Ferrate(VI)
200px Solutions of ferrate (left)
and permanganate (right) |
|
Names | |
---|---|
IUPAC name
Ferrate(VI)
|
|
Systematic IUPAC name
Tetraoxoironbis(olate)[citation needed]
|
|
Other names
Ferrate(2-)
|
|
Identifiers | |
ChEBI | CHEBI:30992 |
ChemSpider | 21865127 |
Jmol 3D model | Interactive image Interactive image |
PubChem | 25000034 |
|
|
|
|
Properties | |
FeO42− | |
Molar mass | 119.843 g mol−1 |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|
|
verify (what is ?) | |
Infobox references | |
Ferrate(VI) is the inorganic anion with the chemical formula [FeO4]2−. It is photosensitive, contributes a pale violet colour to compounds and solutions containing it and is one of the strongest water-stable oxidising species known. Although it is classified as a weak base, concentrated solutions containing ferrate(VI) are corrosive and attack the skin and are only stable at high pH.
Nomenclature
The term ferrate is normally used to mean ferrate(VI), although it can refer to other iron-containing anions, many of which are more commonly encountered than salts of [FeO4]2−. These include the highly reduced species disodium tetracarbonylferrate Na2[Fe(CO)4] and salts of the iron(III) complex tetrachloroferrate [FeCl4]−. Although rarely studied, ferrate(V) [FeO4]3− and ferrate(IV) [FeO4]4− oxyanions of iron also exist. These too are called ferrates.[1]
Synthesis
Ferrate(VI) salts are formed by oxidizing iron in an aqueous medium with strong oxidizing agents under alkaline conditions, or in the solid state by heating a mixture of iron filings and powdered potassium nitrate.[2]
For example, ferrates are produced by heating iron(III) hydroxide with sodium hypochlorite in alkaline solution:[3]
- 2 Fe(OH)
3 + 3 OCl−
+ 4 OH−
→ 2 [FeO
4]2−
+ 5 H
2O + 3 Cl−
The anion is typically precipitated as the barium(II) salt, forming barium ferrate.[3]
Properties
The ferrate(VI) anion is unstable at neutral[2] or acidic pH values, decomposing to iron(III):[3]
- [FeO
4]2−
+ 3 -
e + 8 H+
⇌ Fe3+
+ 4 H
2O
The reduction goes through intermediate species in which iron has oxidation states +5 and +4.[4] These anions are even more reactive than ferrate(VI).[5] In alkaline conditions ferrates are more stable, lasting for about 8 to 9 hours at pH 8 or 9.[5]
Aqueous solutions of ferrates are pink when dilute, and deep red or purple at higher concentrations.[4][6] The ferrate ion is a stronger oxidizing agent than permanganate,[7] and will oxidize chromium(III) to dichromate,[8] and ammonia to molecular nitrogen.[9]
Ferrates are excellent disinfectants, and are capable of removing and destroying viruses.[10]
The ferrate(VI) ion has two unpaired electrons, and is thus paramagnetic. It has a tetrahedral molecular geometry.[4]
See also
References
- ↑ Lua error in package.lua at line 80: module 'strict' not found.
- ↑ 2.0 2.1 Lua error in package.lua at line 80: module 'strict' not found.
- ↑ 3.0 3.1 3.2 Lua error in package.lua at line 80: module 'strict' not found.
- ↑ 4.0 4.1 4.2 Lua error in package.lua at line 80: module 'strict' not found.
- ↑ 5.0 5.1 Lua error in package.lua at line 80: module 'strict' not found.
- ↑ Lua error in package.lua at line 80: module 'strict' not found.
- ↑ Lua error in package.lua at line 80: module 'strict' not found.
- ↑ Lua error in package.lua at line 80: module 'strict' not found.
- ↑ Lua error in package.lua at line 80: module 'strict' not found.
- ↑ Lua error in package.lua at line 80: module 'strict' not found.
- Pages with broken file links
- Articles with unsourced statements from March 2011
- Chemical articles without CAS Registry Number
- Articles without KEGG source
- Articles without UNII source
- Pages using collapsible list with both background and text-align in titlestyle
- Chemical articles using a fixed chemical formula
- Ferrates
- Oxoanions