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Triboracyclopropenyl

The triboracyclopropenyl fragment is a cyclic structural motif in boron chemistry, named for its geometric similarity to cyclopropene. In contrast to nonplanar borane clusters that exhibit higher coordination numbers at boron (e.g., through 3-center 2-electron bonds to bridging hydrides or cations), triboracyclopropenyl-type structures are rings of three boron atoms where substituents at each boron are also coplanar to the ring. Triboracyclopropenyl-containing compounds are extreme cases of inorganic aromaticity. They are the lightest and smallest cyclic structures known to display the bonding and magnetic properties that originate from fully delocalized electrons in orbitals of σ and π symmetry. Although three-membered rings of boron are frequently so highly strained as to be experimentally inaccessible, academic interest in their distinctive aromaticity and possible role as intermediates of borane pyrolysis motivated extensive computational studies by theoretical chemists.[1][2][3][4] Beginning in the late 1980s with mass spectrometry work by Anderson et al. on all-boron clusters, experimental studies of triboracyclopropenyls were for decades exclusively limited to gas-phase investigations of the simplest rings (ions of B3).[4][5][6] However, more recent work has stabilized the triboracyclopropenyl moiety via coordination to donor ligands or transition metals, dramatically expanding the scope of its chemistry.[7][8][9][10]

Both the B3+ fragment and the B3R32− fragment (with electron-sharing B−R bonds) are Hückel-aromatic forms of the triboracyclopropenyl fragment.

Synthesis

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Laser ablation of a mixed target containing iridium and boron generates a cluster beam containing two IrB3− isomers of very similar energy.[8]

For gas-phase spectroscopic studies, triboracyclopropenyl-containing compounds are obtained via laser ablation of boron targets and collimation of the resulting plasma cloud in a flow of inert carrier gas such as helium. The charged molecules of interest are then mass-selected by time-of-flight mass spectrometry. Addition of gases such as N2 or CO to the gas stream affords the corresponding adducts, while addition of metals such as iridium and vanadium to the B target yields the corresponding metal-doped clusters.[11]

 
Na4[B3(NCy2)3]2 • 2 DME is synthesized by direct reduction of a boron precursor.[7]

The sole isolable example of a triboracyclopropenyl anion that persists in solution and in the solid state was identified by Braunschweig and coworkers, who synthesized it by reducing the aminoborane Cl2B=NCy2 (Cy = cyclohexyl) with finely dispersed sodium metal in dimethoxyethane (DME).[7] Cooling of the resulting orange-red solution of the dimeric species Na4[B3(NCy2)3]2 • 2 DME resulted in crystals suitable for X-ray diffraction, by which the structure was determined. Although the detailed reduction mechanism is unknown, it has been suggested that subvalent "R2N−B" intermediates are involved in the formation of such boron clusters.[12]

Structure and bonding

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Due to their special status as the simplest aromatic cycles, the electronic structure of triboracyclopropenyl derivatives has been analyzed with a variety of techniques in computational chemistry. These have ranged from canonical molecular orbital theory to alternative formulations of bonding such as adaptive natural density partitioning theory,[13] the quantum theory of atoms in molecules, natural bond orbital theory, natural orbitals for chemical valence[14] and electron localization function analysis. NICS and ring current calculations have also been used to characterize the aromaticity in such systems by using magnetic criteria.[15] In general, the extremely small size of these cycles implies that their bonding electrons experience substantial Coulomb repulsion, resulting in abnormally high ring strain.[16] This effect is partially compensated for by the stabilization offered by aromatic delocalization.

B3+

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The HOMO and LUMO of B3+ display a2'' and a1' symmetry, respectively. Electron occupation of the former conveys π aromaticity, the latter σ aromaticity.

B3+ displays π aromaticity associated with its a2''-symmetric HOMO. In its singlet electronic ground state, it is a Hückel 2π electron system analogous to the cyclopropenium cation, but it is too reactive to be isolated. It is triangular, with D3h symmetry - all of its B atoms and B-B bond distances are chemically equivalent. The gas-phase adducts B3(N2)3+ and B3(CO)3+ have been computationally studied through ETS-NOCV (extended transition state - natural orbitals for chemical valence) theory, which dissects the changes in energy and electron density that result as a molecule is prepared from a reference state of noninteracting fragments.[17] ETS-NOCV energy decomposition analysis suggests that the N2 and CO adducts are primarily stabilized (by -83.6 and -112.3 kcal/mol respectively) through σ donation of the exocyclic ligands into the highly electron-deficient boron ring. As a result, each was interpreted as a B3+ moiety supported by dative bonding from N2 or CO. The electron deformation density constructed from the NOCVs of this system, together with charges derived from natural bond orbital populations, indicate electron flow from the exocyclic ligand into the ring, which induces all the equivalent bonds of the B3+ core to shorten by approximately 4 pm. π-symmetry interactions are observed with both the weak σ donor N2 and the strong π acceptor ligand CO. However, the out-of-plane π backdonation (from the π system of the B3 ring to the π acceptor orbitals of each ligand) is less stabilizing than the in-plane π backdonation, with strengths of -26.7 and -19.6 kcal/mol for the [B3(CO)2+ + CO] system. This suggests that the minimum-energy configuration of the molecule is one which preserves maximal π aromaticity in the B3+ core.

Just as aromatic species like the cyclopentadienyl anion and the cyclopropenium cation can coordinate to transition metals, it was recently demonstrated that the B3+ ring can bind to metal centers.[18] Laser ablation of a mixed B/Ir target produces two isomers of IrB3−, a B3+ ring coordinated to a formal Ir2- anion. These are a pseudo-planar η2 adduct and a tetrahedral η3 adduct, the latter of which contains an aromatic triboracyclopropenyl fragment. Both are nearly identical in energy and coexist in the generated cluster beam.

 
The Natural Bond Orbital corresponding to the sigma bond between B and Ar in B3Ar3+, displaying 82.6% Ar character and 17.4% B character.[19]
 
AIM analysis reveals strong polarization of the noble gas Ar in the adduct B3Ar3+.[19] Left: The Laplacian of the electron density distribution. Right: The electron density distribution.[20]

Computations suggest that B3+ may even bind inert noble-gas atoms to form an unusual family of compounds B3(Rg)3+ (Rg = rare/noble gas), with nonnegligible bond strengths (from 15 to 30 kcal/mol) that originate from Rg p-orbital σ donicity and a significant degree of charge transfer from Rg to B3+. The possibility of new noble-gas compounds that form exothermally and spontaneously is an opportunity for experimental work.[19][21]

B3

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B3 possesses a singly occupied a1' HOMO (a SOMO) that consists of σ-symmetric orbitals oriented toward the core of the ring, associated with σ delocalization and slightly shorter B-B bond lengths as compared to B3+. It is paramagnetic with a doublet ground state.[22] It is nonpolar, flat and triangular, having D3h symmetry.

B3−

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B3−, with a filled a1' HOMO in D3h symmetry, is considered to be "doubly" aromatic and relatively stable - it simultaneously possesses highly delocalized σ and π electrons in its HOMO and HOMO-1 respectively.[23][24]

B3R32-

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B3R32-, formulated with electron-sharing B−R bonds rather than dative arrows, is isoelectronic to B3+. 8 electrons are assigned to the triboracyclopenyl core, 6 in σ bonding orbitals and 2 in the π system, resulting in Hückel aromaticity. The only experimentally characterized compound of this class is Na4[B3(NCy2)3]2 • 2 DME, a dimer of stacked B3R32- units which are themselves aromatic.[7] Natural bond orbital analysis indicates that this compound is highly stabilized (by roughly 45 kcal/mol) by a donor-acceptor interaction of localized B−B bond orbitals with corresponding B−N antibonding orbital across the ring, in addition to being bound together by electrostatic attraction to bridging Na+ cations identified in the crystal structure. DFT calculations show that the HOMO and HOMO-1 are antisymmetric and symmetric combinations of the π HOMO of an individual ring, respectively - a feature shared with metallocenes. As expected for a species with B−B bonds that have a formal MO bond order of  , the average B-B bond length of 1.62 Å is closer to those of diborene (R-B=B-R) radical cations than B−B single bonds of roughly 1.75 Å.

Spectroscopy and spectrometry

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Triboracyclopropenyl-derived compounds were first identified by their mass-to-charge ratio, as transient species in the mass spectrometry of complex mixtures of cationic boron clusters.[5] Reactive scattering studies with O2 soon followed, revealing the relatively strong bonding within light boron clusters.[6] Subsequently, B3 was isolated in matrices of frozen noble gases and electron paramagnetic resonance spectra were recorded which confirmed its D3h geometry.[22] Hyperfine coupling of the unpaired electron to the 11B nucleus provided an estimate of 15% s-orbital character for the a1' HOMO. The small and nonpolar B3 rings were able to tumble and rotate freely even when confined in the matrix.

In general, triboracyclopropenyl-containing species have been too short-lived and produced in insufficient quantity for transmission-mode infrared spectroscopy. However, dissociating B3(N2)3+ with infrared light and observing the decay of the corresponding mass-to-charge signal via mass spectrometry allowed an effective infrared spectrum of B3(N2)3+ to be recorded.[17][25] This vibrational photodissociation spectrum contained only a single detectable vibration with a redshift of 98 cm−1 relative to gaseous N2, suggesting a highly symmetric B3(N2)3+ adduct with slightly weakened N≡N bonding.

Negatively charged ions containing triboracyclopropenyl have proven amenable to study by photoelectron spectroscopy. By Koopman's theorem, neglecting the effects of strong electron correlation, the kinetic energies of electrons detached by X-rays can be mapped onto binding energies of individual orbitals and reveal the molecular electronic structure.[26][27] Splitting of the resulting spectral peaks from "vibrational progression" (according to the Franck-Condon principle) indicates how ionization at different energies changes specific vibrational frequencies of the molecule, and such effects on bonding are interpreted in terms of changes to the electron configuration. In B3−, an unusually high-intensity and high energy band corresponding to a multielectron or "shake-up" transition (coupled electron detachment and electronic excitation) was observed, suggesting the strong electron correlation present in the triboracyclopropenyl fragment.[4] For IrB3−, vibrational progression from the stretching and breathing vibrations of IrB3 could be assigned in the overlaid spectra of both isomers present in the cluster beam. By comparison to computations, the minimum energy structure of IrB3 could then be formulated as a tetrahedron with an intact, aromatic B3+ moiety.[8]

Reactivity

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Na4[B3(NCy2)3]2 • 2 DME acts as a strong reductant on a variety of substances.[7]

The reactivity of triboracyclopropenyl-containing compounds is relatively under-explored, as only one example has been prepared in the solution phase. The compound reported by Braunschweig, Na4[B3(NCy2)3]2 • 2 DME, is an extremely potent reductant with an oxidation potential of -2.42 V vs. the ferrocene/ferrocenium couple. As a result, it is capable of reducing chloroboranes to afford tetrahedral B clusters, along with reducing PbCl2 directly to metallic Pb. In addition, it will undergo a ring-opening reaction at the B3 moiety by abstracting chlorine atoms from hexachloroethane. This level of reducing power is roughly comparable to an alkali metal, and has not been previously observed for any molecule based on an organic framework.[7]

Although most examples of transition metal-doped trinuclear boron clusters do not contain an aromatic triboracyclopropenyl fragment, the reactivity of such species with small molecules is likely to attract increasing scientific interest. It has been demonstrated under the conditions of mass spectrometry that VB3+ dehydrogenates methane to afford the products VB3CH2+ and H2. A minor side reaction that produces VH+ and eliminates B3CH3 is also operative.[10]

See also

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References

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  1. ^ McKee, Michael L.; Buehl, Michael; Charkin, Oleg P.; Schleyer, Paul v. R. (1993-10-01). "Theoretical investigation of four-center two-electron bonding involving boron derivatives". Inorganic Chemistry. 32 (21): 4549–4554. doi:10.1021/ic00073a014. ISSN 0020-1669.
  2. ^ Korkin, Anatoli A.; Schleyer, Paul v. R.; McKee, Michael L. (1995-02-01). "Theoretical ab Initio Study of Neutral and Charged B3Hn (n = 3-9) Species. Importance of Aromaticity in Determining the Structural Preferences". Inorganic Chemistry. 34 (4): 961–977. doi:10.1021/ic00108a031. ISSN 0020-1669.
  3. ^ Yang, C. L; Zhu, Z. H (2001-08-27). "The ground singlet and low-lying triplet electronic states of B3+". Journal of Molecular Structure: THEOCHEM. 571 (1): 225–229. doi:10.1016/S0166-1280(01)00558-9. ISSN 0166-1280.
  4. ^ a b c Zhai, Hua-Jin; Wang, Lai-Sheng; Alexandrova, Anastassia N.; Boldyrev, Alexander I.; Zakrzewski, Vyacheslav G. (2003-11-01). "Photoelectron Spectroscopy and ab Initio Study of B3- and B4- Anions and Their Neutrals". The Journal of Physical Chemistry A. 107 (44): 9319–9328. Bibcode:2003JPCA..107.9319Z. doi:10.1021/jp0357119. ISSN 1089-5639.
  5. ^ a b Hanley, Luke.; Anderson, Scott L. (1987-09-01). "Production and collision-induced dissociation of small boron cluster ions". The Journal of Physical Chemistry. 91 (20): 5161–5163. doi:10.1021/j100304a007. ISSN 0022-3654.
  6. ^ a b Hanley, Luke; Anderson, Scott L. (1988-09-01). "Oxidation of small boron cluster ions (B+1–13) by oxygen". The Journal of Chemical Physics. 89 (5): 2848–2860. Bibcode:1988JChPh..89.2848H. doi:10.1063/1.454989. ISSN 0021-9606.
  7. ^ a b c d e f Kupfer, Thomas; Braunschweig, Holger; Radacki, Krzysztof (2015-12-07). "The Triboracyclopropenyl Dianion: The Lightest Possible Main-Group-Element Hückel π Aromatic". Angewandte Chemie International Edition. 54 (50): 15084–15088. doi:10.1002/anie.201508670. PMID 26530854.
  8. ^ a b c Czekner, Joseph; Cheung, Ling Fung; Kocheril, G. Stephen; Kulichenko, Maksim; Boldyrev, Alexander I.; Wang, Lai-Sheng (2019-06-24). "High-Resolution Photoelectron Imaging of IrB 3 − : Observation of a π-Aromatic B 3 + Ring Coordinated to a Transition Metal". Angewandte Chemie International Edition. 58 (26): 8877–8881. doi:10.1002/anie.201902406. PMID 31021049. S2CID 131776294.
  9. ^ Chen, Xin; Chen, Teng-Teng; Li, Wan-Lu; Lu, Jun-Bo; Zhao, Li-Juan; Jian, Tian; Hu, Han-Shi; Wang, Lai-Sheng; Li, Jun (2019-01-07). "Lanthanides with Unusually Low Oxidation States in the PrB 3 – and PrB 4 – Boride Clusters". Inorganic Chemistry. 58 (1): 411–418. doi:10.1021/acs.inorgchem.8b02572. ISSN 0020-1669. PMID 30543295. S2CID 56148031.
  10. ^ a b Chen, Qiang; Zhao, Yan-Xia; Jiang, Li-Xue; Li, Hai-Fang; Chen, Jiao-Jiao; Zhang, Ting; Liu, Qing-Yu; He, Sheng-Gui (2018). "Thermal activation of methane by vanadium boride cluster cations VB n + ( n = 3–6)". Physical Chemistry Chemical Physics. 20 (7): 4641–4645. Bibcode:2018PCCP...20.4641C. doi:10.1039/C8CP00071A. ISSN 1463-9076. PMID 29379936.
  11. ^ Jian, Tian; Chen, Xuenian; Li, Si-Dian; Boldyrev, Alexander I.; Li, Jun; Wang, Lai-Sheng (2019). "Probing the structures and bonding of size-selected boron and doped-boron clusters". Chemical Society Reviews. 48 (13): 3550–3591. doi:10.1039/C9CS00233B. ISSN 0306-0012. PMID 31120469. S2CID 162182837.
  12. ^ Wrackmeyer, Bernd (2016). "A Cyclotriborane Dianion and the Triboron Cation: "Light Ends" of the Hückel Rule". Angewandte Chemie International Edition. 55 (6): 1962–1964. doi:10.1002/anie.201510689. ISSN 1521-3773. PMID 26765534.
  13. ^ Tkachenko, Nikolay V.; Boldyrev, Alexander I. (2019-05-08). "Chemical bonding analysis of excited states using the adaptive natural density partitioning method". Physical Chemistry Chemical Physics. 21 (18): 9590–9596. Bibcode:2019PCCP...21.9590T. doi:10.1039/C9CP00379G. ISSN 1463-9084. PMID 31020963. S2CID 131777283.
  14. ^ Mitoraj, Mariusz P.; Michalak, Artur; Ziegler, Tom (2009-04-14). "A Combined Charge and Energy Decomposition Scheme for Bond Analysis". Journal of Chemical Theory and Computation. 5 (4): 962–975. doi:10.1021/ct800503d. ISSN 1549-9618. PMID 26609605.
  15. ^ Pham, Hung Tan; Lim, Kie Zen; Havenith, Remco W. A.; Nguyen, Minh Tho (2016-04-28). "Aromatic character of planar boron-based clusters revisited by ring current calculations". Physical Chemistry Chemical Physics. 18 (17): 11919–11931. Bibcode:2016PCCP...1811919P. doi:10.1039/C5CP07391J. hdl:1854/LU-8549871. ISSN 1463-9084. PMID 26956732. S2CID 205957278.
  16. ^ Himmel, Hans-Jörg (2019-08-19). "Electron-Deficient Triborane and Tetraborane Ring Compounds: Synthesis, Structure, and Bonding". Angewandte Chemie International Edition. 58 (34): 11600–11617. doi:10.1002/anie.201900563. PMID 30786130. S2CID 73514624.
  17. ^ a b Jin, Jiaye; Wang, Guanjun; Zhou, Mingfei; Andrada, Diego M.; Hermann, Markus; Frenking, Gernot (2016-02-05). "The [B 3 (NN) 3 ] + and [B 3 (CO) 3 ] + Complexes Featuring the Smallest π-Aromatic Species B 3 +". Angewandte Chemie International Edition. 55 (6): 2078–2082. doi:10.1002/anie.201509826. PMID 26836340.
  18. ^ Lichtenberger, Dennis L.; Hoppe, Martin L.; Subramanian, Lalitha; Kober, Edward M.; Hughes, Russell P.; Hubbard, John L.; Tucker, David S. (1993-06-01). "Electron distribution and bonding in .eta.3-cyclopropenyl-metal complexes". Organometallics. 12 (6): 2025–2031. doi:10.1021/om00030a011. ISSN 0276-7333.
  19. ^ a b c Li, Zhuo Zhe; Li, An Yong (2017-07-26). "Monocyclic aromatic compounds BnRgn(n−2)+ of boron and rare gases". Physical Chemistry Chemical Physics. 19 (29): 19109–19119. Bibcode:2017PCCP...1919109L. doi:10.1039/C7CP00316A. ISSN 1463-9084. PMID 28702603.
  20. ^ Lu, Tian; Chen, Feiwu (2012). "Multiwfn: A multifunctional wavefunction analyzer". Journal of Computational Chemistry. 33 (5): 580–592. doi:10.1002/jcc.22885. ISSN 1096-987X. PMID 22162017. S2CID 13508697.
  21. ^ Saha, Ranajit; Pan, Sudip; Mandal, Subhajit; Orozco, Mesías; Merino, Gabriel; Chattaraj, Pratim K. (2016-08-17). "Noble gas supported B3+ cluster: formation of strong covalent noble gas–boron bonds". RSC Advances. 6 (82): 78611–78620. Bibcode:2016RSCAd...678611S. doi:10.1039/C6RA16188J. ISSN 2046-2069.
  22. ^ a b Hamrick, Y. M.; Van Zee, R. J.; Weltner, W. (1992-02-01). "Electron-spin resonance and ground states of the boron and aluminum trimers". The Journal of Chemical Physics. 96 (3): 1767–1775. Bibcode:1992JChPh..96.1767H. doi:10.1063/1.462132. ISSN 0021-9606.
  23. ^ Alexandrova, Anastassia N.; Boldyrev, Alexander I.; Zhai, Hua-Jin; Wang, Lai-Sheng (2006-11-01). "All-boron aromatic clusters as potential new inorganic ligands and building blocks in chemistry". Coordination Chemistry Reviews. 18th Main Group Chemistry. 250 (21): 2811–2866. doi:10.1016/j.ccr.2006.03.032. ISSN 0010-8545.
  24. ^ Yang, Li-ming; Wang, Jian; Ding, Yi-hong; Sun, Chia-chung (2007-08-29). "Investigation of the Typical Triangular Structure B 3 in Boron Chemistry: Insight into Bare All-Boron Clusters Used as Ligands or Building Blocks". The Journal of Physical Chemistry A. 111 (37): 9122–9129. Bibcode:2007JPCA..111.9122Y. doi:10.1021/jp074645y. ISSN 1089-5639. PMID 17725336.
  25. ^ Wang, GuanJun; Chi, ChaoXian; Xing, XiaoPeng; Ding, ChuanFan; Zhou, MingFei (2014-01-01). "A collinear tandem time-of-flight mass spectrometer for infrared photodissociation spectroscopy of mass-selected ions". Science China Chemistry. 57 (1): 172–177. doi:10.1007/s11426-013-4979-5. ISSN 1869-1870. S2CID 195203032.
  26. ^ Lineberger, W. Carl (2013-04-01). "Once upon Anion: A Tale of Photodetachment". Annual Review of Physical Chemistry. 64 (1): 21–36. Bibcode:2013ARPC...64...21L. doi:10.1146/annurev-physchem-032511-143753. ISSN 0066-426X. PMID 23216379.
  27. ^ Truhlar, Donald G.; Hiberty, Philippe C.; Shaik, Sason; Gordon, Mark S.; Danovich, David (2019-09-02). "Orbitals and the Interpretation of Photoelectron Spectroscopy and (e,2e) Ionization Experiments". Angewandte Chemie International Edition. 58 (36): 12332–12338. doi:10.1002/anie.201904609. PMID 31081208. S2CID 153290832.
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