<figure><img src="image_1.png" /></figure>

CrossMark

← click for updates

Cite this: *Dalton Trans.*, 2014, **43**,
14181

# New avenues in the directed deprotometallation of aromatics: recent advances in directed cupration

Philip J. Harford,ª Andrew J. Peel,ª Floris Chevallier,ᵇ Ryo Takita,ᶜ,>d
Florence Mongin,ª,ᵇ Masanobu Uchiyama,ª,ᶜ,d and Andrew E. H. Wheatley*ª

Recent advances in the selective deprotometallation of aromatic reagents using alkali metal cuprates are reported. The ability of these synergic bases to effect deprotonation under the influence of a directing group is explored in the context of achieving new and more efficient organic transformations whilst encouraging greater ancillary group tolerance by the base. Developments in our understanding of the structural chemistry of alkali metal cuprates are reported, with both Gilman cuprates of the type R₂CuLi and Lipshutz and related cuprates of the type R₂Cu(X)Li₂ (X = inorganic anion) elucidated and rationalised in terms of ligand steric s. The generation of new types of cuprate motif are introduced through the development of adducts between different classes of cuprate. The use of DFT methods to interrogate the mechanistic pathways towards deprotonative metallation is described. Theoretical model- ling of in situ rearrangements undergone by the cuprate base are discussed, with a view to understanding the relationship between R₂CuLi and R₂Cu(X)Li₂, their interconversion and the implications of this for cuprate reactivity. The advent of a new class of adduct between different cuprate types is developed and interpreted in terms of the options for expelling LiX from R₂Cu(X)Li₂. Applications in the field of medicinal chemistry and (hetero)arene derivatization are explored.

Received 16th April 2014,
Accepted 3rd June 2014

DOI: 10.1039/c4dt01130a

www.rsc.org/dalton

## 1. General introduction

Deprotolithiation has proved to be an enormously powerful method by which to effect the regioselective functionalization of aromatics.¹ Historically, bases such as organolithiums and lithium dialkylamides have typically been employed for this purpose. However, either because they are highly polar or

because they generate polar aryllithiums, their use for the functionalization of sensitive substrates (e.g. bearing functional groups that are prone to nucleophilic attack, rearrangement or elimination) requires strictly controlled conditions. In addition, organolithium compounds react with electrophiles, such as aroyl chlorides, through double addition, limiting synthetic possibilities by rendering the direct synthesis of ketones unlikely.

Recently, the use of organic bases containing two metals has come to the fore. These so-called synergic reagents exhibit behaviour that is different from that of the corresponding monometal bases. Whilst the field is a challenging one, since its inception² in 1999 with the development of the putative lithium zincate Bu[t]{2}Zn(TMP)Li (TMP = 2,2,6,6-tetramethylpiperidine), a variety of complexes of the type (R)ₘ(R')ₙMM' (M = alkali metal, M' = lower polarity metal; R, R' = alkyl, amido, chloro, etc.), and in particular those containing the very hindered TMP ligand, have been reported to act as efficient and

Philip Harford obtained an MSc degree in Natural Sciences in 2008 from the University of Cambridge and is currently studying for his PhD there under the supervision of Dr Andrew Wheatley. His research is focussing on the synthesis of heterobimetallic lithium cuprate bases with particular interest in their structures as derived from X-ray crystallographic studies.

Andrew Peel completed his degree in Natural Sciences at the University of Cambridge in 2013. He is currently undertaking a PhD in Chemistry in the Wheatley group. His research presently focuses on lithium amidocuprate chemistry, with his principal interests being in chemical crystallography. His other interests include growing exotic chilli peppers and playing guitar.

<figure><img src="image_2.png" /></figure>

<footnote>ªDepartment of Chemistry, University of Cambridge, Lensfield Road, Cambridge, CB2 1EW, UK. E-mail: aehw2@cam.ac.uk; Fax: +44 (0)1223 336362;
Tel: +44 (0)1223 763966</footnote>

<footnote>ᵇUMR 6226, Institut des Sciences Chimiques de Rennes, Chimie et Photonique Moléculaires, Université de Rennes 1-CNRS, Campus de Beaulieu, Bâtiment 10A, Case 1003, 35042 - Rennes Cedex, France. E-mail: Florence.Mongin@univ-rennes1.fr</footnote>

<footnote>ᶜAdvanced Elements Chemistry Research Team, RIKEN Center for Sustainable Resource Science (CSRS), and Elements Chemistry Laboratory, RIKEN, 2-1 Hirosawa, Wako-shi, Saitama 351-0198, Japan. E-mail: uchiyama@mol.f.u-tokyo.ac.jp</footnote>

<footnote n="4">⁴Graduate School of Pharmaceutical Sciences, The University of Tokyo, 7-3-1 Hongo, Bunkyo-ku, Tokyo 113-0033, Japan</footnote>
selective superbases.³ These complexes – which now feature Zn, Al, Cu, Mn and Mg as the lower polarity metal – all exhibit 'ate formulations, and, as such, reveal both anionic activation⁴ and reduced aggregation⁵ when suitable reaction media are employed. Recently, more elaborate versions of these complexes have appeared; these include salt-activated organometallic compounds (e.g. “turbo”-Grignard reagents), and synergic pairs of metal amides that complement each other in deprotometallation reactions.³d,g

The present Perspective depicts the behaviour towards aro-
matics of lithium cuprates specifically, and the development
of the concept of Directed ortho Cupration (DoC) that was first
reported in 2007.⁶ Though they were first prepared in the
1950s, evidence for the actual nature of lithium cuprates has
been slow to be forthcoming and it is only recently that solid-
state structural data has appeared for examples of these com-
plexes designed to behave as deprotonating agents. The
present article is divided into five main parts. After this intro-
duction, cuprate synthesis and structural characterisation are
detailed in the second part. Understanding of the structural
principles at work in lithium cuprates is important in order to
fully appreciate differences in their reactivities. As is discussed
below, there has been much debate into whether such differ-
ences in reactivity can be explained in terms of reagent structure.
Recently, however, very interesting work has gone a long way to
explaining the contrasting activities of cuprates (e.g. 7 and 12,
see below) that are now known to be structurally analogous.⁷
After this structural discussion, the scope and applications of
aromatic directed cupration are presented. Discussion then
shifts to the theoretical interrogation of these systems with a
view to understanding their mechanistic chemistry. Finally,
the concluding section seeks to draw together structural evi-
dence and theoretical work with a view to rationalising the
reported reactions and identifying future directions.

2. Advances in the solid-state structural chemistry of alkali metal amidocuprates

**2.1. Lipshutz cuprates: the solid-state evidence**

The most investigated method by which organocopper com-
pounds can provide reactive organic anions is *via* organo-

cuprates. First reported in 1952, Gilman noted that the addition
of 1 equiv. MeLi to CuI resulted in the formation of a highly
reactive and ether-insoluble yellow product thought to be
(MeCu)∞. This dissolved upon addition of further MeLi⁸ to
give (empirically) the lithium cuprate Me₂CuLi ¹.⁹ In 1981, the
replacement of CuI with CuCN to give more reactive cuprates
for halide substitution reactions was proposed. At this time it
was argued that the cyanide anion σ-bonded to Cu,¹⁰ though
while some NMR studies were interpreted in terms of the pres-
ence of such a motif in solution,¹¹ solid-state evidence for the
exact nature of so-called ‘Lipshutz cuprates’ remained elusive.

Initial crystallographic evidence for the structures of
lithium cuprates appeared only in the early 1980s, with
publication of the structures of [Cu₅Ph₆]⁻[Li·4THF]⁺ 2 and
[Li₂Cu₃Ph₆]₂[Li₄Cl₂·10Et₂O] 3.12,13 Shortly thereafter, van Koten
revealed the solid-state structure of the dimer of
(C₆H₄{CH₂NMe₂}-2)₂CuLi 4.14 This structure, in which an 8-
membered metallocycle was supported by amine chelation of
the alkali metal centres agreed well with that previously pro-
posed based on a combination of multinuclear and variable-
temperature NMR spectroscopic studies.15 This period also
saw the publication of evidence suggestive of the true nature
of Lipshutz cuprates in particular. Attempts to fabricate
lithium cuprates from CuI and (halide-free) organolithiums in
the presence of a crown ether yielded both [CuMe₂]⁻ and
[CuPh₂]⁻ ions.16 These linear cuprate ions have been defined
as so-called ‘lower-order’, with the possibility of ‘higher-order’
cuprate formation, in which copper is 3-coordinate, having
been previously invoked to explain the enhanced reactivity of
Lipshutz species.10,17 By 1990 the lack of data supporting such
higher-order cuprates prompted the publication of NMR spec-
troscopic studies on mixtures of the bis(organyl)cuprates
R₂CuLi with LiX (R = Me, Ph; X = I, CN). The identical nature
of the resulting data was argued to be consistent with lower-
order structures in solution.18 However, the controversy contin-
ued with the presentation of contrary spectroscopic evidence,
with the chemical shifts of the Me₂CuLi/LiI system changing
upon the addition of LiCN and the postulated formation of a
Cu–CN interaction.19 That said, alternative explanations, e.g.
LiCN coordination to an R group, remained, and this ambigu-
ity led to the theoretical investigation by Snyder of possible
structural candidates (see section 4). This led to the conclusion
that higher-order structures were less stable than their lower-
order analogues.20 Whilst in response to these finding it was

Floris Chevallier is an Associate Professor at the University of Rennes 1 (Rennes, France). He studied (organic) chemistry at the universities of Orléans and Nantes. He received his PhD in 2004 under the supervision of Prof. Jean-Paul Quintard, for whom he worked on organotin chemistry. In 2005, he joined the group of Prof. Bernhard Breit at the Albert-Ludwigs-Universität Freiburg (Freiburg, Germany) as a postdoctoral researcher, where he focused on supramolecular catalysis. His current research interests include organometallic methodologies and molecular self-assemblies.

Ryo Takita obtained his PhD in 2006 from the University of Tokyo with Prof. Masakatsu Shibasaki. From 2006 to 2007, he worked as a postdoctoral Fellow at Massachusetts Institute of Technology with Professor Timothy M. Swager. He became an Assistant Professor at Kyoto University (2007–2010) and University of Tokyo (2010–2012), and was promoted to Lecturer (2012–2014). He is currently a Deputy Team Leader at RIKEN Center for Sustainable Resource Science (CSRS). His research interests include organic chemistry for unexplored reactivity and functions.
<figure><img src="image_3.png" /></figure>

proposed that CN⁻ might σ-bond to lithium and π-bond to copper,²¹ further theoretical work suggested the former coordinate mode to be more likely than the latter.²²

It is only since 1998 that unambiguous structural evidence for the behaviour of cyanide ligands in the presence of Cu(I) organometallics has appeared in the literature. Initial reports verified the solid-state structures of ion-separated [Bu₉₂Cu]⁻ - [(μ-CN)(Li·THF·PMDTA)₂]⁺ 5 (PMDTA = N,N,N',N'',N''-penta-methyldiethylenetriamine) and the polymer of closely related {(2-Me₂NCH₂C₆H₄)₂Cu}{(μ-CN)(Li·2THF)₂} 6 (Fig. 1).²³,²⁴ In the first of these examples, the use of a strong Lewis base (PMDTA) has induced ion-separation by extruding Li⁺ from the cuprate moiety. Concordant with this and, as is described in section 4, based both on crystallographic and theoretical studies, the ability of the cuprate component of the structure to interact with an alkali metal is contingent not only on the Lewis basicity of the solvent but also on the nature of the Cu-bonded organyl groups. In the case of 5, the adoption of a Cu(μ-Bu')Li motif is not strongly favoured by the choice of potential bridging group. Accordingly, therefore, separated and linear [Bu₉₂Cu]⁻ and [(μ-CN)Li₂]⁺ ions are noted. In contrast, the absence of PMDTA and the utilisation of bifunctional organyl groups in the cuprate ion instead lead to ion-association in 6 via the formation of N(Me₂)-Li interactions.

The issue of cyanide incorporation by cuprates has only recently been revisited. This work first appeared in 2007, with attempts to fabricate and structurally elucidate the proposed Lipshutz cuprate afforded by treating TMPLi with 0.5 equiv. of CuCN (Scheme 1). The imperative for this investigation came from the first reports of Directed *ortho* Cupration (DoC) facilitated by the use of cuprate moieties that incorporate sterically demanding amide ligands.⁶ As noted in section 3.2, a reagent with the putative (Lipshutz) formulation (TMP)₂Cu(CN)Li₂ was found to offer significant potential for aromatic homocoupling processes. X-ray diffraction on the isolated crystals established

<figure><img src="image_4.png" /><figcaption>**Fig. 1** The first solid-state evidence for lithium cyanocuprate structures was revealed by ion-separated 5 and the polymer of 6.</figcaption></figure>

the structure as being a dimer based on monomers of (TMP)₂Cu(CN)Li₂·THF 7 (Fig. 2). The core is based on a classical (NLi)₂ cyclic architecture synonymous with the metallocycle formation of Snaith's vertical²⁵ and lateral²⁶ ring aggregation principles. Peripheral to this core are two cuprate components, based on approximately linear N-Cu-N motifs. The metal-bridging potential of the amido ligands is clearly demonstrated. Crucially, in terms of understanding the structural properties of cyanide-containing cuprates, the ion-associated species formed does not contain a bonded CuCN component in the solid-state. Instead, it closely approximates to the most stable of the structures computed by Snyder in 1994,²⁰ with the cyanide group bridging between alkali metal ions. The manner in which it does this is different for the various metals in the aggregated structure, with each cyanide interacting with three

<figure><img src="image_5.png" /><figcaption>Florence Mongin</figcaption></figure>

Florence Mongin obtained her PhD in Chemistry in 1994 from the University of Rouen (France) under the supervision of Prof. Guy Queguiner. After two years at the Institute of Organic Chemistry of Lausanne (Switzerland) as a postdoctoral Fellow with Prof. Manfred Schlosser, she returned to the University of Rouen as an Assistant Professor in 1997 (HDR in 2003). She took up her present position in 2005 as Professor at the University of

Rennes (France) and was appointed Junior Member of the Institut Universitaire de France in 2009. Her interests include the functionalization of aromatic compounds including heterocycles with recourse to mixed lithium-metal bases.

<figure><img src="image_6.png" /><figcaption>Masanobu Uchiyama</figcaption></figure>

Masanobu Uchiyama obtained his PhD in 1998 from the University of Tokyo with Prof. Koichi Shudo. He worked as an Assistant Professor at Tohoku University (1995–2001) and University of Tokyo (2001–2003), and was promoted to lecturer (2003–2006). He became Associate Chief Scientist at RIKEN in 2006. He is currently a Full Professor at the University of Tokyo (from 2010) and Chief Scientist/Team Leader at RIKEN and RIKEN CSRS

(from 2013). His research interests are in the area of synthetic organic chemistry with an emphasis on organometallic, physical, and computational chemistry.
<figure><img src="image_7.png" /></figure>

<figure><img src="image_8.png" /><figcaption>**Scheme 1** Formation of the dimer of Lipshutz bis(amido)cuprate 7.</figcaption></figure>

<figure><img src="image_9.png" /><figcaption>**Fig. 2** Crystal structure (H atoms omitted) of the dimer of Lipshutz cuprate 7.</figcaption></figure>

different alkali metal centres; spanning two metal ions in near linear σ-fashion and exhibiting an offset side-on bond to the third.

## 2.2. Extending the principle: Lipshutz-type structures

The structural motif revealed by 7 turns out to have a great deal in common with the 6-membered metallocyclic lithio-

cuprate (Ph₂N)₂Cu(NPh₂)Li₂·2OEt₂ 8.²⁷ This species revealed a solid-state monomer comprising a near linear geometry at Cu and both Cu-(μ-N)-Li and Li-(μ-N)-Li bridges (Fig. 3). Taken together, the observation of 7 and 8 suggests that there is nothing unique in the inter-lithium bridging activity of cyanide in the former complex. This idea led us to propose the creation of a series of what might be called 'Lipshutz-type' cuprates. These have the formulation R₂Cu(X)Li₂, such that for 7 X = CN. This idea has been tested by the replacement of CuCN with CuHal (Hal = Cl, Br, I) in essentially the same synthetic sequence as that which yielded 7 (Scheme 2). In the first instance, CuCl was investigated (our interest in this deriving from its ability to promote the deprotonative metallation of 2-chloropyridine as a precursor to benzoylation, see section 3.3). Initial work towards the isolation and characterisation of halide-containing reagent mixtures focused on the deployment of TMPLi and CuCl, with data quickly establishing that solvent conditions capable of promoting the retention of *in situ*-formed LiCl *in solution* (where it is capable of combining with putative R₂CuLi) promoted cuprate reactivity. Importantly, attempts to replicate organic transformations using pre-

<figure><img src="image_10.png" /><figcaption>Andrew Wheatley</figcaption></figure>

Andrew Wheatley obtained his BSc from the University of Kent at Canterbury in 1995. He then worked at Cambridge under the guidance of Dr Ron Snaith, receiving his PhD in 1999 and an MA (Cantab) in 2002. After his PhD studies he undertook a Research Fellowship at Gonville & Caius College before becoming a University Lecturer at Cambridge (2000) and a Fellow of Fitzwilliam College. He has received the Harrison Memorial

Medal from the RSC and more recently he has been a Visiting Associate Professor at Tohoku University, Japan. He is now a University Senior Lecturer at Cambridge.

<figure><img src="image_11.png" /><figcaption>**Fig. 3** Monomeric structure of amidocuprate 8.</figcaption></figure>

<figure><img src="image_12.png" /><figcaption>**Scheme 2** Formation of the dimers of Lipshutz-type bis(amido)cuprates 9, 10 and 12.</figcaption></figure>
<figure><img src="image_13.png" /></figure>

<figure><img src="image_14.png" /><figcaption>Fig. 4 Structure (H atoms omitted) of the crystallographic dimer of chloride 9.</figcaption></figure>

formed (TMP)₂CuLi (section 3) produced distinctly inferior reactivity. Overall, therefore, it could be posited that the optimal reagent adhered to the putative formulation (TMP)₂Cu(Cl)Li₂.²⁸ Corroboration came from subsequent studies conducted on crystalline material isolated from reaction of TMP:Li with CuCl in THF. The resulting structure, of (TMP)₂Cu(Cl)Li₂·THF 9 (Fig. 4), revealed a solid-state dimer based on a (ClLi)₂ core.²⁹ Superficially, the structure is highly analogous to that revealed by both 7 (albeit the Cu-containing rings are now 6- rather than 7-membered) and 8 (albeit the structure is dimeric). As with these structures, 9 incorporates lower-order, near-linear Cu centres.

Comparative research on the synthesis of diaryl ketones using lithiocuprates prepared with LiCl and LiBr has been reported and is discussed in section 3.3. As with chloride-based 9, the dimer of (TMP)₂Cu(Br)Li₂·THF 10 proved straightforward to isolate and characterise.³⁰ The dimeric structure of this species contrasted with that noted previously for monomeric (C₆H₄{CH₂NMeCH₂CH₂NMe₂}-2)₂Cu(Br)Li₂ 11 in which aggregation was inhibited by internal coordination of the alkali metals (Fig. 5).³¹ Finally, the iodide analogue of 9 and 10, (TMP)₂Cu(I)Li₂·THF 12, was also prepared (Fig. 6).³²

The Cu-containing metallocycles in 7 are 7-membered and show near perpendicular geometry at the bridging nitrogen centres, there being only a slight asymmetry here (N1/2–Li2/1 1.995(4)/1.982(5) Å; Cu1–N1/2–Li2/1 91.13(13)/94.92(14)°) in spite of the fact that the two alkali metal centres in the ring have significantly different coordination environments. On moving to the chloride 9 and bromide 10, the most immediate structural change is that the cuprate moieties yield 6-membered rings which are highly asymmetric. This is revealed by the remarkably different N–Li distances and bridging angles at N. For example, in 10 the unsolvated alkali metal ion participates in a relatively short interaction with TMP (N2–Li2 1.963(4) Å compares with N1–Li1(THF) 2.002(5) Å). In a similar vein, the bridging angle at N2 is expanded relative to

that at N1 (cf. 92.81(14) and 85.45(13)°, respectively). The same pattern is clearly seen for chloride 9, but moving to iodide 12, patterns in the bonding parameters depart somewhat from those seen in 9 and 10 in that the extreme asymmetry seen for the 6-membered cuprate metallocycles in the chloride and bromide dimers is present to a much reduced extent. Thus, although N–Li is significantly shorter than N–Li·THF, four very similar Cu–N–Li bond angles (range 93.11 (18)–94.63(18)°) are seen. The N–Li interactions reveal a final point about the cuprate metallocycles in 12. At 1.965 Å (mean) these are shorter than those in 7 (mean 1.989 Å), consistent with the preference of hard Li⁺ for hard nitrogen over soft iodide.

In a similar vein to the synthesis of THF-solvates 7, 9, 10 and 12, the extension in Li–X bonding interactions as Group 17 is descended is noted also for the employment of OEt₂ as Lewis base. The resulting lithiocuprates 13–16 (for X = CN, Cl, Br and I, respectively; Fig. 7) have all been found to be essentially analogous to their THF-solvated counterparts. Poor quality data prevents detailed discussion of 13. However, analysis of the bonding in 14–16 reveals that, in comparison to the THF-solvates discussed above, their 6-membered rings show a higher level of symmetry, in spite of the clearly different alkali metal environments therein.

<figure><img src="image_15.png" /><figcaption>Fig. 5 Monomeric structure of internally stabilized cuprate 11.</figcaption></figure>

<figure><img src="image_16.png" /><figcaption>Fig. 6 Structure of the non-centrosymmetric dimer of 12 (H atoms and iodide centre positional disorder omitted).</figcaption></figure>
<figure><img src="image_17.png" /><figcaption>Fig. 7 The solid-state formulation of diethyl ether-solvated 13–16.</figcaption></figure>

## 2.3. Gilman reagents

Of course, as noted above, the first lithium cuprates to be prepared were not Lipshutz or Lipshutz-type but rather were considered to have the formulation R<sub>2</sub>CuLi (e.g. R = Me 1). These have come to be known as Gilman reagents. In the context of deprotonative cupration, we describe elsewhere in this article (section 3.2) synthetic transformations done in hydrocarbon media that drive the removal of lithium salt from the reaction and which, therefore, promote Gilman cuprate activity. Specifically, lithium cuprates of the type R<sub>m</sub>Cu(NR<sub>2</sub>)<sub>n</sub>Li (m = 1, n = 1; m = 0, n = 2) are relevant to the organic transformations described here and these have not been thoroughly studied historically. The structural possibilities for these systems have only begun to be elucidated in the last few years and this has led the field to be the subject of review.<sup>33</sup>

Concerning lithium (TMP)cuprates, the treatment of TMPcLi with CuCN and various CuX (X = halide) reagents in THF has been described above as yielding 7 and 9, 10 and 12 (and their OEt<sub>2</sub>-solvated analogues 13–16). Bis(amido)cuprate formulations such as these have been shown (see section 3.2) to effect DoC with the TMP ligand acting as a base, enabling homocoupling to give 2,2-biaryls. However, the solution structures of these systems are still not fully established. This study involves not only the elucidation of aggregation state but also understanding of the affinity of (TMP)<sub>2</sub>CuLi for LiX; that is, the question of whether a Lipshutz-type cuprate may interconvert with a Gilman cuprate through the inclusion/exclusion of LiX. As the discussion of recent theoretical studies in section 4 makes clear, this question is one of enormous importance in understanding DoC reactivity. By way of an example, whereas the previous sections of this structural discussion focus on Lipshutz cuprates (TMP)<sub>2</sub>Cu(CN)Li<sub>2</sub>S 7 and 13 (S = THF, OEt<sub>2</sub>) and also Lipshutz-type reagents (TMP)<sub>2</sub>Cu(X)Li<sub>2</sub>S 9, 10, 12 and 14–16 (X = halide; S = THF, OEt<sub>2</sub>), a bis(TMP) Gilman cuprate has been prepared using remarkably similar chemistry. Hence, the reaction of TMPcLi with CuI in the presence of THF (in the ratio 2:1:1) has given (TMP)<sub>2</sub>Cu(I)Li<sub>2</sub>·THF 12 (see above). In contrast, similar reaction in the absence of THF represents a strategy designed to allow the precipitation and removal of lithium halide. This has borne fruit as discussed in the organic synthesis section of this review, where the efficiency with which deprotonative transformations have been achieved was found to correlate with whether or not lithium salt was

<figure><img src="image_18.png" /><figcaption>Fig. 8 The dimer of 17 with H atoms omitted.</figcaption></figure>

<figure><img src="image_19.png" /><figcaption>**Scheme 3** Formation of Gilman reagent 17 accompanied by the expulsion of lithium iodide, which precipitates in the absence of donor solvent and so avoids the formation of 12.</figcaption></figure>

abstracted from the system. In the present case, LiI precipitation facilitated the isolation of Gilman bis(amido)cuprate (TMP)<sub>2</sub>CuLi 17.<sup>32</sup> Crystallography reveals a cyclic dimer in the solid-state (Fig. 8 and Scheme 3). In spite of the known ability of organolithium and organocopper species to exchange (see below) the metal sites in the dimer of 17 revealed hardly any substitutional disorder and the structure compares closely with the 8-membered metallocyclic dimer of MesNHCu(PhNH)-Li·DME 18 (DME = 1,2-dimethoxyethane; Fig. 9).<sup>27</sup> The isolation of 17 proved useful because it provided pure Gilman bis(TMP)cuprate for comparative tests of Lipshutz-type and Gilman cuprates in organic synthesis (section 3.3).

As noted above, the article in which DoC was first presented discussed the synthesis of homocoupled products.<sup>6</sup> However,

<figure><img src="image_20.png" /><figcaption>Fig. 9 The 8-membered metallocyclic dimer of MesNHCu(PhNH)-Li·DME 18.</figcaption></figure>

<figure><img src="image_21.png" /></figure>
<figure><img src="image_22.png" /></figure>

<figure><img src="image_23.png" /><figcaption>**Scheme 4** The formation of Gilman cuprates **19** (R = Ph, n = 3, S = THF) and **20** (R = Me, n = 1, S = TMEDA).</figcaption></figure>

it was also suggested that the synthesis of heterocoupled products could be achieved by using the putative cuprates R(TMP)-Cu(CN)Li₂ (R = alkyl, aryl). To investigate, CuCN was treated with RLi and TMPLi. For R = Ph crystallography now revealed the formation of monomeric PhCu(TMP)Li·3THF **19** (Scheme 4 and Fig. 10). In a similar vein, the ability of putative cuprate Me(TMP)Cu(CN)Li₂ to achieve products in which aryl substrates were methylated led to investigation of the MeLi-CuCN-TMPLi mixture. With crystallisation being aided by the introduction of TMEDA (N,N,N',N'-tetramethylethylenediamine) it proved possible to isolate cuprate MeCu(TMP)Li·TMEDA **20**.³⁴

The observation of a terminal Cu-Ph interaction in **19** is unusual. Whilst it is known from other types of organo-copper compound,³⁵ the only lithiocuprate examples are [Ph₂Cu]⁻-[Li·2(12-crown-4)]⁺ **21** and {[Ph₂Cu]⁻}₂[(Cu·2PPh₃)·{(CN)Li}₂·5THF]₂⁺ **22**,³⁶ whilst the remaining reported terminal Cu-Ar bonds in this area all feature bulky Mes,³⁷ C₆H₃-2,6-Mes₂,³⁸ C₆H₃-2,6-Trip₂ (Trip = C₆H₂-2,4,6-Pr¹)³⁹ or ferrocenyl groups.⁴⁰ Moving to the similarly underpopulated field of heteroleptic organyl(amido)cuprate structural chemistry,⁴¹ **19** fails to demonstrate the aggregation behaviour of aryl(amido)-cuprate MesCu(NBz₂)Li **23** (Bz = benzyl; Fig. 11),⁴² the head-to-tail dimeric structure of which confirmed theoretical expectations. Even in solution, the dimer showed negligible signs of deaggregation.⁴³ However, it was clear that **23** represented the only compound isolable from a Schlenk equilibrium involving a variety of structural isomers in solution.⁴² Methylcuprate ions are even less well documented, having been noted only in

<figure><img src="image_24.png" /><figcaption>**Fig. 11** The dimeric aggregate of MesCu(NBz₂)Li **23**.</figcaption></figure>

[Me₂Cu]⁻-[Li·nS]⁺ (**24** n = 2, S = 12-crown-4; **25** n = 3, S = DME)³⁶,⁴⁴ and the alkyl(phosphido)cuprate MeCu{P(Buₕ)₂}-Li·3THF **26** (Fig. 12).⁴⁵ The observation of a single N-atom bridge between metals in **19** and **20** is interesting in the wider context of synergic amido-reagents. Hitherto, these have frequently revealed metallo cyclic M(µ-R)(µ-N)Li cores, even after isolation from (and including within their structures) Lewis base media. Hence, metallocycle formation has proved unambiguous in aluminates (where M is Group 13)⁴⁶ and zincates (where M is Group 12 and therefore stands comparison with Group 2).⁴⁷ However, in recently observed manganates (where M is Group 7 and therefore stands comparison with Groups 2 and 12),⁴⁸ closure of the ring *via* the formation of an agostic bridge⁴⁹ to match the amido one was much more ambiguous (Scheme 5). Finally, in the present case (where M is Group 11

<figure><img src="image_25.png" /><figcaption>**Fig. 12** Alkyl(phosphido)cuprate **26**.</figcaption></figure>

<figure><img src="image_26.png" /><figcaption>**Fig. 10** Structures of **19** (left) and **20** (right) with H atoms and disorder omitted.</figcaption></figure>
<figure><img src="image_27.png" /><figcaption>**Scheme 5** The cores of synergic bases containing Al, Zn, Mn and Cu. (a) and (b) metallocycle completion via short Li···C approaches of 2.258(4)⁴⁶ᵇ and 2.374(3)⁴⁷ᵈ Å, respectively; (c) the central ring fails to form, with Li···C relatively extended at 2.742(6) Å;⁴⁷ᵃ (d) Cu exhibits a near linear geometry, precluding agostic stabilisation of the alkali metal.</figcaption></figure>

and stands comparison with Group 1) the essentially linear geometry at Cu⁵⁰ clearly prevents the formation of a metallocycle.

## 2.4. Amidocuprate adducts: the abstraction of lithium halide

Recent studies in the rapidly evolving field of so-called synergic base chemistry have focused on minimizing the costs of reagent preparations.⁵¹ This has led to the deployment of DMPH (= cis-2,6-dimethylpiperidine) in place of TMPH. At time of writing, the relative costs of these two amines are £2.62 g⁻¹ (TMPH) and £0.20 g⁻¹ (DMPH), making the potential savings of developing DMP-ligated synergic bases significant.⁵² The adoption of much cheaper amide ligands has gone hand-in-hand with the removal of some of the significant steric hindrance associated with TMP ligands, allowing fundamental changes to the orientation of the amide group and enabling the observation of new amidocuprate structure-types.⁵³

As noted above, the use of diethyl ether as a solvent enabled the synthesis and isolation of Lipshutz-type (TMP)₂Cu-(Cl)Li₂·OEt₂ 14. However, upon exchanging the amide component for DMP a dramatic effect was observed. Initially, the combination of DMPLi with CuCl was attempted in limited (2 equiv.) Et₂O. Reaction led to the isolation of crystalline material that analyzed as a triangulated structure based on a LiCl core and having the formulation [(DMP)₄CuM(Li·OEt₂)₂]-LiCl 27 where optimal refinement of multiple crystallographic datasets suggested a pattern of disorder consistent with M = 0.3 : 0.7 Cu : Li (Scheme 6).

The disorder at one of the metal sites complicates interpretation of the nature of 27 but is interesting because it is suggestive of the phenomenon of exchange between organocopper and organolithium species that has been directly observed spectroscopically in the past.⁵⁴ Overall, two views of 27 present themselves. For M = Li the complex could be viewed as a 1 : 2

adduct between Lipshutz-type (DMP)₂Cu(Cl)Li₂ and DMPLi. However, for M = Cu it can be argued that 27 represents an *adduct* between Gilman cuprate (DMP)₂CuLi·OEt₂ and Lipshutz-type cuprate (DMP)₂Cu(Cl)Li₂·OEt₂. To overcome this ambiguity and to remove the observed metal disorder, solvent mixtures were varied. Ultimately, the use of bulk Et₂O served to reinforce the interpretation of 27 as an adduct between two cuprates, with [(DMP)₂CuLi·OEt₂]₂LiCl 28 being isolated (Scheme 6 and Fig. 13).

It proved possible to replicate the formation of 28 using CuBr (Scheme 7 and Fig. 14). A number of iterations were required to allow the isolation of [(DMP)₂CuLi·OEt₂]₂LiBr 29. Hence, the reaction of BuⁿLi (1 eq. wrt amine) with DMPH to give DMPLi was initially affected in limited Lewis base (2 equiv. Et₂O). However, this afforded [(DMP)₂Cu-Li·OEt₂]₁.₄₅[(DMP)₂CuLi·DMPH]₀.₅₅LiBr 30. This problem could be overcome, in two ways: the use of excess BuⁿLi (wrt amine) or the deployment of bulk Et₂O as solvent. Variation in solvent conditions has therefore been shown to have an effect on the production of adducts 28 and 29, with bulk Et₂O working best for X = Cl and either bulk or 2 equiv. Et₂O best for X = Br. Attempts to extend the new chemistry to X = I demonstrated a need to more stringently control the quantity of Et₂O, with the

<figure><img src="image_28.png" /><figcaption>**Scheme 6** Synthesis of 27 (M = 30 : 70 Cu : Li, n = 2 equiv. wrt Cu) and 28 (M = Cu, n = bulk).</figcaption></figure>
<figure><img src="image_29.png" /></figure>

<figure><img src="image_30.png" /><figcaption>Fig. 13 Adduct [(DMP)₂CuLi·OEt₂]₂LiCl 28. H atoms and minor Et₂O disorder omitted.</figcaption></figure>

<figure><img src="image_31.png" /><figcaption>Scheme 7 Synthesis of 29 (n = bulk; L = OEt₂) and 30 (n = 2 equiv. wrt Cu; L = (OEt₂)₀.₄₅(DMPH)₀.₅₅).</figcaption></figure>

<figure><img src="image_32.png" /><figcaption>Fig. 14 Adduct [(DMP)₂CuLi·OEt₂]₂LiBr 29. H atoms omitted.</figcaption></figure>

use of 1 equiv. wrt Cu yielding [(DMP)₂CuLi·OEt₂]₂LiI 31 (Scheme 8 and Fig. 15).

The metal disorder in 27 notwithstanding, the adduct structures all approximate to C₂ symmetry about a core lithium halide axis. The metal–halide bonds in adducts 28, 29 and 31 extend as Group 17 is descended. Though this is unsurprising in itself, the extension proves not to be consistent. At 1.10, the ratio between Li2–X and the mean of Li1/3–X is greatest for X = I. For both the smaller halides it is 1.04, and this can be rationalised in terms of the relative preference of the alkali metal for interaction with hard and soft donors. The extension

<figure><img src="image_33.png" /><figcaption>Scheme 8 Synthesis of 31 (n = 1 equiv. wrt Cu).</figcaption></figure>

<figure><img src="image_34.png" /><figcaption>Fig. 15 Adduct [(DMP)₂CuLi·OEt₂]₂LiI 31. H atoms and minor disorder omitted.</figcaption></figure>

of metal–nitrogen bonding as a function of halide hardness is also reflected in the Li2–N–Cu angles, which increase in response to the presence of a softer halide. Moreover, a persistent feature of these ether-solvated adducts is distinct asymmetry in both the N–Li bond lengths and bridging angles at nitrogen. This contrasts with the much more symmetrical rings in diethyl ether solvates 14–16 (see section 2.2) in spite of the observation of essentially the same Cu-containing 6-membered rings in which only one of the two Li⁺ ions is solvated by OEt₂. For example, angles at either N in a 6-membered ring deviate by <3° in 14–16 whereas in adducts 28, 29 and 31 they differ by 4.2–6.6°.

The observation of a transition in structure-type from Lipshutz-type dimers to adducts is intriguing. It is also potentially important in terms of rationalising DoC. As is explained in sections 3 and 4 of this review, DoC requires reagents that are formally Lipshutz(-type) but which may generate active monomeric Gilman bases. This revelation – that generation of the active base takes place *in situ* – has prompted an examination of structure-types synonymous with the abstraction of LiX from Lipshutz-type dimers, and it is clear that adducts of the type now discovered can be viewed in these terms.

Since 14–16 and 28, 29 and 31 are all (mono)ether solvates it stands to reason that the choice of amide ligand must be having a significant effect on structure. This idea bears fruit if the steric constraints associated with TMP and DMP ligands are considered. In, for example, the ether-solvated Lipshutz-type chloride dimer of (TMP)₂Cu(Cl)Li₂·OEt₂ 14 it is clear that
<figure><img src="image_35.png" /><figcaption>**Fig. 16** Structures of the 6-membered heterocyclic Lipshutz-type components that form parts of the dimer of TMP-based chloride **14** (top) and DMP-based adduct **28** (bottom). In **14** the piperidide ligands lie flat in order that the axial Me-groups (red) do not sterically interact. In **28** only equatorial Me-groups are present (blue) and the piperidide ligands can reside face-on.</figcaption></figure>

the two TMP ligands bonded to either Cu atom project away from one another so that the two 6-membered piperidide rings lie in a fashion best described as *endo,endo* relative the (ClLi)₂ aggregate core (Fig. 16, top). The need for this to happen is rationalised by considering the positions of the 8 methyl groups associated with this pair of ligands. Four of these methyl groups (blue in Fig. 16) exhibit equatorial positions relative to the piperidide rings while the remaining four are axially disposed. Clearly, the axial Me-groups (red in Fig. 16) would interact with each other in the event that the piperidide ligands, instead of lying *endo,endo*, adopted an *exo,exo* (or face-on) arrangement. Such an arrangement is, however, enabled by the replacement of TMP by DMP in **28**. In this case the two DMP ligands bonded to a given Cu centre can now exhibit a face-on motif that is *exo,exo* with respect to

the structure core (the LiCl vector in **28**) without there being steric interaction between the methyl groups (Fig. 16, bottom).

The fact that, in the absence of steric interaction between methyl groups, the piperidide rings adopt a face-on configuration vexes the question: is this a preferred arrangement? This unfortunately cannot be answered by an analysis of the adduct structures reported here because the ability of the piperidide ligands to adopt a face-on orientation confers significant stability on the structure in terms of steric interactions not only within the monomeric building block but also between Lipshutz-type and Gilman components of the triangulated structure. As suggested by Fig. 17, the *exo,exo* orientation of the amide ligands allows steric congestion at the unsolvated Li⁺ (Li2 in Fig. 13–15) to be acceptable. An *endo,endo* structure would be precluded for obvious reasons while the inability to observe *exo,exo* TMP-based analogues of DMP-based adducts **28–31** may also be explicable on steric grounds.

The adducts so far prepared have demonstrated a significant tendency to retain their structures in hydrocarbon solution. This has best been evidenced by ⁷Li NMR spectroscopy. For the chloride adduct [(DMP)₂CuLi·OEt₂]₂LiCl **28** the bis(amide)-complexed alkali metal is seen at more positive chemical shift (δ 1.83 ppm) than the externally solvated metal ions, which resonate at δ 1.48 ppm, with the two peaks exhibiting a 1:2 ratio. Identical trends are observed for **29** and **31**. The incompletely deprotonated complex [(DMP)₂Cu-Li·OEt₂]₁.₄₅[(DMP)₂CuLi·DMPH]₀.₅₅LiBr **30** presents a yet more interesting spectrum. The unique bis(amide)-complexed alkali metal ion is seen at δ 1.83 ppm, while equivalent integration signals are now also seen at δ 1.66 ppm and δ 1.48 ppm, and these are attributable to Li·DMPH and Li·OEt₂.

Lastly, recent work on the new class of cuprate adduct discussed here has sought to extend our understanding of the generality with which they form by varying the solvent. Reaction of DMPLi with CuBr followed by recrystallization in the presence of THF has afforded [(DMP)₂CuLi·2THF]₂LiBr **32** (Fig. 18 and Scheme 9). In so doing the ability of THF to furnish an adduct has been demonstrated along with the observation that much more extensive solvation of the alkali metals is possible in these structures.

<figure><img src="image_36.png" /><figcaption>**Fig. 17** A schematic of the observed *exo,exo* (left) and less favoured *endo,endo* forms (middle) of DMP-based adducts akin to **28–31** clarifies why only the first option has been seen experimentally. Steric interaction at the structure apex may also explain why TMP-based adducts have not so far been seen (right).</figcaption></figure>

<figure><img src="image_37.png" /></figure>
<figure><img src="image_38.png" /><figcaption>Fig. 18 Adduct [(DMP)₂CuLi·2THF)₂LiBr 32. H atoms omitted.</figcaption></figure>

<figure><img src="image_39.png" /><figcaption>Scheme 9 Synthesis of adduct 32.</figcaption></figure>

# 3. Recent applications of lithium cuprates in organic synthesis

## 3.1. Gilman cuprates and structural interconversion

By employing a Gilman cuprate base, that is of the type R₂CuLi, Gais and co-workers noted in 2008 the attack of (Z)- and (E)-alkenyl sulfoximines at the α-position and the 1,2-metallate rearrangement of the resulting copper derivatives prior to trapping. A pre-complex between the cuprate base and the sulfoximine group was proposed as a possible explanation for the reaction.⁵⁵ However, with the exception of this study, other examples reported in the literature concerning deproto-metallation using cuprate bases have involved aromatic substrates. Moreover, it is noteworthy that these studies have focused on Lipshutz cuprates and, as defined in section 2 of this review, Lipshutz-type cuprates. This emphasis is borne of studies on the Gilman cuprates RCu(TMP)Li·nS (R = Ph, n = 3, S = THF 19, R = Me, n = 1, S = TMEDA 20) and their tendency to include or exclude LiCN. Crucially, the same work established that 20 was relatively inactive in DoC.³⁴ Thus, N,N-diisopropylbenzamide was treated both with pre-isolated 20 and a solution containing 20 and LiCN, prior to electrophilic quenching with I₂. Results showed that iodination proceeded in both cases, but yielding only 37% 2-iodo-N,N-diisopropyl-

benzamide when employing pre-isolated 20. This improved to 89% using the solution containing 20 and LiCN. Clearly, these data pointed to the importance of the presence of a Lipshutz or Lipshutz-type formulation base in solution, albeit the relationship between Gilman cuprate and LiX (X = CN, halide) remained complex.

## 3.2. Lipshutz formulations: efficient DoC reagents

The ability of several lithium cuprate bases to deprotonate aromatic compounds was first evidenced in 2007 by Usui et al.⁶ The efficiency of the bases was evaluated by reacting benzonitrile with a variety of amidocuprates (formally 2 equiv. of cuprate monomer wrt benzonitrile, the cuprate being prepared in situ by the treatment of amidolithium, organolithium and copper cyanide in appropriate ratios) at 0 °C in THF. This was followed by iodolysis after stirring for 3 h at room temperature (in Table 1 the cuprates are expressed formally as monomers). Whereas amidocuprates prepared from CuI failed to give the 2-iodo derivative in satisfying yields (see next section), it was clear that cuprates of Lipshutz formulation promoted DoC of the aromatic in generally high yields (70–93%). In particular, the TMP ligand, one of the bulkiest amide ligands available, was identified as being crucial for both good reactivity and chemoselectivity.

The putative cuprate MeCu(TMP)(CN)Li₂, identified in Table 1 as a very efficient lithium cuprate base for the deprotonation-iodolysis of benzonitrile, was next employed in the attempted functionalization of a variety of other aromatic substrates (Table 2). In this way, the reaction was extended with success to the elaboration of N,N-diisopropylbenzamide, 3-cyanoanisole, 1,3-dimethoxybenzene and 1,3-dicyanobenzene. Notably, the presence of a bromo or iodo group on the benzene ring was tolerated provided that a lower reaction temperature was used (−78 °C, cf. 0 °C in Table 1). Lastly, five-membered aromatic heterocycles could be similarly regioselectively converted at 0 or −40 °C.

<table><caption>**Table 1** Screening of amidocuprates for benzonitrile-directed *ortho* cupration</caption><thead><tr><th>Entry</th><th>Cuprate</th><th>Yield<sup>a</sup> (%)</th></tr></thead><tbody><tr><td>1</td><td>TMPCu(CN)Li</td><td>0</td></tr><tr><td>2</td><td>(TMP)<sub>2</sub>Cu(i)Li<sub>2</sub></td><td>0</td></tr><tr><td>3</td><td>MeCu(TMP)(i)Li<sub>2</sub></td><td>51</td></tr><tr><td>4</td><td>MeCu(NMe<sub>2</sub>)(CN)Li<sub>2</sub></td><td>0</td></tr><tr><td>5</td><td>MeCu(NPr<sub>2</sub>)(CN)Li<sub>2</sub></td><td>53</td></tr><tr><td>6</td><td>(TMP)<sub>2</sub>Cu(CN)Li<sub>2</sub></td><td>74</td></tr><tr><td>7</td><td>MeCu(TMP)(CN)Li<sub>2</sub></td><td>91</td></tr><tr><td>8</td><td>Bu<sup>i</sup>Cu(TMP)(CN)Li<sub>2</sub></td><td>83</td></tr><tr><td>9</td><td>Bu<sup>i</sup>Cu(TMP)(CN)Li<sub>2</sub></td><td>70</td></tr><tr><td>10</td><td>PhCu(TMP)(CN)Li<sub>2</sub></td><td>93</td></tr></tbody></table>

<figure><img src="image_40.png" /></figure>

<footnote>a After purification.</footnote>
<table><caption>**Table 2** DoC of aromatic substrates using MeCu(TMP)(CN)Li₂</caption><thead><tr><th>Entry</th><th>Temp.</th><th>Product</th><th>Yield<sup>a</sup> (%)</th><th>Entry</th><th>Temp.</th><th>Product</th><th>Yield<sup>a</sup> (%)</th></tr></thead><tbody><tr><td>1</td><td>0 °C</td><td>CON(Pr)<sub>2</sub></td><td>92</td><td>6</td><td>-78 °C</td><td>CON</td><td>96</td></tr><tr><td>2</td><td>0 °C</td><td>CN<br>OMe</td><td>90</td><td>7</td><td>-78 °C</td><td>CON(Pr)<sub>2</sub></td><td>100</td></tr><tr><td>3</td><td>0 °C</td><td>OMe</td><td>95</td><td>8</td><td>0 °C</td><td>N<br>S</td><td>90</td></tr><tr><td>4</td><td>0 °C</td><td>CN<br>CN</td><td>90</td><td>9</td><td>0 °C</td><td>O</td><td>70</td></tr><tr><td>5</td><td>-78 °C</td><td>Br</td><td>82</td><td>10</td><td>-40 °C</td><td>Boc</td><td>88</td></tr></tbody></table>

Besides iodine, electrophiles such as D₂O, methyl iodide, allyl bromide, benzoyl chloride and chlorotrimethylsilane were all successfully used to efficiently intercept the arylcuprate intermediate generated by *ortho* deprotometallating N,N-diisopropylbenzamide. These electrophiles afforded the expected deuterated, methylated, allylated, benzoylated and silylated derivatives in yields ranging from 84 to 100% (Table 3). The introduction of a hydroxyl group was achieved in 56% yield by exposure of the cuprate to molecular oxygen at room temperature in the presence of CuCN (1 equiv.).

When the arylcuprates prepared from N,N-diisopropylbenzamide using different putative RCu(TMP)(CN)Li₂ bases were treated with nitrobenzene, selective oxidative ligand coupling took place to furnish either the 2-methylated (R = Me) or the 2-phenylated (R = Ph) cross-coupled derivative, or even the homocoupled product (R = TMP) (Scheme 10).

### 3.3. Replacing cyanide with halide: Lipshutz-type cuprates

Since 2009, Mongin and co-workers have extensively documented the use of a cuprate of (TMP)₂Cu(Cl)Li₂ formulation, which has been structurally characterised as both a THF²⁹ and a diethyl ether⁵³ solvate (dimers of 9 and 14, respectively). In

<table><caption>**Table 3** Electrophilic trapping of the arylcuprate generated from N,N-diisopropylbenzamide</caption><thead><tr><th>Entry</th><th>Electrophile, conditions (E)</th><th>Yield<sup>a</sup> (%)</th></tr></thead><tbody><tr><td>1</td><td>D<sub>2</sub>O, rt, 0.5 h (D)</td><td>100</td></tr><tr><td>2</td><td>MeI, rt, 16 h (Me)</td><td>99</td></tr><tr><td>3</td><td>AllylBr, rt, 16 h (Allyl)</td><td>99</td></tr><tr><td>4</td><td>PhCOCl, 80 °C, 16 h (COPh)</td><td>84</td></tr><tr><td>5</td><td>TMSCl, 50 °C, 16 h (TMS)</td><td>99</td></tr></tbody></table>

synthetic studies, the chloride-containing cuprate was generated either from air-stable CuCl₂·TMEDA by reduction of CuII to CuI using butyllithium (1 equiv.) followed by the addition of TMPLi (2 equiv.)⁵⁶ or, more simply, from CuCl by the addition of TMPLi (2 equiv.).⁵⁷ In spite of the clear structural similarities between the chloride- (9/14) and iodide-containing

<footnote><sup>a</sup> After purification.</footnote>

<footnote><sup>a</sup> After purification.</footnote>
<figure><img src="image_41.png" /></figure>

<figure><img src="image_42.png" /><figcaption>**Scheme 10** Oxidation of arylcuprates coming from N,N-diisopropylbenzamide.</figcaption></figure>

(12/16) lithium cuprates, it is clear that the (TMP)₂Cu(Cl)Li₂ formulation base prepared in situ behaves significantly differently to the (TMP)₂Cu(I)Li₂ ³² formulation base in these systems and, instead, acts rather more like the Lipshutz formulation cuprate (TMP)₂Cu(CN)Li₂ (see above)⁶ inasmuch as it is capable of deprotonating a large range of aromatic substrates. Similar results were achieved recently utilising the bromide-containing Lipshutz-type system (viz. 10 and 15 above) though with less impressive conversions than were typically attainable with the chloride.³⁰ Taken together, these data are consistent with the view, expressed in the structural discussion above, that there is no fundamental change incurred to the cuprate on replacing X = CN (Lipshutz formulation) with X = halide (Lipshutz-type formulation) but rather, as the halide gets softer there is a general trend away from the reactivity patterns seen for the Lipshutz system. Overall, therefore, while structural evidence so far suggests the adherence of both Lipshutz and Lipshutz-type species to the general formula R₂Cu(X)Li₂, reactivity studies suggest that as the softness of X is increased it becomes reasonable to propose a gradual progression in solution to R₂CuLi·LiX.

Reaction conditions were optimized for the chloride-containing cuprate using 2,4-dimethoxypyridine as substrate. Using THF as solvent, the best yield (60%) was recorded by carrying out the reaction with the base (1 equiv.) for 2 h at room temperature before interception with benzoyl chloride. The reaction could be efficiently carried out in toluene containing TMEDA (5 equiv.), but to the detriment of the regioselectivity. Using diethyl ether instead of THF led to the expected ketone in an improved 99% yield (Scheme 11). Meanwhile, the use of mixed organo/amido lithiocuprates resulted in lower yields due to a reduced ability to effect deprotonation and the occurrence of competitive side reactions.

The cuprate generated regioselectively from 2,4-dimethoxypyrimidine could be converted into ketones using 2- and 4-chlorobenzoyl chlorides. The 5-methyl derivative was synthesized in a reasonable yield using methyl iodide whereas a low 19% yield was noted for the 5-allylated derivative (a result that could have been due to the presence of the nucleophilic diazine nitrogen) (Table 4). Using nitrobenzene as an oxidant resulted in formation of the corresponding 5,5'-bipyrimidine in 22% yield.

Reaction conditions for ketone formation were carefully optimized, taking account of both steps, using 2-methoxypyridine as substrate and benzoyl chloride to intercept the intermediate arylcuprate (Table 5). Under the conditions used

<figure><img src="image_43.png" /><figcaption>**Scheme 11** Deprotocupration–benzoylation of 2,4-dimethoxypyrimidine.</figcaption></figure>

<table><caption>**Table 4** Electrophilic trapping of the cuprate coming from 2,4-dimethoxypyrimidine</caption><thead><tr><th>Entry</th><th>Electrophile (E), temp.</th><th>Yield<sup>a</sup> (%)</th></tr></thead><tbody><tr><td>1</td><td>2-ClC<sub>6</sub>H<sub>4</sub>COCl, rt (COC<sub>6</sub>H<sub>4</sub>-2-Cl)</td><td>58</td></tr><tr><td>2</td><td>4-ClC<sub>6</sub>H<sub>4</sub>COCl, 60 °C (COC<sub>6</sub>H<sub>4</sub>-4-Cl)</td><td>52</td></tr><tr><td>3</td><td>MeI, 30 °C (Me)</td><td>62</td></tr><tr><td>4</td><td>AllylBr, rt (Allyl)</td><td>19</td></tr></tbody></table>

a After purification.

above for reaction of 2,4-dimethoxypyrimidine, the expected 3-benzoylpyridine was isolated in 82% yield. By using 0.5 equiv. of cuprate base, the yield was reduced by half, while reducing or extending the deprotonation time was deleterious for the yield.

Interestingly, the temperature at which the quenching step was conducted in the deprotocupration–benzoylation of 2-methoxypyridine was found to have an impact on the course of

<table><caption>**Table 5** Deprotocupration–benzoylation of 2-methoxypyridine</caption><thead><tr><th></th><th></th><th></th><th></th><th></th><th></th></tr><tr><th>Entry</th><th>x</th><th>Solvent</th><th>Time 1</th><th>Temp. 2</th><th>Yield<sup>a</sup> (%)</th></tr></thead><tbody><tr><td>1</td><td>1</td><td>THF</td><td>2 h</td><td>rt</td><td>82</td></tr><tr><td>2</td><td>0.5</td><td>THF</td><td>2 h</td><td>rt</td><td>40</td></tr><tr><td>3</td><td>1</td><td>THF</td><td>0.5 h</td><td>rt</td><td>72</td></tr><tr><td>4</td><td>1</td><td>THF</td><td>6 h</td><td>rt</td><td>62</td></tr><tr><td>5</td><td>1</td><td>THF</td><td>2 h</td><td>60 °C</td><td>66<sup>b</sup></td></tr><tr><td>6</td><td>1</td><td>THF</td><td>2 h</td><td>0 °C</td><td>66</td></tr><tr><td>7</td><td>1</td><td>Et<sub>2</sub>O</td><td>2 h</td><td>rt</td><td>71</td></tr><tr><td>8</td><td>1</td><td>PhMe + TMEDA (5 equiv.)</td><td>2 h</td><td>rt</td><td>49</td></tr><tr><td>9</td><td>1</td><td>Et<sub>2</sub>O + TMEDA (5 equiv.)</td><td>2 h</td><td>rt</td><td>81</td></tr></tbody></table>

a After purification. b The 3,6-disubstituted derivative was also formed in 10% yield.
the reaction. Hence, when trapping was performed at 60 °C the yield decreased on account of the competitive degradation (as observed for extended deprotonation times at room temperature). In contrast, at 0 °C the reaction proved slower. In the case of 2-methoxypyridine, switching solvent medium from THF to diethyl ether or toluene containing TMEDA did not improve the yield. A good yield was restored by using diethyl ether containing dimethyl sulfide (5 equiv.), a cosolvent which has been proven to be useful in deprotocupration reactions.⁵⁸

Besides aroyl chlorides, other electrophiles were also evaluated for their room temperature-reactivity towards the pyridyl-cuprate intermediate (Table 6). Employing 2-phenyloxirane led to both regioisomeric alcohols. Meanwhile, the use of diphenyl disulfide afforded the expected functionalized pyridine more efficiently. Reactions involving conjugate addition were only found to be possible using alkyl propionates, affording the products as (Z) and (E) mixtures in only moderate yields. By using iodine, the expected 3-iodo derivative was formed, but again in a moderate (28%) yield on account of competitive homocoupling taking place. 4-Chlorobenzenesulfonyl chloride and, to a greater extent, dimethylsulfamoyl chloride and tetramethylthiuram behaved as oxidative agents, furnishing the 3,3'-dimer. From 2-fluoropyridine, 3,3'-dimer formation was similarly noted using chlorotrimethylsilane at 50 °C (52% yield), chloranil at 60 °C (94%) and nitrobenzene at room temperature (84%).

<table><caption>**Table 6** Electrophilic trapping of the cuprate generated from 2-methoxy-pyridine</caption><thead><tr><th>Entry</th><th>Electrophile (E)</th><th>Yield(s)<sup>a</sup> (%)</th></tr></thead><tbody><tr><td>1<sup>b</sup></td><td>2-ClC<sub>6</sub>H<sub>4</sub>COCl (COC<sub>6</sub>H<sub>4</sub>-2-Cl)</td><td>56</td></tr><tr><td>2<sup>b</sup></td><td>2-BrC<sub>6</sub>H<sub>4</sub>COCl (COC<sub>6</sub>H<sub>4</sub>-2-Br)</td><td>43</td></tr><tr><td>3<sup>b</sup></td><td>2,6-dichloro-4-methyl-1,3,5-triazine (Cl<sub>2</sub>N<sub>2</sub>O<sub>2</sub>)</td><td>39</td></tr><tr><td>4</td><td>PhSSPh (SPh) (Ph<sub>3</sub>Ph<sub>2</sub>Ph<sub>2</sub>)<sub>2</sub></td><td>22 and 12</td></tr><tr><td>5</td><td>PhSSPh (SPh)</td><td>67</td></tr><tr><td>6</td><td>PhC≡CCO<sub>2</sub>Et [C(Ph)=CHCO<sub>2</sub>Et]</td><td>39 (Z) and 10<sup>c</sup> (E)</td></tr><tr><td>7</td><td>PeC≡CCO<sub>2</sub>Et [C(Pe)=CHCO<sub>2</sub>Et]</td><td>26 (E)</td></tr><tr><td>8</td><td>MeC≡CCO<sub>2</sub>Me [C(Me)=CHCO<sub>2</sub>Me]</td><td>30 (Z) and 17 (E)</td></tr><tr><td>9</td><td>I<sub>2</sub> (I)</td><td>28</td></tr><tr><td>10</td><td>4-ClC<sub>6</sub>H<sub>4</sub>SO<sub>2</sub>Cl (SO<sub>2</sub>C<sub>6</sub>H<sub>4</sub>-4-Cl)</td><td>3</td></tr><tr><td>11</td><td>Me<sub>2</sub>NSO<sub>2</sub>Cl</td><td>—</td></tr><tr><td>12</td><td>[Me<sub>2</sub>NC(S)S]</td><td>—</td></tr></tbody></table>

That azines and diazines can be functionalized through deprotonative metallation at room temperature makes the method described above of interest. Indeed, such π-deficient heterocycles are sensitive to nucleophilic attacks on their C≡N bond due to their low LUMO levels. As a consequence, traditional lithium bases, when they can be employed, in general require very low temperature reaction conditions.⁵⁹ The optimized deprotocupration-arylation conditions were thus applied to the synthesis of different azinic and diazinic ketones (Table 7).²⁸⁻³⁰,⁵⁶,⁵⁷ Good results were observed using 2-substituted pyridine substrates (with the exception of 2-bromopyridine, from which elimination of metal halide to give 2,3-pyridine was suspected),⁶⁰ with TMEDA favouring the reaction and regioselectivities being analogous to those observed using TMPLi.⁵⁹ Except for 4-methoxypyridine and 3,5-dichloropyridine, the reaction required the presence of a substituent at the position adjacent to the ring nitrogen.

In the framework of recent studies, the behaviour of 1,4-dimethoxybenzene and five-membered aromatic heterocycles towards (TMP)<sub>2</sub>Cu(Cl)Li<sub>2</sub> was also investigated (Table 8). Under the reaction conditions used for the functionalization of pyridines described above, 1,4-dimethoxybenzene was converted to its 2-allylated derivative and to diarylketones in medium yields. No improvement was noted by increasing the deprotonation temperature to 40 °C.

Continuing in the same vein, N-Boc indole, furan and thiophene were similarly reacted in the deprotocupration-arylation sequence to afford the expected ketones in approximately 50% yield. In order to reach higher yields, THF had to be replaced by either diethyl ether or diethyl ether containing dimethyl sulfide (5 equiv.). As expected, when this was undertaken, higher conversions were noted, although mixtures of 2-substituted and 2,5-disubstituted thiophenes also formed. From ethyl 2-thiophenecarboxylate and 3-thiophenecarboxylate, the reactions took place at the 5 and 2 position of the aromatic ring respectively, but with a lower chemoselectivity in the latter case. Finally, it was noted that the trapping temperature had an important impact on the efficiency on the reaction, with the best yields being obtained at 60 °C (Table 9).

Whereas the arylcuprates prepared from N,N-diisopropylbenzamide using different RCu(TMP)(CN)Li<sub>2</sub> bases were converted to the 2-methylated (R = Me) or the 2-phenylated (R = Ph) cross-coupled derivative upon treatment by nitrobenzene (Scheme 10),⁶ the arylcuprates obtained by deprotocupration using (TMP)<sub>2</sub>Cu(Cl)Li<sub>2</sub> could be utilised in palladium-catalysed cross-couplings with aryl halides such as 4-iodoanisole and 2-bromopyridine in the presence of catalytic amounts of PdCl<sub>2</sub>(PPh<sub>3</sub>)<sub>2</sub> and dppf (1,1'-bis(diphenylphosphino)ferrocene) (Table 10).⁵⁷

Compared with the reactivities of previously reported lithium-zinc bases, it is clear that the lithiocuprate (TMP)<sub>2</sub>Cu(Cl)Li<sub>2</sub> behaves more like a lithium amide, as it leads to deprotonation of the most acidic hydrogen atoms and is incompatible with reactive functional groups. This, however, is offset by a satisfying reactivity towards a larger range of electrophiles.

<figure><img src="image_44.png" /></figure>

<footnote><sup>a</sup>After purification. <sup>b</sup> Base prepared in the presence of TMEDA (1 equiv.). <sup>c</sup> Estimated yield.</footnote>
<table><caption>**Table 7** Deprotocupration–arylation of azine and diazine substrates</caption><thead><tr><th>Entry</th><th>ClCOAr'</th><th>Product</th><th>Yield<sup>a</sup> (%)</th><th>Entry</th><th>ClCOAr'</th><th>Product</th><th>Yield<sup>a</sup> (%)</th></tr></thead><tbody><tr><td>1</td><td>ClO-CF<sub>3</sub></td><td>MeO-N<sub>2</sub>OCF<sub>3</sub></td><td>60</td><td>16</td><td>ClO-Ph</td><td>Cl<sub>2</sub>COPh</td><td>41<sup>b</sup> (C3), 24<sup>b</sup> (C2)</td></tr><tr><td>2<sup>b</sup></td><td>ClO-Cl</td><td>MeO-N<sub>2</sub>OCF<sub>3</sub></td><td>91</td><td>17</td><td>ClO-Ph</td><td>Cl<sub>2</sub>COPh</td><td>42<sup>b</sup></td></tr><tr><td>3<sup>b</sup></td><td>ClO-Cl</td><td>OMe-N<sub>2</sub>OCF<sub>3</sub></td><td>57</td><td>18</td><td>ClO-Ph</td><td>Cl<sub>2</sub>COPh</td><td>70<sup>b</sup></td></tr><tr><td>4</td><td>ClO-R</td><td>N<sub>2</sub>OCF<sub>3</sub></td><td>85 (R = H)<br>76 (R = 2-Cl)<br>83 (R = 4-Cl)<br>92 (R = 4-CF<sub>3</sub>)</td><td>19</td><td>ClO-Ph</td><td>Cl<sub>2</sub>COPh</td><td>33<sup>b</sup></td></tr><tr><td>8</td><td>ClO-N<sub>2</sub>Cl</td><td>N<sub>2</sub>OCF<sub>3</sub></td><td>72</td><td>20</td><td>ClO-Ph</td><td>Cl<sub>2</sub>COPh</td><td>55<sup>b</sup></td></tr><tr><td>9</td><td>ClO-R</td><td>N<sub>2</sub>OCF<sub>3</sub></td><td>90<sup>b</sup> (R = H)<br>59<sup>b</sup> (R = 2-Cl)<br>80<sup>b</sup> (R = 4-Cl)<br>80<sup>b</sup> (R = 4-OMe)<br>66<sup>b</sup> (R = 3-OMe)</td><td>21</td><td>ClO-Ph</td><td>Cl<sub>2</sub>COPh</td><td>80</td></tr><tr><td>14</td><td>ClO-N<sub>2</sub>Cl</td><td>N<sub>2</sub>OCF<sub>3</sub></td><td>65<sup>b</sup></td><td>22</td><td>ClO-Ph</td><td>Cl<sub>2</sub>COPh</td><td>21</td></tr><tr><td>15</td><td>ClO-Ph</td><td>N<sub>2</sub>OCF<sub>3</sub></td><td>20</td><td>23</td><td>ClO-Ph</td><td>MeO-N<sub>2</sub>COPh</td><td>78<sup>b</sup></td></tr></tbody></table>

### 3.4. New amidocuprate adducts and the formation of reactive species

Lastly, and in line with the investigation of less expensive amide ligands,⁵¹ the effect of replacing TMP with DMP has been studied by Harford *et al.*⁵³ As noted above, attempts to fabricate Lipshutz-type cuprates analogous to 9, 10, 12 and 14–16 instead afforded the series of complexes 28, 29, 31 and 32 that have been interpreted as adducts between Lipshutz-type and Gilman cuprates. The potential importance of this new structure-type is explained fully in the final section of this

review where DFT analysis has suggested that the abstraction of LiX from Lipshutz or Lipshutz-type cuprates is fundamental to incurring *in situ* formation of the reactive base in DoC. It is clear, therefore, that these new adducts can all be viewed in terms of the elimination of 1 equiv. LiX having occurred from the corresponding Lipshutz-type dimer (e.g. 14<sub>2</sub> → 28 + LiCl). Crucial to this view of their importance, using the base prepared *in situ* from DMPLi (4 equiv.) and CuBr (2 equiv.) in THF, N,N-diisopropylbenzamide was readily converted to the corresponding 2-metallated derivative, as shown by subsequent trapping with iodine (80% yield). An essentially

<footnote><sup>a</sup> After purification. <sup>b</sup> Base prepared in the presence of TMEDA (1 equiv.).</footnote>
<table><caption>**Table 10** Palladium-catalysed cross-coupling of arylcuprates</caption><thead><tr><th>Entry</th><th>XAr'</th><th>Product</th><th>Yield<sup>a</sup> (%)</th></tr></thead><tbody><tr><td>1</td><td>X<sup>R</sup></td><td></td><td>64 (X = I, R = OMe)</td></tr><tr><td>2</td><td></td><td></td><td>46 (X = Br, R = OMe)</td></tr><tr><td>3</td><td></td><td></td><td>47 (X = Br, R = F)</td></tr><tr><td>4</td><td></td><td></td><td>64 (X = Br, R = CO<sub>2</sub>Et)</td></tr><tr><td>5</td><td></td><td></td><td>51 (Y = CH, Z = N)</td></tr><tr><td>6</td><td></td><td></td><td>42, 46<sup>b</sup> (Y = Z = N)</td></tr><tr><td>7</td><td></td><td></td><td>39<sup>b</sup></td></tr><tr><td>8</td><td></td><td></td><td>63 (R = H)</td></tr><tr><td>9</td><td></td><td></td><td>54 (R = OMe)</td></tr><tr><td>10</td><td></td><td></td><td>44</td></tr><tr><td>11</td><td></td><td></td><td>36<sup>b</sup></td></tr></tbody></table>

<sup>a</sup> After purification. <sup>b</sup> Deprotonation step performed at 40 °C.

Results suggested higher-order models to be at least 20 kcal mol⁻¹ higher in energy than their lower-order counterparts and that spectroscopic data suggesting higher-order structures could be accommodated by metallocyclic bridged structures containing linear, lower-order copper.⁶² Of most interest, a tandem EXAFS/ab initio study assessed a variety of structural possibilities for the formulation Me₂Cu(CN)Li₂ and concluded that there was a strong likelihood that the structure was as shown in Fig. 19.⁶¹ Plainly, this corresponds closely with that recently noted for complexes 7 and 13 by X-ray diffraction in which the cyanide group bonds only to alkali metal centres.⁶

<figure><img src="image_45.png" /><figcaption>**Fig. 19** Preferred ab initio structure of alkylcuprate Me₂Cu(CN)Li₂.</figcaption></figure>

More recently, among the organocuprate(i) complexes receiving increased attention have been heteroleptic cuprates ([R-Cu-R']⁻). Organyl(amido)cuprates represent an important class of these, particularly since they have now been harnessed to achieve a variety of organic transformations. Thus, 2007 saw publication of the first of several reports that TMP-cuprates of the type RCu(TMP)(CN)Li₂ (R = alkyl, phenyl, TMP) could promote the highly chemoselective DoC of multifunctionalized aromatic compounds.⁶,³⁴,⁵⁷ The arylcuprate intermediates presumed to result from deprotometallation of the aromatic substrate were effectively employed not only in the trapping of electrophiles, but also in oxidative ligand coupling to form new C–C bonds with alkyl/aryl groups (see section 3.2).

The chemistry of organocuprates(i) has traditionally been dominated by two structure types: Gilman cuprates and Lipshutz(-type) cuprates. As revealed above, these have now been structurally elucidated, with the former capable of exhibiting a homodimeric structure and Lipshutz-type cuprates demonstrating heteroaggregate structures based on metallocycles that are either 6-membered (halide-containing) or 7-membered (cyanide-containing, Scheme 12). Overall, with the help of X-ray crystallography, structure–reactivity relationship studies of TMP-cuprates have revealed that (1) the cyclic dimer of Gilman cuprate (TMP)₂CuLi is unreactive in DoC and (2) a variety of Lipshutz-type amidocuprates, including (TMP)₂Cu(CN)Li₂, exhibit enhanced deprotonative reactivity.³²

Further insights into the natures of active cuprate species and the mechanisms by which they exhibit DoC have been gained through DFT study of the derivatisation of N,N-dimethylbenzamide. The deprotonation process using MeCu(NMe₂)(CN)Li₂·2OMe₂ as a model Lipshutz cuprate is summarized in Scheme 13.³²

<figure><img src="image_46.png" /><figcaption>**Scheme 12** Structures of Gilman and Lipshutz-type cuprates (top) and monoGilman-type cuprates with solvent coordination (bottom, S = solvent molecule).</figcaption></figure>

<figure><img src="image_47.png" /></figure>
<figure><img src="image_48.png" /><figcaption>Deprotonation by an amido ligand</figcaption></figure>

<figure><img src="image_49.png" /><figcaption>Ligand exchange process - Deprotonation of Me₂NH by an alkyl ligand</figcaption></figure>

**Scheme 13** Proposed reaction pathways for the DoC of N,N-dimethylbenzamide using Lipshutz cuprate MeCu(NMe₂)(CN)Li₂·2OMe₂. Energy changes and bond lengths at the B3LYP/6-31+G* and SVP (Cu) level of theory are shown in kcal mol⁻¹ and Å, respectively.

In common with the reaction pathways previously proposed for TMP-zincates²,⁴⁷ and TMP-aluminates,⁴⁶ two plausible pathways were discovered for regioselective DoM (Directed *ortho* Metallation). These differ in terms of whether the deprotonation step is triggered by the amido or the alkyl ligand in the cuprate. Although in Scheme 13 the formation of **IM2**<sub>L</sub> represents a thermodynamically favorable outcome, the pathway by which the alkyl ligand promotes the *ortho* deprotonation (**IM1**<sub>L</sub>-**TS1**<sub>L</sub>-**IM2**<sub>L</sub>) is kinetically unfavorable on account of there being a relatively high energy transition state (TS<sub>1</sub><sub>L</sub>, ΔG‡ = 40.8 kcal mol<sup>-1</sup>). In contrast, TS<sub>2</sub><sub>L</sub> represents the transition state immediately preceding amido ligand-promoted deprotonation (**IM3**<sub>L</sub>-**TS2**<sub>L</sub>-**IM4**<sub>L</sub>). While the activation barrier to TS<sub>2</sub><sub>L</sub> formation is somewhat high (+27.7 kcal mol<sup>-1</sup>) relative to reaction pre-complex **IM3**<sub>L</sub>, it is still reasonably accessible and can be viewed as allowing metalated intermediate **IM4**<sub>L</sub> to form. The ligand exchange step (**IM5**<sub>L</sub>-**TS3**<sub>L</sub>-**IM2**<sub>L</sub>), a process seen in TMP-zincate chemistry⁴⁷ but not in TMP-aluminate chemistry,⁴⁶ has a higher activation barrier (+31.3 kcal mol<sup>-1</sup>). Taken together with the observation of heterocoupling processes achieved using organyl(amido)cuprate reagents (discussed in section 3.2) it is reasonable to conclude that the ligand exchange step would be difficult in DoC.

Interestingly, investigations into possible DoC pathways using the Lipshutz reagent MeCu(NMe₂)(CN)Li₂·2OMe₂ have led to the identification of another *ortho* cupration pathway that involves an *active monomeric Gilman complex* (Scheme 12,

bottom). Importantly, the monomeric structure-type of this so-called *mono*Gilman species has been established experimentally using TMP-cuprates isolated from various Lewis basic media.³⁴ Calculations that take the Lipshutz reagent MeCu(NMe₂)(CN)-Li₂·2OMe₂ as a starting point suggest that the *mono*Gilman complexes **IM1**<sub>G</sub> and **IM3**<sub>G</sub> can be formed by the elimination of solvated LiCN (Scheme 14). Although **IM1**<sub>G</sub> is more stable than **IM3**<sub>G</sub>, its alkyl ligand fails to promote the deprotonative step in the reaction (**IM1**<sub>G</sub>-**TS1**<sub>G</sub>-**IM2**<sub>G</sub>), this sequence having a very high activation energy (+40.3 kcal mol<sup>-1</sup>). In contrast, the pathway **IM3**<sub>G</sub>-**TS2**<sub>G</sub>-**IM4**<sub>G</sub>, in which deprotonation is promoted by the amido ligand in the *mono*Gilman base, has a very low activation barrier (+14.9 kcal mol<sup>-1</sup> with respect to **IM3**<sub>G</sub>) *en route* to **IM4**<sub>G</sub>. Although the total activation energy (26.0 kcal mol<sup>-1</sup>) from **RT**<sub>L</sub> to **TS2**<sub>G</sub> is comparable to that from **RT**<sub>L</sub> to **TS2**<sub>L</sub> (23.8 kcal mol<sup>-1</sup>, in Scheme 13), it is noteworthy that the *mono*Gilman-pathway *does not require more than 15 kcal mol<sup>-1</sup> for any individual step*, and this contrasts with the Lipshutz pathway (which requires more than 27 kcal mol<sup>-1</sup> for the deprotonation step **IM3**<sub>L</sub>-**TS2**<sub>L</sub>). As with the Lipshutz system, quenching of the amine Me₂NH (**IM5**<sub>G</sub>-**TS3**<sub>G</sub>-**IM2**<sub>G</sub>) appears to be unlikely to proceed on account of the rather high energy difference between **RT**<sub>L</sub> and **TS3**<sub>G</sub> (more than 28 kcal mol<sup>-1</sup>), though the activation barrier to reach **TS3**<sub>G</sub> is entropically permissible at 22.4 kcal mol<sup>-1</sup>.

Oxidative ligand coupling involving the putative arylcuprate intermediate generated from the DoC of N,N-diisopropylbenza-
### Deprotonation by an alkyl ligand

<figure><img src="image_50.png" /></figure>

### Deprotonation by an amido ligand

<figure><img src="image_51.png" /></figure>

### Ligand exchange process - Deprotonation of Me₂NH by an alkyl ligand

<figure><img src="image_52.png" /><figcaption>**Scheme 14** Reaction pathways for the DoC of N,N-dimethylbenzamide using Lipshutz cuprate MeCu(NMe₂)(CN)Li₂·2OMe₂ and proceeding via a *mono*Gilman intermediate. Energy changes and bond lengths at the B3LYP/6-31+G* and SVP (Cu) level of theory are shown in kcal mol⁻¹ and Å, respectively.</figcaption></figure>

<figure><img src="image_53.png" /><figcaption>**Scheme 15** Oxidative ligand coupling employing an arylcuprate intermediate.</figcaption></figure>

mide by MeCu(TMP)(CN)Li₂ has been discussed in section 3.2 – with the use of nitrobenzene affording 2-methyl-N,N-diisopropylbenzamide (Scheme 15).⁶ This result clearly shows that the methyl ligand is retained by the copper centre in the arylcuprate intermediate and this bears out the theoretical work described here. A significant increase in the activation energy of deprotonation starting from a Gilman *dimer* has been found theoretically,³² again in agreement with experimental findings described in this section.

The most recent structural studies into bis(amido)cuprates have revealed the formation of triangulated complexes best viewed as adducts between Gilman and Lipshutz-type monomers. These are discussed in detail in section 2.4. Moreover, the adduct [(DMP)₂CuLi·OEt₂]₂LiBr 29 has been shown (see section 3.4) to be an effective DoC reagent.⁵³ In the wake of recent DFT work, this has led to speculation that the adduct can deaggregate to give an active *mono*Gilman base. In this vein, preliminary calculations on the simplified Lipshutz-type
<figure><img src="image_54.png" /><figcaption>**Scheme 16** The interconversion of a Lipshutz-type and a Gilman dimer ($L_D$ and $G_D$) at B3LYP/631SVP level ($ΔE$ [$ΔG$] are in kcal mol$^{-1}$). "LiCl" = $1/4[\text{LiCl}((\text{OMe}_2)]_4 - \text{OMe}_2$.</figcaption></figure>

dimer of $(\text{Me}_2\text{N})_2\text{Cu(Cl)}\text{Li}_2 \cdot \text{OMe}_2$ ($L_D$) have revealed an enthalpic preference for eliminating a solvated lithium halide to form Gilman dimer $G_D$ via adduct $L_M G_M$, though the effects of entropy mean that the system is a finely balanced one, as reflected by the very small values of $ΔG$ (Scheme 16).

A further important step that it is necessary for $L_M G_M$ to participate in if it is to be viewed as a contender for DoC is its dissociation to generate $L_M$ and the participation of this in a pre-reaction complex with, for example, N,N-dimethylbenzamide. Data point to this sequence increasing $ΔG$ by 6.1 kcal mol$^{-1}$ with the initial dissociation of $L_M G_M$ raising $ΔG$ by 15.4 kcal mol$^{-1}$ (Scheme 17). In comparison to the $\text{IM3G-}TS2_G-\text{IM4}_G$ pathway modelled above (see Scheme 14) for sourcing monoGilman agents from a Lipshutz cuprate starting material, it is clear that the recently reported cuprate adducts can also be viewed as viable sources of monoGilman active species. This is consistent with their demonstrated ability (discussed in section 3.4) as DoC reagents.⁵³

To summarize, DoM using Lipshutz-type amidocuprates or amidocuprate adducts can be viewed as proceeding *via* the formation of a monoGilman intermediate, and in organyl(amido)-cuprate systems the alkyl ligand is retained by the copper centre in the intermediate arylcuprate species, indicating that ligand scrambling does not occur.

<figure><img src="image_55.png" /><figcaption>**Scheme 17** Conversion of adduct $L_M G_M$ to a monoGilman-(N,N-dimethylbenzamide) complex ($\text{IM1}_G$) at B3LYP/631SVP level.</figcaption></figure>

## 5. Conclusions

The relatively new field of directed aromatic *ortho* metallation using synergic reagents has been significantly expanded through the deployment of lithium cuprates. Though these systems are not new in themselves it is only recently that unambiguous structural evidence for their nature has been forthcoming. Subsequent to spectroscopic and theoretical investigations on cyanide-containing lithium cuprates, it was only in 1998 that the first clear evidence for the behaviour of the cyanide ion was presented.²³,²⁴ More recently, the crystallographic elucidation of 7 revealed that the classic Lipshutz system $(\text{TMP})_2\text{Cu(CN)}\text{Li}_2 \cdot \text{THF}$ incorporated bonds between cyanide and lithium, with the lower polarity metal being ligated only by two diametrically opposed amide ligands.⁶ Gratifyingly, this observation was concordant with calculations reported as long ago as 1995!⁶¹ Subsequent to this, it rapidly became apparent that the replacement of cyanide with halide (= X) in $(\text{TMP})_2\text{Cu(X)}\text{Li}_2 \cdot \text{THF}$ (X = Cl 9, Br 10, I 12) had no very significant effect on lithium cuprate structure. This allows cyanide- and halide-containing TMP-cuprates to be discussed in terms of the existence of a series of cuprates that can be regarded as, to a greater or lesser extent, Lipshutz-type. This can be interpreted in terms of the elimination of LiX to give a Gilman cuprate (which is highly active, see below), though we have also seen that if X is very soft then unreactive Gilman dimers may be isolated. It should also be noted, though, that the observation of a common Lipshutz-type cuprate dimer for various X groups is also consistent with the recent suggestion that differing reactivities of cyanide and iodide complexes may be defined by the structures of reaction intermediates rather than those of the substrates themselves.⁷ That said, the general inefficiency of Gilman reagents in DoC is clear. The implication of these data is that for DoC to proceed with optimum efficiency, a Lipshutz-type cuprate is necessary as the starting point.

Recent calculations have added a remarkable new insight to the structural and synthetic data noted above. Namely, that whereas the employment of a Lipshutz-type cuprate is necessary for efficient DoC to proceed (as evidenced synthetically and also proposed on the basis of reaction coordinates plotted in the previous section), the active species is a Gilman monomer created *in situ* by the expulsion of LiX from the Lipshutz-type substrate. DFT analysis reveals a compelling reaction pathway
<figure><img src="image_56.png" /></figure>

for the elimination of LiX prior to formation of a pre-reaction complex between aromatic substrate and Gilman monomer and, interestingly, also suggests that the formation of a reactive Gilman monomer from the corresponding dimer is, in fact, relatively unlikely. Again, this is borne out by structural and synthetic work.

Most recently, the isolation and characterisation of a new class of lithium cuprate that is best viewed as representing an adduct between Lipshutz-type and Gilman monomers has presented a new way of envisaging the *in situ* generation of reactive cuprates for DoC. The abstraction of LiX from a Lipshutz-type dimer turns out to be enthalpically plausible. Moreover, calculations suggest that deaggregation of the resulting adduct and coordination of the formed (active) Gilman monomer by an aromatic substrate provides another compelling pathway for DoC. Overall, it is clear that, like Lipshutz-type dimers, the triangulated adducts reported here can be interpreted as plausible sources of the active cuprate species required for DoC.

The interpretation of theoretical data in terms of solid-state structures has afforded significant new insights into routes towards active *mono*Gilman species. For example, adducts such as **28** have introduced new possibilities regarding the elimination of LiX from Lipshutz-type cuprates. Of course, these data have implications for our view of the solution behaviour of lithium cuprates and direct monitoring of the aggregation behaviour of these systems in solution, examples of which have been reported recently,⁴² will represent an increasingly significant part of forthcoming work. Attention is also turning to heteroleptic cuprates. Though these are reported for **19** and **20**, heteroleptic bis(amido)cuprates represent the next target for structural elucidation and it is expected that they will be able to take two forms: the first will be mixed dimers or adducts such as $(AM)_2Cu(X)Li_2 \cdot (AM')_2Cu(X)Li_2$ and $(AM)_2Cu(X)Li_2 \cdot (AM')_2CuLi$ while the second will take the form of structures that incorporate heteroleptic monomers such as AMCu$(AM')(X)Li_2$ (where AM and AM' are different amides). This work is rendered particularly important by the observation of distinctly contrasting amide orientations (cf. TMP in **14**₂ and DMP in **28**) and attempts to fabricate mixed DMP/TMP-cuprates are ongoing. Moreover, the ability of DMP to result in relatively inexpensive cuprating agents opens up new possibilities in terms of varying the amide components of cuprate bases (e.g., different ring size, substitution pattern, introducing chirality) in order to develop a full understanding of the steric requirements necessary for effective DoC.

## Acknowledgements

Much of this work was supported by the U.K. EPSRC (EP/J500380/1). A.W. would like to acknowledge the graduate students who have contributed to the work in the past (Drs James Morey and Joanna Haywood) and also the GB Sasakawa and Daiwa Foundations and the Royal Society for support with travel and international collaboration. A.W. and M.U. thank

the Japan Society for the Promotion of Science. M.U. and R.T. acknowledge Drs Shinsuke Komagawa, Shinya Usui, Ching-Yuan Liu, Yotaro Matsumoto and Keiichi Hirano, and Professors Yuichi Hashimoto, Shuji Yasuike and Jyoji Kurita for their contributions to the work. M.U. also thanks JSPS KAKENHI (S) (No. 24229011), Takeda Science Foundation, The Asahi Glass Foundation, Daiichi-Sankyo Foundation of Life Sciences, Mochida Memorial Foundation, Tokyo Biochemical Research Foundation, Foundation NAGASE Science Technology Development, Yamada Science Foundation and Sumitomo Foundation. R.T. acknowledges JSPS Grant-in-Aid for Young Scientists (A) (No. 25713001). F.C. and F.M. would like to acknowledge the graduate students who have contributed to the work (Dr Tan Tai Nguyen and Ms Nada Marquise) and the Agence Nationale de la Recherche (ACTIVATE program) for financial support. F.M. also thanks the Institut Universitaire de France and Rennes Métropole. Thanks go to Professor Paul Raithby and Dr Tom Robinson (Bath) for X-ray crystallographic studies. Calculations were performed on the RIKEN Super Combined Cluster (RSCC) and RIKEN Integrated Cluster of Clusters (RICC).

## References

1. (a) H. W. Gschwend and H. R. Rodriguez, *Org. React.*, 1979, **26**, 1; (b) P. Beak and V. Snieckus, *Acc. Chem. Res.*, 1982, **15**, 306; (c) V. Snieckus, *Chem. Rev.*, 1990, **90**, 879; (d) T. G. Gant and A. I. Meyers, *Tetrahedron*, 1994, **50**, 2297; (e) M. Schlosser, *Organometallics in Synthesis*, ed. M. Schlosser, Wiley, New York, 2nd edn, 2002, ch. 1.

2. Y. Kondo, M. Shilai, M. Uchiyama and T. Sakamoto, *J. Am. Chem. Soc.*, 1999, **121**, 3539.

3. (a) R. E. Mulvey, *Organometallics*, 2006, **25**, 1060; (b) R. E. Mulvey, F. Mongin, M. Uchiyama and Y. Kondo, *Angew. Chem., Int. Ed.*, 2007, **46**, 3802; (c) R. E. Mulvey, *Acc. Chem. Res.*, 2009, **42**, 743; (d) B. Haag, M. Mosrin, H. Ila, V. Malakhov and P. Knochel, *Angew. Chem., Int. Ed.*, 2011, **50**, 9794; (e) F. Mongin and M. Uchiyama, *Curr. Org. Chem.*, 2011, **15**, 2340; (f) R. E. Mulvey, *Dalton Trans.*, 2013, **42**, 6676; (g) F. Mongin and A. Harrison-Marchand, *Chem. Rev.*, 2013, **113**, 7563.

4. (a) G. Wittig, *Angew. Chem.*, 1958, **70**, 65; (b) W. Tochtermann, *Angew. Chem., Int. Ed. Engl.*, 1966, **5**, 351.

5. A. Harrison-Marchand and F. Mongin, *Chem. Rev.*, 2013, **113**, 7470.

6. S. Usui, Y. Hashimoto, J. V. Morey, A. E. H. Wheatley and M. Uchiyama, *J. Am. Chem. Soc.*, 2007, **129**, 15102.

7. M. Neumeier and R. M. Gschwind, *J. Am. Chem. Soc.*, 2014, **136**, 5765.

8. H. Gilman, R. Jones and L. Woods, *J. Org. Chem.*, 1952, **17**, 1630.

9. H. House, W. Respess and G. Whitesides, *J. Org. Chem.*, 1966, **31**, 3128.

10. B. H. Lipshutz, R. S. Wilhelm and D. M. Floyd, *J. Am. Chem. Soc.*, 1981, **103**, 7672.
Perspective

11 G. Whitesides, W. Fisher, J. San Filipo, R. Bashe and H. House, *J. Am. Chem. Soc.*, 1969, **91**, 4871.

12 P. G. Edwards, R. W. Gellert, M. W. Marks and R. Bau, *J. Am. Chem. Soc.*, 1982, **104**, 2072.

13 H. Hope, D. Oram and P. P. Power, *J. Am. Chem. Soc.*, 1984, **106**, 1149.

14 (a) G. van Koten and J. G. Noltes, *J. Chem. Soc., Chem. Commun.*, 1972, 940; (b) G. van Koten, J. T. B. H. Jastrzebski, F. Muller and C. H. Stam, *J. Am. Chem. Soc.*, 1985, **107**, 697.

15 G. van Koten and J. G. Noltes, *J. Am. Chem. Soc.*, 1979, **101**, 6593.

16 H. Hope, M. Olmstead, P. Power, J. Sandell and X. Xu, *J. Am. Chem. Soc.*, 1985, **107**, 4337.

17 H. O. House, D. G. Koepsell and W. J. Campbell, *J. Org. Chem.*, 1972, **37**, 1003.

18 S. Bertz, *J. Am. Chem. Soc.*, 1990, **112**, 4031.

19 B. H. Lipshutz, S. Sharma and E. L. Ellsworth, *J. Am. Chem. Soc.*, 1990, **112**, 4032.

20 J. Snyder, D. Spangler, J. Behling and B. Rossiter, *J. Org. Chem.*, 1994, **59**, 2665.

21 B. Lipshutz and B. James, *J. Org. Chem.*, 1994, **59**, 7585.

22 J. Snyder and S. Bertz, *J. Org. Chem.*, 1995, **60**, 4312.

23 C. Kronenberg, J. Jastrzebski, A. Spek and G. van Koten, *J. Am. Chem. Soc.*, 1998, **120**, 9688.

24 G. Boche, F. Bosold, M. Marsch and K. Harms, *Angew. Chem., Int. Ed.*, 1998, **37**, 1684.

25 D. R. Armstrong, D. Barr, R. Snaith, W. Clegg, R. E. Mulvey, K. Wade and D. Reed, *J. Chem. Soc., Dalton Trans.*, 1987, 1071.

26 D. R. Armstrong, D. Barr, W. Clegg, S. M. Hodgeson, R. E. Mulvey, D. Reed, R. Snaith and D. S. Wright, *J. Am. Chem. Soc.*, 1989, **111**, 4719.

27 P. Reiss and D. Fenske, *Z. Anorg. Allg. Chem.*, 2000, **626**, 1317.

28 K. Snégaroff, T. T. Nguyen, N. Marquise, Y. S. Halauko, P. J. Harford, T. Roisnel, V. E. Matulis, O. A. Ivashkevich, F. Chevallier, A. E. H. Wheatley, P. C. Gros and F. Mongin, *Chem. – Eur. J.*, 2011, **17**, 13284.

29 N. Marquise, P. J. Harford, F. Chevallier, T. Roisnel, A. E. H. Wheatley, P. C. Gros and F. Mongin, *Tetrahedron Lett.*, 2013, **54**, 3154.

30 N. Marquise, P. J. Harford, F. Chevallier, T. Roisnel, V. Dorcet, A.-L. Gagez, S. Sablé, L. Picot, V. Thiéry, A. E. H. Wheatley, P. C. Gros and F. Mongin, *Tetrahedron*, 2013, **69**, 10123.

31 C. M. P. Kronenburg, C. H. M. Amijs, J. T. B. H. Jastrzebski, M. Lutz, A. L. Spek and G. van Koten, *Organometallics*, 2002, **21**, 4662.

32 S. Komagawa, S. Usui, J. Haywood, P. J. Harford, A. E. H. Wheatley, Y. Matsumoto, K. Hirano, R. Takita and M. Uchiyama, *Angew. Chem., Int. Ed.*, 2012, **51**, 12081.

33 R. P. Davies, *Coord. Chem. Rev.*, 2011, 255, 1226.

34 J. Haywood, J. V. Morey, A. E. H. Wheatley, C.-Y. Liu, S. Yasuike, J. Kurita, M. Uchiyama and P. R. Raithby, *Organometallics*, 2009, **28**, 38.

35 (a) S. Gambarotta, S. Strologo, C. Floriani and A. Chiesi-Villa, *Organometallics*, 1984, **3**, 1444; (b) A. M. Dattelbaum and J. D. Martin, *Polyhedron*, 2006, **25**, 349; (c) R. Fischer, H. Gorls and M. Westerhausen, *Organometallics*, 2007, **26**, 3269.

36 (a) H. Hope, M. M. Olmstead, P. P. Power, J. Sandell and X. Xu, *J. Am. Chem. Soc.*, 1985, **107**, 4337; (b) R. P. Davies and S. Hornauer, *Eur. J. Inorg. Chem.*, 2005, 51.

37 R. P. Davies and S. Hornauer, *Chem. Commun.*, 2007, 304.

38 (a) M. Niemeyer, *Organometallics*, 1998, **17**, 4649; (b) C.-S. Hwang and P. P. Power, *Bull. Korean Chem. Soc.*, 2003, **24**, 605.

39 (a) C.-S. Hwang and P. P. Power, *J. Am. Chem. Soc.*, 1998, **120**, 6409; (b) C.-S. Hwang and P. P. Power, *J. Am. Chem. Soc.*, 1999, **18**, 697.

40 R. Bomparola, R. P. Davies, T. Gray and A. J. P. White, *Organometallics*, 2009, **28**, 4632.

41 R. M. Gschwind, *Chem. Rev.*, 2008, **108**, 3029.

42 R. P. Davies, S. Hornauer and P. B. Hitchcock, *Angew. Chem., Int. Ed.*, 2007, **46**, 5191.

43 (a) R. K. Dieter and M. Tokles, *J. Am. Chem. Soc.*, 1987, **109**, 2040; (b) R. K. Dieter and T. W. Hanks, *Organometallics*, 1992, **11**, 3549; (c) B. E. Rossiter, M. Eguchi, G. Miao, N. M. Swingle, A. E. Hernandez, D. Vickers, E. Fluckiger, R. G. Patterson and K. V. Reddy, *Tetrahedron*, 1993, **49**, 965.

44 M. John, C. Auel, C. Behrens, M. Marsch, K. Harms, F. Bosold, R. M. Gschwind, P. R. Rajamohanan and G. Boche, *Chem. – Eur. J.*, 2000, **6**, 3060.

45 S. F. Martin, J. R. Fishpaugh, J. M. Power, D. M. Giolando, R. A. Jones, C. M. Nunn and A. H. Cowley, *J. Am. Chem. Soc.*, 1988, **110**, 7226.

46 (a) M. Uchiyama, H. Naka, Y. Matsumoto and T. Ohwada, *J. Am. Chem. Soc.*, 2004, **126**, 10526; (b) H. Naka, M. Uchiyama, Y. Matsumoto, A. E. H. Wheatley, M. McPartlin, J. V. Morey and Y. Kondo, *J. Am. Chem. Soc.*, 2007, **129**, 1921; (c) J. García-Álvarez, E. Hevia, A. R. Kennedy, J. Klett and R. E. Mulvey, *Chem. Commun.*, 2007, 2402; (d) H. Naka, J. V. Morey, J. Haywood, D. J. Eisler, M. McPartlin, F. García, H. Kudo, Y. Kondo, M. Uchiyama and A. E. H. Wheatley, *J. Am. Chem. Soc.*, 2008, **130**, 16193.

47 (a) M. Uchiyama, T. Miyoshi, Y. Kajihara, T. Sakamoto, Y. Otani, T. Ohwada and Y. Kondo, *J. Am. Chem. Soc.*, 2002, **124**, 8514; (b) W. Clegg, S. H. Dale, E. Hevia, G. W. Honeyman and R. E. Mulvey, *Angew. Chem., Int. Ed.*, 2006, **45**, 2370; (c) M. Uchiyama, Y. Matsumoto, D. Nobuto, T. Furuyama, K. Yamaguchi and K. Morokuma, *J. Am. Chem. Soc.*, 2006, **128**, 8748; (d) Y. Kondo, J. V. Morey, J. M. Morgan, P. R. Raithby, D. Nobuto, M. Uchiyama and A. E. H. Wheatley, *J. Am. Chem. Soc.*, 2007, **129**, 12734; (e) W. Clegg, J. Garcia-Álvarez, P. Garcia-Álvarez, D. V. Graham, R. W. Harrington, E. Hevia, A. R. Kennedy, R. E. Mulvey and L. Russo, *Organometallics*, 2008, 27, 2654.

48 J. Garcia-Álvarez, A. R. Kennedy, J. Klett and R. E. Mulvey, *Angew. Chem., Int. Ed.*, 2007, **46**, 1105.
49 J. M. Cole, P. G. Waddell, A. E. H. Wheatley, G. J. McIntyre, A. J. Peel, C. W. Tate and D. J. Linton, *Organometallics*, 2014, DOI: 10.1021/om500271p.

50 P. P. Power, K. Ruhlandt-Senge and S. C. Shoner, *Inorg. Chem.*, 1991, **30**, 5013.

51 (a) R. Campbell, B. Conway, G. S. Fairweather, P. García-Álvarez, A. R. Kennedy, J. Klett, R. E. Mulvey, C. T. O'Hara and G. M. Robertson, *Dalton Trans.*, 2010, 511; (b) B. Conway, P. García-Álvarez, A. R. Kennedy, J. Klett, R. E. Mulvey and S. D. Robertson, *New J. Chem.*, 2010, **34**, 1707.

52 D. R. Armstrong, J. A. Garden, A. R. Kennedy, S. A. Leenhouts, R. E. Mulvey, P. O'Keefe, C. T. O'Hara and A. Steven, *Chem. – Eur. J.*, 2013, **19**, 13492.

53 P. J. Harford, A. J. Peel, J. P. Taylor, S. Komagawa, P. R. Raithby, T. P. Robinson, M. Uchiyama and A. E. H. Wheatley, *Chem. – Eur. J.*, 2014, **20**, 3908.

54 C. M. P. Kronenburg, J. T. B. H. Jastrzebski, J. Boersma, M. Lutz, A. L. Spek and G. van Koten, *J. Am. Chem. Soc.*, 2002, **124**, 11675.

55 H.-J. Gais, C. V. Rao and R. Loo, *Chem. – Eur. J.*, 2008, **14**, 6510.

56 T. T. Nguyen, F. Chevallier, V. Jouikov and F. Mongin, *Tetrahedron Lett.*, 2009, **50**, 6787.

57 T. T. Nguyen, N. Marquise, F. Chevallier and F. Mongin, *Chem. – Eur. J.*, 2011, **17**, 10405.

58 (a) T. Fujisawa, Y. Kurita, M. Kawashima and T. Sato, *Chem. Lett.*, 1982, 1641; (b) P. Kocienski and C. Barber, *Pure Appl. Chem.*, 1990, **62**, 1933; (c) P. Ashworth, B. Broadbelt, P. Jankowski, P. Kocienski, A. Pimm and R. Bell, *Synthesis*, 1995, 199.

59 (a) G. Queguiner, F. Marsais, V. Snieckus and J. Epsztajn, *Adv. Heterocycl. Chem.*, 1991, **52**, 187; (b) F. Mongin and G. Queguiner, *Tetrahedron*, 2001, **57**, 4059; (c) A. Turck, N. Plé, F. Mongin and G. Queguiner, *Tetrahedron*, 2001, **57**, 4489; (d) M. Schlosser and F. Mongin, *Chem. Soc. Rev.*, 2007, **36**, 1161; (e) F. Chevallier and F. Mongin, *Chem. Soc. Rev.*, 2008, **37**, 595; (f) P. C. Gros and Y. Fort, *Eur. J. Org. Chem.*, 2009, 4199.

60 G. Queguiner, F. Marsais, V. Snieckus and J. Epsztajn, *Adv. Heterocycl. Chem.*, 1991, **52**, 187.

61 T. L. Stemmler, T. M. Barnhart, J. E. Penner-Hahn, C. E. Tucker, P. Knochel, M. Bohme and G. Frenking, *J. Am. Chem. Soc.*, 1995, **117**, 12489.

62 S. H. Bertz, G. Miao and M. Eriksson, *Chem. Commun.*, 1996, 815.