Antimony trichloride

| Stereo structural formula of antimony trichloride | Ball and stick model of antimony trichloride

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Names
Preferred IUPAC name

Antimony trichloride

Systematic IUPAC name

Trichlorostibane

Other names

Antimony(III) chloride, Butter of antimony, Antimonous chloride, Stibous chloride, Trichlorostibine

Identifiers

CAS Number

* 10025-91-9 Y

3D model (JSmol)

* Interactive image

ChEBI |

* CHEBI:74856 N

ChemSpider |

* 23199 Y

EC Number |

* 233-047-2

KEGG |

* C15235 N

MeSH | Antimony+trichloride

PubChem CID

* 24814

RTECS number |

* CC4900000

UNII |

* J281401KK3 Y

UN number | 1733

InChI

* InChI=1S/3ClH.Sb/h3*1H;/q;;;+3/p-3 Y

Key: FAPDDOBMIUGHIN-UHFFFAOYSA-K Y

* 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

SMILES

* Cl[Sb](Cl)Cl

Properties

Chemical formula

| 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)

Solubility in water

| 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 acetone, ethanol, CH2Cl2, phenyls, ether, dioxane, CS2, CCl4, CHCl3, cyclohexane, 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]

Magnetic susceptibility (χ)

| −86.7·10−6 cm3/mol

Refractive index (nD)

| 1.46[1]
Structure

Crystal structure

| Orthorhombic

Dipole moment

| 3.93 D (20 °C)[3]
Thermochemistry

Heat capacity (C)

| 183.3 J/mol·K[3]

Std molar
entropy (S ~~o~~ 298)

| 110.5 J/mol·K[3]

Std enthalpy of
formation (ΔfH⦵298)

| −381.2 kJ/mol[3]

Gibbs free energy (ΔfG˚)

| −322.5 kJ/mol[3]
Hazards
Safety data sheet | ICSC 1224
GHS pictograms | [5]
GHS Signal word | Danger

GHS hazard statements

| H314, H411[5]

GHS precautionary statements

| P273, P280, P305+351+338, P310[5]
NFPA 704 (fire diamond)  |

Flash point | Non-flammable
Lethal dose or concentration (LD, LC):

LD50 (median dose)

| 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]
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 YN ?)
Infobox references

Tracking categories (test):

* PairSizeSet

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.

## Contents

* 1 Preparation
* 2 Reactions
* 3 Structure
* 4 Uses
* 5 References in popular culture
* 6 References

## 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 Sb4O5Cl2 which on heating to 460° under argon converts to Sb8O11Cl12.[7]

SbCl3 readily forms complexes with halides, but the stoichiometries are not a good guide to the composition;[7] for example, the (C5H5NH)SbCl4 contains a chain anion with distorted SbIII octahedra. Similarly the salt (C4H9NH3)2SbCl5 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 L2SbCl3.[9]

While SbCl3 is only a weak Lewis base,[7] some complexes, such as the carbonyl complexes Fe(CO)3(SbCl3)2 and Ni(CO)3SbCl3, 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 reagent for detecting vitamin A and related carotenoids in the Carr-Price test. The antimony trichloride reacts with the carotenoid to form a blue 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; [11] a mordant; and in the production of other antimony salts. Its solution is used as an analytical reagent for chloral, aromatics, and vitamin A.[12] 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.[13]

## References in popular culture

In episode 2 of the third season of the popular British program All Creatures Great and Small (adapted from chapter six of the book 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

1. ↑ 1.0 1.1 1.2 "Antimony Trichloride, SbCl3". https://antimony.atomistry.com/antimony_trichloride.html.
2. ↑ 2.0 2.1 2.2 2.3 2.4 2.5 Seidell, Atherton; Linke, William F. (1952). Solubilities of Inorganic and Organic Compounds. Van Nostrand.
3. ↑ 3.0 3.1 3.2 3.3 3.4 3.5 3.6 3.7 3.8 "Antimony(III) chloride". http://chemister.ru/Database/properties-en.php?dbid=1&id=1978.
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), http://webbook.nist.gov (retrieved 2014-05-28)
5. ↑ 5.0 5.1 5.2 5.3 Sigma-Aldrich Co., Antimony(III) chloride. Retrieved on 2014-05-29.
6. ↑ 6.0 6.1 NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0036.html.
7. ↑ 7.0 7.1 7.2 7.3 Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. pp. 558–571. ISBN 978-0-08-022057-4. https://books.google.com/books?id=OezvAAAAMAAJ&q=0-08-022057-6&dq=0-08-022057-6&source=bl&ots=m4tIRxdwSk&sig=XQTTjw5EN9n5z62JB3d0vaUEn0Y&hl=en&sa=X&ei=UoAWUN7-EM6ziQfyxIDoCQ&ved=0CD8Q6AEwBA.
8. ↑ Zarychta, B.; Zaleski, J. "Phase transitions mechanism and distortion of SbCl3−6 octahedra in bis(n-butylammonium) pentachloroantimonate(III) (C4H9NH3)2[SbCl5]". Z. Naturforsch. B 2006, 61, 1101–1109. Abstract (PDF)
9. ↑ 9.0 9.1 "Antimony: Inorganic Chemistry" R. Bruce King Encyclopedia of Inorganic Chemistry Editor R Bruce King (1994) John Wiley and Sons ISBN 0-471-93620-0
10. ↑ 10.0 10.1 Wells A.F. (1984) Structural Inorganic Chemistry 5th edition, pp. 879 - 884, Oxford Science Publications, ISBN 0-19-855370-6
11. ↑ Shiv Hydromet
12. ↑ Patnaik, P. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8.
13. ↑ Wilkinson, John A. (1931). "Liquid Hydrogen Sulfide as a Reaction Medium." (in EN). Chemical Reviews 8 (2): 237–250. doi:10.1021/cr60030a005. ISSN 0009-2665.

* v
* t
* e

Antimony compounds

* SbBr3
* Sb(C2H3O2)3
* SbCl3
* SbCl5
* SbF3
* SbF5
* SbH3
* SbI3
* Sb2O3
* Sb2O4
* Sb2O5
* Sb2S3
* Sb2S5
* Sb2(SO4)3
* Sb2Se3
* Sb2Te3

* v
* t
* e

Salts and covalent derivatives of the chloride ion

HCl |  |  |  | He

|
|
|
|

LiCl | BeCl2 | BCl3
B2Cl4 | CCl4 | NCl3
ClN3 | Cl2O
ClO2
Cl2O7 | ClF
ClF3
ClF5 | Ne
NaCl | MgCl2 | AlCl
AlCl3 | SiCl4 | P2Cl4
PCl3
PCl5 | S2Cl2
SCl2
SCl4 | Cl2 | Ar
KCl | CaCl
CaCl2 | ScCl3 | TiCl2
TiCl3
TiCl4 | VCl2
VCl3
VCl4
VCl5 | CrCl2
CrCl3
CrCl4 | MnCl2 | FeCl2
FeCl3 | CoCl2
CoCl3 | NiCl2 | CuCl
CuCl2 | ZnCl2 | GaCl2
GaCl3 | GeCl2
GeCl4 | AsCl3
AsCl5 | Se2Cl2
SeCl4 | BrCl | KrCl
RbCl | SrCl2 | YCl3 | ZrCl3
ZrCl4 | NbCl4
NbCl5 | MoCl2
MoCl3
MoCl4
MoCl5
MoCl6 | TcCl4 | RuCl3 | RhCl3 | PdCl2 | AgCl | CdCl2 | InCl
InCl2
InCl3 | SnCl2
SnCl4 | SbCl3
SbCl5 | Te3Cl2
TeCl4 | ICl
ICl3 | XeCl
XeCl2
CsCl | BaCl2 |  | HfCl4 | TaCl5 | WCl2
WCl3
WCl4
WCl5
WCl6 | Re3Cl9
ReCl4
ReCl5
ReCl6 | OsCl4 | IrCl2
IrCl3
IrCl4 | PtCl2
PtCl4 | AuCl
AuCl3 | Hg2Cl2,
HgCl2 | TlCl | PbCl2,
PbCl4 | BiCl3 | PoCl2,
PoCl4 | AtCl  | RnCl2
FrCl | RaCl2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
LaCl3 | CeCl3 | PrCl3 | NdCl2,
NdCl3 | PmCl3 | SmCl2,
SmCl3 | EuCl2,
EuCl3 | GdCl3 | TbCl3 | DyCl2,
DyCl3 | HoCl3 | ErCl3 | TmCl2
TmCl3 | YbCl2
YbCl3 | LuCl3
AcCl3 | ThCl4 | PaCl5 | UCl3
UCl4
UCl5
UCl6 | NpCl4 | PuCl3 | AmCl2
AmCl3 | CmCl3 | BkCl3 | CfCl3 | EsCl3 | Fm  | Md  | No  | LrCl3

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*[CID]: Compound ID
*[H314]: Causes severe skin burns and eye damage
*[H411]: Toxic to aquatic life with long lasting effects
*[P273]: Avoid release to the environment
*[P280]: Wear protective gloves/protective clothing/eye protection/face protection
*[P305+351+338]: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do – continue rinsing
*[P310]: Immediately call a POISON CENTER or doctor/physician
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