Antimony trichloride

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Antimony trichloride
Antimony trichloride solid.jpeg
Stereo structural formula of antimony trichloride SbCl3.png
Stereo structural formula of antimony trichloride
Ball and stick model of antimony trichloride Antimony-trichloride-3D-balls.png
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 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 233-047-2
KEGG
MeSH Antimony+trichloride
PubChem CID
RTECS number
  • CC4900000
UNII
UN number 1733
  • InChI=1S/3ClH.Sb/h3*1H;/q;;;+3/p-3 Yes check.svgY
    Key: FAPDDOBMIUGHIN-UHFFFAOYSA-K Yes check.svgY
  • 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
AppearanceColorless 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) [2]
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) [3]
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) [4]
693.7 g/100 g (45 °C) [3]
Solubility in acetone 537.6 g/100 g (18 °C) [3] [4]
Solubility in benzoyl chloride 139.2 g/100 g (15 °C)
169.5 g/100 g (25 °C) [4]
2.76 kg/100 g (70 °C) [3]
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) [3]
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) [3]
Vapor pressure 13.33 Pa (18.1 °C) [4]
0.15 kPa (50 °C)
2.6 kPa (100 °C) [5]
-86.7·10−6 cm3/mol
1.46 [1]
Structure
Orthorhombic
3.93 D (20 °C) [4]
Thermochemistry
183.3 J/mol·K [4]
Std molar
entropy (S⦵298)
110.5 J/mol·K [4]
-381.2 kJ/mol [4]
-322.5 kJ/mol [4]
Hazards
GHS labelling:
GHS-pictogram-acid.svg GHS-pictogram-pollu.svg [2]
Danger
H314, H411 [2]
P273, P280, P305+P351+P338, P310 [2]
NFPA 704 (fire diamond)
NFPA 704.svgHealth 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).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

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

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 Antimony trichloride solution.JPG
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, [7] some complexes, such as the 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 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; 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]

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 Ken 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.

Related Research Articles

<span class="mw-page-title-main">Antimony</span> Chemical element, symbol Sb and atomic number 51

Antimony is a chemical element with the symbol Sb (from Latin stibium) and atomic number 51. A lustrous gray metalloid, it is found in nature mainly as the sulfide mineral stibnite (Sb2S3). Antimony compounds have been known since ancient times and were powdered for use as medicine and cosmetics, often known by the Arabic name kohl. The earliest known description of the metalloid in the West was written in 1540 by Vannoccio Biringuccio.

<span class="mw-page-title-main">Aluminium chloride</span> Chemical compound

Aluminium chloride, also known as aluminium trichloride, is an inorganic compound with the formula AlCl3. It forms a hexahydrate with the formula [Al(H2O)6]Cl3, containing six water molecules of hydration. Both the anhydrous form and the hexahydrate are colourless crystals, but samples are often contaminated with iron(III) chloride, giving them a yellow colour.

<span class="mw-page-title-main">Thionyl chloride</span> Inorganic compound (SOCl2)

Thionyl chloride is an inorganic compound with the chemical formula SOCl2. It is a moderately volatile, colourless liquid with an unpleasant acrid odour. Thionyl chloride is primarily used as a chlorinating reagent, with approximately 45,000 tonnes per year being produced during the early 1990s, but is occasionally also used as a solvent. It is toxic, reacts with water, and is also listed under the Chemical Weapons Convention as it may be used for the production of chemical weapons.

<span class="mw-page-title-main">Phosphorus pentachloride</span> Chemical compound

Phosphorus pentachloride is the chemical compound with the formula PCl5. It is one of the most important phosphorus chlorides/oxychlorides, others being PCl3 and POCl3. PCl5 finds use as a chlorinating reagent. It is a colourless, water-sensitive solid, although commercial samples can be yellowish and contaminated with hydrogen chloride.

<span class="mw-page-title-main">Phosphorus trichloride</span> Chemical compound

Phosphorus trichloride is an inorganic compound with the chemical formula PCl3. A colorless liquid when pure, it is an important industrial chemical, being used for the manufacture of phosphites and other organophosphorus compounds. It is toxic and reacts readily with water to release hydrogen chloride.

<span class="mw-page-title-main">Rhodium(III) chloride</span> Chemical compound

Rhodium(III) chloride refers to inorganic compounds with the formula RhCl3(H2O)n, where n varies from 0 to 3. These are diamagnetic solids featuring octahedral Rh(III) centres. Depending on the value of n, the material is either a dense brown solid or a soluble reddish salt. The soluble trihydrated (n = 3) salt is widely used to prepare compounds used in homogeneous catalysis, notably for the industrial production of acetic acid and hydroformylation.

Antimony pentafluoride is the inorganic compound with the formula SbF5. This colourless, viscous liquid is a strong Lewis acid and a component of the superacid fluoroantimonic acid, formed upon mixing liquid HF with liquid SbF5 in 1:1 ratio. It is notable for its strong Lewis acidity and the ability to react with almost all known compounds.

<span class="mw-page-title-main">Arsenic pentoxide</span> Chemical compound

Arsenic pentoxide is the inorganic compound with the formula As2O5. This glassy, white, deliquescent solid is relatively unstable, consistent with the rarity of the As(V) oxidation state. More common, and far more important commercially, is arsenic(III) oxide (As2O3). All inorganic arsenic compounds are highly toxic and thus find only limited commercial applications.

Titanium(III) chloride is the inorganic compound with the formula TiCl3. At least four distinct species have this formula; additionally hydrated derivatives are known. TiCl3 is one of the most common halides of titanium and is an important catalyst for the manufacture of polyolefins.

<span class="mw-page-title-main">Antimony pentachloride</span> Chemical compound

Antimony pentachloride is a chemical compound with the formula SbCl5. It is a colourless oil, but typical samples are yellowish due to dissolved chlorine. Owing to its tendency to hydrolyse to hydrochloric acid, SbCl5 is a highly corrosive substance and must be stored in glass or PTFE containers.

<span class="mw-page-title-main">Arsenic trichloride</span> Chemical compound

Arsenic trichloride is an inorganic compound with the formula AsCl3, also known as arsenous chloride or butter of arsenic. This poisonous oil is colourless, although impure samples may appear yellow. It is an intermediate in the manufacture of organoarsenic compounds.

<span class="mw-page-title-main">Antimony pentoxide</span> Chemical compound

Antimony pentoxide (molecular formula: Sb2O5) is a chemical compound of antimony and oxygen. It contains antimony in the +5 oxidation state.

<span class="mw-page-title-main">Indium(III) chloride</span> Chemical compound

Indium(III) chloride is the chemical compound with the formula InCl3. This salt is a white, flaky solid with applications in organic synthesis as a Lewis acid. It is also the most available soluble derivative of indium. This is one of three known indium chlorides.

Technetium compounds are chemical compounds containing the chemical element technetium. Technetium can form multiple oxidation states, but often forms in the +4 and +7 oxidation states. Because technetium is radioactive, technetium compounds are extremely rare on Earth.

Antimony trifluoride is the inorganic compound with the formula SbF3. Sometimes called Swarts' reagent, is one of two principal fluorides of antimony, the other being SbF5. It appears as a white solid. As well as some industrial applications, it is used as a reagent in inorganic and organofluorine chemistry.

<span class="mw-page-title-main">Bismuth chloride</span> Chemical compound

Bismuth chloride (or butter of bismuth) is an inorganic compound with the chemical formula BiCl3. It is a covalent compound and is the common source of the Bi3+ ion. In the gas phase and in the crystal, the species adopts a pyramidal structure, in accord with VSEPR theory.

Antimony pentasulfide is an inorganic compound of antimony and sulfur, also known as antimony red. It is a nonstoichiometric compound with a variable composition. Its structure is unknown. Commercial samples are contaminated with sulfur, which may be removed by washing with carbon disulfide in a Soxhlet extractor.

<span class="mw-page-title-main">Berkelium compounds</span> Any chemical compound having at least one berkelium atom

Berkelium forms a number of chemical compounds, where it normally exists in an oxidation state of +3 or +4, and behaves similarly to its lanthanide analogue, terbium. Like all actinides, berkelium easily dissolves in various aqueous inorganic acids, liberating gaseous hydrogen and converting into the trivalent oxidation state. This trivalent state is the most stable, especially in aqueous solutions, but tetravalent berkelium compounds are also known. The existence of divalent berkelium salts is uncertain and has only been reported in mixed lanthanum chloride-strontium chloride melts. Aqueous solutions of Bk3+ ions are green in most acids. The color of the Bk4+ ions is yellow in hydrochloric acid and orange-yellow in sulfuric acid. Berkelium does not react rapidly with oxygen at room temperature, possibly due to the formation of a protective oxide surface layer; however, it reacts with molten metals, hydrogen, halogens, chalcogens and pnictogens to form various binary compounds. Berkelium can also form several organometallic compounds.

Niobium(III) chloride also known as niobium trichloride is a compound of niobium and chlorine. The binary phase NbCl3 is not well characterized but many adducts are known.

References

  1. 1 2 3 "Antimony Trichloride, SbCl3".
  2. 1 2 3 4 Sigma-Aldrich Co., Antimony(III) chloride. Retrieved on 2014-05-29.
  3. 1 2 3 4 5 6 Seidell, Atherton; Linke, William F. (1952). Solubilities of Inorganic and Organic Compounds. Van Nostrand.
  4. 1 2 3 4 5 6 7 8 9 "Antimony(III) chloride".
  5. ↑ 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)
  6. 1 2 NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
  7. 1 2 3 4 Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. pp. 558–571. ISBN   978-0-08-022057-4.
  8. ↑ Zarychta, B.; Zaleski, J. "Phase transitions mechanism and distortion of SbCl3−
    6     octahedra in bis(n-butylammonium) pentachloroantimonate(III) (C
    4    H
    9    NH
    3    )
    2    [SbCl
    5    ]    ". Z. Naturforsch. B 2006, 61, 1101–1109. Abstract (PDF)
  9. 1 2 "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. 1 2 Wells A.F. (1984) Structural Inorganic Chemistry 5th edition, pp. 879 - 884, Oxford Science Publications, ISBN   0-19-855370-6
  11. ↑ Patnaik, P. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN   0-07-049439-8.
  12. ↑ Wilkinson, John A. (1931). "Liquid Hydrogen Sulfide as a Reaction Medium". Chemical Reviews. 8 (2): 237–250. doi:10.1021/cr60030a005. ISSN   0009-2665.
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