"General Chemistry II" is a basic subject of the first year of the Degree in Chemistry and the Degree in Chemical Engineering. It forms part of the fundamental module and is a complement to the subject of the same course "General Chemistry I" (first semester). These two subjects are the basis of the chemistry subjects of the basic module.



The theoretical contents of "General Chemistry II" are put into practice in the subject of the first year of the Degree in Chemistry "Experimental Methodology in Chemistry".



The first part of the subject begins with the study of two of the main fields of Chemistry such as Kinetics and Thermodynamics. Regarding the first one, the necessary knowledge about the rate of reactions is acquired, which allows carrying out experimental studies on this subject. Thermodynamics is the main tool to carry out studies on the energetic changes that accompany chemical and physical processes, as well as to address the study of equilibrium and spontaneity of the processes. In fact, the study of the equilibrium state is deepened, which includes the chemical equilibrium itself and the equilibrium between phases in one-component systems. From a professional point of view, with these tools, we can find out how fast a product can be obtained industrially, what energy is needed to produce it, or what is the performance of the process in question. In addition, we can also determine which are the most appropriate conditions to optimize these parameters.

The second part of the subject deals with the study of equilibria in solution. As an introductory way, the dependence of the equilibrium constants with the ionic force is described, and the concentration constants are introduced, as well as the characteristic terminology of the different types of reactions involved in the equilibria. It then goes on to describe the four fundamental pillars on which chemistry in solution is based: acid-base reactions, complex formation, precipitation and finally oxidation-reduction reactions. For the four types of reactions, the numerical and graphical methodologies that allow solving the chemical problems of equilibrium in solution are explained.



"General Chemistry II" is the starting point for other subjects of higher courses. Specifically, in the Degree in Chemistry three subjects from the basic module of the second year: "Physical Chemistry I", "Experimentation in Physical Chemistry" and "Analytical Chemistry I" and also subjects from the third year of the same degree. In the case of the Degree in Chemical Engineering, it is important to control the contents obtained in "General Chemistry II" to study the subjects "Applied Thermodynamics" and "Kinetics of Chemical Processes" in the second year of the degree.

In this subject, the bases of Chemical Kinetics and Thermodynamics are studied, as well as Ionic Equilibria in Solutions.



COMPETENCIES

In this subject, the student develops the following competencies:

1.Understanding and use of the principles and basic theory of the chemical reaction of different types of substances.

2.Understanding and use of mathematical tools and data analysis processes in a scientific environment.

3.Capacity for observation, analysis and presentation of results in the field of chemistry and other experimental sciences

4.Knowledge and use of reference styles of scientific literature in oral and written communication.

5. Know the most frequent sources of information and documentation in experimental sciences and demonstrate their efficient use.







LEARNING RESULTS

The student achieves the following Learning Results related to the afore mentioned competencies:



Chemical kinetics

-Adequately interpretS the experimental results of a chemical reaction to quantify the reaction rate and to predict the reaction mechanism.



Thermodynamics

-AnalyzeS, calculateS and interpretS the energy changes that occur in chemical processes.

-Using the entropy concept predicts the direction and extent to which chemical and physical changes occur



Chemical/physical Equilibrium

-Using thermodynamic concepts, quantitatively and qualitatively describes the chemical equilibrium and the effect of external factors on it.

- Evaluates and analyzes the conditions for phase changes to occur in pure substances and for these phases to be in equilibrium.

- Identifies the relationships between the different chemical equilibria and the variables that can change the equilibrium conditions.

- Predicts the reactions that take place (neutralization, titration, masking, coprecipitation, etc...) when mixing different substances in solution and deduces the majority species present at equilibrium.

- Handles the appropriate methodologies to solve numerically and graphically the problems associated with equilibria in solution

The contents of the course "General Chemistry II" are theoretical and are applied through problem solving. In the Chemistry Degree, the laboratory practices related to these theoretical contents are developed in the subject "Experimental Methodology in Chemistry"



I. CHEMICAL KINETICS.

REACTION RATE. Factors that affect the rate of reaction. Differential velocity equation. Reaction order. Experimental methods to determine the rate of reaction. Initial velocity method. Integrated rate equations. half-reaction period. Influence of temperature on the reaction rate.



MECHANISMS OF CHEMICAL REACTIONS. elementary processes. Complex processes. Obtaining the rate equation consistent with a given mechanism: Approximation of the limiting stage. Steady state approximation. Collision theory: activation energy.Transition state theory. Energy profile of an elemental reaction and a complex reaction. Catalysis.



II. CHEMICAL THERMODYNAMICS.

THERMOCHEMISTRY. Job. Heat. First Law of thermodynamics. Internal energy and enthalpy. Experimental determination of heats of reaction. Calorimetry Enthalpies of reaction and standard formation. Link energies. Effect of temperature on the enthalpy of a reaction.



CHEMICAL THERMODYNAMICS. ENTROPY AND FREE ENERGY. Entropy concept. Calculation of entropy. Second principle of thermodynamics. Criterion of spontaneity and balance in a closed system. Entropy calculations for different types of processes. General condition of spontaneity and equilibrium: Gibbs free energy. Helmholtz free energy. Entropy at the molecular level. Third Principle. Gibbs free energy change of a reaction.Coupled reactions.



III. CHEMICAL EQUILIBRIUM. Chemical potential and material equilibrium. The equilibrium constant. Influence of temperature on the equilibrium constant. Modification of the equilibrium state. Chemical equilibrium in non-electrolytic solutions. Chemical equilibrium in electrolyte solutions.



IV. PHASE EQUILIBRIUM IN PURE SUBSTANCES. Liquid-vapour balance. Vapor pressure. Dependence of Pv with temperature. Solid-vapor equilibrium. Solid-liquid balance. Thermodynamic treatment of phase equilibria. Phase diagram. Critical state. Phase rule.



V. EQUILIBRIA IN DISSOLUTION. Types of equilibrium constants. Ionic force. Activity coefficients. Debye-Hückel theory.



ACID-BASE EQUILIBRIA. The role of the solvent. Acid-base behavior of water. Strength of acids and bases. Acid-base balance calculations. The mass balance. Electroneutrality equation. Proton balance equation. Numerical and graphic resolution of the acid-base balance. Weak monoprotic and polyprotic protoliths. Buffer solutions. Buffer capacity.



VI. COMPLEX FORMATION EQUILIBRIA. Description of the balance. Types of complexes. Monodentate and polydentate ligands. Addition complexes and chelates. Stability and inertia. Equilibrium constants: successive and global. Mass balance equations. Balance calculations. logarithmic diagrams. Influence of pH. Applications: Masking.



VII. PRECIPITATION EQUILIBRIA. Description of heterogeneous equilibrium. Solubility product. Solubility. Factors that affect solubility. saline effect. Common ion effect. parasitic reactions. logarithmic diagrams. Fractional precipitation. Influence of pH. Influence of complex formation reactions. Applications.



VIII. OXIDATION-REDUCTION EQUILIBRIA. Introduction. Standard electrode potential. Types of redox processes. Nersts equation. Equilibrium constant. Equilibrium potential. Redox system of water. Factors on the electrode potential. dismutation.



IX. SOLUTIONS. Types of solutions. Partial molar properties. Multicomponent systems and chemical potential. Thermodynamic properties of ideal solutions. non-ideal solutions. electrolyte solutions. Colligative properties.

The course includes master classes (M) where the theoretical concepts of each content are given. Group or individual activities can also be carried out so that the student can discuss the given contents.



In order to achieve the learning results of the subject, the master classes are complemented with classroom practices (GA) where in a reasoned way and analyzing data and results, practical problems are solved. The problems can be solved individually or in groups and the results are obtained together, always guided by the teacher. These problems constitute a model for the student on their own or in a group to solve similar situations that can be evaluated.



Likewise, seminars are held where doubts are resolved and unknown situations are evaluated, using the knowledge that the students are acquiring in their learning process and reasoning the ideas.



In the second part of the course, classes are taught in computer rooms (GO). Through the MEDUSA program, acid-base equilibria, complex formation, precipitation and oxidation-reduction exercises are solved graphically.

• Final Assessment System
• Tools and qualification percentages:
  • Written test to be taken (%): 75
  • Realization of Practical Work (exercises, cases or problems) (%): 25

The general evaluation criteria are:

- Degree of knowledge of the contents

- Data analysis and critical achievement of results

- Use of scientific language

- Clarity in reasoning



The evaluable tasks required during the course are obligatory and consist of:

- Individual or group reports on the quantitative resolution of problems about chemical reactions and chemical equilibrium situations

- Individual or group questionnaires carried out both in person and on-line, focused on the development of the analysis and diagnosis of unknown situations.

The sum of the grade obtained in these two tasks will constitute 25% of the final grade.

- Final test, whose grade will account for 75% of the final grade.

Likewise, active attendance in face-to-face classes and participation in required tasks are taken into account.



For non-face-to-face evaluable tasks, the corresponding feedback is provided to promote the learning process. The tasks carried out in the face-to-face sessions, the feedback will be collective in said sessions.



To pass, 5 points out of 10 are required and it is a requirement to obtain a minimum of 4 points out of 10 in the final test, this score being balanced between all parts of the test.



If the minimum required grade is not achieved in the final test, the grade for the subject is the one obtained in said test.



If the final test grade is greater than or equal to the minimum required grade, the final grade constitutes 75% of the final test grade and 25% of the grade for the evaluable tasks carried out during the course.

If a student cannot perform the evaluable tasks scheduled during the course, the grade for the subject is the one obtained in the final test. If this is the case, the teaching staff must be notified in writing within the period stipulated by the evaluation regulations.



Failure to take the scheduled test means renunciation of the call.

It consists of a written test and it is necessary to obtain a minimum of 5 points out of 10, this score being balanced between all the parts of the test.

If the grades obtained throughout the course are positive, they are taken into account and the final grade consists of 75% of said test and 25% of the tasks. On the contrary, if the grades for the tasks are negative, it is not taken into account in the final grade for the subject and this is 100% of the grade for the final test.

Basic bibliography

- R.H. Petrucci, W.S. Harwood ,F.G. Herring, "Química General", (8. ed.), Prentice Hall, Madrid, 2003

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

- P. Atkins, L. Jones, "Principios de Química. Los caminos del descubrimiento", (3. ed.), Médica Panamericana, 2009.

- A. J. Bard "Equilibrio Químico" Ediciones del Castillo, 1977.

In-depth bibliography

- D.W. Oxtoby, H.P.Gillis, N.H. Nachtrieb, "Principles of Modern Chemistry", (5. ed.), Brooks Cole, 2002.
- R. Levine, "Fisicoquímica", 1 eta 2 liburukiak, (5. ed.), Mac Graw Hill, 2004.
- R.J.Silbey, R.A.Alberty, "Kimika fisikoa", Argitalpen serbitzua UPV/EHU, 2006.
- M.S.Silberberg, "Química General", McGraw Hill, México, 2002.
- I.Urretxa , J.Iturbe, "Kimikako Problemak", Udako Euskal Unibertsitatea, 1999.
- Skoog, West, Holler, Crouch, "Fundamentos de Química Analítica", 8ª edición, Thomson, 2005.
-- M. Silva, J. Barbosa, "Equilibrios Iónicos y sus Aplicaciones Analíticas", Síntesis, 2002.

Web addresses

http://webbook.nist.gov/chemistry/
http://www.chem1.com/acad/webtext/virtualtextbook.html
http://www.buruxkak.org