Description of the subject



In this subject students begin their training by learning to formulate, a basic aspect for a graduate in Pharmacy. Next, the atomic models are explained, both the first ones and the current ones.



This subject is intended to endow students with the basic knowledge of the composition of matter (atoms, molecules, bonds, etc.), the changes that matter can undergo (chemical reactions) and the physical and chemical properties resulting from this composition. Besides, within the section of Inorganic Chemistry, students acquire initial knowledge about the different families of chemical elements, their properties and their biological and pharmacological interest.



Contextualisation of the subject



The objectives of this degree include training pharmacists, highly qualified professionals in drugs and in their impact on

health. Drugs are usually synthetic chemical substances. Having a solid knowledge in chemistry is essential for the appropriate management and use of medicines. Knowledge of the basic principles of General Chemistry and, in particular, of Inorganic Chemistry is essential for the suitable management of drugs.



According to the CIN / 2137/2008 order, which establishes the requirements for the verification of the official university qualifications that qualify for the practice of the profession of Pharmacist, the curriculum of the degree must have a

Chemistry module with a minimum of 54 ECTS.



Within this module of Chemistry, the subject General and Inorganic Chemistry is taught at first, the first semester of the first year.



This subject, in its section of General Chemistry, lays the basic knowledge on chemistry, reinforcing the knowledge that the students bring from High School and widening it from a university viewpoint.



That is, the subject is basic to be able to take the other subjects of the chemistry module of the degree (Organic Chemistry, Physicochemistry, Analytics, etc.). Therefore, as stated before, this subject is set in the first course and first semester of the degree and is basic to be able to take the remaining subjects of the chemistry module.

Skills / Learning outcomes



SKILLS



1.Analyze the different atomic models and the disadvantages of each of them.



2.Know the Periodic Table and the relationship between the electronic configurations of the elements and certain

properties.



3.Know the different bond models and relate the chemical properties of the compounds with the type of bond established

between ions, atoms and molecules.



4.Know and understand the characteristic properties of the elements and their compounds, as well as their application in

the pharmaceutical field.



5.Identify the different types of chemical reactions (acid-base and redox) that take place in solution and perform

stoichiometric calculations.



6.Formulate and name chemical compounds.



7.Know the general properties of metallic and non-metallic elements, and inorganic compounds, especially those of

sanitary interest.



8.Know the features and properties of coordination compounds, especially their functions and applications in biological

processes.



9.Use basic techniques and materials in a chemistry laboratory.



10.Estimate the risks associated with the use of chemical substances and laboratory processes.



TRANSVERSAL SKILLS



Written communication, teamwork, information search.



LEARNING OUTCOMES



1.The student recognizes the different chemical compounds, both inorganic and organic, and he/she is able to formulate

and name them according to the IU-PAC rules.



2.The student is able to locate the chemical elements of the Periodic Table and relate their electronic configurations with

their physical and chemical properties.



3.The student recognizes the different bond models and he/she is able to relate the physical and chemical properties of the

compounds with its structure.



4.The student handles the units of concentration of the solutions and knows their properties.

5.The student recognizes the different types of chemical reactions (acid-base and redox) and the chemical equilibria in

solution.



6.The student knows the characteristic properties of chemical elements and their compounds.



7.The student is able to apply the theoretical knowledge acquired in laboratory practicals and during the resolution of

issues and problems.



8.The student knows the risks associated with the use of chemical substances and laboratory processes.



9.The student knows the suitable experimental procedures for the transformation, separation, isolation and purification of

compounds, including the use of appropriate scientific equipment for synthesis.



10.The student knows how to prepare reports, summaries and presentations of theoretical and(or) experimental works,

both individual or as a part of a group, with a critical thinking and using the appropriate scientific language.

COURSE CONTENTS, THEORETICAL & APPLIED

Theoretical and practical contents



I. Introduction



1. Organic and inorganic nomenclature



2. Atoms, molecules, solutions: units of concentration



3. Acid-base theories



Definitions of Arrhenius and Bronsted-Lowry. Proof of the acid nature. Conjugated pairs. Hydrolysis and buffer solutions.

Definition of Lewis. Lux-Flood and Franklin model. Pearson model



4. Red-Ox Systems



Standard potential. The electrochemical series. Nernst equation. Diagrams of red-ox potentials. Disproportion.



II. Atomic structure and Periodicity



5. Models for the monoelectronic atom



The atom according to quantum mechanics: Schrödinger equation. Uncertainty principle. Probability. The wave function

and its physical meaning. Quantum numbers and atomic orbitals. Topology of the hydrogenoid atomic orbitals



6. Polyelectronic atoms



Polyelectronic atoms. Construction principle: Pauli Principle and Rules of Hund. Electronic configuration: Aufbau Principle.

Configuration in the ground state. Shielding, penetration and effective nuclear charge. The Periodic Table. Groups and

periods. Periodic properties.



III. Chemical bonding



7. Electrostatic model: ionic bonding



Ionic crystals. Born-Haber cycle and reticular energy. Properties of the ionic solid. Partial ionic character. Polarization and

directionality.



8. Covalent bonding



Valence-bond model. Hybrid orbitals and molecular geometry. The valence-shell electron-pair repulsion (VSEPR) model.

Molecular Orbital method. Linear combination of atomic orbitals (LCAO): bonding character and combination rules. Sigma

and pi bonds in diatomic molecules of second period elements. Polyatomic molecules.



9. Stereochemistry of an isolated molecule



Symmetry and structure. Operations and elements of symmetry. Point groups. Idealized Geometries: structural rigidity.



10. Intermolecular forces



Van der Waals bonding: molecular crystals. Polarity in the molecules. Hydrogen bond.



11.Metallic bonding



Metallic bonding and properties of metallic crystals. Band Theory. Magnetic Prop-erties. Semiconductors



12.Bonding in coordination compounds



Rule of the 18 electrons. Valence Bond Theory. Crystal field theory. Crystal field stabilization energy. Optical and magnetic

properties. Covalence Effects.



IV. Reactivity and Equilibria in solution:



13.Inorganic acids and bases



Bronsted-Lowry acidity of metal ions, hydracids, oxacids. Amphoteric substances Study of the Strength of the Lewis acids

and bases.



14.Oxidation-reduction reactions. Electromotive force diagrams. Lattimer diagrams. Frost diagrams



V. Descriptive Inorganic Chemistry



15. Descriptive of the non-metallic elements and their compounds. Variation of their properties along the Periodic Table.

Physical and chemical properties. Most important compounds.



16. Metal elements of s and p blocks. Properties, preparation and most important compounds.



17. Transition elements. Properties, preparation and most important compounds.



VI. Introduction to bioinorganic chemistry:



18. Bioinorganic chemistry I



Concept. The elements of the human body: concepts of essential and toxic. Incorporation of the elements in the evolution

of living beings. Toxicity of inorganic species. Contamination.



19. Bioinorganic chemistry II



Main functions of the metallic elements. Biological importance of Fe, Cu, Co, Mn. Metalloporphyrins. Transport of oxygen

and electrons. Metalloenzymes. Model systems.





LABORATORY PRACTICALS



Practical 1: Titration of commercial vinegar



Practical 2: Titration of a hydrogen peroxide solution



Practical 3: Acid-base reactions



Practical 4: Independent behavior of ions



Practical 5: Preparation of two copper compounds



Practical 6: Redox reactions



Practical 7: Preparation of iron(II) oxalate and potassium tris(oxalate)ferrate(III) trihydrate



Practical 8: Determination of the formula of a hydrate



Practical 9: Types of chemical reactions



Practical 10: Precipitation reactions: recognition of metal ions



COMPUTER PRACTICALS



Practical I. Acid-base systems

Practical II. Acid-base titration curves

Practical III. Lattice energy of ionic solids

Practical IV. Geometry of Molecules

Assessment

-Continuous assessment system

-Final assessment system

Assessment tools and percentages

-Carrying out a written exam:80%

-Test exam:6%

-Individual tasks:14%

To pass the subject the following sections must be passed:

-Inorganic and Organic Chemistry Nomenclature

-Theoretical section

-Practical section

The following requirements must be fulfilled to pass the subject:

-The mark of the final exam must be at least 4. The contents of this exam are so relevant and, thus, its percentage in the final mark is so high

-The mark of the lab practicals must be at least 5

-It is mandatory to pass the nomenclature exam for passing the subject. In order to pass the exam 75% of the proposed formulas/names must be correct. This exam will be held in October, and it can be also overcome in the final exam at any of the 2 calls. In no case will a fourth exam be held to pass this test. Failing this exam will imply not passing the subject.

-If any of the previous requirements is not fulfilled, the final mark will be at most 4.5.

-Moreover, if any of the sections (nomenclature, theoretical section or practical section) is not passed, the final mark will be at most 4.5.

-If in the ordinary call a student, in addition to the theoretical test, also has to do the nomenclature exam, it would be possible to save the mark of one of these exams as long as the next conditions are fulfilled:

o In the case that the nomenclature exam is passed but the theoretical exam is failed, the nomenclature mark will be saved if in the theoretical exam the mark is at least 3/10.

o In the case that the theoretical exam is passed but the nomenclature exam is failed, the theoretical mark will be saved if in the nomenclature exam the mark is at least 10/20.

Ordinary exam call: guidelines and declining to sit

To pass the subject the following sections must be passed:

-Inorganic and Organic Chemistry Nomenclature

-Theoretical and Practical section

A written exercise of Inorganic and Organic Chemistry Nomenclature will be held in October. Passing this exam (75% of the proposed formulas) is essential to pass the subject, although it does not contribute to the final mark.

The nomenclature can be overcome in the final exam at any of the 2 calls. In no case will a fourth exam be held to pass this test.

EVALUATION TOOLS AND CRITERIA

Sections for assessment:

1) Theoretical section: 80%

2) Practical section: 20%

CRITERIA

-Passing the nomenclature exam is essential to pass the subject.

-Written exams, as they are official documents, must be submitted with the appropriate presentation. Therefore, a penalty in the final mark may be applied if this requirement is not met, for instance, if they are written in pencil, they contain crossed out and disordered paragraphs, letters of doubtful reading or spelling mistakes.

-All the exam answers must be properly reasoned to be considered correct, except for the test type.

-The use of any type of electronic material in examinations is not allowed, except a calculator.

- The student who copies in an assessment activity of the subject (exam, computer-practical, report, etc.) will receive the corresponding punishment in accordance with UPV/EHU rules.

ASSESSMENT MODALITIES:

1) Modality I (final assessment).

All students can benefit from continuous assessment. There will be a Nomenclature exam, a written exam of open questions and problems for the theoretical section and a practical exam (encompassing laboratory and computer parts) for the practical section.

The evaluation in this modality will consist of three differentiated sections:

1.- Nomenclature exam (the student must pass it to do the theoretical exam).

2.- Theoretical exam (the student must pass it to do the practical exam).

3.- Practical exam.

According to the Grading Regulations in Undergraduate Studies, students who do not wish to participate in the continuous assessment system should inform the lecturer of the course by giving him/her a signed document, specifying the date, before the end of the week 9.

2) Modality II (continuous assessment).

Attendance at all sessions with activities subject to continuous assessment is mandatory.

75% of the theoretical section will be evaluated through a final exercise and the remaining 25% will be evaluated through 2 continuous assessment activities (15% and 10%, respectively).

The practical section will be entirely assessed through continuous assessment (20% of the total mark).

The assessment activities will be carried out on the dates scheduled in the "Continuous Assessment Calendar".

Skills

1) Specific skills of the subject (94.4%)

2) Transversal skills: written communication (5.6%).

The "written communication" transversal skill will be assessed by presenting a report of one of the Laboratory practicals.

To pass the subject, students must obtain a minimum passing mark in each of the sections (theoretical and practice).

If one of the sections is not pas, the maximum mark will be 4.5.

• Continuous Assessment System
• Final Assessment System
• Tools and qualification percentages:
  • Written test to be taken (%): 72
  • Multiple-Choice Test (%): 12
  • Individual works (%): 4
  • Team projects (problem solving, project design)) (%): 12

Assessment

-Continuous assessment system

-Final assessment system

Assessment tools and percentages

-Carrying out a written exam: 80%

-Test exam: 6%

-Individual tasks: 14%



To pass the subject the following sections must be passed:

-Inorganic and Organic Chemistry Nomenclature

-Theoretical section

-Practical section

More concisely, the following requirements must be fulfilled to pass the subject:

-The mark of the final exam must be at least 4. The contents of this exam are so relevant and, thus, its percentage in the final mark is so high.

-The mark of the lab practicals must be at least 5.

-It is mandatory to pass the nomenclature exam for passing the subject. In order to pass the exam 75% of the proposed formulas/names must be correct. This exam will be held in October, and it can be also overcome in the final exam at any of the 2 calls. In no case will a fourth exam be held to pass this test. Failing this exam will imply not passing the subject.

-If any of the previous requirements is not fulfilled, the final mark will be at most 4.5.

-Moreover, if any of the sections (nomenclature, theoretical section or practical section) is not passed, the final mark will be at most 4.5.

-If in the ordinary call a student, in addition to the theoretical test, also has to do the no-menclature exam, it would be possible to save the mark of one of these exams as long as the next conditions are fulfilled:

o In the case that the nomenclature exam is passed but the theoretical exam is failed, the nomenclature mark will be saved if in the theoretical exam the mark is at least 3/10.

o In the case that the theoretical exam is passed but the nomenclature exam is failed, the theoretical mark will be saved if in the nomenclature exam the mark is at least 10/20.



Ordinary exam call: guidelines and declining to sit

To pass the subject the following sections must be passed:

-Inorganic and Organic Chemistry Nomenclature

-Theoretical section

-Practical section

A written exercise of Inorganic and Organic Chemistry Nomenclature will be held in Octo-ber. Passing this exam (75% of the proposed formulas) is essential to pass the subject, alt-hough it does not contribute to the final mark. The nomenclature can be overcome in the final exam at any of the 2 calls. In no case will a fourth exam be held to pass this test.



EVALUATION TOOLS AND CRITERIA

Sections for assessment:

1) Theoretical section: 80%

2) Practical section: 20%



CRITERIA

-Passing the nomenclature exam is essential to pass the subject.

-Written exams, as they are official documents, must be submitted with the appropriate presentation. Therefore, a penalty in the final mark may be applied if this requirement is not met, for instance, if they are written in pencil, they contain crossed out and disordered para-graphs, letters of doubtful reading or spelling mistakes.

-All the exam answers must be properly reasoned to be considered correct, except for the test type.

-The use of any type of electronic material in examinations is not allowed, except a calcu-lator.

- The student who copies in an assessment activity of the subject (exam, computer-practical, report, etc.) will receive the corresponding punishment in accordance with UPV/EHU rules.

ASSESSMENT MODALITIES:

1) Modality I (final assessment).

All students can benefit from continuous assessment. There will be a Nomenclature ex-am, a written exam of open questions and problems for the theoretical section and a practi-cal exam (encompassing laboratory and computer parts) for the practical section.

The evaluation in this modality will consist of three differentiated sections:

1.- Nomenclature exam (the student must pass it to do the theoretical exam).

2.- Theoretical exam (the student must pass it to do the practical exam).

3.- Practical exam.



According to the Grading Regulations in Undergraduate Studies, students who do not wish to participate in the continuous assessment system should inform the lecturer of the course by giving him/her a signed document, specifying the date, before the end of the week 9.

2) Modality II (continuous assessment).

Attendance at all sessions with activities subject to continuous assessment is mandato-ry.

75% of the theoretical section will be evaluated through a final exercise and the remaining 25% will be evaluated through 2 continuous assessment activities (15% and 10%, respective-ly).The practical section will be entirely assessed through continuous assessment (20% of the total mark).The assessment activities will be carried out on the dates scheduled in the "Con-tinuous Assessment Calendar".

In the event that the health circumstances make it impossible to carry out a face-to-face assessment, a non-face-to-face assessment system will be enabled, from which the stu-dents will be properly advised.

Skills

1) Specific skills of the subject (94.4%)

2) Transversal skills: written communication (5.6%).

The "written communication" transversal skill will be assessed by

EXTRAORDINARY CALL

The assessment will be made according to Modality I (final assessment).



DECLINING TO SIT

If a student does not turn up to the exam he/she will not be assessed (NO SHOW).

Periodic table
Labcoat and security glasses

Basic bibliography

- Basic bibliography

-Conelly, N. G.; Damhus, T.; Hartshorn, R. M.; Hutton, A. T.: Nomenclature of inorganic chemistry. IUPAC recommendations 2005 (Red Book). Ed. The Royal Society of Chemistry: Cambridge, UK (2005). ISBN 0-85404-438-8

-Favre, H. A.; Powell, W. H.: Nomenclature of organic chemistry. IUPAC recommenda-tions and preferred name 2013 (Blue Book). Ed. The Royal Society of Chemistry: Cambridge, UK (2013). ISBN 978-0-85404-182-4

- Chang, R.; Goldsby, K. A.: Chemistry, 12th Ed. McGraw-Hill, (2016)

- Shriver, D. F.; Atkins, P. W;. Langford, C. H.: Inorganic Chemistry. 2nd Ed., Oxford University Press, (1994)

- Shriver & Atkins: Inorganic Chemistry. 4th Ed., McGraw-Hill. (2008)

- Housecroft, C. E., Sharpe, A. G.: Inorganic Chemistry. 4th Ed., Pearson; (2012)

- Petrucci, R. H., Herring F. G.; Madura, J.D.; Bissonnette C.: General Chemistry: Principles and Modern Applications. 10th Ed., Pearson Education: (2011)





Useful websites

- Materials employed during the lectures will be accessible on https://egela1819.ehu.eus

- Periodic table and properties:

https://www.webelements.com/

http://www.chemicalelements.com/

In-depth bibliography

In-depth bibliography
-Cotton, F. A., Wilkinson, G., Murillo C. A., Bockman, M.: Advanced Inorganic Chemis-try. 6ª Ed., John Wiley & Sons: New York, (1999)
-Huheey, J. E., Keiter, E. A., Keiter, R. L.: Química Inorgánica. Principios de Estructura y Reactividad. 4th Ed. Oxford University Press. (1997)
-Rayner-Canham, G.; Overton, T.: Descriptive Inorganic Chemistry. 6th Ed., Macmillan learning, (2014)
- Rodgers, G. E.: Introduction to coordination, solid state, and descriptive inorganic chemistry. McGraw-Hill: New York, (1994)
-Ochiai, E-I.: Bioinorganic Chemistry. A survey. 1st Ed. Academic Press: (2008)

Journals

Web addresses

Useful websites
- Materials employed during the lectures will be accessible on https://egela.ehu.eus/
- Periodic table and properties:
- https://www.webelements.com/
- http://www.chemicalelements.com/