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.

Answered by Robert S. Chemistry tutor

7689 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

In order to find the [H+] ion content of H2SO4 (Sulphuric Acid), why must you divide by two after using the formula for pH calculation?


Can you help me with the question: "State and explain the trend in boiling temperature of hydrogen halides down the group"?


Why does ice float on water?


Plan out a 4 step organic synthesis to form N-methyl Butanamide from 1-Bromopropane. Include relevant reagents and conditions for each reaction. Include 1 mechanism for one of the stages.


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences