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can someone tell me what is the rule for naming the coordination compound in which bothvanion and cation are complex??

jash goswami , 12 Years ago
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Aman Bansal

Last Activity: 12 Years ago

Dear Jash,

Coordination complexes have their own classes of isomers, different magnetic properties and colors, and various applications (photography, cancer treatment, etc), so it makes sense that they would have a naming system as well. Consisting of a metal and ligands, their formulas follow the pattern[Metal Anions Neutrals]±Charge, while names are written Prefix Ligands Metal(Oxidation State).

 

  1. 1. Introduction
  2. 2. Naming Coordination Complexes
    1. 2.1. Rules for Naming the Ligands
    2. 2.2. Rules for Naming the Metal Center & Oxidation State
  3. 3. Writing Formulas of Coordination Complexes
  4. 4. References
  5. 5. Outside Links
  6. 6. Problems
  7. 7. Answers
  8. 8. Contributors

 

 

Introduction

According to the Lewis base theory, ligands are Lewis bases since they can donate electrons to the central metal atom. The metals, in turn, are Lewis acids since they accept electrons. Coordination complexes consist of a ligand and a metal center cation. The overall charge can be positive, negative, or neutral. Coordination compounds are complex or contain complex ions: 

  • Complex Cation: [CO(NH3)6]3+
  • Complex Anion: [CoCl4(NH3)2]-
  • Neutral Complex: [CoCl3(NH3)3]
  • Coordination Compound: K4[Fe(CN)6]

A ligand can be an anion or a neutral molecule that donates an electron pair to the complex. Ex: NH3, H2O, Cl-. The number of ligands that attach to a metal depends on whether the ligand is monodentate, bidentate, or polydentate. For more information, see Ligands and Chelation.

 

Naming Coordination Complexes

Given Formula → Write Name

To begin naming coordination complexes, here are some things to keep in mind.  

  1. Ligands are named first in alphabetical order.
  2. The name of the metal comes next.
  3. The oxidation state of the metal follows, noted by a Roman numeral in parentheses (II, IV).                                                               

Rules for Naming the Ligands

1. Ligands that act as anions which end in "-ide" are replaced with an ending "-o" (e.g., Chloride → Chloro).

Anions ending with "-ite" and "-ate" are replaced with endings "-ito" and "-ato" respectively (e.g., Nitrite → Nitrito, Nitrate → Nitrato).

 

Anionic Monodentate Ligands
F- Fluoro OH- Hydroxo
Cl- Chloro SO42- Sulfato
Br- Bromo S2O32-- Thiosulfato
I- Iodo NO2- Nitrito-N-; Nitro
O2- Oxo ONO- Nitrito-O-; Nitrito
CN- Cyano SCN- Thiocyanato-S-; Thiocyanato
NC- Isocyano NCS- Thiocyanato-N-; Isothiocyanato

2. Most neutral molecules that are ligands carry their normal name. The few exceptions are the first four on the chart: ammine, aqua, carbonyl, and nitrosyl.

 

Neutral Monodentate Ligands
NH3 Ammine
H2O Aqua
CO Carbonyl
NO Nitrosyl
CH3NH2 Methylamine
C5H5N Pyridine

(Note: Ammine is spelled with two m''s when referring to a ligand. Amines are something else.)

Polydentate ligands follow the same rules for anions and neutral molecules.

 

en Ethylenediamine
ox2- Oxalato
EDTA4- Ethylenediaminetetraacetato

3. The number of ligands present in the complex is indicated with the prefixes di, tri, etc. The exceptions are polydentates that have a prefix already in their name (en and EDTA4- are the most common). When indicating how many of these are present in a coordination complex, put the ligand''s name in parentheses and use bis, tris, and tetrakis.

 

  Normal Polydentates
1 mono -
2 di bis
3 tri tris
4 tetra tetrakis
5 penta -
6 hexa -

Prefixes always go before the ligand name; they are not taken into account when putting ligands in alphabetical order. Note that "mono" often is not used. 

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