Inorganic Chemistry
Keywords |
Classification |
Keyword |
OFICIAL |
Chemistry |
Instance: 2020/2021 - 1S
Cycles of Study/Courses
Teaching language
Suitable for English-speaking students
Objectives
Deepen the knowledge on coordination chemistry: electronic properties, magnetic and chemical reactions of ctransition metal ion compounds.
Recognize the applications of inorganic compounds in several applied areas.
Learning outcomes and competences
Know the basics of Solid State Chemistry and Materials Chemistry
Know how to prepare bulk materials, understand defects and ionic transport.
Know how to give examples of materials and know their applications: Oxides, nitrides and metal fluorides. Calcogenides, intercalation compounds and metal rich phases. Structures with network organization. Hydrides and materials for hydrogen storage. Inorganic pigments. Chemistry of semiconductors. Molecular materials and fullerene anions.
Understand the concepts of Nano Chemistry through its basic principles: Nanosciences and Nanotechnologies.
Deepen the knowledge on the Chemistry of Coordination CompoundsKnow how to identify isomers. To know the chemical bonding models of the coordination compounds: Crystal field theory and ligand field. Understand the reactions in metallic complexes: equilibrium of complexation. Effects of stereochemical nature. Change to spin state. Effect of Jahn-Teller. Irving-Williams Series. Inert-labile character. Chelate effect, macrocyclic effect.
Understanding electronic spectroscopy in metal complexes
Know how to identify the free ion terms and use the Tanabe-Sugano diagrams. Interoperating the electronic spectra: electronic transitions: rules of selection and intensity of the bands
Know the basic concepts of Magnetismapplied to ccomplexes.
Know the basics of Organometallic ChemistryUnderstand the chemical bond in organometallic complexes: rule of the 18 electrons. Know how to characterize the type of organometallic compounds
Working method
Presencial
Pre-requirements (prior knowledge) and co-requirements (common knowledge)
General Chemistry
Program
- Overview of atomic structure and chemical bonding
1.1 Schrödinger equation and its meaning
1.2 Atomic orbitals and quantum numbers
1.3 Polyelectrotic atoms
1.4 Periodic properties
1.5 Models of covalent bonding
- Metallic bonding
2.1 Bonding models
2.2 Structure of metals
2.3 Unit cells
2.4 Alloys
2.5 Metal nanoparticles
2.6 Magnetic properties of metals
- Ionic bonding
3.1 The ionic model and the size of ions
3.2 Hydrated salts
3.3 Polarization and covalency
3.4 Ionic crystal structures
3.5 Crystal structures of polyatomic ions
3.6 The bonding continuum
- Inorganic thermodynamics
4.1 Thermodynamics of the formation of compounds
4.2 Formation of ionic compounds
4.3 Born-Haber cycle
4.4 Thermodynamics of solution processes
4.5 Formation of covalent compounds
- Solvent systems and acid-base behaviour
5.1 Solvents
5.2 Bronsted-Lowry acids and bases
5.3 Trends in acid-base behaviour
5.4 Acid-base reactions of oxides
5.5 Lewis acids and bases
5.6 Hard-soft acid-base concepts
5.7 Applications of HSAB concepts
5.8 Biological aspects.
- Oxidation and reduction
6.1 Review of basic concepts
6.2 Determination of oxidation numbers
6.3 Difference between oxidation number and formal charge
6.4 Periodic variations of oxidation numbers
6.5 Redox reactions
6.6 Quantitative aspects of half-reactions
6.7 Electrode potentials as thermodynamic functions
6.8 Latimer diagrams
6.9 Pourbaix diagrams
6.10 Redox synthesis
6.11 Biological aspects
7 Transition metal complexes
7.1 Transition metals
7.2 Metal complexes
7.3 Stereochemistry in metal complexes
7.4 Isomerism in metal complexes
7.5 Nomenclature of transition metal complexes
7.6 Bonding theories for transition metal complexes
7.7 Crystal-field theory
7.8 Electronic spectra
7.9 Ligand-field theory
7.10 Thermodynamic vs. kinetic factors
7.11 Synthesis of coordination compounds
7.12 Coordination compounds and the HSAB concept
7.13 Biological aspects
Mandatory literature
Weller,M., Rourke, J., Overton, T., Armstrong, F.; Inorganic Chemistry, 7th Edition, OUP
Atkins Peter William 1940- 070;
Shriver & Atkins inorganic chemistry. ISBN: 978-0-19-926463-6
Complementary Bibliography
Catherine E. Housecroft, Alan G. Sharpe;; Inorganic Chemistry, 4th edition, Pearson
Teaching methods and learning activities
Theoretical Lectures:
These classes will be online. The slides presented in the classes will be available on the course page. Internet sites and files will be available to complement the UC study. The UP Moodle platform will be used in the management of UC.
Theoretical-practical classes:
Solving problems related to the subject taught in theoretical classes. Students will form groups of 3 and / or 2 students. Groups will have to prepare problem solving at home to be presented during TP classes.
keywords
Physical sciences > Chemistry > Inorganic chemistry
Physical sciences > Chemistry > Molecular chemistry
Physical sciences > Chemistry > Heterogeneous catalysis
Physical sciences > Chemistry > Structural chemistry
Physical sciences > Chemistry > Homogeneous catalysis
Technological sciences > Technology > Nanotechonology
Evaluation Type
Distributed evaluation with final exam
Assessment Components
designation |
Weight (%) |
Exame |
60,00 |
Participação presencial |
20,00 |
Teste |
20,00 |
Total: |
100,00 |
Amount of time allocated to each course unit
designation |
Time (hours) |
Estudo autónomo |
110,00 |
Frequência das aulas |
52,00 |
Total: |
162,00 |
Eligibility for exams
The final grade of the TP classes must be equal to or greater than 9.0/20.0
Calculation formula of final grade
The students will be evaluated in three components, two of continuous evaluation that will take place during the teaching semester and a final exam (
E). The two components of continuous evaluation are: i)
TP: teamwork in problem solving in the pratical classes; ii)
T: online tests to be performed every two weeks.
The final grade will be:
FINAL GRADE= (0.60 x E) + (0.20 x T) + (0,20 x TP)where
E is the grade of the final exam (in presence, must be ≥ 8,0,
T is the average of the 5 best tests (online) and
TP is the classification of the group work (must be ≥ 9,0).
Special assessment (TE, DA, ...)
Worker Students:Worker students can follow the general rules of evaluation or they can be evaluated only by final exam.
Students that cannot attend TP classes:
Students that cannot attend TP classes due to schedule incompatibility or other reasons deemed valid by the responsible professors, can be evaluates only be the final exam.
Classification improvement
Final exam. The final grade will be the exam grade.
Observations
Due to the uncertainty of the evolution of COVID-19 pandemics, it may be necessary to change the face-to-face evaluation.
All students that miss any evaluation due to COVID-19 symptoms must contact the responsible professors as soon as possible, to find an alternative form of evaluation.