Chemistry:Iron(II) acetate
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| Names | |
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| IUPAC name
Iron(II) acetate
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| Other names
Ferrous acetate
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| Identifiers | |
3D model (JSmol)
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PubChem CID
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| Properties | |
| C4H6FeO4 | |
| Molar mass | 173.933 g·mol−1 |
| Appearance | White crystals (anhydrous) Light green crystals (tetrahydrate) |
| Odor | Odorless |
| Density | 1.734 g/cm3 (−73 °C)[1] |
| Melting point | 190–200 °C (374–392 °F; 463–473 K) decomposes[2][3] |
| Soluble[2] | |
| Structure | |
| Orthorhombic, oP75 (200 K) | |
| Pbcn, No. 60 (200 K)[1] | |
| 2/m 2/m 2/m (200 K) | |
a = 18.1715(4) Å, b = 22.1453(5) Å, c = 8.2781(2) Å (200 K) α = 90°, β = 90°, γ = 90°
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| Hazards | |
| GHS pictograms |  [3]
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| GHS Signal word | Warning |
| H315, H319, H335[3] | |
| P261, P305+351+338[3] | |
| NFPA 704 (fire diamond) | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
Iron(II) acetate is a coordination complex with formula Fe(CH3COO)2. It is a white solid, although impure samples can be slightly colored.[1] A light green tetrahydrate is also known, which is highly soluble in water.
Preparation and structure
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Iron powder reacts with acetic acid in electrolysis to give the ferrous acetate, with evolution of hydrogen gas:[1]
- Fe + 2 CH3CO2H → Fe(CH3CO2)2 + H2
It can also be made from the insoluble, olive green, Iron(II) carbonate.[citation needed]
It adopts a polymeric structure with octahedral Fe(II) centers interconnected by acetate ligands. It is a coordination polymer.[1]
A hydrated form be made by the reaction of ferrous oxide or ferrous hydroxide with acetic acid.[5]
Reaction of scrap iron with acetic acid affords a brown mixture of various iron(II) and iron(III) acetates that are used in dyeing.[6]
Uses
Ferrous acetate is used as a mordant by the dye industry. Ebonizing wood is one such process.[7]
References
- ↑ 1.0 1.1 1.2 1.3 1.4 1.5 Weber, Birgit; Betz, Richard; Bauer, Wolfgang; Schlamp, Stephan (2011). "Crystal Structure of Iron(II) Acetate". Zeitschrift für anorganische und allgemeine Chemie 637: 102–107. doi:10.1002/zaac.201000274.
- ↑ 2.0 2.1 Lide, David R., ed (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN 978-1-4200-9084-0.
- ↑ 3.0 3.1 3.2 3.3 Sigma-Aldrich Co., Iron(II) acetate. Retrieved on 2014-05-03.
- ↑ "MSDS of Ferrous acetate". Fisher Scientific. https://www.fishersci.ca/viewmsds.do?catNo=AC305370500.
- ↑ "Synthesis of Iron(II) acetate hydrate (ferrous acetate)". http://www.ims.demokritos.gr/people/tbou/iron_acetate.html.
- ↑ Wildermuth, Egon; Stark, Hans; Friedrich, Gabriele; Ebenhöch, Franz Ludwig; Kühborth, Brigitte; Silver, Jack; Rituper, Rafael (2000). "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a14_591.
- ↑ Ebonizing Wood with Ferric Acetate
Acetyl halides and salts of the acetate ion
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| 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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