Lithium bis(trimethylsilyl)amide

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Lithium bis(trimethylsilyl)amide
Li-HMDS.svg
Monomer (does not exist)
Cyclic Trimer of Lithium bis(trimethylsilyl)amide Structural formula V1.svg
Cyclic trimer
The real "Li N(Sitms2 )2".png
Names
Preferred IUPAC name
Lithium 1,1,1-trimethyl-N-(trimethylsilyl)silanaminide
Other names
Lithium hexamethyldisilazide
Hexamethyldisilazane lithium salt
Identifiers
  • 4039-32-1 checkY
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.021.569 Edit this at Wikidata
UNII
Properties
C6H18LiNSi2
Molar mass 167.326 g/mol
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
THF, hexane, toluene
Acidity (pKa) 26
Hazards
Main hazards flammable, corrosive
Related compounds
Related compounds
 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).
☒N  (what is checkY☒N ?)
Infobox references

Lithium bis(trimethylsilyl)amide is a lithiated organosilicon compound with the formula LiN(SiMe3)2. It is commonly abbreviated as LiHMDS (lithium hexamethyldisilazide - a reference to its conjugate acid HMDS) and is primarily used as a strong non-nucleophilic base and as a ligand. Like many lithium reagents, it has a tendency to aggregate and will form a cyclic trimer in the absence of coordinating species.

Preparation[]

LiHMDS is commercially available, but it can also be prepared by the deprotonation of bis(trimethylsilyl)amine with n-butyllithium.[1] This reaction can be performed in situ.[2]

HN(SiMe3)2 + C4H9Li → LiN(SiMe3)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 non-nucleophilic base.[3] Its conjugate acid has a pKa of ~26,[4] making it is less basic than other lithium bases, such as LDA (pKa of conjugate acid ~36), but it is more sterically hindered and hence less nucleophilic. It can be used to form various organolithium compounds, including acetylides[3] or lithium enolates.[2]

LiHMDS EnolateFormation.png

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 [(Me3Si)2N]2S as a precursor with pre-formed S–N bonds. [(Me3Si)2N]2S is prepared by the reaction of lithium bis(trimethylsilyl)amide and sulfur dichloride (SCl2).

2 [(CH3)3Si]2NLi + SCl2 → [((CH3)3Si)2N]2S + 2 LiCl

The [((CH3)3Si)2N]2S reacts with the combination of SCl2 and sulfuryl chloride (SO2Cl2) to form S4N4, trimethylsilyl chloride, and sulfur dioxide:[5]

2[((CH3)3Si)2N]2S + 2SCl2 + 2SO2Cl2 → S4N4 + 8 (CH3)3SiCl + 2SO2

As a ligand[]

LiHMDS can react with a wide range of metal halides, by a salt metathesis reaction, to give metal bis(trimethylsilyl)amides.

MXx + x Li(hmds) → M(hmds)x + x LiX
(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 nonpolar organic solvents, this often makes them more reactive than the corresponding metal halides, which can be difficult to solubilise. The steric bulk of the ligands causes their complexes to be discrete and monomeric; further increasing their reactivity. Having a built-in base, these compounds conveniently react with protic ligand precursors to give other metal complexes and hence are important precursors to more complex coordination compounds.[6]

Niche uses[]

LiHMDS is volatile and has been discussed for use for atomic layer deposition of lithium compounds.[7]

Structure[]

Like many organolithium reagents, lithium bis(trimethylsilyl)amide can form aggregates in solution. The extent of aggregation depends on the solvent. In coordinating solvents, such as ethers[8] and amines,[9] the monomer and dimer are prevalent. In the monomeric and dimeric state, one or two solvent molecules bind to lithium centers. With ammonia as donor base lithium bis(trimethylsilyl)amide forms a trisolvated monomer that is stabilized by intermolecular hydrogen bonds.[10][11] In noncoordinating solvents, such as aromatics or pentane, the complex oligomers predominate, including the trimer.[9] In the solid state structure is trimeric.[12]

LiHMDS aggregation.png
LiHMDS-tmeda complex.png
LiHMDS adduct with TMEDA 		Li2(Sitms2)2(THF)2.png
THF solvated dimer: (LiHMDS)2•THF2 		The real "Li N(Sitms2 )2".png
Trimer, solvent free: (LiHMDS)3

See also[]

References[]

  1. ^ Amonoo-Neizer, E. H.; Shaw, R. A.; Skovlin, D. O.; Smith, B. C. (1966). "Lithium Bis(Trimethylsilyl)Amide and Tris(Trimethylsilyl)Amine". Inorg. Synth. Inorganic Syntheses. 8: 19–22. doi:10.1002/9780470132395.ch6. ISBN 978-0-470-13239-5.
  2. ^ Jump up to: 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.; Collective Volume, 9, p. 197
  3. ^ Jump up to: a b Wu, George; Huang, Mingsheng (July 2006). "Organolithium Reagents in Pharmaceutical Asymmetric Processes". Chemical Reviews. 106 (7): 2596–2616. doi:10.1021/cr040694k. PMID 16836294.
  4. ^ Fraser, Robert R.; Mansour, Tarek S.; Savard, Sylvain (August 1985). "Acidity measurements on pyridines in tetrahydrofuran using lithiated silylamines". The Journal of Organic Chemistry. 50 (17): 3232–3234. doi:10.1021/jo00217a050.
  5. ^ Maaninen, A.; Shvari, J.; Laitinen, R. S.; Chivers, T (2002). Coucouvanis, Dimitri (ed.). "Compounds of General Interest". Inorganic Syntheses. New York: John Wiley & Sons, Inc. 33: 196–199. doi:10.1002/0471224502.ch4.
  6. ^ Michael Lappert, Andrey Protchenko, Philip Power, Alexandra Seeber (2009). Metal Amide Chemistry. Weinheim: Wiley-VCH. doi:10.1002/9780470740385. ISBN 0-470-72184-7.CS1 maint: multiple names: authors list (link)
  7. ^ Hämäläinen, Jani; Holopainen, Jani; Munnik, Frans; Hatanpää, Timo; Heikkilä, Mikko; Ritala, Mikko; Leskelä, Markku (2012). "Lithium Phosphate Thin Films Grown by Atomic Layer Deposition". Journal of the Electrochemical Society. 159 (3): A259–A263. doi:10.1149/2.052203jes.
  8. ^ Lucht, Brett L.; Collum, David B. (1995). "Ethereal Solvation of Lithium Hexamethyldisilazide: Unexpected Relationships of Solvation Number, Solvation Energy, and Aggregation State". Journal of the American Chemical Society. 117 (39): 9863–9874. doi:10.1021/ja00144a012.
  9. ^ Jump up to: a b Lucht, Brett L.; Collum, David B. (1996). "Lithium Ion Solvation: Amine and Unsaturated Hydrocarbon Solvates of Lithium Hexamethyldisilazide (LiHMDS)". Journal of the American Chemical Society. 118 (9): 2217–2225. doi:10.1021/ja953029p.
  10. ^ Neufeld, R.; Michel, R.; Herbst-Irmer, R.; Schöne, R.; Stalke, D. (2016). "Introducing a Hydrogen-Bond Donor into a Weakly Nucleophilic Brønsted Base: Alkali Metal Hexamethyldisilazides (MHMDS, M = Li, Na, K, Rb and Cs) with Ammonia". Chem. Eur. J. 22: 12340–12346. doi:10.1002/chem.201600833. PMID 27457218.
  11. ^ 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.
  12. ^ Rogers, Robin D.; Atwood, Jerry L.; Grüning, Rainer (1978). "The crystal structure of N-lithiohexamethyldisilazane, [LiN(SiMe3)2]3". J. Organomet. Chem. 157 (2): 229–237. doi:10.1016/S0022-328X(00)92291-5.
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