Chapter 23 – Transition Metals and Coordination Compounds
*Know how to write electron configurations for transition metal atoms and ions presented in Chemistry I (see section 4.4 and 4.7)
*Know how to determine oxidation state of a metal presented in Chemistry I (see section 9.9)
Define:
- Complex ion
- Ligand
- Coordination compound
- Coordinate covalent bond
- Coordination number
- Chelate, chelating agents
- Isomer
- Structural isomer
- Stereoisomer
- Coordination isomer
- Linkage isomer
- Geometric isomer
- cis versus trans
- fac versus mer
- Optical isomer
- Weak field versus strong field ligand
- High spin versus low spin complex
DO:
- Predict periodic trends in atomic radius, ionization energy and electronegativity for transition metals
- Identify ligands as monodentate, bidentate or polydentate
- Identify the common geometries of coordination complexes (octahedral, tetrahedral, square planar, linear)
- Explain the difference between a ligand and an ion in a complex such as [Ni(H2O)6]SO4
- Explain bonding in Lewis acid-Lewis base terms
- Differentiate between structural isomers (coordination and linkage) and stereoisomers (geometric and optical)
- Use crystal field theory to explain d-orbital splitting in octahedral complexes
- Explain the relationship between the splitting of the d-orbitals and color
- Use crystal field theory to predict the number of unpaired electrons and the magnetic properties of coordination complexes
- Discuss the role of EDTA as a chelating agent, especially for toxic heavy metals
- Recognize the role of transition metals in biomolecules (such as hemoglobin, cytochrome c, chlorophyll and carbonic anhydrase) and pharmaceuticals (cisplatin)