journals

Journal of Chemical Education, American Chemical Society.

Web addresses

http://www.ehu.es/zorrilla/juanma/qw6.html

(A Compilation of Dozens of Websites Dedicated to Various Topics in Chemistry)Pagasarri