Abstract
While main group elements have four valence orbitals accessible for bonding, quadruple bonding to main group elements is extremely rare. Here we report that main group element boron is able to form quadruple bonding interactions with iron in the BFe(CO)3- anion complex, which has been revealed by quantum chemical investigation and identified by mass-selected infrared photodissociation spectroscopy in the gas phase. The complex is characterized to have a B-Fe(CO)3− structure of C3v symmetry and features a B-Fe bond distance that is much shorter than that expected for a triple bond. Various chemical bonding analyses indicate that the complex involves unprecedented B≣Fe quadruple bonding interactions. Besides the common one electron-sharing σ bond and two Fe→B dative π bonds, there is an additional weak B→Fe dative σ bonding interaction. This finding of the new quadruple bonding indicates that there might exist a wide range of boron-metal complexes that contain such high multiplicity of chemical bonds.
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Introduction
Chemical bonding is among the most fundamental concepts in modern chemistry. Depending upon the availability of valence orbitals and electrons, an atom can form single or multiple covalent chemical bonds with neighboring atoms in forming stable compounds. Since the discovery of Re–Re quadruple bond in 1964 by Cotton and coworkers1,2, metal–metal multiple bonding with bond orders of four to six has been extensively explored for transition metals and actinides3,4,5,6,7,8,9,10,11,12,13,14,15,16,17,18. Main group elements of the periodic table may form single, double, and triple bonds between two atoms, that is, the maximum bond order can only be three as exemplified in alkyne. Triple bonds between two main group atoms are well established, and a large number of triple-bonded molecules are known19,20,21,22,23,24,25,26. As main group elements have nsnp four valence orbitals accessible for bonding, it has been speculated that a further extension to bond order of four for main group elements should in principle be possible. Diatomic C2 and its isoelectronic molecules CB−, BN, and CN+ each having eight valence electrons were claimed to be quadruple-bonded molecules, comprising not only one σ- and two π-bonds, but also one weak ‘inverted’ bond27. However, this quadruple bond assignment has been debated, which has stimulated hot discussion28,29,30. Quadruple bonding of carbon to uranium with rich valence shell (sdf) has been reported to exist in the triatomic uranium carbide oxide molecule CUO and related species, due to availability of both 2p and unhybridized 2s orbitals of carbon46 analyses shown in Supplementary Table 2. The semi-localized results indicate that the B–Fe bonding interactions in BFe(CO)3− involve two 5c-2e σ bonds and two 5c-2e π bonds. It should be mentioned that here there is some mixing of the B–Fe and Fe-CO bonding MOs, but the major components and shapes of MOs resemble those of the classical electron-pair bonding models. The above bonding analysis also indicates that the B–Fe bonding interactions have quite small effect on the Fe-to-CO 2π* back-donation interactions in the Fe(CO)3− fragment. Charge analyses in Supplementary Table 4 also indicate that the negative charge is largely located on the Fe(CO)3 moiety. The antisymmetric CO stretching frequency (1841 cm−1) of BFe(CO)3− is only slightly higher than that of free Fe(CO)3− (1780 cm−1), but is lower than those of neutral Fe(CO)4 and Fe(CO)5.
Figure 4 qualitatively illustrates the bonding picture of BFe(CO)3− and its correlation to the interacting fragments B and Fe(CO)3−. The major interactions between B and Fe(CO)3− involve one σp-type (14a1) Fe–B electron-sharing bonding, two degenerate π-type (10e) Fe→B dative bonding, and one σs-type (13a1) B→Fe dative bonding, leading to the aforementioned quadruple bonding. The ground state BFe(CO)3− anion can thus be regarded as being formed via the interactions between the ground state 2P-B atom with the (2s)2(2pz)1 configuration and the Fe(CO)3− fragment in its 2A1 electronic ground state with (a1)1(e)4(e)4 configuration. The B≣Fe quadruple bonding interactions are further characterized using the principal interacting orbital (PIO) approach47. The calculated PIOs and PIMOs shown in Supplementary Figs. 8–11 clearly reveal the fourfold bonding interactions between B and Fe in the BFe(CO)3− anion, which further support the above assignment.
The strengths of the above-mentioned pairwise orbital interactions can be quantitatively estimated by the EDA-NOCV method48,49. The numerical results calculated at the M06-2X /TZ2P level are listed in Supplementary Table 5. The EDA-NOCV calculations suggest that 43% of the attractive forces in BFe(CO)3− are due to orbital (covalent) interactions. The breakdown of the orbital interaction term ∆Eorb into individual orbital contributions reveals that the four bonding components contribute 42.8% (σp), 46.6% (two π), and 8.2% (σs) of the orbital bonding interactions. Although the fourth component (σs B→Fe dative bonding interaction) is much weaker than the electron-sharing σp and two Fe→B dative π bonding interactions, it has a calculated interaction energy of 18.4 kcal/mol, indicating that it is a non-negligible, albeit weak, bonding interaction. The deformation densities Δρ(σ) and Δρ(π) that are connected to the σ and π interactions in BFe(CO)3− are displayed in Supplementary Table 5. The deformation densities Δρ show the direction of the charge flow and the orbitals that are involved, where the color code of the charge flow is red → blue. The results clearly indicate the electron-sharing bonding nature of the stronger σp interaction and the dative bonding character of the two π and the weaker σs interactions. The weaker σs interaction is strongly polarized with obvious charge flow from B atom to Fe(CO)3−. In contrast, the two degenerate π interactions show reversed charge flow from Fe(CO)3− to B.
To make certain that these single-configuration quantum chemical methods are reliable, the wavefunction of BFe(CO)3− is further examined in a multi-configurational framework. Ab initio CASSCF calculation involving 12 valence electrons in a space of 12 MOs was performed at the M06-2X optimized geometry, and the Löwdin natural orbitals (NOs) were analyzed using the CASSCF density matrix. The six strongly occupied and six weakly occupied natural orbitals and their occupation numbers (NOONs) are displayed in Supplementary Fig. 12. There is no significant occupation number of B–Fe antibonding NOs, 1σ*0.05π*0.182σ*0.11, indicating that the multi-reference feature of this molecule is not very large. The B≣Fe effective bond order (EBO)9 based on the ground-state CASSCF wavefunctions is calculated as 3.7, which is rather close to four and further supports the B≣Fe quadruple bonding assignment.
In summary, the BFe(CO)3− anion complex has been identified by a combined quantum chemical and experimental study. The anion is generated in the gas phase and is studied by mass-selected infrared photodissociation spectroscopy. The complex has been characterized to have a cylindrical BFe(CO)3− structure with C3v symmetry and a very short B–Fe bond distance. Electronic structure and chemical bonding analyses indicate that the complex exhibits an unprecedented B≣Fe quadruple bonding interactions, featuring one electron-sharing σ bond, two Fe→B dative π bonds as well as one additional weak B→Fe dative σ bonding interaction. The results extend the maximum bond order of boron element to four. This study reveals that a variety of such quadruple-bonded systems of main-group and transition-metal elements may exist in inorganic and organometallic chemistry.
Methods
Experimental details
The anion complexes were generated in the gas phase using a pulsed laser vaporization/supersonic expansion ion source. A bulk target compressed from an isotopically enriched (11B- or 10B-depleted) or natural abundance boron powder was used. The ions were produced from the laser vaporization process in expansions of helium seeded with 5−10% CO using a pulsed valve (General Valve, Series 9) at 0.5−1.0 MPa backing pressure. After free expansion and cooling, the anions were skimmed into a second chamber where they were pulse-extracted into a Wiley−McLaren type time-of-flight mass spectrometer. The anions of interest were mass-selected and decelerated into the extraction region of a second collinear time-of-flight mass spectrometer, where they were dissociated by a tunable IR laser. The tunable IR laser used is generated by a KTP/KTA//AgGaSe2 optical parametric oscillator/amplifier system (OPO/OPA, Laser Vision) pumped by a Nd: YAG laser, producing about 0.5−1.0 mJ per pulse in the range of 1600−2200 cm−1. Resonant absorption leads to fragmentation of the anion complex. The infrared photodissociation spectrum is obtained by monitoring the yield of the fragment anion as a function of the dissociation IR laser wavelength and normalizing to parent anion signal.
Computational methods
Geometry optimization and vibrational frequency calculations of the most stable structure of BFe(CO)3− were performed using the density functional theory (DFT) methods with the PBE50,51, B3LYP52,53, and M06-2X 54 functionals using the ADF 2016 program packages [ADF 2016.101, http://www.scm.com]. The Slater-type-orbital (STO) basis sets with the quality of triple-ζ plus two polarization functions (TZ2P)55 were applied with the consideration of scalar-relativistic (SR) effects at the zero-order regular approximation (ZORA)56. In order to obtain more accurate B–Fe bond distance, a series of single-point calculations at different B–Fe distances were carried out using a domain-based local pair natural orbital coupled cluster method, DLPNO-CCSD(T)57,58,59, with the def2-TZVP basis sets (11s6p2d1f)/[5s3p2d1f] for the B, C and O, and (17s11p7d1f)/[6s4p4d1f] for Fe60. The DLPNO-CCSD(T) calculations were performed with the ORCA program package61.
The chemical bonding properties were analysed by employing several different methods including adaptive natural density partitioning (AdNDP)46 and the principal interacting orbital (PIO)47. The def2-TZVP basis sets, (11s6p2d1f)/[5s3p2d1f] for the B, C, and O, and (17s11p7d1f)/[6s4p4d1f] for Fe in Gaussian 09 program62, were applied in the AdNDP calculations. For determining the most stable structure of BFe(CO)3−, BFe(CO)4−, and BFe(CO)5−, B3LYP with Dunning’s correlation consistent basis sets aug-cc-pVTZ63, (10s5p2d1f)/[4s3p2d1f] for B, C, and O, and (20s16p8d2f1g)/[7s6p4d2f1g] for Fe64 were applied with Gaussian 09 program. The PIO analyses were also carried out using the Gaussian 09 program with aug-cc-pVTZ basis sets.
The multi-configurational complete-active-space SCF (CASSCF)65 calculations were performed using the MOLPRO 2012.1 program package to examine the description of electronic configurations based on the DFT-optimized geometries with the Dunning’s correlation consistent basis sets aug-cc-pVTZ63, (10s5p2d1f)/[4s3p2d1f] for B, C, and O, and (20s16p8d2f1g)/[7s6p4d2f1g] for Fe64. The active space used 12 valence electrons in 12 orbitals (12e,12o), which includes six occupied orbitals and six unoccupied orbitals at the frontier region of the molecular orbitals.
Data availability
The data that support the findings of this study are available within the article and the associated Supplementary Data. Any other data are available from the corresponding author upon request.
References
Cotton, F. A. et al. Mononuclear and polynuclear chemistry of rhenium (III): its pronounced homophilicity. Science 145, 1305–1307 (1964).
Cotton, F. A. Metal–metal bonding in [Re2X8]2- ions and other metal atom clusters. Inorg. Chem. 4, 334–336 (1965).
Cotton, F. A., Murillo, C. A. & Walton, R. A. Multiple bonds between metal atoms. (Springer Science & Business Media, 2005).
Chisholm, M. H. & Macintosh, A. M. Linking multiple bonds between metal atoms: clusters, dimers of “dimers”, and higher ordered assemblies. Chem. Rev. 105, 2949–2976 (2005).
Nguyen, T. et al. Synthesis of a stable compound with fivefold bonding between two chromium (I) centers. Science 310, 844–847 (2005).
Frenking, G. Building a quintuple bond. Science 310, 796–797 (2005).
Wagner, F. R., Noor, A. & Kempe, R. Ultrashort metal–metal distances and extreme bond orders. Nat. Chem. 1, 529–536 (2009).
Tsai, Y.-C. & Chang, C.-C. Recent progress in the chemistry of quintuple bonds. Chem. Lett. 38, 1122–1129 (2009).
Roos, B. O., Borin, A. C. & Gagliardi, L. Reaching the maximum multiplicity of the covalent chemical bond. Angew. Chem. Int. Ed. 46, 1469–1472 (2007).
Frenking, G. & Tonner, R. Theoretical chemistry: the six-bond bound. Nature 446, 276–277 (2007).
Weinhold, F. & Landis, C. R. High bond orders in metal-metal bonding. Science 316, 61–63 (2007).
Collman, J. P. & Boulatov, R. Heterodinuclear transition‐metal complexes with multiple metal–metal bonds. Angew. Chem. Int. Ed. 41, 3948–3961 (2002).
Eisenhart, R. J., Clouston, L. J. & Lu, C. C. Configuring bonds between first-row transition metals. Acc. Chem. Res. 48, 2885–2894 (2015).
Falvello, L. R., Foxman, B. M. & Murillo, C. A. Fitting the pieces of the puzzle: the δ bond. Inorg. Chem. 53, 9441–9456 (2014).
Lyngdoh, R. H. D., Schaefer, H. F. III & King, R. B. Metal-metal (MM) bond distances and bond orders in binuclear metal complexes of the first row transition metals titanium through zinc. Chem. Rev. 118, 11626–11706 (2018).
Gagliardi, L. & Roos, B. O. Quantum chemical calculations show that the uranium molecule U2 has a quintuple bond. Nature 433, 848–851 (2005).
Knecht, S., Jensen, H. J. A. & Saue, T. Relativistic quantum chemical calculations show that the uranium molecule U2 has a quadruple bond. Nat. Chem. 11, 40–44 (2019).
Hu, H. S. & Kaltsoyannis, N. The shortest Th-Th distance from a new type of quadruple bond. Phys. Chem. Chem. Phys. 19, 5070–5076 (2017).
Fischer, R. C. & Power, P. P. π-bonding and the lone pair effect in multiple bonds involving heavier main group elements: developments in the new millennium. Chem. Rev. 110, 3877–3923 (2010).
Zhou, M. F. et al. OCBBCO: a neutral molecule with some boron-boron triple bond character. J. Am. Chem. Soc. 124, 12936–12937 (2002).
Li, S. D., Zhai, H. J. & Wang, L. S. B2(BO)2 2− - diboronyl diborene: a linear molecule with a triple boron-boron bond. J. Am. Chem. Soc. 130, 2573–2579 (2008).
Braunschweig, H. et al. Ambient-temperature isolation of a compound with a boron-boron triple bond. Science 336, 1420–1422 (2012).
Frenking, G. & Holzmann, N. A boron-boron triple bond. Science 336, 1394–1395 (2012).
Zhang, X. X. et al. Realization of an Al≡Al triple bond in the gas-phase Na3Al2 - cluster via double electronic transmutation. Angew. Chem. Int. Ed. 57, 14060–14064 (2018).
Sekiguchi, A., Kinjo, R. & Ichinohe, M. A stable compound containing a silicon-silicon triple bond. Science 305, 1755–1757 (2004).
Stender, M., Phillips, A. D., Wright, R. J. & Power, P. P. Synthesis and characterization of a digermanium analogue of an alkyne. Angew. Chem. Int. Ed. 41, 1785–1787 (2002).
Shaik, S. et al. Quadruple bonding in C2 and analogous eight-valence electron species. Nat. Chem. 4, 195–200 (2012).
Shaik, S., Rzepa, H. S. & Hoffmann, R. One molecule, two atoms, three views, four bonds? Angew. Chem. Int. Ed. 52, 3020–3033 (2013).
Markus, H. & Frenking, G. The chemical bond in C2. Chem. Eur. J. 22, 4100–4108 (2016).
Xu, L. T. & Dunning, T. H. Jr Insights into the perplexing nature of the bonding in C2 from generalized valence bond calculations. J. Chem. Theory Comput. 10, 195–201 (2014).
Hu, H.-S., Qiu, Y.-H., **ong, X.-G., Schwarz, W. E. & Li, J. On the maximum bond multiplicity of carbon: unusual C≣U quadruple bonding in molecular CUO. Chem. Sci. 3, 2786–1796 (2012).
Qiu, Y. H., Hu, H. S. & Li, J. Quadruple bonding of carbon in terminal carbides. Sci. China Chem. 57, 426–434 (2014).
Papakondylis, A., Miliordos, E. & Mavridis, A. Carbonyl boron and related systems: An ab initio study of B-X and YB≡BY (1Σg +), where X= He, Ne, Ar, Kr, CO, CS, N2 and Y= Ar, Kr, CO, CS, N2. J. Phys. Chem. A 108, 4335–4340 (2004).
Ducati, L. C., Takagi, N. & Frenking, G. Molecules with all triple bonds: OCBBCO, N2BBN2, and [OBBBBO]2 −. J. Phys. Chem. A 113, 11693–11698 (2009).
Mitoraj, M. P. & Michalak, A. Multiple boron-boron bonds in neutral molecules: an insight from the extended transition state method and the natural orbitals for chemical valence scheme. Inorg. Chem. 50, 2168–2174 (2011).
Braunschweig, H. & Colling, M. Transition metal complexes of boron-synthesis, structure and reactivity. Coord. Chem. Rev. 223, 1–51 (2001).
Braunschweig, H., Kollann, C. & Rais, D. Transition‐metal complexes of boron-new insights and novel coordination modes. Angew. Chem. Int. Ed. 45, 5254–5274 (2006).
Wang, X. F., Roos, B. O. & Andrews, L. Calculations and matrix infrared spectra of terminal borylene complexes FB=MF2. Angew. Chem. Int. Ed. 49, 157–160 (2010).
Tzelia, D. & Mavridisb, A. Electronic structure and bonding of the 3d transition metal borides, MB, M=Sc, Ti, V, Cr, Mn, Fe, Co, Ni, and Cu through all electron ab initio calculations. J. Chem. Phys. 128, 034309 (2008).
Borin, A. C. & Gobbo, J. P. Low-lying singlet and triplet electronic states of RhB. J. Phys. Chem. A. 112, 4394–4398 (2008).
Jian, T., Cheung, L. F., Chen, T. T. & Wang, L. S. Bismuth–boron multiple bonding in BiB2O- and Bi2B-. Angew. Chem. Int. Ed. 56, 9551–9555 (2017).
Wang, G., Chi, C., **ng, X., Ding, C. & Zhou, M. A collinear tandem time-of-flight mass spectrometer for infrared photodissociation spectroscopy of mass-selected ions. Sci. China Chem. 57, 172–177 (2014).
Pyykkö, P., Riedel, S. & Patzschke, M. Triple‐bond covalent radii. Chem. Eur. J. 11, 3511–3520 (2005).
Brandhorst, K. & Grunenberg, J. Characterizing chemical bond strengths using generalized compliance constants. ChemPhysChem 8, 1151–1156 (2007).
Brandhorst, K. & Grunenberg, J. How strong is it? The interpretation of force and compliance constants as bond strength descriptors. Chem. Soc. Rev. 37, 1558–1567 (2008).
Zubarev, D. Y. & Boldyrev, A. I. Develo** paradigms of chemical bonding: adaptive natural density partitioning. Phys. Chem. Chem. Phys. 10, 5207–5217 (2008).
Zhang, J. X., Sheong, F. K. & Lin, Z. Y. Unravelling chemical interactions with principal interacting orbital analysis. Chem. Eur. J. 24, 9639–9650 (2018).
Michalak, A., Mitoraj, M. & Ziegler, T. Bond orbitals from chemical valence theory. J. Phys. Chem. A 112, 1933–1939 (2008).
Mitoraj, M. P., Michalak, A. & Ziegler, T. A combined charge and energy decomposition scheme for bond analysis. J. Chem. Theory Comput. 5, 962–975 (2009).
Ernzerhof, M. & Scuseria, G. E. Assessment of the Perdew–Burke–Ernzerhof exchange-correlation functional. J. Chem. Phys. 110, 5029–5036 (1999).
Hammer, B., Hansen, L. B. & Nørskov, J. K. Improved adsorption energetics within density-functional theory using revised Perdew-Burke-Ernzerhof functionals. Phys. Rev. B 59, 7413 (1999).
Becke, A. D. Density functional thermochemistry. III. The role of exact exchange. J. Chem. Phys. 98, 5648–5652 (1993).
Lee, C., Yang, W. & Parr, R. G. Development of the Colle-Salvetti correlation-energy formula into a functional of the electron density. Phys. Rev. B 37, 785–789 (1988).
Zhao, Y. & Truhlar, D. G. The M06 suite of density functionals for main group thermochemistry, thermochemical kinetics, noncovalent interactions, excited states, and transition elements: two new functionals and systematic testing of four M06-class functionals and 12 other functionals. Theor. Chem. Acc. 120, 215–241 (2008).
van Lenthe, E. & Baerends, E. J. Optimized Slater‐type basis sets for the elements 1–118. J. Comput. Chem. 24, 1142–1156 (2003).
van Lenthe, E., Baerends, E.-J. & Snijders, J. G. Relativistic regular two‐component Hamiltonians. J. Chem. Phys. 99, 4597–4610 (1993).
Riplinger, C. & Neese, F. An efficient and near linear scaling pair natural orbital based local coupled cluster method. J. Chem. Phys. 138, 034106 (2013).
Riplinger, C., Pinski, P., Becker, U., Valeev, E. F. & Neese, F. Sparse maps-A systematic infrastructure for reduced-scaling electronic structure methods. II. Linear scaling domain based pair natural orbital coupled cluster theory. J. Chem. Phys. 144, 024109 (2016).
Riplinger, C., Sandhoefer, B., Hansen, A. & Neese, F. Natural triple excitations in local coupled cluster calculations with pair natural orbitals. J. Chem. Phys. 139, 134101 (2013).
Schäfer, A., Huber, C. & Ahlrichs, R. Fully optimized contracted Gaussian basis sets of triple zeta valence quality for atoms Li to Kr. J. Chem. Phys. 100, 5829–5835 (1994).
Neese, F. The ORCA program system. WIREs Comput. Mol. Sci. 2, 73–78 (2012).
Frisch, M. J. et al. Gaussian 09, Revision C.01. (Gaussian, Inc., Wallingford CT, 2009).
Dunning, T. H. Jr Gaussian basis sets for use in correlated molecular calculations. I. The atoms boron through neon and hydrogen. J. Chem. Phys. 90, 1007–1023 (1989).
Balabanov, N. B. & Peterson, K. A. Systematically convergent basis sets for transition metals. I. All-electron correlation consistent basis sets for the 3d elements Sc–Zn. J. Chem. Phys. 123, 064107 (2005).
Celani, P. & Werner, H.-J. Multireference perturbation theory for large restricted and selected active space reference wave functions. J. Chem. Phys. 112, 5546–5557 (2000).
Acknowledgements
This work was supported by National Natural Science Foundation of China (grant nos 21433005, 21688102, 21590792, and 91426302). The calculations were done using supercomputers at the Southern University of Science and Technology (SUSTech) and Tsinghua National Laboratory for Information Science and Technology.
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The experiments were performed at East China University of Technology by C.C., L.M. and M.L. The theoretical calculations were performed at Tsinghua University by J.W., Y.Z. and W.L. M.Z., H.H. and J.L. wrote the paper and supervised the experimental and theoretical parts. All authors discussed the results and commented on the manuscript at all stages.
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Chi, C., Wang, JQ., Hu, HS. et al. Quadruple bonding between iron and boron in the BFe(CO)3− complex. Nat Commun 10, 4713 (2019). https://doi.org/10.1038/s41467-019-12767-5
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DOI: https://doi.org/10.1038/s41467-019-12767-5
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