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

7568 Views

See similar Chemistry A Level tutors

Related Chemistry A Level answers

All answers ▸

What is the oxidation number of Mn in K2MnO4?


Flask Q (volume = 1.00 x 103 cm3 ) is filled with ammonia (NH3) at 102 kPa and 300 K. Calculate the mass of ammonia in flask Q. (Gas constant R = 8.31 J K−1 mol−1 )


Chlorine, 15 g, is contained in a vessel with a volume of 0.80 dm3 at 330 K. Calculate the pressure exerted when the chlorine is treated as a perfect (ideal) gas giving your answer in terms of kPa


Explain, in terms of atomic energy levels, how an atomic emission spectrum is formed


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