If the
complex is an ion, the formula for the complex is surrounded by square brackets with the overall charge at the right outside the brackets.
Example 1: [Cu(NH3)4]2+ is the tetraamminecopper(II) ion
Example 2: [Cr(OH)6]3– is the hexahydroxidochromate(II) ion
Example 3: [CuCl4]2– is the tetrachloridocuprate(II) ion
If the complex is a
cation, the
name of the complex is simply followed by the
word ion (
Example 1).
If the complex is an
anion, the suffix
ate replaces the
last syllable in the metal name (
Examples 2 and 3).
For some metals appearing in anions, the Latin name is used (Example 3).
Fe is iron in a cation and ferrate in an anion.
Cu is copper in a cation and cuprate in an anion.
Ag is silver in a cation and argentate in an anion.
Ionic complexes exist as
compounds with a counter ion (anion or cation depending on the charge on the complex) that is NOT in the coordination sphere.
The name of the compound is the name of the cation followed by the name of the anion where either of these may be the complex.
Example 4: Na[Al(OH)4] is sodium tetrahydroxidoaluminate(III)
Example 5: [Ag(NH3)4]OH is tetraamminesilver(I) hydroxide