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
Answered by Robert S. Chemistry tutor

8334 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

What is the mechanism for nucleophilic addition reactions at carbonyls?


Draw the shape of an SF6 and SF4 molecule, indicating bond angles and any lone pairs which may influence these. What shape is the SF6 molecule?


How can you tell what shape a molecule is going to be?


Explain why the first ionisation energy of sulfur is different from that of phosphorus.


We're here to help

contact us iconContact ustelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

MyTutor is part of the IXL family of brands:

© 2025 by IXL Learning