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Names | |||
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IUPAC names
Tetrachlorostannane
Tin tetrachloride Tin(IV) chloride | |||
Other names
Stannic chloride
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Identifiers | |||
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3D model (JSmol)
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ChemSpider | |||
ECHA InfoCard | 100.028.717 | ||
EC Number |
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PubChem CID
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RTECS number |
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UNII | |||
UN number | 1827 | ||
CompTox Dashboard (EPA)
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Properties | |||
SnCl4 | |||
Molar mass | 260.50 g/mol (anhydrous) 350.60 g/mol (pentahydrate) | ||
Appearance | Colorless fuming liquid | ||
Odor | Acrid | ||
Density | 2.226 g/cm3 (anhydrous) 2.04 g/cm3 (pentahydrate) | ||
Melting point | −34.07 °C (−29.33 °F; 239.08 K) (anhydrous) 56 °C (133 °F; 329 K) (pentahydrate) | ||
Boiling point | 114.15 °C (237.47 °F; 387.30 K) | ||
hydrolysis,very hygroscopic (anhydrous) very soluble (pentahydrate) | |||
Solubility | soluble in alcohol, benzene, toluene, chloroform, acetone, kerosene, CCl4, methanol, gasoline, CS2 | ||
Vapor pressure | 2.4 kPa | ||
−115·10−6 cm3/mol | |||
Refractive index (nD)
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1.512 | ||
Structure | |||
monoclinic (P21/c) | |||
Hazards | |||
GHS labelling: | |||
Danger | |||
H314, H412 | |||
P260, P264, P273, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P405, P501 | |||
NFPA 704 (fire diamond) | |||
Safety data sheet (SDS) | ICSC 0953 | ||
Related compounds | |||
Other anions
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Tin(IV) fluoride Tin(IV) bromide Tin(IV) iodide | ||
Other cations
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Carbon tetrachloride Silicon tetrachloride Germanium tetrachloride Lead(IV) chloride | ||
Related compounds
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Tin(II) chloride | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Tin(IV) chloride, also known as tin tetrachloride or stannic chloride, is an inorganic compound of tin and chlorine with the formula SnCl4. It is a colorless hygroscopic liquid, which fumes on contact with air. It is used as a precursor to other tin compounds.[1] It was first discovered by Andreas Libavius (1550–1616) and was known as spiritus fumans libavii.
It is prepared from reaction of chlorine gas with tin at 115 °C (239 °F):
Anhydrous tin(IV) chloride solidifies at −33 °C to give monoclinic crystals with the P21/c space group. It is isostructural with SnBr4. The molecules adopt near-perfect tetrahedral symmetry with average Sn–Cl distances of 227.9(3) pm.[2]
Tin(IV) chloride is well known as a Lewis acid. Thus it forms hydrates. The pentahydrate SnCl4·5H2O was formerly known as butter of tin. They all consist of [SnCl4(H2O)2] molecules together with varying amounts of water of crystallization. The additional water molecules link together the molecules of [SnCl4(H2O)2] through hydrogen bonds.[3] Although the pentahydrate is the most common hydrate, lower hydrates have also been characterised.[4]
Aside from water, other Lewis bases form adducts with SnCl4. These include ammonia and organophosphines. The complex [SnCl6]2− is formed with hydrochloric acid making hexachlorostannic acid.[1]
Anhydrous tin(IV) chloride is a major precursor in organotin chemistry. Upon treatment with Grignard reagents, tin(IV) chloride gives tetraalkyltin compounds:[5]
Anhydrous tin(IV) chloride reacts with tetraorganotin compounds in redistribution reactions:
These organotin halides are useful precursors to catalysts (e.g., dibutyltin dilaurate) and polymer stabilizers.[6]
SnCl4 is used in Friedel–Crafts reactions as a Lewis acid catalyst.[1] For example, the acetylation of thiophene to give 2-acetylthiophene is promoted by tin(IV) chloride.[7] Similarly, tin(IV) chloride is useful for the nitrations.[8]
Stannic chloride was used as a chemical weapon in World War I, as it formed an irritating (but non-deadly) dense smoke on contact with air. It was supplanted by a mixture of silicon tetrachloride and titanium tetrachloride near the end of the war due to shortages of tin.[9]
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