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Antimony(III) acetate

Antimony(III) acetate is the compound of antimony with the chemical formula of Sb(CH3CO2)3. It is a white powder, is moderately water-soluble, and is used as a catalyst in the production of polyesters.

Antimony(III) acetate
Antimony(III) acetate
Names
IUPAC name
Antimony(III) acetate
Other names
Antimony triacetate
Acetic acid, antimony(3+) salt
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.027.312 Edit this at Wikidata
RTECS number
  • AF4200000
UNII
  • InChI=1S/3C2H4O2.Sb/c3*1-2(3)4;/h3*1H3,(H,3,4);/q;;;+3/p-3 checkY
    Key: JVLRYPRBKSMEBF-UHFFFAOYSA-K checkY
  • InChI=1/3C2H4O2.Sb.3H/c3*1-2(3)4;;;;/h3*1H3,(H,3,4);;;;/q;;;+3;;;/p-3/r3C2H4O2.H3Sb/c3*1-2(3)4;/h3*1H3,(H,3,4);1H3/q;;;+3/p-3
    Key: NSMVVPJZMRQLMR-ZHOQVWKLAW
  • InChI=1/3C2H4O2.Sb/c3*1-2(3)4;/h3*1H3,(H,3,4);/q;;;+3/p-3
    Key: JVLRYPRBKSMEBF-DFZHHIFOAU
  • O=C(C)O[Sb](OC(C)=O)OC(C)=O
Properties
Sb(CH3COO)3
Appearance White powder
Density 1.22 g/cm3 (20 °C)
Melting point 128.5 °C (263.3 °F; 401.6 K) (decomposes to Sb2O3)
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1
0
0
Lethal dose or concentration (LD, LC):
4480 mg/kg (rat)
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 0.5 mg/m3 (as Sb)[1]
REL (Recommended)
 TWA 0.5 mg/m3 (as Sb)[1]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Preparation

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It can be prepared by the reaction of antimony(III) oxide with acetic anhydride:

Sb2O3 + 3 C4H6O3 → 2 Sb(CH3CO2)3

Structure

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The crystal structure of antimony(III) acetate has been determined by X-ray crystallography. It consists of discrete Sb(OAc)3 monomers with monodentate acetate ligands. The monomers are linked together into chains by weaker C=O···Sb intermolecular interactions.[2]

References

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  1. ^ a b NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
  2. ^ Hall, M.; Sowerby, D. B. (1980). "Antimony(III) acetate and thioacetate: spectra and crystal structures". J. Chem. Soc., Dalton Trans. (8): 1292–1296. doi:10.1039/DT9800001292.
 

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