Kevin
Yurkerwich
,
Daniela
Buccella
,
Jonathan G.
Melnick
and
Gerard
Parkin
*
Department of Chemistry, Columbia University, New York, New York 10027, USA. E-mail: parkin@columbia.edu
First published on 25th May 2010
A series of tris(2-mercapto-1-tert-butylimidazolyl)hydroborato gallium compounds have been synthesized. While GaI3 and GaCl3 afford mononuclear {[TmBut]Ga} compounds, namely {[TmBut]GaI}I, {[TmBut]GaCl}[GaCl4], and [κ2-TmBut]2GaI, the reactions of “GaI”, Ga[GaCl4] and (HGaCl2)2 yield compounds that feature Ga–Ga bonds, namely [TmBut]GaGaI3, [TmBut]GaGaCl3, {[TmBut]GaGa[TmBut]}I2, {[TmBut]GaGa[TmBut]}[GaCl4]2, {[TmBut]Ga(GaI2)Ga[TmBut]}I and {[TmBut]GaGa[TmBut]}{[μ-κ1,κ2-TmBut]GaI2GaI2GaI}2. These Ga–Ga bonded compounds may be formally regarded as donor–acceptor adducts between monovalent [TmBut]Ga and various trivalent moieties; for example, [TmBut]GaGaI3 may be described as an adduct of [TmBut]Ga and GaI3, while {[TmBut]Ga(GaI2)Ga[TmBut]}+ is an adduct between two molecules of [TmBut]Ga and [GaI2]+. Comparison of the structure of [TmBut]Ga→B(C6F5)3 with that of [TmBut]In→B(C6F5)3 indicates that [TmBut]Ga is a more effective Lewis base than is [TmBut]In.
Scheme 1 |
In addition to {[TmBut]GaX}+ (X = Cl, I), which feature one [TmBut] ligand per gallium, the 2:1 complex [κ2-TmBut]2GaI (2), which exhibits κ2 coordination of the [TmBut] ligands, has also been obtained from the reaction of [TmBut]K with GaI3 (2:1 molar ratio). The ability to isolate {[TmBut]GaX}+ and [κ2-TmBut]2GaI provides an interesting comparison with the related indium system. Specifically, the indium counterparts of {[TmBut]GaX}+ have not been reported, while the indium analogue of [κ2-TmBut]2GaI exists as an ion pair, {[TmBut]2In}I,2a in which the indium is octahedrally coordinated to the two [TmBut] ligands in a κ3 manner.6
Another notable difference between the gallium and indium systems is that treatment of [TmBut]M (M = K, Tl) with “GaI”7,8 does not simply yield monovalent9 [TmBut]Ga, the analogue of [TmBut]In,2a but rather gives compounds that feature gallium–gallium bonds, namely (i) dinuclear [TmBut]GaGaI3 (3) and {[TmBut]GaGa[TmBut]}I2 (4)[I]210 and (ii) trinuclear {[TmBut]Ga(GaI2)Ga[TmBut]}I (5)[I] (Schemes 2 and 3), depending on the reaction conditions. In addition to these discrete dinuclear and trinuclear compounds, the ion pair {[TmBut]GaGa[TmBut]}{[μ-κ1,κ2-TmBut]GaI2GaI2GaI}2 that features both dinuclear and trinuclear moieties has been isolated, of which the anionic {[μ-κ1,κ2-TmBut]GaI2GaI2GaI}− (6)− species features an unprecedented [μ-κ1,κ2-TmBut] coordination mode in which the ligand bridges a chain of metal atoms.
Scheme 2 |
Scheme 3 |
The formation of each of these dinuclear and trinuclear compounds may be rationalized in terms of disproportion of “GaI” to gallium metal and GaI3,8 of which the latter would react with [TmBut]K to generate [TmBut]GaI2 (vide supra). Thus, dinuclear [TmBut]GaGaI3 may be formally regarded as a donor–acceptor adduct between monovalent [TmBut]Ga and trivalent GaI3,11 while {[TmBut]GaGa[TmBut]}2+ may be viewed as a donor–acceptor adduct between [TmBut]Ga and {[TmBut]Ga}2+. Similarly, trinuclear {[TmBut]Ga(GaI2)Ga[TmBut]}I is formally derived from a 2:1 ratio of [TmBut]Ga and GaI3. It is also worth noting that the isolation of {[TmBut]Ga(GaI2)Ga[TmBut]}I is best achieved at low temperature (−35 °C), and that solutions in MeCN convert to a mixture comprising [TmBut]GaGaI3 and {[TmBut]GaGa[TmBut]}2+ at room temperature.
The molecular structures of [TmBut]GaGaI3, {[TmBut]GaGa[TmBut]}I2, {[TmBut]Ga(GaI2)Ga[TmBut]}I and {[TmBut]GaGa[TmBut]}{[μ-κ1,κ2-TmBut]GaI2GaI2GaI}2 have been determined by X-ray diffraction, as illustrated respectively in Fig. 1–4. The Ga–Ga bond lengths of [TmBut]GaGaI3 [2.4138(4) and 2.4254(3) Å],12 {[TmBut]GaGa[TmBut]}2+ [2.412(2) Å], {[TmBut]Ga(GaI2)Ga[TmBut]}+ [2.4586(5) Å] and {[μ-κ1,κ2-TmBut]GaI2GaI2GaI}− [2.406(3) and 2.412(2) Å] are comparable to twice the covalent radius of gallium (2.44 Å,13 2.48 Å14) and are typical for compounds with Ga–Ga single bonds.15
Fig. 1 Molecular structure of [TmBut]GaGaI3 (from benzene). |
Fig. 2 Molecular structure of {[TmBut]GaGa[TmBut]}I2 (only the cation is shown). |
Fig. 3 Molecular structure of {[TmBut]Ga(GaI2)Ga[TmBut]}+. |
Fig. 4 Molecular structure of {[μ-κ1,κ2-TmBut]GaI2GaI2GaI}−. |
{[TmBut]GaGa[TmBut]}2+ and {[TmBut]Ga(GaI2)Ga[TmBut]}+ are of particular note because there are no other structurally characterized cationic dinuclear and trinuclear gallium compounds listed in the Cambridge Structural Database16 and catenation is not common for gallium.17 Furthermore, in view of the analogy between [TmR], tris(pyrazolyl)hydroborato [TpRR′] and cyclopentadienyl [CpR] ligands, it is interesting to note that the {[TpRR′]GaGa[TpRR′]}2+ and {[CpR]GaGa[CpR]}2+ counterparts of {[TmBut]GaGa[TmBut]}2+ have not been reported, even though such species are isoelectronic with the recently reported neutral zinc complexes CpRZnZnCpR,18 the first examples of compounds with Zn–Zn bonds.19
The chloride complexes Ga[GaCl4] and (HGaCl2)220 may also be used to synthesize compounds with Ga–Ga bonds. For example, Ga[GaCl4] reacts with [TmBut]Tl to give [TmBut]GaGaCl3 (7) (Scheme 4), while treatment of [TmBut]K with (HGaCl2)2 yields {[TmBut]GaGa[TmBut]}[GaCl4]210 (8) (Scheme 5), both of which have been structurally characterized by X-ray diffraction. While the mechanism for formation of {[TmBut]GaGa[TmBut]}2+ in the latter reaction is not known, it is pertinent to note that Lewis bases promote reductive dehydrogenation of (HGaCl2)2,20,21 which thereby provides a means to generate {[TmBut]GaGa[TmBut]}2+.
Scheme 4 |
Scheme 5 |
Since [TmBut]GaGaX3 (X = Cl, I) and {[TmBut]GaGa[TmBut]}2+ may be formally regarded as donor–acceptor adducts between monovalent [TmBut]Ga and the respective trivalent moiety, GaI3 and {[TmBut]Ga}2+, we sought evidence for the existence of [TmBut]Ga in this system.22 In this regard, support for the accessibility of [TmBut]Ga is provided by the observation that the simple adduct [TmBut]Ga→B(C6F5)3 (9) may be isolated via the reaction of [TmBut]K and (HGaCl2)2 in the presence of B(C6F5)3 (Scheme 5). Furthermore, the bridging sulfido complex [TmBut]GaSGaCl3 (10) may be obtained from the reaction of [TmBut]K with (HGaCl2)2 in the presence of sulfur (Scheme 5). In view of the fact that [TpBut2]Ga reacts with elemental chalcogens to give the terminal chalcogenido complexes [TpBut2]GaE (E = S, Se, Te),23 the formation of [TmBut]GaSGaCl3 is consistent with a sequence in which in situ generated [TmBut]Ga reacts with sulfur to give the terminal sulfido complex [TmBut]GaS, which is subsequently trapped by GaCl3, although other mechanisms are possible.24
The molecular structure of [TmBut]GaSGaCl3 has been determined by X-ray diffraction (Fig. 5), thereby demonstrating that the Ga–S bonds for the bridging sulfido ligand [2.2024(6) and 2.2153(6) Å] are shorter than those for the [TmBut] ligand (2.30–2.31 Å), an observation which is in accord with the L2X nature of [TmBut],25 such that the Ga–[TmBut] interaction is appropriately described as a composite of covalent and dative covalent bonds. The gallium sulfido bond lengths are, nevertheless, comparable to the values for other bridging sulfido complexes,26 but are considerably longer than that for the terminal sulfido complex [TpBut2]GaS [2.093(2) Å].23a The similarity of the two gallium–sulfido bond lengths is significant in view of the fact that the gallium centers in the isolated fragments, namely monovalent [TmBut]Ga and trivalent GaCl3, are electronically distinct. However, in view of the zwitterionic nature of the bonding within [TmBut]Ga(+)–S–Ga(−)Cl3, both gallium centers in the sulfido complex are trivalent and the Ga–S bond lengths are comparable.
Fig. 5 Molecular structure of [TmBut]GaSGaCl3. |
Comparison of the structure of [TmBut]Ga→B(C6F5)3 (Fig. 6) with that of the indium counterpart provides a means to assess the relative abilities of the [TmBut]Ga and [TmBut]In moieties to serve as a Lewis base. Specifically, the deviation of the B(C6F5)3 ligand from planarity, as indicated by the magnitude of Σ(C–B–C) provides a simple indication of the strength of the interaction with the Lewis base.27 On this basis, Σ(C–B–C) for [TmBut]Ga→B(C6F5)3 [342.2°]28 is smaller than that for [TmBut]In→B(C6F5)3 [347.9°],2a thereby indicating that the lone pair on gallium is more available for bonding than is that on indium, an observation which is in accord with the so-called “inert pair effect” being more prevalent for the heavier element.29 Support for the greater Lewis basicity of [TmBut]Ga, as implied by the structural differences between [TmBut]Ga→B(C6F5)3 and [TmBut]In→B(C6F5)3, is provided by DFT calculations which indicate that coordination of B(C6F5)3 to [TmBut]Ga (−23.7 kcal mol−1) is more exothermic than is coordination to [TmBut]In (−19.3 kcal mol−1).
Fig. 6 Molecular structure of [TmBut]GaB(C6F5)3. |
It is also pertinent to note that the 5.7° difference in Σ(C–B–C) for [TmBut]Ga→B(C6F5)3 and [TmBut]In→B(C6F5)3 is distinctly larger than the corresponding difference for ArGa→B(C6F5)3 and ArIn→B(C6F5)3 counterparts; for example, Σ(C–B–C) for (2,6-C6H3Trip2)Ga→B(C6F5)3 (337.5°)27b and (2,6-C6H3Trip2)In→B(C6F5)3 (339.3°)30 differ by only 1.9°. As such, this observation demonstrates that supporting ligands can exert differential effects on the relative Lewis basicities of monovalent gallium and indium centers.
Footnote |
† Electronic supplementary information (ESI) available: Experimental details and crystallographic data. CCDC reference numbers 763457–763470. For ESI and crystallographic data in CIF or other electronic format see DOI: 10.1039/c0sc00145g |
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