General Inorganic Chemistry
Objectives
To introduce and rationalize the diversity of inorganic compounds exhibited by the various elements of the Periodic Table. This subject develops along two parts: main group elements (s and p blocks) and transition elements (d block).
General characterization
Code
2227
Credits
6.0
Responsible teacher
António Jorge Dias Parola, Carlos Lodeiro Espino
Hours
Weekly - 4
Total - 64
Teaching language
Português
Prerequisites
Available soon
Bibliography
1 - W. Henderson, Main Group Chemistry, Royal Society of Chemistry, 2000.
2 - M. Weller, T. Overton, J. Rourke, F. Armstrong, Inorganic Chemistry, 7th ed., Oxford University Press, 2018.
3 - F. A. Cotton, G. Wilkinson, P. L. Gaus, Basic Inorganic Chemistry, 3rd ed., Wiley, 1995.
4 - G. Svehla, Vogel''s Qualitative Inorganic Analysis, 7th ed., Longman, 1996. (for lab lessons)
Teaching method
The teaching of Inorganic Chemistry (CR) is spread over 26 h of theoretical lessons, complemented by 9 h of exercises and problems solving. The experimental part comprises 24 h of laboratory practice.
Evaluation method
Assessment
1. The final grade (NF) is given by:
NF = 0.25 x P + 0.75 x T
where P is the laboratory grade and T the theoretical grade, both round to the one decimal place.
2. The theoretical part is evaluated by 3 mini-tests or by exam, being necessary to have a test average or exam grade ≥ 9.5 to pass the theoretical part..
3. This UC has frequency, given by the completion of practical work with delivery of the respective questionnaires (in the next practical class) and eventual discussion of them, being necessary to have a grade ≥ 9.5 to pass the practical part.
Subject matter
Contents
1. Theoretical lessons
1.1. Introduction. Review of atomic structure: quantum numbers, orbitals, electronic configuration. Effective nuclear charge. Periodic table trends.
1.2. Main group chemistry.
1.2.1. Group 1: hydrogen and alcaline metals. Solubility of salts in water: lattice energy, hydration enthalpy, solution enthalpy.
1.2.2. Group 2: alkaline earth metals.
1.2.3. Group 13.
1.2.4. Group 14.
1.2.5. Group 15. Redox representations: Latimer, Frost and Pourbaix diagrams.
1.2.6. Group 16.
1.2.7. Group 17: halogens.
1.3. Transition metal chemistry.
1.3.1. The transition elements: their discivery and position in the periodic table. The d block and the f block.
1.3.2. Coordination compounds: origins; ligands; nomenclature.
1.3.3. Isomerism in coordination compounds.
1.3.4. Bond theories in coordination compounds.
1.3.4.1. Crystal Field Theory. Magnetism and colour of coordination compoundsOctahedral, tetrahedral and square planar complexes. Spectrochemical series.
1.3.4.2. Molecular Orbital Theory: review of concepts. Ligand Field Theory: pi bonding: pi acceptor and donor groups; pi backbonding.
1.3.5. Chemical equilibrium in coordination compounds: partial and global constants. Complexometry. Dependence of equilibrium on pH: conditional constants. Calculations: mass balance.
1.3.6. Stability of coordination compounds: chelation effect; Irving-Williams series; Hard Soft Acid Base (HSAB) principle.
2. Practical lessons
2.1. Exercises and problems related to the theoretical lessons.
3. Laboratory lessons
3.1. Calculations and preparation of solutions.
3.2. Coordination chemistry I - Synthesis of colbalt pigments.
3.3. Main Group chemistry I - Groups 1 and 2.
3.4. Main Group chemistry II - Groups 14 e 15.
3.5. Main Group chemistry III - Groups 16 e 17.
3.6. Coordination chemistry II - Nernst equation for the ferrocyanide/ferricyanide redox pair
3.7. Coordination chemistry III - (a) Cu(II) complexes with different ligand fields; (b) Determination of the stability constant for [FeSCN]2+; (c) Determination of the stoichiometry of the complex formed between Ni(II) and EDTA.
3.8. Coordination chemistry IV - Reactions of copper, iron and silver ions. (Laboratory test.)