Editing Coordination complex (section)

==Nomenclature of coordination complexes==
The basic procedure for naming a complex is:
# When naming a complex ion, the ligands are named before the metal ion.
# The ligands' names are given in alphabetical order. Numerical prefixes do not affect the order.
#* Multiple occurring monodentate ligands receive a prefix according to the number of occurrences: ''di-'', ''tri-'', ''tetra-'', ''penta-'', or ''hexa-''.
#* Multiple occurring polydentate ligands (e.g., ethylenediamine, oxalate) receive ''bis-'', ''tris-'', ''tetrakis-'', etc.
#* Anions end in ''o''.  This replaces the final 'e' when the anion ends with '-ide', '-ate' or '-ite', e.g. ''chloride'' becomes ''chlorido'' and ''sulfate'' becomes ''sulfato''. Formerly, '-ide' was changed to '-o' (e.g. ''chloro'' and ''cyano''), but this rule has been modified in the 2005 IUPAC recommendations and the correct forms for these ligands are now ''chlorido'' and ''cyanido''.<ref name="iupac_org">{{cite web |url= http://www.iupac.org/fileadmin/user_upload/databases/Red_Book_2005.pdf |title= Nomenclature of Inorganic Chemistry IUPAC Recommendations 2005 |at= section 1.6.4 (p. 10–11) |publisher= [[IUPAC]] |access-date= 2016-03-06 |archive-url= https://web.archive.org/web/20141222172055/http://www.iupac.org/fileadmin/user_upload/databases/Red_Book_2005.pdf |archive-date= 2014-12-22 |url-status= dead }}</ref>
#* Neutral ligands are given their usual name, with some exceptions: NH<sub>3</sub> becomes ''[[ammine]]''; H<sub>2</sub>O becomes ''aqua'' or ''aquo''; CO becomes ''carbonyl''; NO becomes ''nitrosyl''.
# Write the name of the central atom/ion.  If the complex is an anion, the central atom's name will end in ''-ate'', and its Latin name will be used if available (except for mercury).
# The oxidation state of the central atom is to be specified (when it is one of several possible, or zero), and should be written as a Roman numeral (or 0) enclosed in parentheses.
# Name of the cation should be preceded by the name of anion. (if applicable, as in last example)

Examples:
{|class="wikitable"
!metal
!changed to
|-
|cobalt
|cobaltate
|-
|aluminium
|aluminate
|-
|chromium
|chromate
|-
|vanadium
|vanadate
|-
|copper
|cuprate
|-
|iron
|ferrate
|}

: [Cd(CN)<sub>2</sub>(en)<sub>2</sub>] → dicyanidobis(ethylenediamine)cadmium(II)
: [CoCl(NH<sub>3</sub>)<sub>5</sub>]SO<sub>4</sub> → pentaamminechloridocobalt(III) sulfate
: [Cu(H<sub>2</sub>O)<sub>6</sub>] <sup>2+</sup>  → hexaaquacopper(II) ion
: [CuCl<sub>5</sub>NH<sub>3</sub>]<sup>3−</sup> → amminepentachloridocuprate(II) ion
: K<sub>4</sub>[Fe(CN)<sub>6</sub>] → potassium hexacyanidoferrate(II)
: [NiCl<sub>4</sub>]<sup>2−</sup> → tetrachloridonickelate(II) ion (The use of chloro- was removed from IUPAC naming convention)<ref name="iupac_org" />

The coordination number of ligands attached to more than one metal (bridging ligands) is indicated by a subscript to the Greek symbol [[mu (letter)|μ]] placed before the ligand name. Thus the [[Dimer (chemistry)|dimer]] of [[aluminium trichloride]] is described by Al<sub>2</sub>Cl<sub>4</sub>(μ<sub>2</sub>-Cl)<sub>2</sub>.

Any anionic group can be electronically stabilized by any cation. An anionic complex can be stabilised by a hydrogen cation, becoming an acidic complex which can dissociate to release the cationic hydrogen. This kind of complex compound has a name with "ic" added after the central metal. For example, H<sub>2</sub>[Pt(CN)<sub>4</sub>] has the name tetracyanoplatinic (II) acid.