|Preferred IUPAC name
|Systematic IUPAC name
Antimony(III) chloride, Butter of antimony, Antimonous chloride, Stibous chloride, Trichlorostibine
3D model (JSmol)
CompTox Dashboard (EPA)
|Molar mass||228.11 g·mol−1|
|Appearance||Colorless solid, very hygroscopic|
|Density||3.14 g/cm3 (25 °C)|
2.51 g/cm3 (150 °C)
|Melting point||73.4 °C (164.1 °F; 346.5 K) |
|Boiling point||223.5 °C (434.3 °F; 496.6 K)|
|601.1 g/100 mL (0 °C)|
985.1 g/100 mL (25 °C)
1.357 kg/100 mL (40 °C)
|Solubility||Soluble in 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)
693.7 g/100 g (45 °C)
|Solubility in acetone||537.6 g/100 g (18 °C)|
|Solubility in benzoyl chloride||139.2 g/100 g (15 °C)|
169.5 g/100 g (25 °C)
2.76 kg/100 g (70 °C)
|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)
|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)
|Vapor pressure||13.33 Pa (18.1 °C)|
0.15 kPa (50 °C)
2.6 kPa (100 °C)
Refractive index (nD)
|3.93 D (20 °C)|
Heat capacity (C)
Std enthalpy of
Gibbs free energy (ΔfG˚)
|Safety data sheet||ICSC 1224|
|GHS Signal word||Danger|
|P273, P280, P305+351+338, P310|
|NFPA 704 (fire diamond)|
|Lethal dose or concentration (LD, LC):|
LD50 (median dose)
|525 mg/kg (oral, rat)|
|NIOSH (US health exposure limits):|
|TWA 0.5 mg/m3 (as Sb)|
|TWA 0.5 mg/m3 (as Sb)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
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.
With more water it forms Sb4O5Cl2 which on heating to 460° under argon converts to Sb8O11Cll2.
SbCl3 readily forms complexes with halides, but the stoichiometries are not a good guide to the composition, for example the (C5H5NH)SbCl4 contains a chain anion with distorted SbIII octahedra. Similarly the salt (C4H9NH3)2SbCl5 contains a polymeric anion of composition [SbCl52−]n with distorted octahedral SbIII.
With nitrogen donor ligands, L, complexes with a stereochemically active lone-pair are formed, for example Ψ-trigonal bipyramidal LSbCl3 and Ψ-octahedral L2SbCl3.
In the gas phase SbCl3 is pyramidal with a Cl-Sb-Cl angle of 97.2° and a bond length of 233 pm. 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.
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 stubs 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. 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.
In episode 12 of the third season of the popular British program All Creatures Great and Small, several calves died following an episode of nonspecific gastroenteritis, the cause of which was later determined to be ingestion of antimony trichloride present in a solution used to dissolve their horn stubs.
|Wikimedia Commons has media related to Antimony trichloride.|