View source for Organolithium reagent

{{short description|Chemical compounds containing C–Li bonds}}

In [[organometallic chemistry]], '''organolithium reagents''' are [[chemical compound]]s that contain [[carbon]]–[[lithium]] (C–Li) [[Chemical bond|bonds]]. These reagents are important in [[organic synthesis]], and are frequently used to transfer the organic group or the lithium atom to the substrates in synthetic steps, through [[nucleophilic addition]] or simple [[deprotonation]].<ref name=analytical>
{{cite book| last = Zabicky | first = Jacob | chapter = Analytical aspects of organolithium compounds| title = PATAI'S Chemistry of Functional Groups.| publisher = John Wiley & Sons, Ltd | year = 2009| isbn = 9780470682531 | doi =  10.1002/9780470682531.pat0304}}</ref> Organolithium reagents are used in industry as an initiator for [[anionic polymerization]], which leads to the production of various [[elastomers]]. They have also been applied in [[asymmetric synthesis]] in the pharmaceutical industry.<ref name=orglipharm>
{{cite journal| title = Organolithium Reagents in Pharmaceutical Asymmetric Processes| author = Wu, G.
|author2=Huang, M.| journal = Chem. Rev.| year = 2006| volume = 106| issue = 7
| pages = 2596–2616| doi = 10.1021/cr040694k| pmid=16836294}}</ref> Due to the large difference in [[electronegativity]] between the carbon atom and the lithium atom, the C−Li bond is highly [[ionization|ionic]]. Owing to the polar nature of the C−Li bond, organolithium reagents are good [[nucleophile]]s and strong bases. For laboratory organic synthesis, many organolithium reagents are commercially available in solution form. These reagents are highly reactive, and are sometimes [[pyrophoricity|pyrophoric]]. [[File:Glasbottles containing Butyllithium, Buli.jpg|thumb|right|Glass bottles containing butyllithium]]
[[File:Sec-butyllithium-2D-skeletal.png|thumb|right|230px|A ''sec''-butyllithium aggregate in which each of the four ''sec''-butyl groups is associated with one face of the tetrahedron formed from four lithium atoms]]

==History and development==
Studies of organolithium reagents began in the 1930s and were pioneered by [[Karl Ziegler]], [[Georg Wittig]], and [[Henry Gilman]]. In comparison with [[Grignard reaction|Grignard (magnesium) reagents]], organolithium reagents can often perform the same reactions with increased rates and higher yields, such as in the case of [[metalation]].<ref name="Eisch2002">{{cite journal|last1=Eisch|first1=John J.|title=Henry Gilman: American Pioneer in the Rise of Organometallic Chemistry in Modern Science and Technology†|journal=Organometallics|volume=21|issue=25|year=2002|pages=5439–5463|issn=0276-7333|doi=10.1021/om0109408}}</ref>
Since then, organolithium reagents have overtaken Grignard reagents in common usage.<ref name =chemorgli>{{cite book|editor = Rappoport, Z. |editor2=Marek, I.|title = The Chemistry of Organolithium Compounds (2 parts)|publisher = John Wiley & Sons, Ltd |year = 2004|isbn = 978-0-470-84339-0}}</ref>

== Structure ==
Although simple alkyllithium species are often represented as monomer RLi, they exist as aggregates ([[oligomer]]s) or polymers.<ref name=leadstructure /> 
The degree of aggregation depends on the organic substituent and the presence of other ligands.<ref name=Reich>{{cite journal|last=Reich|first=Hans J.|title=Role of Organolithium Aggregates and Mixed Aggregates in Organolithium Mechanisms|journal=Chemical Reviews|year=2013|volume=113|issue=9|pages=7130–7178|doi=10.1021/cr400187u|pmid=23941648}}</ref><ref name=Strohmann /> These structures have been elucidated by a variety of methods, notably <sup>6</sup>Li, <sup>7</sup>Li, and <sup>13</sup>C [[NMR spectroscopy]] and X-ray diffraction analysis.<ref name="analytical"/> [[Computational chemistry]] supports these assignments.<ref name =leadstructure>{{cite book| last1 = Stey |first1 = Thomas |last2 = Stalke |first2 = Dietmar |chapter = Lead structures in lithium organic chemistry|title = PATAI'S Chemistry of Functional Groups.|publisher = John Wiley & Sons, Ltd |year = 2009|isbn = 9780470682531|doi = 10.1002/9780470682531.pat0298}}</ref>

=== Nature of carbon–lithium bond ===
[[File:Allyllithium.svg|thumb|right|150x100px|Delocalized electron density in allyllithium reagents]] 
The relative [[electronegativity|electronegativities]] of carbon and lithium suggest that the C−Li bond will be highly polar.<ref name=gopakomar>
{{cite book| last1 = Jemmis | first1 = E.D.| last2 = Gopakumar | first2 = G. | chapter = Theoretical studies in organolithium chemistry| title = PATAI'S Chemistry of Functional Groups.| publisher = John Wiley & Sons, Ltd | year = 2009| isbn = 9780470682531 | doi = 10.1002/9780470682531.pat0297}}</ref><ref name=streiwieser>{{cite journal| title = Perspectives on Computational Organic Chemistry| author = Streiwieser, A.| journal = J. Org. Chem.| year = 2009| volume = 74| issue = 12| pages = 4433–4446| doi = 10.1021/jo900497s | pmid = 19518150| pmc = 2728082}}</ref><ref name=bickelhaupt>{{cite journal| title = Covalency in Highly Polar Bonds. Structure and Bonding of Methylalkalimetal Oligomers (CH3M)n (M = Li−Rb; n = 1, 4)| author = Bickelhaupt, F. M.| journal = J. Chem. Theory Comput.| year = 2006| volume = 2| issue = 4| pages = 965–980| doi = 10.1021/ct050333s | pmid = 26633056|display-authors=etal}}</ref>
However, certain organolithium compounds possess properties such as solubility in nonpolar solvents that complicate the issue.
<ref name="gopakomar"/> While most data suggest the C−Li bond to be essentially ionic, there has been debate as to how much [[covalent]] character exists in it.<ref name=streiwieser/><ref name=bickelhaupt/>  One estimate puts the percentage of ionic character of alkyllithium compounds at 80 to 88%.<ref>{{Cite journal|last=Weiss|first=Erwin|date=November 1993|title=Structures of Organo Alkali Metal Complexes and Related Compounds|journal=Angewandte Chemie International Edition in English|language=en|volume=32|issue=11|pages=1501–1523|doi=10.1002/anie.199315013|issn=0570-0833}}</ref>

In allyl lithium compounds, the lithium cation coordinates to the face of the carbon π bond in an η<sup>3</sup> fashion instead of a localized, carbanionic center, thus, allyllithiums are often less aggregated than alkyllithiums.<ref name=Reich /><ref name=Fraenkelallyllithium>
{{cite journal| title = Observation of a Partially Delocalized Allylic Lithium and the Dynamics of Its 1,3 Lithium Sigmatropic Shift| author = Fraenkel, G.|author2=Qiu, Fayang| journal = J. Am. Chem. Soc.| year = 1996| volume = 118| issue = 24| pages = 5828–5829| doi = 10.1021/ja960440j}}</ref> In aryllithium complexes, the lithium cation coordinates to a single carbanion center through a Li−C σ type bond.<ref name=Reich /><ref name=Fraenkel>
{{cite journal| title = The carbon-lithium bond in monomeric arllithium: Dynamics of exchange, relaxation and rotation| author = Fraenkel. G| journal = J. Am. Chem. Soc.| year = 1995| volume = 117| issue = 23| pages = 6300–6307| doi = 10.1021/ja00128a020 |display-authors=etal}}</ref>
{{multiple image| direction = vertical| width = 180 |height = 400| footer = Solid state structures of methyllithium tetramers, ''n-''butyllithium hexamers and polymeric ladder of phenyllithium| image1 = Methyllithium-tetramer-2-3D-balls.png| image2 = Butyllithium-hexamer-from-xtal-3D-balls-A.png| image3 = Phenyllithium-chain-from-xtal-Mercury-3D-balls.png}}

===Solid state structure===
[[File:Building block of alkyllithium aggregates.png|thumb|270px|left|Tetrahedron and octahedron metal cores formed by aggregation of the Li3 triangle - carbanion coordinate complex<ref name=leadstructure />]]

Like other species consisting of polar subunits, organolithium species aggregate.<ref name=Strohmann>{{cite journal|last=Strohmann|first=C|title=Structure Formation Principles and Reactivity of Organolithium Compounds.|journal= Chem. Eur. J.|year=2009|volume=15|issue=14|pages=3320–3334|url=http://onlinelibrary.wiley.com/store/10.1002/chem.200900041/asset/3320_ftp.pdf?v=1&t=hnc3zl4k&s=90cd763c5affe82ca5d8208a75ea074deede3187|doi=10.1002/chem.200900041|pmid=19260001|display-authors=etal}}</ref><ref name=Power>{{cite journal|last=Power|first=P.P|author2=Hope H.|title=Isolation and crystal structures of the halide-free and halide-rich phenyllithium etherate complexes [(PhLi.Et2O)4] and [(PhLi.Et2O)3.LiBr].|journal=Journal of the American Chemical Society|year=1983|volume=105|issue=16|pages=5320–5324|doi=10.1021/ja00354a022}}</ref>
Formation of aggregates is influenced by [[electrostatic]] interactions, the coordination between lithium and surrounding solvent molecules or polar additives, and steric effects.<ref name=Strohmann />

A basic building block toward constructing more complex structures is a carbanionic center interacting with a Li<sub>3</sub> triangle in an η<sup>3</sup>- fashion.<ref name=leadstructure />
In simple alkyllithium reagents, these triangles aggregate to form tetrahedron or octahedron structures. For example, [[methyllithium]], [[ethyllithium]] and [[tert-Butyllithium|''tert''-butyllithium]] all exist in the tetramer [RLi]<sub>4</sub>. Methyllithium exists as tetramers in a [[cubane-type cluster]] in the solid state, with four lithium centers forming a tetrahedron. Each methanide in the tetramer in methyllithium can have [[agostic]] interaction with lithium cations in adjacent tetramers.<ref name=leadstructure /><ref name=Strohmann />
Ethyllithium and ''tert''-butyllithium, on the other hand, do not exhibit this interaction, and are thus soluble in non-polar hydrocarbon solvents. Another class of alkyllithium adopts hexameric structures, such as [[n-butyllithium|''n''-butyllithium]], isopropyllithium, and cyclohexanyllithium.<ref name=leadstructure />

[[File:dimerliamide.jpg|thumb|250px|left|LDA dimer with THF coordinated to Li cations]]

Common lithium amides, e.g. [[lithium bis(trimethylsilyl)amide]] and [[lithium diisopropylamide]], are also subject to aggregation.<ref name="Williard, P. G.; Salvino, J. M. 1993 1–3">{{cite journal|author1=Williard, P. G. |author2=Salvino, J. M. |journal=[[Journal of Organic Chemistry]]|year=1993| volume=58|issue=1|pages=1–3|title=Synthesis, isolation, and structure of an LDA-THF complex |doi=10.1021/jo00053a001}}</ref> Lithium amides adopt polymeric-ladder type structures in non-coordinating solvent in the solid state, and they generally exist as dimers in ethereal solvents. In the presence of strongly donating ligands, tri- or tetrameric lithium centers are formed. 
<ref name=Liamides>{{cite book| last1 = Hilmersson | first1 = Goran| last2 = Granander | first2 = Johan | chapter = Structure and dynamics of chiral lithium amides| title = PATAI'S Chemistry of Functional Groups.| publisher = John Wiley & Sons, Ltd | year = 2009| isbn = 9780470682531 | doi = 10.1002/9780470682531.pat0342}}</ref>
For example, LDA exists primarily as dimers in THF.<ref name="Williard, P. G.; Salvino, J. M. 1993 1–3"/> The structures of common lithium amides, such as lithium diisopropylamide (LDA) and lithium hexamethyldisilazide (LiHMDS) have been extensively studied by Collum and coworkers using [[NMR spectroscopy]].<ref name=Collumamides>{{cite journal| title = Lithium Diisopropylamide: Solution Kinetics and Implications for Organic Synthesis| author = Collum, D.B.| journal = Angew. Chem. Int. Ed. | year = 2007| volume = 49| issue = 17| pages = 3002–3017| doi = 10.1002/anie.200603038 | pmid = 17387670|display-authors=etal}}</ref>
Another important class of reagents is silyllithiums, extensively used in the synthesis of organometallic complexes and polysilane [[dendrimers]].<ref name=Strohmann /><ref name=lithiosilanes>{{cite journal|title=Lithiosilanes and their application to the synthesis of polysilane dendrimers |author=Sekiguchi, Akira.|journal=Coord. Chem. Rev.|year=2000 |volume=210 |pages=11–45 |doi=10.1016/S0010-8545(00)00315-5 |display-authors=etal}}</ref>
In the solid state, in contrast with alkyllithium reagents, most silyllithiums tend to form monomeric structures coordinated with solvent molecules such as THF, and only a few silyllithiums have been characterized as higher aggregates.<ref name=Strohmann />
This difference can arise from the method of preparation of silyllithiums, the steric hindrance caused by the bulky alkyl substituents on silicon, and the less polarized nature of Si−Li bonds. The addition of strongly donating ligands, such as TMEDA and (-)-[[sparteine]], can displace coordinating solvent molecules in silyllithiums.<ref name=Strohmann />

===Solution structure===
It is possible for organolithium reagents adopt structures in solution that differ from the solid state.<ref name=Reich /><ref name=solutionenolate>{{cite journal| title = Solution Structures of Lithium Enolates, Phenolates, Carboxylates, and Alkoxides in the Presence of N,N,N′,N′-Tetramethylethylenediamine: A Prevalence of Cyclic Dimers| author = Collum, D. B.| journal = J. Org. Chem.| year = 2008| volume = 73| issue = 19| pages = 7743–7747| doi = 10.1021/jo801532d | pmid = 18781812|display-authors=etal| pmc = 2636848}}</ref> NMR spectroscopy has emerged as a powerful tool for the studies of organolithium aggregates in solution. For alkyllithium species, C−Li ''J'' coupling can often used to determine the number of lithium interacting with a carbanion center, and whether these interactions are static or dynamic.<ref name=Reich /> Separate NMR signals can also differentiate the presence of multiple aggregates from a common monomeric unit.<ref name=reich103>{{cite journal| title = Aggregation and reactivity of phenyllithium solutions| author = Reich, H. J.| journal = J. Am. Chem. Soc.| year = 1998| volume = 120| issue = 29| pages = 7201–7210| doi = 10.1021/ja980684z |display-authors=etal}}</ref>

Organolithium compounds bind [[Lewis base]]s such as [[tetrahydrofuran]] (THF), [[diethyl ether]] (Et<sub>2</sub>O), tetramethylethylene diamine (TMEDA) or [[hexamethylphosphoramide]] (HMPA).<ref name=leadstructure /> [[Methyllithium]] is a special case: its tetrameric structure is unaffected by ether or even HMPA.<ref name=Strohmann /> On the other hand, THF deaggregates hexameric butyl lithium: the tetramer is the main species, and ΔG for interconversion between tetramer and dimer is around 11 kcal/mol.<ref name=McGarrity>{{cite journal| title = High-field proton NMR study of the aggregation and complexation of n-butyllithium in tetrahydrofuran| author = McGarrity, J. F.|author2=Ogle, C.A.| journal = J. Am. Chem. Soc.| year = 1985| volume = 107| issue = 7| pages = 1805–1810| doi = 10.1021/ja00293a001}}</ref> TMEDA can also chelate to the lithium cations in ''n''-butyllithium and form solvated dimers such as [(TMEDA) LiBu-n)]<sub>2</sub>.<ref name=leadstructure /><ref name = Reich /> Phenyllithium has been shown to exist as a distorted tetramer in the crystallized ether solvate, and as a mixture of dimer and tetramer in ether solution.<ref name =Reich />

{| border="1" class="wikitable"  style="text-align:center; margin-left: auto; margin-right: auto; border: none;"
|+ Solvated alkyllithium aggregate structures<ref name=Reich />
! Alkyl group
! Solvent
! Structure
|-
| rowspan=2 | methyl || THF || tetramer
|-
| ether/HMPA || tetramer
|-
| rowspan=3 | ''n''{{nbh}}butyl || pentane || hexamer
|-
| ether || tetramer
|-
| THF || tetramer-dimer
|-
| ''sec''{{nbh}}butyl || pentane || hexamer-tetramer
|-
| isopropyl || pentane || hexamer-tetramer
|-
| rowspan=2 | ''tert''{{nbh}}butyl || pentane || tetramer
|-
| THF || monomer
|-
| rowspan=2 | phenyl || ether || tetramer-dimer
|-
| ether/HMPA || dimer
|}

===Structure and reactivity===
As the structures of organolithium reagents change according to their chemical environment, so do their reactivity and selectivity.<ref name=Strohmann /><ref name=whatsgoingon>{{cite journal| title = What's going on with these lithium reagents| author = Reich, H. J.| journal = J. Org. Chem.| year = 2012| volume = 77| issue = 13| pages = 5471–5491| doi = 10.1021/jo3005155| pmid = 22594379}}</ref>
One question surrounding the structure-reactivity relationship is whether there exists a correlation between the degree of aggregation and the reactivity of organolithium reagents. It was originally proposed that lower aggregates such as monomers are more reactive in alkyllithiums.<ref name=Strohmann44>
{{cite book| last = Wardell| first = J.L. | chapter = Chapter 2| title = Comprehensive Organometallic Chemistry, Vol. 1| edition = 1st| editor = Wilinson, G. |editor2=Stone, F. G. A. |editor3=Abel, E. W.| publisher = Pergamon| location = New York| year = 1982| isbn = 978-0080406084}}</ref> 
However, reaction pathways in which dimer or other oligomers are the reactive species have also been discovered,<ref name=Strohmann24b>{{cite journal| title = Crystal Structures of n-BuLi Adducts with (R,R)-TMCDA and the Consequences for the Deprotonation of Benzene| author = Strohmann, C.|author2=Gessner, V.H.| journal = J. Am. Chem. Soc.| year = 2008| volume = 130| issue = 35| pages = 11719–11725| doi =  10.1021/ja8017187| pmid=18686951}}</ref> and for lithium amides such as LDA, dimer-based reactions are common.<ref name=Collumldareview>{{cite journal| title = Lithium Diisopropylamide: Solution Kinetics and Implications for Organic Synthesis| author = Collum, D. B.| journal = Angew. Chem. Int. Ed.| year = 2007| volume = 46| issue = 17| pages = 3002–3017| doi = 10.1002/anie.200603038 | pmid = 17387670|display-authors=etal}}</ref> 
A series of solution kinetics studies of LDA-mediated reactions suggest that lower aggregates of enolates do not necessarily lead to higher reactivity.<ref name=Collumamides/>

Also, some Lewis bases increase reactivity of organolithium compounds.<ref name=Chalk>{{cite journal|last=Chalk|first=A.J|author2=Hoogeboom, T.J|title=Ring metalation of toluene by butyllithium in the presence of N,N,N′,N′-tetramethylethylenediamine|journal= J. Organomet. Chem.|year=1968|volume=11|pages=615–618|doi=10.1016/0022-328x(68)80091-9}}</ref>
<ref name=Reich2>{{cite journal|last=Reich|first=H.J|author2=Green, D.P|title=Spectroscopic and Reactivity Studies of Lithium Reagent - HMPA Complexes|journal=Journal of the American Chemical Society|year=1989|volume=111|issue=23|pages=8729–8731|doi=10.1021/ja00205a030}}</ref>
However, whether these additives function as strong chelating ligands, and how the observed increase in reactivity relates to structural changes in aggregates caused by these additives are not always clear.<ref name=Chalk/><ref name=Reich2/>
For example, TMEDA increases rates and efficiencies in many reactions involving organolithium reagents.<ref name =Strohmann /> Toward alkyllithium reagents, TMEDA functions as a donor ligand, reduces the degree of aggregation,<ref name =leadstructure /> and increases the nucleophilicity of these species.<ref name=Williard>{{cite journal|last=Williard|first=P.G|author2=Nichols, M.A|title=Solid-state structures of n-butyllithium-TMEDA, -THF, and -DME complexes|journal=Journal of the American Chemical Society|year=1993|volume=115|issue=4|pages=1568–1572|doi=10.1021/ja00057a050}}</ref>
However, TMEDA does not always function as a donor ligand to lithium cation, especially in the presence of anionic oxygen and nitrogen centers. For example, it only weakly interacts with LDA and LiHMDS even in hydrocarbon solvents with no competing donor ligands.<ref name=Collumtmedagood>{{cite journal| title = Is N,N,N,N-Tetramethylethylenediamine a Good Ligand for Lithium?| author = Collum, D.B.| journal = Acc. Chem. Res.| year = 1992| volume = 25| issue = 10| pages = 448–454| doi = 10.1021/ar00022a003}}</ref>
In imine lithiation, while THF acts as a strong donating ligand to LiHMDS, the weakly coordinating TMEDA readily dissociates from LiHMDS, leading to the formation of LiHMDS dimers that is the more reactive species. Thus, in the case of LiHMDS, TMEDA does not increase reactivity by reducing aggregation state.<ref name=Collumimine>{{cite journal| title = Solvent- and substrate-dependent rates of imine metalations by lithium diisopropylamide: understanding the mechanisms underlying krel| author = Bernstein, M.P.|author2=Collum, D.B.| journal = J. Am. Chem. Soc.| year = 1993| volume = 115| issue = 18| pages = 8008–8010| doi = 10.1021/ja00071a011}}</ref> Also, as opposed to simple alkyllithium compounds, TMEDA does not deaggregate lithio-acetophenolate in THF solution.<ref name=Reich /><ref name=Seebach>{{cite journal|last=Seebach|first=D|title=Structure and Reactivity of Lithium Enolates. From Pinacolone to Selective C-Alkylations of Peptides. Difficulties and Opportunities Afforded by Complex Structures.|journal=Angew. Chem. Int. Ed. |year=1988|volume=27|issue=12|pages=1624–1654|url=http://onlinelibrary.wiley.com/store/10.1002/anie.198816241/asset/198816241_ftp.pdf?v=1&t=hnc87p5u&s=0a5c03a2a79fd94ea5461e768687e4b5fc7d4f3b|doi=10.1002/anie.198816241}}</ref>
The addition of HMPA to lithium amides such as LiHMDS and LDA often results in a mixture of dimer/monomer aggregates in THF. However, the ratio of dimer/monomer species does not change with increased concentration of HMPA, thus, the observed increase in reactivity is not the result of deaggregation. The mechanism of how these additives increase reactivity is still being researched.<ref name=whatsgoingon />

== Reactivity and applications==
The C−Li bond in organolithium reagents is highly polarized. As a result, the carbon attracts most of the [[electron density]] in the bond and resembles a carbanion. Thus, organolithium reagents are strongly basic and nucleophilic. Some of the most common applications of organolithium reagents in synthesis include their use as nucleophiles, strong bases for deprotonation, initiator for polymerization, and starting material for the preparation of other organometallic compounds.

===As nucleophile===

====Carbolithiation reactions====
As nucleophiles, organolithium reagents undergo carbolithiation reactions, whereby the carbon-lithium bond adds across a carbon''–''carbon double or triple bond, forming new organolithium species.<ref name=Intracarbolithiation>{{cite book| last1 = Fananas | first1 = Francisco | last2 = Sanz | first2 = Roberto| chapter = Intramolecular carbolithiation reactions| title = PATAI'S Chemistry of Functional Groups.| publisher = John Wiley & Sons, Ltd | year = 2009| isbn = 9780470682531 | doi = 10.1002/9780470682531.pat0341}}</ref> This reaction is the most widely employed reaction of organolithium compounds. Carbolithiation is key in anionic polymerization processes, and [[n-butyllithium|''n''-butyllithium]] is used as a catalyst to initiate the polymerization of [[styrene]], butadiene, or isoprene or mixtures thereof.<ref name=Hsieh>Heinz-Dieter Brandt, Wolfgang Nentwig1, Nicola Rooney, Ronald T. LaFlair, Ute U. Wolf, John Duffy, Judit E. Puskas, Gabor Kaszas, Mark Drewitt, Stephan Glander "Rubber, 5. Solution Rubbers" in Ullmann's Encyclopedia of Industrial Chemistry, 2011, Wiley-VCH, Weinheim. {{doi|10.1002/14356007.o23_o02}}</ref><ref name=anionicpolymer>
{{cite book| last1 = Baskaran | first1 = D.| last2 = Müller | first2 = A.H.| chapter = Anionic Vinyl Polymerization| title = Controlled and living polymerizations: From mechanisms to applications| publisher = Wiley-VCH Verlag GmbH & Co. KGaA| location = Weinheim, Germany| year = 2010| doi = 10.1002/9783527629091.ch1| isbn = 9783527629091}}</ref>

:[[File:Anionic polymerization of styrene initiated by sec-BuLi.png|450px|Anionic polymerization of styrene initiated by ''sec''-butyllithium|center]]

Another application that takes advantage of this reactivity is the formation of carbocyclic and heterocyclic compounds by [[Intramolecular reaction|intramolecular]] carbolithiation.<ref name=Intracarbolithiation /> As a form of anionic cyclization, intramolecular carbolithiation reactions offer several advantages over [[radical cyclization]]. First, it is possible for the product cyclic organolithium species to react with electrophiles, whereas it is often difficult to trap a radical intermediate of the corresponding structure. Secondly, anionic cyclizations are often more regio- and stereospecific than radical cyclization, particularly in the case of 5-hexenyllithiums. Intramolecular carbolithiation allows addition of the alkyl-, [[vinyllithium]] to triple bonds and mono-alkyl substituted double bonds. Aryllithiums can also undergo addition if a 5-membered ring is formed. The limitations of intramolecular carbolithiation include difficulty of forming 3 or 4-membered rings, as the intermediate cyclic organolithium species often tend to undergo ring-openings.<ref name=Intracarbolithiation /> Below is an example of intramolecular carbolithiation reaction. The lithium species derived from the lithium–halogen exchange cyclized to form the vinyllithium through 5-exo-trig ring closure. The vinyllithium species further reacts with electrophiles and produce functionalized cyclopentylidene compounds.<ref name=intra18>{{cite journal| title = Preparation and facile cyclization of 5-alkyn-1-yllithiums| author = Bailey, W.F.| journal = Tetrahedron Lett.| year = 1989| volume = 30| issue = 30| pages = 3901–3904| doi = 10.1016/S0040-4039(00)99279-7 |display-authors=etal}}</ref>

:[[File:Intramolecular carbolithiation'.png|470px|A sample stereoselective intramolecular carbolithiation reaction|center]]

====Addition to carbonyl compounds====
Nucleophilic organolithium reagents can add to electrophilic carbonyl double bonds to form carbon''–''carbon bonds. They can react with [[aldehydes]] and [[ketones]] to produce [[alcohols]]. The addition proceeds mainly via polar addition, in which the nucleophilic organolithium species attacks from the equatorial direction, and produces the axial alcohol.<ref name=Carey>{{cite book| last = Carey | first = Francis A. | chapter = Organometallic compounds of Group I and II metals| title = Advanced Organic Chemistry: Reaction and Synthesis Pt. B| publisher = Springer| edition = Kindle| year = 2007| isbn = 978-0-387-44899-2}}</ref> Addition of lithium salts such as LiClO<sub>4</sub> can improve the stereoselectivity of the reaction.<ref name=Ashby>{{cite journal|last=Ashby|first=E.C.|author2=Noding, S.R.|title=The effects of added salts on the stereoselectivity and rate of organometallic compound addition to ketones|journal=J. Org. Chem.|year=1979|volume=44|issue=24|pages=4371–4377|doi=10.1021/jo01338a026}}</ref>

:[[File:LiClO4 increase selectivity.png|500px|center|LiClO4 increase selectivity of t BuLi]]

When the ketone is sterically hindered, using Grignard reagents often leads to reduction of the carbonyl group instead of addition.<ref name=Carey /> However, alkyllithium reagents are less likely to reduce the ketone, and may be used to synthesize substituted alcohols.<ref name=Yamatakaddorgli>{{cite book| last = Yamataka | first = Hiroshi | chapter = Addition of organolithium reagents to double bonds| title = PATAI'S Chemistry of Functional Groups.| publisher = John Wiley & Sons, Ltd | year = 2009| isbn = 9780470682531 | doi =  10.1002/9780470682531.pat0310}}</ref> Below is an example of ethyllithium addition to adamantone to produce tertiary alcohol.<ref name=adamantone>{{cite journal| title = Über adamantan und dessen derivate IX. In 2-stellung substituierte derivate| author = Landa, S.| journal = Collection of Czechoslovak Chemical Communications| year = 1967| volume = 72| issue = 2| pages = 570–575| doi = 10.1135/cccc19670570 |display-authors=etal}}</ref>

:[[File:Li add to adamantone.png|350px|center|Li add to adamantone]]

Organolithium reagents are also better than Grignard reagents in their ability to react with carboxylic acids to form ketones.<ref name=Carey /> This reaction can be optimized by carefully controlling the amount of organolithium reagent addition, or using trimethylsilyl chloride to quench excess lithium reagent.<ref name=carey114>{{cite journal| title = Preparation of methyl ketones by the sequential treatment of carboxylic acids with methyllithium and chlorotrimethylsilane| author = Rubottom, G.M.|author2=Kim, C| journal = J. Org. Chem.| year = 1983| volume = 48| issue = 9| pages = 1550–1552| doi =  10.1021/jo00157a038}}</ref> A more common way to synthesize ketones is through the addition of organolithium reagents to [[Weinreb amide]]s (''N''-methoxy-''N''-methyl amides). This reaction provides ketones when the organolithium reagents is used in excess, due to chelation of the lithium ion between the ''N''-methoxy oxygen and the carbonyl oxygen, which forms a tetrahedral intermediate that collapses upon acidic work up.<ref name=weinreb>{{cite journal| title = A One-Pot Synthesis of Ketones and Aldehydes from Carbon Dioxide and Organolithium Compounds | author = Zadel, G.|author2=Breitmaier, E.| journal = Angew. Chem. Int. Ed.| year = 1992| volume = 31| issue = 8| pages = 1035–1036| doi = 10.1002/anie.199210351}}</ref>

:[[File:Li add to weinreb.png|450px|center|Li add to weinreb]]

Organolithium reagents also react with [[carbon dioxide]] to form, after workup, [[carboxylic acids]].<ref name=liaddtocbx>{{cite journal| title = Methoxymethyl ethers. An activating group for rapid and regioselective metalation| author = Ronald, R.C.| journal = Tetrahedron Lett.| year = 1975| volume = 16| issue = 46| pages = 3973–3974| doi = 10.1016/S0040-4039(00)91212-7}}</ref>

In the case of [[enone]] substrates, where two sites of nucleophilic addition are possible (1,2 addition to the carbonyl carbon or 1,4 [[conjugate addition]] to the β carbon), most highly reactive organolithium species favor the 1,2 addition, however, there are several ways to propel organolithium reagents to undergo conjugate addition. First, since the 1,4 adduct is the likely to be the more thermodynamically favorable species, conjugate addition can be achieved through equilibration (isomerization of the two product), especially when the lithium nucleophile is weak and 1,2 addition is reversible. Secondly, adding donor ligands to the reaction forms heteroatom-stabilized lithium species which favors 1,4 conjugate addition. In one example, addition of low-level of HMPA to the solvent favors the 1,4 addition. In the absence of donor ligand, lithium cation is closely coordinated to the oxygen atom, however, when the lithium cation is solvated by HMPA, the coordination between carbonyl oxygen and lithium ion is weakened. This method generally cannot be used to affect the regioselectivity of alkyl- and aryllithium reagents.<ref name=14conjugate>{{cite journal| title = Michael addition of organolithium compounds. A Review| author = Hunt, D.A.| journal = Org. Prep. Proc. Int.| year = 1989| volume = 21| issue = 6| pages = 705–749| doi = 10.1080/00304948909356219}}</ref><ref name=12vs14>{{cite journal| title = Regioselectivity of Addition of Organolithium Reagents to Enones: The Role of HMPA| author = Reich, H. J.|author2=Sikorski, W. H.| journal = J. Org. Chem.| year = 1999| volume = 64| issue = 1| pages = 14–15| doi = 10.1021/jo981765g| pmid = 11674078}}</ref>

:[[File:1,4vs1,2_addition1.svg|center|480px|1,4vs1,2 addition]]

Organolithium reagents can also perform enantioselective nucleophilic addition to carbonyl and its derivatives, often in the presence of chiral ligands. This reactivity is widely applied in the industrial syntheses of pharmaceutical compounds. An example is the Merck and Dupont synthesis of [[Efavirenz]], a potent [[HIV]] reverse transcriptase inhibitor. Lithium acetylide is added to a prochiral ketone to yield a chiral alcohol product. The structure of the active reaction intermediate was determined by NMR spectroscopy studies in the solution state and X-ray crystallography of the solid state to be a cubic 2:2 tetramer.<ref name=MerckDupont>{{cite journal| title = NMR Spectroscopic Investigations of Mixed Aggregates Underlying Highly Enantioselective 1,2-Additions of Lithium Cyclopropylacetylide to Quinazolinones| author = Collum, D.B.| journal = J. Am. Chem. Soc.| year = 2001| volume = 123| issue = 37| pages = 9135–9143| doi = 10.1021/ja0105616 | pmid = 11552822|display-authors=etal}}</ref>

:[[File:Merck synthesis of Efavirenz.png|center|700px|Merck synthesis of Efavirenz]]

====S<sub>N</sub>2 type reactions====
Organolithium reagents can serve as nucleophiles and carry out S<sub>N</sub>2 type reactions with alkyl or allylic halides.<ref name=inversionSn2>{{cite journal| title = Stereospecific coupling reactions between organolithium reagents and secondary halides| author = Sommmer, L.H.|author2=Korte, W. D.| journal = J. Org. Chem.| year = 1970| volume = 35| pages = 22–25| doi = 10.1021/jo00826a006}}</ref>
Although they are considered more reactive than Grignard reagents in alkylation, their use is still limited due to competing side reactions such as radical reactions or metal''–''halogen exchange. Most organolithium reagents used in alkylations are more stabilized, less basic, and less aggregated, such as heteroatom stabilized, aryl- or allyllithium reagents.<ref name=Reich /> HMPA has been shown to increase reaction rate and product yields, and the reactivity of aryllithium reagents is often enhanced by the addition of potassium alkoxides.<ref name=Carey /> Organolithium reagents can also carry out nucleophilic attacks with [[epoxides]] to form alcohols.

:[[File:SN2 inversion with benzyllithium.png|550px|center|SN2 inversion with benzyllithium]]

===As base===
Organolithium reagents provide a wide range of [[basicity]]. [[tert-Butyllithium|''tert''-Butyllithium]], with three weakly electron donating alkyl groups, is the strongest base commercially available ([[pKa]] = 53).  As a result, the acidic protons on −OH, −NH and −SH are often protected in the presence of organolithium reagents. Some commonly used lithium bases are alkyllithium species such as [[n-butyllithium|''n''-butyllithium]] and lithium dialkylamides (LiNR<sub>2</sub>). Reagents with bulky R groups such as lithium diisopropylamide (LDA) and lithium bis(trimethylsilyl)amide (LiHMDS) are often sterically hindered for nucleophilic addition, and are thus more selective toward deprotonation. Lithium dialkylamides (LiNR<sub>2</sub>) are widely used in [[enolate]] formation and [[aldol]] reaction.<ref name=Reich3 /> The reactivity and selectivity of these bases are also influenced by solvents and other counter ions.

====Metalation====
Metalation with organolithium reagents, also known as '''lithiation''' or lithium-hydrogen exchange, is achieved when an organolithium reagent, most commonly an alkyllithium, abstracts a proton and forms a new organolithium species. 
{{NumBlk|:|<chem title="Lithium hydrogen exchange">R-H + R'Li -> RLi + R'H</chem>|{{EquationRef|1}}}}

Common metalation reagents are the butyllithiums. ''tert''-Butyllithium and ''sec''-butyllithium are generally more reactive and have better selectivity than ''n''-butyllithium, however, they are also more expensive and difficult to handle.<ref name=Reich3 /> Metalation is a common way of preparing versatile organolithium reagents. The position of metalation is mostly controlled by the [[acidity]] of the C-H bond. Lithiation often occurs at a position α to electron withdrawing groups, since they are good at stabilizing the electron-density of the anion. Directing groups on aromatic compounds and [[heterocyclic compound|heterocycles]] provide regioselective sites of metalation; directed ortho metalation is an important class of metalation reactions. Metalated sulfones, acyl groups and α-metalated amides are important intermediates in chemistry synthesis. Metalation of allyl ether with alkyllithium or LDA forms an anion α to the oxygen, and can proceed to [[2,3-Wittig rearrangement]]. Addition of donor ligands such as TMEDA and HMPA can increase metalation rate and broaden substrate scope.<ref name=Leroux>''The Preparation of Organolithium Reagents and Intermediates'' Leroux.F., Schlosser. M., Zohar. E., Marek. I., Wiley, New York. 2004. {{ISBN|978-0-470-84339-0}}</ref> [[Chiral]] organolithium reagents can be accessed through asymmetric metalation.<ref name=asymmetalation />

:[[File:Directed ortho metalation2.png|500px|Directed ortho metalation|center]]

[[Directed ortho metalation]] is an important tool in the synthesis of regiospecific substituted [[aromatic]] compounds. This approach to lithiation and subsequent quenching of the intermediate lithium species with electrophile is often better than the electrophilic aromatic substitution due to its high regioselectivity. This reaction proceeds through deprotonation by organolithium reagents at the positions α to the direct metalation group (DMG) on the aromatic ring. The DMG is often a functional group containing a [[heteroatom]] that is Lewis basic, and can coordinate to the Lewis-acidic lithium cation. This generates a complex-induced proximity effect, which directs deprotonation at the α position to form an aryllithium species that can further react with electrophiles. Some of the most effective DMGs are amides, [[carbamate]]s, [[sulfone]]s and [[sulfonamide]]s. They are strong electron-withdrawing groups that increase the acidity of alpha-protons on the aromatic ring. In the presence of two DMGs, metalation often occurs ortho to the stronger directing group, though mixed products are also observed. A number of heterocycles that contain acidic protons can also undergo ortho-metalation. However, for electron-poor heterocycles, lithium amide bases such as LDA are generally used, since alkyllithium has been observed to perform addition to the electron-poor heterocycles rather than deprotonation. In certain transition metal-arene complexes, such as [[ferrocene]], the transition metal attracts electron-density from the arene, thus rendering the aromatic protons more acidic, and ready for ortho-metalation.<ref name=Clayden>{{cite book| last = Clayden| first = Jonathan | chapter = Directed metallization of aromatic compounds| title = PATAI'S Chemistry of Functional Groups.| publisher = John Wiley & Sons, Ltd | year = 2009| isbn = 9780470682531 | doi = 10.1002/9780470682531.pat0306}}</ref>

====Superbases====
{{main|Superbase}}
Addition of potassium alkoxide to alkyllithium greatly increases the basicity of organolithium species.<ref name=Schlosser2>{{cite journal|last=Schlosser|first=M|title=Superbases for organic synthesis|journal=Pure Appl. Chem.|year=1988|volume=60|issue=11|pages=1627–1634|doi=10.1351/pac198860111627|doi-access=free}}</ref> The most common "superbase" can be formed by addition of KOtBu to butyllithium, often abbreviated as "LiCKOR" reagents. These "superbases" are highly reactive and often stereoselective reagents. In the example below, the LiCKOR base generates a stereospecific crotylboronate species through metalation and subsequent lithium-metalloid exchange.<ref name=Roush>{{cite journal| title = Enantioselective synthesis using diisopropyl tartrate modified (E)- and (Z)-crotylboronates: Reactions with achiral aldehydes| author = Roush, W.R.| journal = Tetrahedron Lett.| year = 1988| volume = 29| issue = 44| pages = 5579–5582| doi = 10.1016/S0040-4039(00)80816-3 |display-authors=etal}}</ref>

:[[File:Superbase;.png|center|550px|Superbase]]

=====Asymmetric metalation=====
Enantioenriched organolithium species can be obtained through [[asymmetric synthesis|asymmetric]] metalation of prochiral substrates. Asymmetric induction requires the presence of a [[chiral]] ligand such as (-)-[[sparteine]].<ref name=asymmetalation>{{cite book| last1 = Hoppe | first1 = Dieter | last2 = Christoph | first2 = Guido| chapter = Asymmetric deprotonation with alkyllithium– (−)-sparteine| title = PATAI'S Chemistry of Functional Groups.| publisher = John Wiley & Sons, Ltd | year = 2009| isbn = 9780470682531 | doi = 10.1002/9780470682531.pat0313}}</ref> The enantiomeric ratio of the chiral lithium species is often influenced by the differences in rates of deprotonation. In the example below, treatment of ''N''-Boc-''N''-benzylamine with ''n''-butyllithium in the presence of (-)-sparteine affords one enantiomer of the product with high [[enantiomeric excess]]. Transmetalation with trimethyltinchloride affords the opposite enantiomer.<ref name=NBocbenzylamines>{{cite journal| title = (−)-Sparteine-Mediated α-Lithiation of N-Boc-N-(p-methoxyphenyl)benzylamine: Enantioselective Syntheses of (S) and (R) Mono- and Disubstituted N-Boc-benzylamines| author = Park, Y.S.| journal = J. Am. Chem. Soc.| year = 1996| volume = 118| issue = 15| pages = 3757–3758| doi = 10.1021/ja9538804 |display-authors=etal}}</ref>

:[[File:Asymmetric synthesis with nBuLi and (-)-sparteine.png|600px|center|Asymmetric synthesis with nBuLi and (-)-sparteine]]

====Enolate formation====

Lithium [[enolate]]s are formed through deprotonation of a C−H bond α to the carbonyl group by an organolithium species. Lithium enolates are widely used as nucleophiles in carbon''–''carbon bond formation reactions such as [[aldol condensation]] and alkylation. They are also an important intermediate in the formation of [[silyl enol ether]].

:[[File:Li enolate 2.png|center|750x125px|Sample aldol reaction with lithium enolate]]

Lithium enolate formation can be generalized as an acid''–''base reaction, in which the relatively acidic proton α to the carbonyl group (pK =20-28 in DMSO) reacts with organolithium base. Generally, strong, non-nucleophilic bases, especially lithium amides such LDA, LiHMDS and LiTMP are used. THF and DMSO are common solvents in lithium enolate reactions.<ref name=valnotenolate />

The stereochemistry and mechanism of enolate formation have gained much interest in the chemistry community. Many factors influence the outcome of enolate stereochemistry, such as steric effects, solvent, polar additives, and types of organolithium bases. Among the many models used to explain and predict the selectivity in stereochemistry of lithium enolates is the Ireland model.<ref name=Ireland>{{cite journal| title = The ester enolate Claisen rearrangement. Stereochemical control through stereoselective enolate formation| author = Ireland. R. E.| journal = J. Am. Chem. Soc.| year = 1976| volume = 98| issue = 10| pages = 2868–2877| doi = 10.1021/ja00426a033 |display-authors=etal}}</ref>

In this assumption, a monomeric LDA reacts with the carbonyl substrate and form a cyclic Zimmerman–Traxler type [[transition state]]. The (E)-enolate is favored due to an unfavorable ''syn-pentane'' interaction in the (Z)-enolate transition state.<ref name=valnotenolate />

:[[File:Ireland model enolate1.svg|center|540px|Ireland model for lithium enolate stereoselectivity. In this example, the (E) enolate is favored.]]

Addition of polar additives such as HMPA or DMPU favors the formation of (Z) enolates. The Ireland model argues that these donor ligands coordinate to the lithium cations, as a result, carbonyl oxygen and lithium interaction is reduced, and the transition state is not as tightly bound as a six-membered chair. The percentage of (Z) enolates also increases when lithium bases with bulkier side chains (such as LiHMDS) are used.<ref name=valnotenolate /> However, the mechanism of how these additives reverse stereoselectivity is still being debated.

There have been some challenges to the Ireland model, as it depicts the lithium species as a monomer in the transition state. In reality, a variety of lithium aggregates are often observed in solutions of lithium enolates, and depending on specific substrate, solvent and reaction conditions, it can be difficult to determine which aggregate is the actual reactive species in solution.<ref name=valnotenolate>{{cite book| last1 = Valnot | first1 = Jean-Yves | last2 = Maddaluno | first2 = Jacques| chapter = Aspects of the synthesis, structure and reactivity of lithium enolates| title = PATAI'S Chemistry of Functional Groups.| publisher = John Wiley & Sons, Ltd | year = 2009| isbn = 9780470682531 | doi = 10.1002/9780470682531.pat0345}}</ref>

=== Lithium–halogen exchange ===
{{main|Metal-halogen exchange#Lithium-halogen exchange}}

Lithium–halogen exchange involves heteroatom exchange between an organohalide and organolithium species.
{{NumBlk|:|<chem title="Lithium-Halogen exchange">R-Li + R'-X -> R-X + R'-Li</chem>|{{EquationRef|2}}}}
Lithium–halogen exchange is very useful in preparing new organolithium reagents. The application of lithium–halogen exchange is illustrated by the Parham cyclization.<ref name=parham>{{cite journal| title = Aromatic organolithium reagents bearing electrophilic groups. Preparation by halogen-lithium exchange| author = Parham, W.P.|author2=Bradsher, C.K.| journal = Acc. Chem. Res.| year = 1982| volume = 15| issue = 10| pages = 300–305| doi = 10.1021/ar00082a001}}</ref>

:[[File:Parham cyclization in MitoSpin'.png|center|580px|Parham cyclization in MitoSpin]]

===Transmetalation===
Organolithium reagents are often used to prepare other organometallic compounds by transmetalation. Organocopper, [[organotin]], organosilicon, organoboron, organophosphorus, [[organocerium]] and organosulfur compounds are frequently prepared by reacting organolithium reagents with appropriate electrophiles.

{{NumBlk|:|<math chem title="Transmetalation">\ce{R-M} + \textit{n-}\ce{BuLi -> {R-Li} +}\ \textit{n-}\ce{BuM}</math>|{{EquationRef|3}}}}

Common types of transmetalation include Li/Sn, Li/Hg, and Li/Te exchange, which are fast at low temperature.<ref name=Reich3 /> The advantage of Li/Sn exchange is that the tri-alkylstannane precursors undergo few side reactions, as the resulting n-Bu<sub>3</sub>Sn byproducts are unreactive toward alkyllithium reagents.<ref name=Reich3>''Organolithium Reagents'' Reich, H.J. 2002 https://organicchemistrydata.org/hansreich/resources/organolithium/organolithium_data/orgli-primer.pdf</ref> In the following example, vinylstannane, obtained by [[hydrostannylation]] of a terminal alkyne, forms vinyllithium through transmetalation with n-BuLi.<ref name=stannane>{{cite journal| title = Useful new organometallic reagents for the synthesis of allylic alcohols by nucleophilic vinylation| author = Corey, E.J.|author2=Wollenberg, R.H.| journal = J. Org. Chem.| year = 1975| volume = 40| issue = 15| pages = 2265–2266| doi = 10.1021/jo00903a037}}</ref>

:[[File:Li Sn exchange.png|center|550px|Li Sn exchange]]

Organolithium can also be used in to prepare organozinc compounds through transmetalation with zinc salts.<ref name=organozinc>{{cite journal| title = An Improved Method for the Palladium Cross-Coupling Reaction of Oxazol-2-ylzinc Derivatives with Aryl Bromides| author = Reeder, M.R.| journal = Org. Process Res. Dev.| year = 2003| volume = 7| issue = 5| pages = 696–699| doi = 10.1021/op034059c |display-authors=etal}}</ref>

:[[File:Organozincfrom li.png|center|550px|Organozinc reagents from alkyllithium]]

Lithium diorganocuprates can be formed by reacting alkyl lithium species with copper(I) halide. The resulting organocuprates are generally less reactive toward aldehydes and ketones than organolithium reagents or Grignard reagents.<ref name=pathwayofcuprate>{{cite journal| title = Reaction Pathway of the Conjugate Addition of Lithium Organocuprate Clusters to Acrolein| author = Nakamura, E.| journal = J. Am. Chem. Soc.| year = 1997| volume = 119| issue = 21| pages = 4900–4910| doi = 10.1021/ja964209h |display-authors=etal}}</ref>

:[[File:1,4 cuprate addition.png|center|390px|1,4 cuprate addition]]

== Preparation ==
Most simple alkyllithium reagents, and common lithium amides are commercially available in a variety of solvents and concentrations. Organolithium reagents can also be prepared in the laboratory. Below are some common methods for preparing organolithium reagents.

===Displacement of a leaving group===
In [[lithium-halogen exchange]], reduction of alkyl halide with metallic lithium can afford simple alkyl and aryl organolithium reagents.<ref name=Carey />
{{NumBlk|:|<chem title="Reduction with metal lithium">R-X + 2Li -> R-Li + Li-X</chem>|{{EquationRef|4}}}}

''tert-''Butyllithium or ''n-''butyllithium are the most commonly used reagents for generating new organolithium species through lithium halogen exchange. Lithium–halogen exchange is mostly used to convert aryl and alkenyl iodides and bromides with ''sp2'' carbons to the corresponding organolithium compounds. The reaction is extremely fast, and often proceed at −60 to −120&nbsp;°C.<ref name=Leroux />

Industrial preparation of organolithium reagents is achieved using this method by treating the alkyl chloride with metal lithium containing 0.5''–''2% [[sodium]]. The conversion is highly [[exothermic]]. The sodium initiates the radical pathway and increases the rate.<ref name=Schlosser>"Organometallics in Organic Synthesis", Schlosser, M., Ed, Wiley: New York, 1994. {{ISBN|0-471-93637-5}}</ref> The reduction proceeds via a radical pathway. Below is an example of the preparation of a functionalized lithium reagent using reduction with lithium metal.<ref name=reductLi>{{cite journal| title = Obtention of 2,2-(diethoxy) vinyl lithium and 2-methyl-4-ethoxy butadienyl lithium by arene-catalysed lithiation of the corresponding chloro derivatives. Synthetic applications| author = Si-Fodil, M.| journal = Tetrahedron Lett.| year = 1998| volume = 39| issue = 49| pages = 8975–8978| doi = 10.1016/S0040-4039(98)02031-0 |display-authors=etal}}</ref> Sometimes, lithium metal in the form of fine powders are used in the reaction with certain catalysts such as [[naphthalene]] or 4,4’-di-t-butylbiphenyl (DTBB). Another substrate that can be reduced with lithium metal to generate alkyllithium reagents is sulfides. Reduction of sulfides is useful in the formation of functionalized organolithium reagents such as alpha-lithio ethers, sulfides, and silanes.<ref name=Cohen>{{cite journal|last=Cohen|first=T|author2=Bhupathy. M|title=Organoalkali compounds by radical anion induced reductive metalation of phenyl thioethers|journal=Acc. Chem. Res.|year=1989|volume=22|issue=4|pages=152–161|doi=10.1021/ar00160a006}}</ref>

:[[File:Reduction with li metal.png|center|480px|Reduction with Li metal]]

===Metalation===
{{Further|Metalation#Reactivity and applications}}
A second method of preparing organolithium reagents is a metalation (lithium hydrogen exchange). The relative acidity of hydrogen atoms controls the position of lithiation.

This is the most common method for preparing alkynyllithium reagents, because the terminal hydrogen bound to the ''sp'' carbon is very acidic and easily deprotonated.<ref name=Carey /> For aromatic compounds, the position of lithiation is also determined by the directing effect of substituent groups.<ref name=Snieckus>{{cite journal|last=Snieckus|first=V|title=Directed ortho metalation. Tertiary amide and O-carbamate directors in synthetic strategies for polysubstituted aromatics|journal=Chem. Rev.|year=1990|volume=90|issue=6|pages=879–933|doi=10.1021/cr00104a001}}</ref> Some of the most effective directing substituent groups are alkoxy, amido, sulfoxide, sulfonyl. Metalation often occurs at the position ortho to these substituents. In heteroaromatic compounds, metalation usually occurs at the position ortho to the heteroatom.<ref name=Carey /><ref name=Snieckus />

:[[File:Organolithium Reagents Prepared Metalation.svg|center|700px]]

===Transmetalation===
{{Further|Transmetalation#Applications}}
The fourth method to prepare organolithium reagents is through transmetalation. This method can be used for preparing vinyllithium.

===Shapiro reaction===
In the [[Shapiro reaction]], two equivalents of strong alkyllithium base react with p-tosylhydrazone compounds to produce the vinyllithium, or upon quenching, the olefin product.

==Handling==
Organolithium compounds are highly reactive species and require specialized handling techniques. They are often corrosive, flammable, and sometimes [[pyrophoric]] (spontaneous ignition when exposed to air or moisture).<ref name=Letchford>{{cite journal|last1=Schwindeman|first1=James A.|last2=Woltermann|first2=Chris J.|last3=Letchford|first3=Robert J.|title=Safe handling of organolithium compounds in the laboratory|journal=Chemical Health and Safety|volume=9|issue=3|year=2002|pages=6–11|issn=1074-9098|doi=10.1016/S1074-9098(02)00295-2}}</ref> Alkyllithium reagents can also undergo thermal decomposition to form the corresponding alkyl species and lithium hydride.<ref name=Gellert>{{cite journal|last=Gellert|first=H|author2=Ziegler, K.|title=Organoalkali compounds. XVI. The thermal stability of lithium alkyls.|journal=Liebigs Ann. Chem.|year=1950|volume=567|pages=179–185|doi=10.1002/jlac.19505670110}}</ref>  Organolithium reagents are typically stored below 10&nbsp;°C. Reactions are conducted using [[air-free technique]]s.<ref name=Letchford /> The concentration of alkyllithium reagents is often determined by [[titration]].<ref>{{cite journal|author1=Juaristi, E. |author2=Martínez-Richa, A. |author3=García-Rivera, A. |author4=Cruz-Sánchez, J. S. |title=Use of 4-Biphenylmethanol, 4-Biphenylacetic Acid and 4-Biphenylcarboxylic Acid/Triphenylmethane as Indicators in the Titration of Lithium Alkyls. Study of the Dianion of 4-Biphenylmethanol|journal=The Journal of Organic Chemistry|year=1983|volume=48|issue=15|pages=2603–2606|doi=10.1021/jo00163a038}}</ref><ref>{{cite web |url= http://www.scripps.edu/shenvi/Education_files/titration.pdf| title=Titrating Soluble RM, R2NM and ROM Reagents |access-date= 2014-06-04 }}</ref><ref>{{cite web |url= https://www.chem.tamu.edu/rgroup/gladysz/documents/alkylreagents.pdf |title= Methods for Standardizing Alkyllithium Reagents (literature through 2006) |access-date= 2014-06-04 }}</ref>

Organolithium reagents react, often slowly, with ethers, which nonetheless are often used as solvents.<ref>{{cite journal | title = Directed Ortho-Lithiation of Phenylcarbamic Acid 1,l-Dimethylethyl Ester (N-Boc-aniline). Revision and Improvements |author1=Stanetty, P. |author2=Koller, H. |author3=Mihovilovic, M. | journal = [[J. Org. Chem.]] | year = 1992 | volume = 57 | pages =  6833–6837 | doi = 10.1021/jo00051a030 | issue = 25}}</ref>
{| class="wikitable"
|+Approximate half-lives of common lithium reagents in typical solvents
! Solvent!!Temp
! n-BuLi
! s-BuLi
! t-BuLi
! MeLi
! CH<sub>2</sub>=C(OEt)-Li
! CH<sub>2</sub>=C(SiMe<sub>3</sub>)-Li
|-
|THF || style="text-align:right;" | −40&nbsp;°C
|
|
|338 min
|
|
|
|-
| THF || style="text-align:right;" | −20&nbsp;°C
|
|
| 42 min
|
|
|
|-
|THF || style="text-align:right;" | 0&nbsp;°C
|17 h
|
|
|
|
|
|-
| THF || style="text-align:right;" | 20&nbsp;°C
|107 min
|
|
|
| >15 h
| 17 h
|-
| THF || style="text-align:right;" | 35&nbsp;°C
| 10 min
|
|
|
|
|
|-
| THF/TMEDA || style="text-align:right;" | −20&nbsp;°C
| 55 h
|
|
|
|
|
|-
| THF/TMEDA || style="text-align:right;" |  0&nbsp;°C
| 340 min
|
|
|
|
|
|-
| THF/TMEDA || style="text-align:right;" | 20&nbsp;°C
| 40 min
|
|
|
|
|
|-
| Ether || style="text-align:right;" | −20&nbsp;°C
|
|
| 480 min
|
|
|
|-
| Ether || style="text-align:right;" | 0&nbsp;°C
|
|
| 61 min
|
|
|
|-
| Ether || style="text-align:right;" | 20&nbsp;°C
| 153 h
|
| <30 min
|
|
| 17 d
|-
| Ether || style="text-align:right;" | 35&nbsp;°C
| 31 h
|
|
|
|
|
|-
| Ether/TMEDA || style="text-align:right;" |  20&nbsp;°C
| 603 min
|
|
|
|
|
|-
| DME || style="text-align:right;" | −70&nbsp;°C
|
| 120 min
| 11 min
|
|
|
|-
| DME || style="text-align:right;" | −20&nbsp;°C
| 110 min
| 2 min
| ≪2 min
|
|
|
|-
| DME || style="text-align:right;" | 0&nbsp;°C
| 6 min
|
|
|
|
|
|}

== See also ==

* [[Alkynylation]]
* [[Carbon]]
* [[Grignard reagent]]
* [[HSAB concept]]
* [[Isotopes of lithium]]
* [[Lithium]]
* [[Organometallic]]

==Further reading==
*{{cite journal|author1= Reich, H. J. |author2= Borst, J. P |author3= Dykstra, R. R.|author4=Green, P. D. |journal=[[J. Am. Chem. Soc.]]|year=1993| volume=115|issue= 19 |pages= 8728–8741|title= A nuclear magnetic resonance spectroscopic technique for the characterization of lithium ion pair structures in THF and THF/HMPA solution| doi= 10.1021/ja00072a028}}

==References==
{{Reflist|colwidth=30em}}

{{Lithium compounds}}
{{ChemicalBondsToCarbon}}
{{Authority control}}

[[Category:Lithium compounds]]
[[Category:Organolithium compounds]]