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Iron(II) cyanide is an inorganic compound with the empirical formula Fe(CN) 2. It ... Text is available under the Creative Commons Attribution-ShareAlike 4.0 License; ...
Iron(II) chloride tetrahydrate, FeCl 2 ·4H 2 O. In chemistry, iron(II) refers to the element iron in its +2 oxidation state. The adjective ferrous or the prefix ferro-is often used to specify such compounds, as in ferrous chloride for iron(II) chloride (FeCl 2). The adjective ferric is used instead for iron(III) salts, containing the cation Fe 3+.
It is usually available as the salt potassium ferrocyanide, which has the formula K 4 Fe(CN) 6. [Fe(CN) 6] 4− is a diamagnetic species, featuring low-spin iron(II) center in an octahedral ligand environment. Although many salts of cyanide are highly toxic, ferro- and ferricyanides are less toxic because they tend not to release free cyanide. [1]
Despite the fact that it is prepared from cyanide salts, Prussian blue is not toxic because the cyanide groups are tightly bound to iron. [25] Both ferrocyanide (( Fe 2+ (CN) 6 ) 4− ) and ferricyanide (( Fe 3+ (CN) 6 ) 3− ) are particularly stable and non-toxic polymeric cyanometalates due to the strong iron coordination to cyanide ions.
An example of a low-spin iron(III) complex is [Fe(CN) 6] 3−. The cyanide ligands may easily be detached in [Fe(CN) 6] 3−, and hence this complex is poisonous, unlike the iron(II) complex [Fe(CN) 6] 4− found in Prussian blue, [16] which does not release hydrogen cyanide except when dilute acids are added. [17]
In these cases the oxidation number (the same as the charge) of the metal ion is represented by a Roman numeral in parentheses immediately following the metal ion name. For example, in uranium(VI) fluoride the oxidation number of uranium is 6. Another example is the iron oxides. FeO is iron(II) oxide and Fe 2 O 3 is iron(III) oxide.
The goal of the antidote was to generate a large pool of ferric iron (Fe 3+) to compete for cyanide with cytochrome a 3 (so that cyanide will bind to the antidote rather than the enzyme). The nitrites oxidize hemoglobin to methemoglobin , which competes with cytochrome oxidase for the cyanide ion.
Cyanometallates or cyanometalates are a class of coordination compounds, most often consisting only of cyanide ligands. [1] Most are anions. Cyanide is a highly basic and small ligand, hence it readily saturates the coordination sphere of metal ions.