Lithium bis(trimethylsilyl)amide
![]() Monomer (does not exist)
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![]() Cyclic trimer
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Names | |
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Preferred IUPAC name
Lithium 1,1,1-trimethyl-N-(trimethylsilyl)silanaminide | |
Other names
Lithium hexamethyldisilazide
Hexamethyldisilazane lithium salt | |
Identifiers | |
3D model (
JSmol ) |
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ChemSpider | |
ECHA InfoCard
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100.021.569 |
PubChem CID
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UNII | |
CompTox Dashboard (EPA)
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Properties | |
LiN(Si(CH3)3)2 | |
Molar mass | 167.33 g·mol−1 |
Appearance | White solid |
Density | 0.86 g/cm3 at 25 °C |
Melting point | 71 to 72 °C (160 to 162 °F; 344 to 345 K) |
Boiling point | 80 to 84 °C (176 to 183 °F; 353 to 357 K) (0.001 mm Hg) |
decomposes | |
Solubility | Most aprotic solvents |
Acidity (pKa) | 26 |
Hazards | |
Occupational safety and health (OHS/OSH): | |
Main hazards
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flammable, corrosive |
Related compounds | |
Related compounds
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Sodium bis(trimethylsilyl)amide Potassium bis(trimethylsilyl)amide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Lithium bis(trimethylsilyl)amide is a lithiated
Preparation
LiHMDS is commercially available, but it can also be prepared by the deprotonation of
- HN(Si(CH3)3)2 + C4H9Li → LiN(Si(CH3)3)2 + C4H10
Once formed, the compound can be purified by sublimation or distillation.
Reactions and applications
As a base
LiHMDS is often used in organic chemistry as a strong
![](http://upload.wikimedia.org/wikipedia/commons/thumb/3/34/LiHMDS_EnolateFormation.png/500px-LiHMDS_EnolateFormation.png)
where Me = CH3. As such, it finds use in a range of coupling reactions, particularly carbon-carbon bond forming reactions such as the Fráter–Seebach alkylation and mixed Claisen condensations.
An alternative synthesis of tetrasulfur tetranitride entails the use of S(N(Si(CH3)3)2)2 as a precursor with pre-formed S–N bonds. S(N(Si(CH3)3)2)2 is prepared by the reaction of lithium bis(trimethylsilyl)amide and sulfur dichloride (SCl2).
- 2 LiN(Si(CH3)3)2 + SCl2 → S(N(Si(CH3)3)2)2 + 2 LiCl
The S(N(Si(CH3)3)2)2 reacts with the combination of SCl2 and sulfuryl chloride (SO2Cl2) to form S4N4, trimethylsilyl chloride, and sulfur dioxide:[5]
- 2 S(N(Si(CH3)3)2)2 + 2 SCl2 + 2 SO2Cl2 → S4N4 + 8 (CH3)3SiCl + 2 SO2
As a ligand
Li(HMDS) can react with a wide range of metal halides, by a salt metathesis reaction, to give metal bis(trimethylsilyl)amides.
- MXn + n Li(HMDS) → M(HMDS)n + n LiX
where X = Cl, Br, I and sometimes F
Metal bis(trimethylsilyl)amide complexes are lipophilic due to the ligand and hence are soluble in a range of
Niche uses
LiHMDS is volatile and has been discussed for use for atomic layer deposition of lithium compounds.[7]
Structure
Like many
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TMEDA
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THF solvated dimer: [(LiHMDS)2(THF)2]
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![]() Trimer, solvent free: [(LiHMDS)3] |
See also
References
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- ^ a b Danheiser, R. L.; Miller, R. F.; Brisbois, R. G. (1990). "Detrifluoroacetylative Diazo Group Transfer: (E)-1-Diazo-4-phenyl-3-buten-2-one". Organic Syntheses. 73: 134; Collected Volumes, vol. 9, p. 197.
- ^ PMID 16836294.
- .
- ISBN 9780471208259.
- ISBN 978-0-470-72184-1.)
{{cite book}}
: CS1 maint: multiple names: authors list (link - .
- .
- ^ .
- PMID 27457218.
- ^ Neufeld, R.: DOSY External Calibration Curve Molecular Weight Determination as a Valuable Methodology in Characterizing Reactive Intermediates in Solution. In: eDiss, Georg-August-Universität Göttingen. 2016.
- .