Antimony trichloride

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Antimony trichloride
Stereo structural formula of antimony trichloride
Stereo structural formula of antimony trichloride
Ball and stick model of antimony trichloride
Ball and stick model of antimony trichloride
Names
Preferred IUPAC name
Antimony trichloride
Systematic IUPAC name
Trichlorostibane
Other names
Antimony(III) chloride, Butter of antimony, Antimonous chloride, Stibous chloride, Trichlorostibine
Identifiers
3D model (
JSmol
)
ChEBI
ChemSpider
ECHA InfoCard
 100.030.031 Edit this at Wikidata
EC Number
  • 233-047-2
KEGG
MeSH Antimony+trichloride
RTECS number
  • CC4900000
UNII
UN number 1733
  • InChI=1S/3ClH.Sb/h3*1H;/q;;;+3/p-3 checkY
    Key: FAPDDOBMIUGHIN-UHFFFAOYSA-K checkY
  • InChI=1S/3ClH.Sb/h3*1H;/q;;;+3/p-3
    Key: FAPDDOBMIUGHIN-UHFFFAOYSA-K
  • InChI=1/3ClH.Sb/h3*1H;/q;;;+3/p-3
    Key: FAPDDOBMIUGHIN-DFZHHIFOAK
  • Cl[Sb](Cl)Cl
Properties
Cl3Sb
Molar mass 228.11 g·mol−1
Appearance Colorless solid, very
hygroscopic
Odor Sharp, pungent
Density 3.14 g/cm3 (25 °C)
2.51 g/cm3 (150 °C)[1]
Melting point 73.4 °C (164.1 °F; 346.5 K)[5]
Boiling point 223.5 °C (434.3 °F; 496.6 K)
601.1 g/100 ml (0 °C)[1]
985.1 g/100 mL (25 °C)
1.357 kg/100 mL (40 °C)[2]
Solubility Soluble in
selenium(IV) oxychloride
Insoluble in pyridine, quinoline
, organic bases
Solubility in acetic acid 143.9 g/100 g (0 °C)
205.8 g/100 g (10 °C)
440.5 g/100 g (25 °C)[3]
693.7 g/100 g (45 °C)[2]
Solubility in acetone 537.6 g/100 g (18 °C)[2][3]
Solubility in benzoyl chloride 139.2 g/100 g (15 °C)
169.5 g/100 g (25 °C)[3]
2.76 kg/100 g (70 °C)[2]
Solubility in hydrochloric acid 20 °C:
8.954 g/ g (4.63% w/w)
8.576 g/ g (14.4% w/w)
7.898 g/ g (36.7% w/w)[2]
Solubility in p-Cymene 69.5 g/100 g (-3.5 °C)
85.5 g/100 g (10 °C)
150 g/100 g (30 °C)
2.17 kg/100 g (70 °C)[2]
Vapor pressure 13.33 Pa (18.1 °C)[3]
0.15 kPa (50 °C)
2.6 kPa (100 °C)[4]
-86.7·10−6 cm3/mol
1.46[1]
Structure
Orthorhombic
3.93 D (20 °C)[3]
Thermochemistry
183.3 J/mol·K[3]
110.5 J/mol·K[3]
Std enthalpy of
formation
(ΔfH⦵298)
 -381.2 kJ/mol[3]
-322.5 kJ/mol[3]
Hazards
GHS labelling:
GHS05: CorrosiveGHS09: Environmental hazard[5]
Danger
H314, H411[5]
P273, P280, P305+P351+P338, P310[5]
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
2
0
1
Flash point Non-flammable
Lethal dose or concentration (LD, LC):
525 mg/kg (oral, rat)
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 0.5 mg/m3 (as Sb)[6]
REL (Recommended)
 TWA 0.5 mg/m3 (as Sb)[6]
Safety data sheet (SDS) ICSC 1224
Related compounds
Other anions
 Antimony trifluoride
Antimony tribromide
Antimony triiodide
Other cations
 Nitrogen trichloride
Phosphorus trichloride
Arsenic trichloride
Bismuth chloride
Related compounds
 Antimony pentachloride
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 ?)

Antimony trichloride is the chemical compound with the formula SbCl3. It is a soft colorless solid with a pungent odor and was known to alchemists as butter of antimony.

Preparation

Antimony trichloride is prepared by reaction of chlorine with antimony, antimony tribromide, antimony trioxide, or antimony trisulfide. It also may be made by treating antimony trioxide with concentrated hydrochloric acid.

Reactions

Antimony trichloride solution in hydrochloric acid

SbCl3 is readily hydrolysed and samples of SbCl3 must be protected from moisture. With a limited amount of water it forms antimony oxychloride releasing hydrogen chloride:

SbCl3 + H2O → SbOCl + 2 HCl

With more water it forms Sb
4O
5Cl
2 which on heating to 460° under argon converts to Sb
8O
11Cl
12.[7]

SbCl3 readily forms complexes with halides, but the stoichiometries are not a good guide to the composition;[7] for example, the (C
5H
5NH)SbCl
4 contains a chain anion with distorted SbIII octahedra. Similarly the salt (C
4H
9NH
3)
2SbCl
5 contains a polymeric anion of composition [SbCl2−
5]
n with distorted octahedral SbIII.[8]

With nitrogen donor ligands, L, complexes with a stereochemically active lone-pair are formed, for example Ψ-trigonal bipyramidal LSbCl3 and Ψ-octahedral L
2SbCl
3.[9]

While SbCl3 is only a weak Lewis base,

carbonyl complexes Fe(CO)
3(SbCl
3)
2 and Ni(CO)
3SbCl
3, are known.[9]

Structure

In the gas phase SbCl3 is pyramidal with a Cl-Sb-Cl angle of 97.2° and a bond length of 233 pm.[10] In SbCl3 each Sb has three Cl atoms at 234 pm showing the persistence of the molecular SbCl3 unit, however there are a further five neighboring Cl atoms, two at 346 pm, one at 361 pm, and two at 374 pm. These eight atoms can be considered as forming a bicapped trigonal prism. These distances can be contrasted with BiCl3 which has three near neighbors at 250 pm, with two at 324 pm, and three at a mean of 336 pm. The point to note here is that the all eight close neighbours of Bi are closer than the eight closest neighbours of Sb, demonstrating the tendency for Bi to adopt higher coordination numbers.[10][7]

Uses

SbCl3 is a

complex that can be measured by colorimetry
.

Antimony trichloride has also been used as an adulterant to enhance the louche effect in absinthe. It has been used in the past to dissolve and remove horn buds from calves without having to cut them off.

It is also used as a catalyst for polymerization, hydrocracking, and chlorination reactions; as a mordant; and in the production of other antimony salts. Its solution is used as an analytical reagent for chloral, aromatics, and vitamin A.[11] It has a very potential use as a Lewis acid catalyst in synthetic organic transformation.

A solution of antimony trichloride in liquid hydrogen sulfide is a good conductor, though the applications of such are limited by the very low temperature or high pressure required for hydrogen sulfide to be liquid.[12]

References in popular culture

In episode 2 of the third season of the popular British program

All Things Wise and Wonderful), several calves died at Kate Billings farm following an episode of nonspecific gastroenteritis
, the cause of which was later determined to be ingestion of antimony trichloride present in a topical "butter of antimony" solution painted on to cauterize and remove their horn buds.

References

Wikimedia Commons has media related to Antimony trichloride.
  1. ^ a b c "Antimony Trichloride, SbCl3".
  2. ^ a b c d e f Seidell, Atherton; Linke, William F. (1952). Solubilities of Inorganic and Organic Compounds. Van Nostrand.
  3. ^ a b c d e f g h i "Antimony(III) chloride".
  4. ^ Antimony trichloride in Linstrom, Peter J.; Mallard, William G. (eds.); NIST Chemistry WebBook, NIST Standard Reference Database Number 69, National Institute of Standards and Technology, Gaithersburg (MD) (retrieved 2014-05-28)
  5. ^ a b c d Sigma-Aldrich Co., Antimony(III) chloride. Retrieved on 2014-05-29.
  6. ^ a b NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
  7. ^
    ISBN 978-0-08-022057-4
    .
  8. Z. Naturforsch. B 2006, 61, 1101–1109. Abstract (PDF)
  9. ^
    ISBN 0-471-93620-0
  10. ^
    ISBN 0-19-855370-6
  11. ISBN 0-07-049439-8
    .
  12. ISSN 0009-2665
    .
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