Consider the transition metal complex [CoCl3(CO)3]. What is a) The oxidation state of the metal centre. b) The dn configuration of the metal centre. c) The co-ordination number of the metal centre.
a) +3. Cl ligands carry a negative charge while CO ligands are neutral so the all together the ligands have a charge of -3. Since the complex is neutral overall, the metal must cancel out the charge of the ligands, so it is +3.
b) d6. Co is in group 9 so it is d9 in its neutral state. To find the dn configuration, simply subtract the oxidation state (+3) from the neutral state dn configuration.
c) 6. Each ligand forms a single bond to the metal. Since there are 6 of them, the metal co-ordination number is 6.
RS
Related Chemistry A Level answers
All answers ▸Explain what happens to the boiling and solubility of alcohols as their chain length increases
Why is CO2 a linear molecule whereas H2O has a v-shaped geometry?
Explain how a hydroxynitrile is produced from a ketone
Write an expression and units for equilibrium constant for this reaction: 2SO2(g)+O2(g)<-->2SO3(g)