ECTS credits ECTS credits: 6
ECTS Hours Rules/Memories Student's work ECTS: 99 Hours of tutorials: 3 Expository Class: 24 Interactive Classroom: 24 Total: 150
Use languages Spanish, Galician
Type: Ordinary Degree Subject RD 1393/2007 - 822/2021
Center Faculty of Mathematics
Call: First Semester
Teaching: Sin Docencia (En Extinción)
Enrolment: No Matriculable (Sólo Planes en Extinción)
The overall objective is to provide students Grade Math basic knowledge of chemistry related to the electronic structure of atoms, the chemical bond and the different models that describe it, as well as acid-base and redox processes.
Theory classes program:
1. Basis of the modern theory of the atom [4 h]
1.1. Elemental application of the ondulatory mechanics.
1.2. The quantum numbers.
1.3. Electronic structure of atoms.
1.4. Periodic table.
1.5. Covalent, ionic and metallic radio.
1.6. Ionization energy.
1.7. Electron affinity.
2. General approach to the chemical bond: covalent bond [3 h]
2.1. Lewis theory.
2.2. Writing Lewis structures.
2.3. Formal charge.
2.4. Resonance.
2.5. Exceptions to the octet rule.
2.6. Valence Shell Electron Pair Repulsion Theory (VSEPR).
2.7. Molecular geometry.
2.8. Dipole moment: polar and nonpolar molecules.
3. Valence bond model. Molecular orbital theory [4 h]
3.1. Valence bond method.
3.2. Hybridization of atomic orbitals.
3.3. Types of hybrid orbitals.
3.4. Multiple covalent bonds.
3.5. Molecular Orbital Theory (TOM).
3.6. Combination of atomic orbitals: dihydrogen molecular orbitals.
3.7. Molecular orbital for homonuclear diatomic molecules of period 2 elements.
3.8. Energy levels diagrams.
3.9. Molecular orbitals of heteronuclear diatomic molecules.
3.10. Introduction to the Band Theory.
4. Ionic bonding model [1 h]
4.1. Structural aspects.
4.2. Energy considerations: lattice energy.
4.3. Born-Haber cycles.
4.4. Ionic model deviations: polarization effects.
5. Intermolecular interactions [1 h]
5.1. Orientation forces.
5.2. Inductive forces.
5.3. Dispersion forces.
5.4. Hydrogen bonding.
6. Matter aggregation states [1 h]
6.1. Properties of solids, liquids and gases.
6.2. Crystalline solids. Types of crystal lattices.
6.3. Phase changes.
6.4. Phase diagrams.
7. Basis of chemical thermodynamics [1 h]
7.1. Heat changes and thermochemistry.
7.2. Spontaneity of physical and chemical changes.
8. Chemical equilibrium in solution: acids and bases I [4 h]
8.1. Definitions of acids and bases.
8.2. Self-ionization of water and pH scale.
8.3. Bronsted-Lowry acid-base theory.
8.4. Ionization constants. Strong and weak acids and bases.
8.5. Percent ionization.
8.6. Polyprotic acids.
8.7. Acid rain.
9. Acids and bases II [4 h]
9.1. Behavior of the salts in aqueous solution: Hydrolysis.
9.2. Buffer solutions.
9.3. Acid-base indicators.
9.4. Neutralization reactions and titration curves.
10. Oxidation-reduction reactions [5 h]
10.1. Review of fundamental concepts.
10.2. Adjustment reactions: ion-electron method.
10.3. Oxidizing and reducing agents.
10.4. Standard electrode potential.
10.5. Nernst equation.
10.6. Primary and secondary batteries.
10.7. Electrolysis.
Program of computer room/chemistry laboratory:
I) Computer room [2 h]
3D Visualization of orbitals, molecules and crystal lattices.
II) Lab practices [9 h]
1. Safety. Labware and basic lab operations.
2. Displacement reactions. Precipitation and filtration.
3. Reactions among species in solution: redox and chemical equilibrium.
Basic textbooks:
• Petrucci, R.H.; Harwood, W.S. y Herring, F.G.: Química General: principios y aplicaciones modernas, 11ª ed.; Prentice Hall, 2017.
Available online from: http://sfx.bugalicia.org/san/ebooksearch/
Complementary, further reading:
• Atkins, P. y Jones, L.: Principios de Química, 5ª ed.; Ed. Médica Panamericana, 2012.
• Brown, T.L.; LeMay Jr., H.E. y Mur, C.J.: Química: La Ciencia Central, 12ª ed.; Pearson Educación, 2014.
• Chang, R. y Goldsby K.A.: Química, 12ª ed.; McGraw-Hill, 2016.
• Kotz, J.C. y Treichel, P.M.: Química y Reactividad Química, 6ª ed.; Thomson, 2005.
• Masterton, W.L. y Hurley, C.N.: Química. Principios y Reacciones, 4ª ed.; Paraninfo Cengage -Learning, 2003.
• Peterson, W.R. Nomenclatura de las sustancias químicas, 4ªed., Editorial Reverté, 2015.
• Reboiras, M.D.: Problemas resueltos de Química: la ciencia básica, Ediciones Paraninfo S.A., 2007.
Competences to be achieved by the student are those listed in the Verification Report of the Mathematics Degree:
• Basic and general competences : CB1, CB2, CB3, CB4, CB5, CG2, CG5.
• Transversal competences: CT1, CT2, CT3, CT4, CT5.
• Specific competences: CE1, CE6, CE7, CE8, CE9.
In addition to contributing to achieve these competences, this subject will allow the student to achieve the following specific objectives in Chemistry:
• Able to solve any basic problem concerning the electron configuration of the chemical elements and predict a number of periodic properties.
• Analyze the different types of chemical bonding that can occur when elements interact to form compounds and study how the different type of bond that present conditions the properties thereof. Understand and manage 3D molecular visualization programs.
• Develop your ability to solve theoretical questions and numerical problems related to acid-base and redox chemical processes and critically analyze the results.
• Understand and correctly use the material and the basic operations of a chemical laboratory.
During the course, students will be able to contact directly with the teaching staff to make any questions or resolve any doubts related to the subject, using the various channels available to the USC (Web Mail, Virtual Campus, MS TEAMS).
All the didactic material used throughout the course 2024-25 will be available to the student in the "Virtual Classroom" of the subject.
The criteria established in the Mathematics Degree Verification Report (continuous formative assessment combined with a final exam) and applied in the 2024-25 academic year will be followed.
• The final exam (60%) and the continuous assessment (40%) obtained in the 2024-25 academic year will be taken into account in the overall grade. The final grade obtained in the subject will be the final exam if it is higher than the grade resulting from weighing it with the continuous assessment.
• Students who do not take the final exam will receive a grade of "NOT PRESENTED."
• The same criteria will be applied for the second opportunity.
In the event of fraudulent completion of exercises or exams, the "Regulations for the Evaluation of Student Academic Performance and Grade Review" will be applied.
Maria Soledad Garcia Tasende
- Department
- Inorganic Chemistry
- Area
- Inorganic Chemistry
- Phone
- 881814954
- soledad.garcia [at] usc.es
- Category
- Professor: University Lecturer
| 01.15.2026 10:00-14:00 | Grupo de examen | Classroom 06 |
| 06.23.2026 10:00-14:00 | Grupo de examen | Classroom 06 |