Tin(IV) chloride
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Names | |||
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IUPAC names
Tetrachlorostannane
Tin tetrachloride Tin(IV) chloride |
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Other names
Stannic chloride
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Identifiers | |||
7646-78-8 ![]() 10026-06-9 (pentahydrate) ![]() |
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ChemSpider | 22707 ![]() |
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EC Number | 231-588-9 | ||
Jmol 3D model | Interactive image | ||
PubChem | 24287 | ||
RTECS number | XP8750000 | ||
UN number | 1827 | ||
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Properties | |||
SnCl4 | |||
Molar mass | 260.50 g/mol (anhydrous) 350.60 g/mol (pentahydrate) |
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Appearance | colorless to slightly yellow fuming liquid | ||
Odor | acrid | ||
Density | 2.226 g/cm3 (anhydrous) 2.04 g/cm3 (pentahydrate) |
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Melting point | −34.07 °C (−29.33 °F; 239.08 K) (anhydrous) 56 °C (133 °F; 329 K) (pentahydrate) |
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Boiling point | 114.15 °C (237.47 °F; 387.30 K) | ||
decomposes (anhydrous) very soluble (pentahydrate) |
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Solubility | soluble in alcohol, benzene, toluene, chloroform, acetone, kerosene, CCl4, methanol, gasoline, CS2 | ||
Vapor pressure | 2.4 kPa | ||
Refractive index (nD)
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1.512 | ||
Structure | |||
monoclinic (P21/c) | |||
Vapor pressure | {{{value}}} | ||
Related compounds | |||
Other anions
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Tin(IV) fluoride Tin(IV) bromide Tin(IV) iodide |
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Other cations
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Carbon tetrachloride Silicon tetrachloride Germanium tetrachloride Tin(II) chloride Lead(IV) chloride |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references | |||
Tin(IV) chloride, also known as tin tetrachloride or stannic chloride is a inorganic compound with the formula SnCl4. At room temperature it is a colourless liquid, which fumes on contact with air, giving a stinging odor. It is used as precursor to other tin compounds.[1] It was first discovered by Andreas Libavius (1550–1616) and was known as "spiritus fumans libavii".
Contents
Preparation
It is prepared from reaction of chlorine gas with elemental tin at 115 °C (239 °F).
- Sn + 2 Cl2 → SnCl4
Structure
Anhydrous tin(IV) chloride solidifies at −33 °C to give monoclinic crystals with the P21/c space group; making it isostructural to solidified SnBr4. Within this the molecules adopt near perfect tetrahedral symmetry with average Sn–Cl distances of 227.9(3) pm.[2]
Several forms of hydrated tin tetrachloride are known. They all consist of [SnCl4(H2O)2] molecules together with varying amouts of water of crystallization. The additional water molecules link together the molecules of [SnCl4(H2O)2] through hydrogen bonds.[3] Although the pentahydrate is most common of the hydrates, lower hydrates have also been characterised.[4]
Reactions
Anhydrous tin(IV) chloride is a Lewis acid. It forms adducts with ammonia, organophosphines, and other Lewis bases. When mixed with a small amount of water a semi-solid crystalline mass of the pentahydrate, SnCl4.5H2O is formed. This solid was formerly known as butter of tin. With hydrochloric acid the complex [SnCl6]2− is formed making the so-called hexachlorostannic acid.[1]
Precursor to organotin compounds
Anhydrous tin(IV) chloride is a major precursor in organotin chemistry. Upon treatment with Grignard reagents, tin(IV) chloride give tetraalkyltin compounds:[5]
- SnCl4 + 4 RMgCl → SnR4 + 4 MgCl2
Anhydrous tin(IV) chloride reacts with tetraorganotin compounds in redistribution reactions:
- SnCl4 + SnR4 → 2 SnCl2R2
These organotin halides are more useful than the tetraorganotin derivatives.
Applications in organic synthesis
Although a specialized application, SnCl4 is used in Friedel-Crafts reactions as a Lewis acidic catalyst for alkylation and cyclisation.[1] Stannic chloride is used in chemical reactions with fuming (90%) nitric acid for the selective nitration of activated aromatic rings in the presence of inactivated ones.[6]
Uses
The main application of SnCl4 is as a precursor to organotin compounds, which are used as catalysts and polymer stabilizers.[7] It can be used in a sol-gel process to prepare SnO2 coatings (for example for toughening glass); nanocrystals of SnO2 can be produced by refinements of this method.
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 substituted for by a mixture of silicon tetrachloride and titanium tetrachloride near the end of the War due to shortages of tin.[8]
References
- ↑ 1.0 1.1 1.2 Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5
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- ↑ G. G. Graf "Tin, Tin Alloys, and Tin Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2005 Wiley-VCH, Weinheim. doi:10.1002/14356007.a27_049
- ↑ Lua error in package.lua at line 80: module 'strict' not found..
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- Chlorides
- Tin compounds
- Metal halides