Diverse outcomes of CO2 fixation using alkali metal amides including formation of a heterobimetallic lithiumsodium carbamato-anhydride via lithiumsodium bis-hexamethyldisilazide

The activation and fixation of small molecules is a fertile field of research currently at the cutting edge of inorganic and organometallic chemistry. Along with fundamental interest, the goal of small molecule activation is to convert common small molecules such as N2, O2 and CO2 to higher value products, achieved through a variety of chemical means. For example, Arnold recently demonstrated small molecule activation of N2, CO and CO2 using a uranium based tris(aryloxide), giving a range of complexes such as [U(OAr)3]2(m-N2) and the ynediolate complex of the form [U(OAr)3]2(m-Z :Z-C2O2). 4

2][3] Along with fundamental interest, the goal of small molecule activation is to convert common small molecules such as N 2 , O 2 and CO 2 to higher value products, achieved through a variety of chemical means. 1 For example, Arnold recently demonstrated small molecule activation of N 2 , CO and CO 2 using a uranium based tris(aryloxide), giving a range of complexes such as [U(OAr) 3 ] 2 (m-N 2 ) and the ynediolate complex of the form [U(OAr) 3 ] 2 (m-Z 1 :Z 1 -C 2 O 2 ). 4 Transition metals such as iron and manganese have been used to activate molecular oxygen, both in synthetic chemistry 5 and in nature with the best known example in the transport of oxygen in blood of vertebrates by the iron protein haemoglobin. 6,7arbon dioxide is a molecular Jekyll and Hyde, famous as it is the primary carbon source for life on earth; but infamous because of its role as a greenhouse gas.Attempts to capture and sequester CO 2 are currently the focus of many scientific efforts worldwide. 8The stability of CO 2 presents a significant challenge in terms of its activation due to the strong C-O double bonds present, exemplified by the high enthalpy value of À393.51 kJ mol À1 . 2,9onetheless, there are many methods available in this regard.For example, nature uses enzymes that employ CO 2 or its hydrated form to carry out a carboxylation reaction to form a new C-C bond. 9CO 2 can also be utilised in the synthesis of polymers, as in the reaction with cyclohexane oxide catalysed by zinc crotonate. 10n spite of this widespread interest, few studies have looked at CO 2 insertion into reactive alkali metal-nitrogen bonds, 11 with much greater attention being paid to transition metals and group 14 elements.Such insertion reactions and concomitant formations of carbamate functionalities adds to the diversity of CO 2 chemistry, which attracts widespread interest across capture technologies, 12 industry and agriculture. 13The paucity of work carried out on alkali metal amides is perhaps surprising given the widespread utility of these amides in synthesis.Lithium diisopropylamide (LDA) is the most common utility amide, first utilised in 1950 in reactions with esters. 14The structure of LDA in the solid state was elucidated in 1991, revealing an eye-catching helical arrangement with near-linear N-Li-N-Li units, 15 with a more recent study establishing an equilibrium of trimers and tetramers in toluene. 16Another class of compound that has received much synthetic interest are pyrroles.This is due to the prevalence of the five-membered ring in areas ranging from agricultural chemistry 17 to the pharmaceutical industry. 18erein we report the different outcomes of the insertion reactions of CO 2 into common utility lithium amides, namely LDA and lithium pyrrolide.Extending our study to reactions between CO 2 and the mixed lithium-sodium 1,1,1,3,3,3-hexamethyldisilazide (HMDS) system, THFÁLi(m-HMDS) 2 NaÁ2THF, reveals a remarkable carbamato-anhydride product, which retains both lithium and sodium in its polymeric chain structure.
The lithium-nitrogen bonding in lithium pyrrolide has recently been elucidated, and suggests that the insertion of CO 2 into lithium pyrrolide should be possible. 19To this end, pyrrole was reacted with n BuLi in hexane at 0 1C, then CO 2 was bubbled through the resulting suspension for 30 minutes.Adding THF produced colourless crystals of the polymeric carbamate [{(THF)ÁLi(CO 2 NC 4 H 4 )} N ] (1) (Scheme 1), as determined by X-ray crystallography (Fig. 1).7) Å for the other. 27Due to the widespread nature of the five membered ring, it should come as no surprise to find that N-CO 2 based structural motifs such as that seen in polymeric 1 are present in a variety of biologically active compounds, which have found use as potential cyclotoxic antitumor agents to antiretroviral therapies. 28,29ext we turned to LDA.The reactive Li-N bond present would be ideal for use in CO 2 activation presumably furnishing the corresponding lithium carbamate complex.To this end, diisopropylamine was deprotonated with n BuLi in hexane, N,N,N 0 ,N 00 ,N 00 -pentamethyldiethylenetriamine (PMDETA) was introduced and CO 2 was bubbled through this solution for 10 minutes.Cooling the resulting solution to À33 1C gave crystals identified as [{(iPr 2 NCOOLi) 12 (iPr 2 NCOOH) 2 }] (2) (Scheme 1 and Fig. 2) by X-ray crystallography.
The centrosymmetric structure of 2 is a discrete dodecanuclear cluster comprising 12 lithium diisopropylamido-carbamate units and two carbamic acids that occupy terminal positions.Note there is no PMDETA present in the structure, though subsequent experiments have shown that PMDETA addition is necessary in order to obtain crystals.The Li cations are bonded to three, four or five oxygen atoms, depending upon their position in the structure.Those bonded to three oxygen atoms (Li1) occupy a slightly distorted trigonal environment (average angle of 1191).The four coordinate Li centres are all in a distorted tetrahedral environment, with t 4 values ranging from 0.80-0.84(Li2).There are two lithium centres in the molecule bonded to five oxygen atoms (Li3), both in a distorted square pyramidal molecular geometry (average bond angle of 94.71).
The two carbamic acid groups present at the terminal positions of the Li-O core presumably result from adventitious hydrolysis, likely due to the CO 2 source being dry ice.However, the reaction is   reproducible and the CO 2 is passed through a CaCl 2 drying tube prior to addition.This is a relatively rare example of such a feature, with only a few examples of carbamic acid groups structurally characterised. 30,31In 2 the metallic core skeleton shows a distorted Li 4 O 4 cubane that is linked to a perfect central Li 2 O 2 planar square (all internal angles 901) via a m-(O-N) bond.The corner oxygen atoms of the cubane are connected to the remaining Li of the Li 2 O 2 square by a carbamate in a kO;kO 1 bridging mode.The C-O distances in the carbamate units within the cubane section of 2 are consistent with those seen in 1, with values generally in the range of 1.25-1.26Å, again longer than in the parent CO 2 molecule. 8he bridging carbamates have slightly different bond lengths, with one generally shorter than the other (1.235(4) vs. 1.275(5) and 1.267(3) vs. 1.288(3)Å), presumably due to the bridging nature.
The carbamic acid molecules have bond lengths that would be expected for a carboxylic acid derived species, with a C-O double bond of 1.227(3) Å and a C-OH single bond of 1.321(4) Å, though the OH group is not visible in either IR or NMR spectra, perhaps due to the lower number of such groups in comparison to the carbamate groups within the complex.
Diisopropylamide species have been used in CO 2 activation before, notably by Sperrle who obtained a hafnium carbamate complex. 32Interestingly, the structure of this complex is simpler than the Li analogue here, having an 8-coordinate hafnium atom bound by four DA-derived carbamate units. 32e next attempted to expand fixation of CO 2 into another major class of utility amide; namely those based on alkali metal HMDS compounds. 33Previous studies have shown M-HMDS species are able to activate CO 2 .Insertion into U-(HMDS) 4 is followed by a series of silyl migration steps, furnishing an isocyanate complex. 34The presence of an isocyanate is also implicated by Kemp et al., who probed the insertion reactions of CO 2 into group two complexes based on a HMDS core. 35We wanted to probe the effects of CO 2 addition specifically on mixed alkali metal species, based on work carried out by Williard which disclosed the structures of these mixed alkali metal HMDS complexes to be dimeric. 36As such, these species would be primed for CO 2 insertion in two distinct sites within the same molecule, between the Li-N bond and Na-N bond for example.However, to the best of our knowledge it is exceptionally rare to generate a mixed alkali metal product from a mixed alkali metal starting material. 37,38o this end, a 1 : 1 NaHMDS : LiHMDS mixture was dissolved in THF, and then CO 2 was bubbled through it for 10 minutes at À78 1C.On warming to room temperature, a yellow solution formed.Cooling this solution to À33 1C deposited crystals, revealed by X-ray crystallography to be the unique lithium-sodium carbamato-anhydride polymer [{(Me 3 Si)NC(QO)OC(QO)N(H)(SiMe 3 )} 2 LiNa(THF) 4 ] N , (3) (Scheme 1 and Fig. 3).Repeated attempts confirmed the reproducibility of this reaction with yields spanning the range 45-51%.Disorder in THF and Me 3 Si groups in 3 rules out a discussion of its bond angles and lengths though its molecular connectivity is unambiguous.Interestingly, when LiHMDS and NaHMDS were reacted separately with CO 2 , only intractable gels were formed, implying the origin of 3 is synergistic.
The structure of 3 exists as an infinite chain of silylamidosubstituted anhydride units held together by alternating Li and Na cations.The Li cations are four-coordinate in a distorted tetrahedral environment (t 4 = 0.78), each coordinated to four oxygens from two chelating anhydride molecules.The Na cations are six-coordinate, bonded to two oxygen and two nitrogen atoms from two individual anhydride units.The nitrogen and oxygen atoms are in the backbone of the anhydride, thus directing polymer formation.The Na coordination sphere is completed by two THF ligands.Therefore the anhydride unit adopts a ditopic arrangement in terminally binding to Na through one O centre and chelating the Li through two oxygen centres on the opposite face.
Given the unexpected nature of 3, a literature search was done which found no evidence for crystallographically characterised alkali metal anhydrides.However, CO 2 has previously been used in the synthesis of an anhydride derived compound, namely hexahydro-4,7-dimethyl-1-oxatetrazonine-2,9-dione. 39he synthesis involved the addition of CO 2 to either a mixture of the parent dihydrizine and HN(SiMe 3 ) 2 or directly reacting CO 2 with the corresponding disilane. 39ased on the stoichiometry of 3, it appears that two trimethylsilyl units and one oxygen atom have been lost from the reaction, which also shows the formation of a new NH group.As for how compound 3 may have formed, Maron and Mazzanti investigated the conversion of CO 2 to isocyanates at uranium centres, postulating that multiple N-Si bond cleavage reactions occurred, leading to the release of hexamethyldisiloxane. 34 This could be a potential pathway in this reaction, explaining the loss of both the oxygen atom and the silylamido groups.The NH group present within the polymer backbone could have been formed either through adventitious hydrolysis or the presence of some HMDS(H) within the reaction.In any case, the anhydride can also be isolated in its hydrolysed form using H 2 O work-up, with the parent compound featuring two NH groups in the backbone.
In conclusion, we have demonstrated that common utility alkali metal amides can be utilised in CO 2 insertion reactions, providing a route to the formation of alkali metal carbamate species.Through judicious choice of amide, different molecular architectures can be obtained, ranging from polymeric through to discrete species.A novel alkali metal anhydride species is also presented through the activation of CO 2 , revealing an exceptionally rare reaction where a mixed lithium-sodium precursor produces a mixed lithium-sodium product, itself a rare example of a heterobimetallic alkali metal polymer.

Carbamate 1
adopts a polymeric ladder of alternating, fused 4-membered (LiO) 2 and 8-membered (LiO) 4 rings, with a THF donor ligand completing the Li coordination.The structure contains only one Li environment, confirmed both in the solid and solution state (see ESI †).This environment comprises four oxygen atoms in a distorted tetrahedron, three from the carbamate units and the fourth from THF.The mean Li-O-Li bond angle is 1091, ranging from 123.8(3)1 to 90.5(2)1 (t 4 = 0.81). 20The (LiO) 2 ring forms a near perfect square, with internal angles of 90.5(2)1 and 89.5(2)1 at Li and O respectively.Least squares planes through the 4-and 8-membered rings make a dihedral angle of 1381.Though ladder motifs are well known in lithium amide chemistry 21-25 to our knowledge this is the first such ladder motif found in lithium carbamate chemistry.The Li cation is m 3 with respect to the carbamate oxygens (Li-O range 1.870(5)-2.020(6)Å) and is effectively equidistant between the carbamate O atom and THF O atom [Li1-O2 and Li1-O3 distance 1.943(5) vs. 1.959(6)Å respectively].The carbamate C-O distances are longer than those seen in the parent CO 2 molecule 8 and are intermediate between C-O single and double bonds.Robertson et al. probed the reaction products of CO 2 insertion into LiTMP observing a similar distance for the C-O bond as seen in 1 [values of 1.255(2) and 1.261(2) Å]. 26 Snaith et al. also observed similar distances to those of 1 when studying CO 2 insertion products of lithium diphenylamide, with values of 1.251(7)/1.256(7)Å for one carbamate unit and 1.264(7)/1.243(

Scheme 1
Scheme 1 CO 2 fixation reactions carried out in this work.