Tin(IV) chloride
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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
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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 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.
Preparation
It is prepared from reaction of chlorine gas with tin at 115 °C (239 °F).
- Sn + 2Cl
2 → SnCl
4
Structure
Anhydrous tin(IV) chloride solidifies at −33 °C to give
Reactions
Tin(IV) chloride is well known as a
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]
Applications
Precursor to organotin compounds
Anhydrous tin(IV) chloride is a major precursor in organotin chemistry. Upon treatment with Grignard reagents, tin(IV) chloride gives tetraalkyltin compounds:[5]
- SnCl4 + 4 RMgCl → SnR4 + 4 MgCl2
Anhydrous tin(IV) chloride reacts with tetraorganotin compounds in
- SnCl4 + SnR4 → 2 SnCl2R2
These organotin halides are useful precursors to catalysts (e.g., dibutyltin dilaurate) and polymer stabilizers.[6]
Organic synthesis
SnCl4 is used in
Safety
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]
References
- ^ ISBN 0-12-352651-5.)
{{cite book}}
: CS1 maint: multiple names: authors list (link - .
- .
- PMID 15071197.
- ISBN 978-0-08-037941-8.
- .
- S2CID 98109571.
- ISBN 978-1-4437-3840-8..
External links
- International Chemical Safety Card 0953
- tinchemical.com/products (industrial uses) at the Wayback Machine (archived 2005-02-28)