Iron(III) acetate

Iron(III) acetate[1]

Names
IUPAC name

iron(III) acetate

Other names

basic iron(III) acetate , iron(III) oxyacetate, iron(III) Acetate

Identifiers

CAS Number

* 1834-30-6 Y

3D model (JSmol)

* Interactive image
* coordination complex: Interactive image

ChemSpider |

* 144555

PubChem CID

* 164887

UNII |

* CZZ8832SI5 Y

InChI

* InChI=1/3C2H4O2.Fe/c3*1-2(3)4;/h3*1H3,(H,3,4);/q;;;+3/p-3

Key: PVFSDGKDKFSOTB-DFZHHIFOAZ

SMILES

* CC(=O)[O-].CC(=O)[O-].CC(=O)[O-].[Fe+3]

* coordination complex: O1[C-](C)O[Fe+3]6([O-2]23)([OH2])(O[C-](C)O4)O[C-](C)O[Fe+3]24([OH2])(O[C-](C)O5)O[C-](C)O[Fe+3]135([OH2])O[C-]C(C)O6

Properties

Chemical formula

| C14H27Fe3O18
Molar mass | 650.9 g/mol
Appearance  | brownish-red powder

Solubility in water

| Insoluble
Solubility | soluble in ethanol[2]

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Infobox references

Tracking categories (test):

* SizeSet

Ferric acetate is the acetate salt of the coordination complex [Fe3O(OAc)6(H2O)3]+ (OAc− is CH3CO2−). Commonly the salt is known as "basic iron acetate".[3] The formation of the red-brown complex was once used as a test for ferric ions.[4]

## Contents

* 1 Structure and synthesis
* 2 Reactions
* 3 Related compounds
* 4 Uses
* 5 See also
* 6 References

## Structure and synthesis

Basic iron acetate forms on treating aqueous solutions of iron(III) sources with acetate salts.[5] A typical precursor is freshly precipitated iron oxide/hydroxide, which is halide-free.[6]

Early work showed that the cation is trinuclear.[7] The Fe centres are equivalent, each being octahedral, being bound to six oxygen ligands, including a triply bridging oxide at the center of the equilateral triangle.[8] The compound was an early example of a molecular complex of iron that features an oxide ligand. The cation has idealized D3h symmetry.

## Reactions

The terminal aqua ligands on the trimetallic framework can be substituted with other ligands, such as pyridine and dimethylformamide. Many different salts are known by exchanging the anion, e.g. [Fe3(μ3-O)(OAc)6(H2O)3]Cl. Reduction of the cation affords the neutral mixed-valence derivative that contains one ferrous and two ferric centers.[3] Mixed metal species are known such as [Fe2CoO(OAc)6(H2O)3].[9]

## Related compounds

Chromium(III), ruthenium(III), vanadium(III), and rhodium(III) form analogous compounds.[10] Iron(III) acetate (lacking the oxo ligand) has been claimed as a red coloured compound from the reaction of silver acetate and iron(III) chloride.[11]

## Uses

Materials prepared by heating iron, acetic acid, and air, loosely described as basic iron acetates, are used as dyes and mordants.[3]

Iron acetate is often brushed upon untreated wood to give it an aged appearance.

## See also

* Iron(II) acetate
* Cobalt(II) acetate
* Rhodium(II) acetate
* Manganese(III) acetate
* Chromium(III) acetate

## References

1. ↑ Lide, David R., ed (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. pp. 4–63. ISBN 0-8493-0487-3.
2. ↑ "Iron(III) Acetate". http://www.endmemo.com/chem/compound/fec2h3o2_3.php.
3. ↑ 3.0 3.1 3.2 J., Burgess; M. V., Twigg (2005). R. Bruce, King; J., Wiley. eds. Encyclopedia of inorganic chemistry (2nd ed.). New York: Wiley. ISBN 978-0-470-86078-6.
4. ↑ H., Brearley; F., Ibbotson (1902). The Analysis of Steel-Works Materials. London ; New York: Longmans, Green. http://www.clpdigital.org/jspui/handle/10493/809.
5. ↑ W., Simon (March 2007). Manual of Chemistry. p. 474. ISBN 978-1406733358.
6. ↑ H. Lux (1963). "Basic Iron(III) Acetate". in Georg Brauer. Handbook of Preparative Inorganic Chemistry. p. 1508.
7. ↑ Weinland, R.; Dinkelacker, P. (July 1909). "Über Salze einer Hexaacetato(formiato)-trichrombase. II". Berichte der Deutschen Chemischen Gesellschaft 42 (3): 2997–3018. doi:10.1002/cber.19090420318. https://zenodo.org/record/1426357.
8. ↑ Figgis, B. N.; Robertson, G. B. (13 February 1965). "Crystal-Molecular Structure and Magnetic Properties of Cr3(CH3.COO)6OCl.5H2O". Nature 205 (4972): 694–695. doi:10.1038/205694a0. Bibcode: 1965Natur.205..694F. This paper describes the isostructure chromium and iron compounds.
9. ↑ Blake, Antony B.; Yavari, Ahmad; Hatfield, William E.; Sethulekshmi, C. N. (1985). "Magnetic and spectroscopic properties of some heterotrinuclear basic acetates of chromium(III), iron(III), and divalent metal ions". Journal of the Chemical Society, Dalton Transactions (12): 2509. doi:10.1039/DT9850002509.
10. ↑ Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils, ed., Inorganic Chemistry, San Diego/Berlin: Academic Press/De Gruyter, ISBN 0-12-352651-5
11. ↑ Paul, Ram C.; Narula, Ramesh C.; Vasisht, Sham K. (December 1978). "Iron(III) acetates". Transition Metal Chemistry 3 (1): 35–38. doi:10.1007/BF01393501.

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Acetyl halides and salts of the acetate ion

AcOH |  |  |  | He
LiOAc | Be(OAc)2
BeAcOH | B(OAc)3 | AcOAc
ROAc | NH4OAc | AcOOH | FAc | Ne
NaOAc | Mg(OAc)2 | Al(OAc)3
ALSOL
Al(OAc)2OH
Al2SO4(OAc)4 | Si  | P  | S  | ClAc | Ar
KOAc | Ca(OAc)2 | Sc(OAc)3 | Ti(OAc)4 | VO(OAc)3 | Cr(OAc)2
Cr(OAc)3 | Mn(OAc)2
Mn(OAc)3 | Fe(OAc)2
Fe(OAc)3 | Co(OAc)2,
Co(OAc)3 | Ni(OAc)2 | Cu(OAc)2 | Zn(OAc)2 | Ga(OAc)3 | Ge  | As(OAc)3 | Se  | BrAc | Kr
RbOAc | Sr(OAc)2 | Y(OAc)3 | Zr(OAc)4 | Nb  | Mo(OAc)2 | Tc  | Ru(OAc)2
Ru(OAc)3
Ru(OAc)4 | Rh2(OAc)4 | Pd(OAc)2 | AgOAc | Cd(OAc)2 | In  | Sn(OAc)2
Sn(OAc)4 | Sb(OAc)3 | Te  | IAc | Xe
CsOAc | Ba(OAc)2 |  | Hf  | Ta  | W  | Re  | Os  | Ir  | Pt(OAc)2 | Au  | Hg2(OAc)2,
Hg(OAc)2 | TlOAc
Tl(OAc)3 | Pb(OAc)2
Pb(OAc)4 | Bi(OAc)3 | Po  | At  | Rn
Fr  | Ra  |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
La(OAc)3 | Ce(OAc)x | Pr  | Nd  | Pm  | Sm(OAc)3 | Eu(OAc)3 | Gd(OAc)3 | Tb  | Dy(OAc)3 | Ho(OAc)3 | Er  | Tm  | Yb(OAc)3 | Lu(OAc)3
Ac  | Th  | Pa  | UO2(OAc)2 | Np  | Pu  | Am  | Cm  | Bk  | Cf  | Es  | Fm  | Md  | No  | Lr

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