![]() ![]() For example, an iron-containing anion would contain the term "ferrate" instead of "iron" a copper-containing one would be called a "cuprate", one with gold would be called an "aurate" and so on. If the complex ion is an anion and the element's symbol does not match its name in English, the Latin name of the metal is usually used rather than the English one. However, if the complex ion containing the metal is an anion, the metal is given the suffix "-ate", sometimes replacing its normal ending. The metal is named following the ligands, and its charge or oxidation state is listed using Roman numerals.ĬlO 4, dichlorobis(ethylenediamine) cobalt(III) perchlorate.For example, if you are comparing a compound with two CO ligands to another that has only one, you might call them "the dicarbonyl compound" and "the monocarbonyl compound", respectively. If you need to stress that only one ligand of a certain type is present, you could use the numbering adjective "mono". Instead, for more complicated ligands like this, we use the following system: ligandsįor example, is tetrakis(triphenylphosphine)palladium(0). We avoid saying "di" to describe something that already contains a "di". The di means that there are two amino groups in the ligand. For example, they may already contain prefixes denoting a number, such as ethylene diamine, NH 2CH 2CH 2NH 2. In the examples above, there were six waters, "hexaaqua", six ammines, "hexaammine", and five waters, "pentaaqua". If there is more than one ligand of the same kind, then the number of ligands is indicated as follows:.(NO 3) 2, penta aqua chlorocobalt(III) nitrate (aqua before chloro) If two different ligands are found in the complex, they are listed alphabetically. Neutral ligands keep their regular names, but the two common molecules H 2O and NH 3 are called "aqua" and "ammine", respectively. Note that anionic ligands generally end in "o" in the name of a coordination compound. Ligands are listed in front of the metal.īr 2, hexa amminecopper(II) bromide (ammine ligand before copper metal).Anything outside of brackets is the counterion or counterions. In the formula, you can always tell one ion from the other because the complex ion (metal plus ligands) is always enclosed in square brackets. If there is a cation and an anion, the cation is named first.Ĭl 2, hexaaquanickel(II) chloride (nickel cation before chloride anion) Coordination compounds often contain a "complex" ion, with ligands attached to the metal ion, as well as a counterion, to balance charge.The names of coordination compounds tend to be pretty long because of the number of pieces involved, but they usually follow a trend. It's sometimes useful to be able to be able to read the name of a compound and understand what that means. The pink color of the hexaaquacobalt(II) ion is produced again (only paler, of course, because it is more dilute).\) Adding water to the right-hand side of the equilibrium has the effect of moving the position of equilibrium to the left. This reaction can be easily reversed by adding water to the solution. Chloride ions are bigger than water molecules, and there isn't room to fit six of them around the central cobalt ion. Notice the change in the co-ordination of the cobalt. The high chloride ion concentration pushes the position of the equilibrium to the right according to Le Chatelier's Principle. Concentrated hydrochloric acid has a chloride ion concentration of approximately 10 mol dm -3. \nonumber \]Ĭoncentrated hydrochloric acid is used as the source of chloride ions because it provides a very high concentration compared to what is possible with, say, sodium chloride solution. ![]()
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