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Nomenclature of Coordination Complexes
(Self quiz after overview)
Anion Name Bromide, Br- 2 - Carbonate, CO 3 Chloride, Cl- Cyanide, CN- Fluoride, F- Hydroxide, OH 2 - -
Oxalate, C 2 O (^4) EDTA
Neutral Ligand Ammonia, NH Water, H2O Carbon Monoxide, CO Ethylenediamine, en
Metal Aluminum Chromium Cobalt Copper Gold Iron Manganese Nickel Platinum Zinc
Overview: Ligands = attached atoms or molecules
Ligand Name Bromo Carbonato Chloro Cyano Fluoro Hydroxo Oxalato Ethylenediamine tetracetato
Ligand Name Ammine Aqua Carbonyl Ethylenediamine
Anion Name Aluminate Chromate Cobaltate Cuprate Aurate Ferrate Manganate Nickelate Platinate Zincate
If more than one ligand is attached then,
2 = di 3 = tri 4 = tetra 5 = penta 6 = hexa
If the ligand has di, tri, tetra, in its name or is a dentate molecule, and you want to indicate you have more than one of them then use,
2 = bis 3= tris 4 = tetrakis
EDTA wrapped around a metal ion.
The Dentates
Bidentates – two bites Oxalate (ox) Ethylenediamine (en) Malate (mal)
Tridentate – three bites Citrate (cit)
Hexadentate – six bites EDTA
How to name complex ions that are positively charged.
The name of the transition metal comes at the end of the name along with a Roman numeral indicating its charge,
Ex: Co(NH 3 ) 6 3+^ = hexamminecobalt(III) Fe(H 2 O)2+ 6 2+^ = hexaquairon(II) Ni(en) (^2) 2+^ = bis(ethylenediamine)nickel(II) Cu(CO) 4 = tetracarbonylcopper(II)
Now, every compound has both a positive part and a negative part, like NaCl is really Na+^ and Cl-. The same is true for complex ions only the positive and negative parts can be really large and complex (which is why they are called complex ions).
In the above examples I gave several positive ions and their name, but each of them also has a negative part that goes with them. Consider the following compounds,
Ex: Co(NH 3 ) 6 Cl 3 = hexamminecobalt(III) chloride Fe(H 2 O) 6 (OH) 2 = hexaquairon(II) hydroxide Ni(en) 2 SO 4 = bis(ethylenediamine)nickel(II) sulfate Cu(CO) 4 CO 3 = tetracarbonylcopper(II) carbonate
In each case an anion has been added to the complex ion. This completes the structure and produces an overall neutral compound that could be stored in a bottle in our storeroom. You will notice that the nomenclature has not changed much from what we learned about transition metal nomenclature, you name the metal ion, indicate its charge with a Roman Numeral, and then add the anion onto the end. Only in this case the positive ion is large and complex but the nomenclature is the same.
Problems
- Name the following compounds,
Cu(OH) 42 -
Na 3 AuCl (^4)
Mo(CN) 64 -
Fe(CO) 6 ScCl (^6)
[Cr(NH 3 ) 3 (H 2 O) 3 ]Cl (^3)
[Pt(NH 3 ) 5 Cl]Br (^3)
[Pt(en) 2 Cl 2 ]Cl (^2)
[Co(en) 3 ] 2 (SO 4 ) (^3)
K 4 [Fe(CN) 6 ]
Na 2 [NiCl 4 ]
Pt(NH 3 ) 2 Cl (^4)
(NH 4 ) 2 [Ni(C 2 O 4 ) 2 (H 2 O) 2 ]
[Ag(NH 3 ) 2 ][Ag(CN) 2 ]
[CoBr(NH 3 ) 5 ]SO (^4)
[Fe(NH 3 ) 6 ][Cr(CN) 6 ]
[Co(SO 4 )(NH 3 ) 5 ]+
[Fe(OH)(H 2 O) 5 ]2+
- Write the formula of the following coordination compounds.
hexaammineiron(III) nitrate
ammonium tetrachlorocuprate(II)
sodium monochloropentacyanoferrate(III)
potassium hexafluorocobaltate(III)
- Give the number of d electrons for each of the complexes listed below. Are the
complexes paramagnetic or diamagnetic?
d electrons Paramagnetic or Diamagnetic
Pd(NH 3 ) 2 Cl
Ru (CO) 6 3+
Ni(H 2 O) 6 2+
HgCl 42 -
- Give the number of d electrons for each of the complexes listed below. Are the
complexes paramagnetic or diamagnetic?
d electrons Paramagnetic or Diamagnetic
Pd(NH 3 ) 2 Cl d8 Diamagnetic
Ru (CO) 6 3+^ d5 Paramagnetic
Ni(H 2 O) 6 2+^ d8 Paramagnetic
HgCl 4 2-^ d10 Diamagnetic
