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| IUPAC name | Tin tetrachloride Tin(IV) chloride |
| Other names | Stannic chloride |
| Identifiers | |
| CAS number | [7646-78-8] |
| Properties | |
| Molecular formula | SnCl4 |
| Molar mass | 260.50 g/mol |
| Appearance | fuming liquid |
| Density | 2.226 g/ml, liquid |
| Melting point |
-33 °C |
| Boiling point |
114.1 °C |
| Solubility in water | Decomposes |
| Viscosity | ? cP at ? °C |
| Hazards | |
| EU classification | Corrosive (C) |
| R-phrases | R34, R52/53 |
| S-phrases | S1/2, S7/8, S26, S45, S61 |
| Related compounds | |
| Other anions | Tin(IV) fluoride Tin(IV) bromide Tin(IV) iodide |
| Other cations | Tin(II) chloride Germanium tetrachloride Lead(IV) chloride |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox references |
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Tin(IV) chloride, also known as tin tetrachloride or stannic chloride is a chemical compound with the formula SnCl4. At room temperature it is a colourless liquid, which fumes on contact with air, giving a stinging odour. It was first discovered by A Libavius (1550-1616) and was known as "spiritus fumans libavii" .[1]
Contents |
Preparation
It is prepared from reaction of chlorine gas with elemental tin.
Reactions
When mixed with a small amount of water a semi-solid crystalline mass of the pentahydrate, SnCl4.5H2O is formed.[1] This was formerly known as butter of tin[1]. This compound has been shown to be best described as [SnCl4(H2O)2.3H2O, consisting of cis-[SnCl4(H2O)2 units linked in chains with three hydrate water molecules.[2]
With hydrochloric acid the complex [SnCl62− is formed making the so-called hexachlorostannic acid.[1]
Anhydrous tin(IV) chloride is a strong Lewis acid and complexes with e.g. ammonia, phosphine and phosphorus pentachloride are known.[1] SnCl4 is used in Friedel-Crafts reactions as a catalyst for homogeneous alkylation and cyclisation.[1]
With Grignard reagents tetraalkyltin compounds can be prepared:[3]
- SnCl4 + RMgCl → SnR4
Uses
Stannic chloride was used as a chemical weapon in World War I. It is also used in the glass container industry for making an external coating containing tin(IV) oxide which toughens the glass. It is a starting material for organotin compounds.
Stannic chloride is used in chemical reactions with fuming (90%) nitric acid for the selective nitration of activated aromatic rings in the presence of unactivated ones.[4]
References
- ^ a b c d e f Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0123526515
- ^ Structures of di-μ-hydroxobis[aquatrichlorotin(IV)]-1,4-dioxane(1/3), di-μ-hydroxobis[aquatrichlorotin(IV)]-1,8-epoxy-p-menthane(1/4), di-m-hydroxobis[aquatribromotin(IV)]-1,8-epoxy-p-menthane(1/4), di-μ-hydroxobis[aquatrichlorotin(IV)], and cis-diaquatetrachlorotin(IV) , Journal of the Chemical Society, Dalton Transactions: Inorganic Chemistry (1972-1999) (1980), (6), 949-53
- ^ Greenwood, Norman N.; Earnshaw, A. (1997). Chemistry of the Elements, 2nd Edition, Oxford: Butterworth-Heinemann. ISBN 0-7506-3365-4.
- ^ Thurston, D. E. et al. (1990). Synthesis 81–84.
External links
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- This page was last modified on 27 July 2008, at 11:38.
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