Boron Oxide B5O6− Cluster as a Boronyl-Based Inorganic Analog of Phenolate Anion

Boron oxide clusters have structural richness and exotic chemical bonding. We report a quantum chemical study on the binary B₅O₆⁻ cluster, which is relatively oxygen-rich. A global structural search reveals planar C_2v (¹A₁) geometry as the global minimum structure, featuring a heteroatomic hexagonal B₃O₃ ring as its core. The three unsaturated B sites are terminated by two boronyl (BO) groups and an O⁻ ligand. The B₅O₆⁻ cluster can be faithfully formulated as B₃O₃(BO)₂O⁻. This structure is in stark contrast to that of its predecessors, C_s B₅O₅⁻ and T_d B₅O₄⁻, both of which have a tetrahedral B center. Thus, there exists a major structural transformation in B₅O_n⁻ series upon oxidation, indicating intriguing competition between tetrahedral and heterocyclic structures. The chemical bonding analyses show weak 6π aromaticity in the B₅O₆⁻ cluster, rendering it a boronyl analog of phenolate anion (C₆H₅O⁻) or boronyl boroxine. The calculated vertical detachment energy of B₅O₆⁻ cluster is 5.26 eV at PBE0, which greatly surpasses the electron affinities of halogens (Cl: 3.61 eV), suggesting that the cluster belongs to superhalogen anions.

Introduction

Boron is an electron-deficient element with the capacity to build strong covalent bonds with other elements. Owing to boron’s high affinity to oxygen, boron oxide clusters readily form, exhibiting usual structures and exotic chemical bonding (Doyle, 1988; Peiris et al., 1997; Zhai et al., 2007a; Zhai et al., 2007b; Drummond et al., 2007; Li et al., 2008; Shao et al., 2009; Tai and Nguyen, 2009; Yao et al., 2009; Braunschweig et al., 2010; Tai et al., 2010; Zhai et al., 2011; Guo et al., 2013; Li et al., 2013; Miao et al., 2013; Zhai et al., 2014a; Chen et al., 2014; Tian et al., 2015a; Tian et al., 2015b; Zhao et al., 2016; Li et al., 2018; Feng et al., 2019; Li et al., 2019). Elemental boron clusters are intrinsically electron-deficient themselves (Zhai et al., 2003; Alexandrova et al., 2006), and therefore boron oxide clusters are anticipated to be even more electron-deficient. In boron-rich oxide clusters, the boronyl (BO) group has recently emerged as an interesting inorganic ligand (Zhai et al., 2014a), which features a robust B≡O triple bond. In fact, the diatomic BO and BO⁻ species are isoelectronic to CN and CN⁻/CO, respectively. In addition, boronyl is a monovalent σ radical, thus leading to isolobal analogy between the BO and H ligands. As the oxidation proceeds, direct B−B bonding gradually diminishes. Consequently, heteroatomic B−O rings start to appear, which serve as the structural core of boron oxide clusters. Such a heteroatomic ring can be rhombic, pentagonal, hexagonal, or polycyclic, giving rise to a diversity of boron oxide cluster structures that mimic aromatic hydrocarbons (including polycyclic aromatic hydrocarbons, PAHs). Among these is the heterocyclic hexagonal B₃O₃ ring, whose relevant clusters are classified as inorganic benzenes. Typical examples are boroxine (B₃O₃H₃) and, more recently, the boronyl boroxine B₃O₃(BO)₃ cluster (Li et al., 2013).

It is interesting and invaluable to follow the oxidation process of a specific bare boron cluster, step by step. The effort should help precisely identify a variety of cluster structures and structural transformations. Along this line, the B₅O_n⁻ clusters are an intriguing and informative system, which have been extensively studied in the past years (Yao et al., 2009; Zhai et al., 2011; Tian et al., 2015b), (Chen et al., 2012; Chen et al., 2013), (Zhai et al., 2002), including a number of gas-phase spectroscopic works. The B₅⁻ cluster assumes double-chain ribbon geometry with a “W” shape (Zhai et al., 2002), while the B₅⁺ cluster is pentagonal (Alexandrova et al., 2006). The B₅O_n⁻ (n = 1–3) clusters are entirely dictated by boronyl groups, whose number increases steadily from 1 to 3, reducing the size of boron core from rhombic B₄ to triangular B₃ and then to dimer B₂ (Zhai et al., 2011; Chen et al., 2012; Chen et al., 2013). The first one or two boronyl ligands are terminally attached to the boron core, whereas the third one occupies a bridging position. The coordination pattern is similar to a hydrogen ligand in boranes, demonstrating the BO/H isolobal analogy. It is noted that all B₅O_n⁻ (n = 0–3) clusters are perfectly planar. In the B₅O₄⁻ cluster (Yao et al., 2009), a tetrahedral geometry occurs, which is still governed by boronyl ligands, except that their number increases to four. It can be formulated as B(BO)₄⁻, being isovalent to BH₄⁻ or CH₄. The B₅O₅⁻ cluster inherits the tetrahedral geometry of B₅O₄⁻ upon substitution of one boronyl terminal by a linear OBO unit (Tian et al., 2015b). What is next in the sequential oxidation process of bare B₅ cluster? Would the tetrahedral geometry persist? What new type of structure would appear? These remain to be open questions in the field.

In the present work, we are motivated to address the abovementioned issues. We report on the structural, electronic, and chemical bonding properties of boron oxide B₅O₆⁻ cluster via computer global searches and quantum chemical calculations. It turns out that the global minimum (GM) structure of B₅O₆⁻ cluster features a heterocyclic B₃O₃ core, whose three unsaturated B sites are decorated by two BO ligands and one O⁻ unit. Herein, the abbreviation “GM” refers to a structure that is lowest in energy on the potential energy surface of a specific molecular system, which is routinely used in physical chemistry or cluster literature. The hexagonal B₃O₃ core is stabilized by a moderately delocalized 6π system, thus rendering the B₅O₆⁻ cluster a boronyl-based analog of benzene, akin to boroxine or boronyl boroxine (Li et al., 2013). In terms of the overall chemical bonding pattern, it is proposed that the B₅O₆⁻ cluster closely mimics phenolate anion (C₆H₅O⁻). The relatively localized extra charge (O⁻) in B₅O₆⁻ cluster gives rise to high vertical detachment energy (VDE) beyond 5 eV, indicating that the cluster is a superhalogen anion (Gutsev and Boldyrev, 1984; Srivastava, 2022; Kandalam et al., 2015; A Technical Note).

Methods

The GM structural searches for B₅O₆⁻ cluster were carried out at the PBE0/3-21G level using the coalescence kick (CK) algorithm (Saunders, 2004; Sergeeva et al., 2011). A total of 8000 stationary points were probed on its potential energy surface (4000 for singlet and triplet states each). The identified low-lying isomers were then fully reoptimized at the PBE0/6-311+G(d) level and their relative energies evaluated, including zero-point energy (ZPE) corrections. The vibrational frequencies were calculated at the same level to ensure that the reported structures are true minima on the potential energy surface.

Our further effort to assess the energetics for top candidate structures is as follows. First, the PBE0-D3/6-311+G(d) calculations were carried out to take into account dispersion correction. Second, comparative B3LYP-D3/6-311+G(d) calculations were carried out to check for consistency of density functionals; the PBE0 and B3LYP functionals have been widely considered to be complementary with each other. Third, single-point CCSD(T)/6-311+G(d) calculations (Purvis and Bartlett, 1982) were carried out on the basis of optimized PBE0-D3/6-311+G(d) geometries, which shall serve as a benchmark of the energetics data. All four sets of energetics data are highly consistent.

The NBO 6.0 program (Glendening et al., 2013) was used for the natural bond orbital (NBO) (Reed et al., 1988) analysis, which offers Wiberg bond indices (WBIs) and natural atomic charges. Chemical bonding was elucidated via canonical molecular orbital (CMO) analysis, adaptive natural density partitioning (AdNDP) (Zubarev and Boldyrev, 2008), and electron local functions (ELFs) (Silvi and Savin, 1994). To assess π aromaticity, nucleus-independent chemical shifts (NICSs) were also calculated (Schleyer et al., 1996), which were supplemented by the isochemical shielded surface (ICSS) analysis (Guo et al., 2020). The latter was performed using the Multiwfn program (Lu and Chen, 2012). The VDEs were calculated using the time-dependent PBE0 (TD-PBE0) (Bauernschmitt and Ahlrichs, 1996; Casida et al., 1998) and outer valence Green’s function (OVGF) (von Niessen et al., 1984; Zakrzewski and von Niessen, 1993; Zakrzewski and Ortiz, 1995) methods and at the single-point CCSD(T) level. All the electronic structure calculations were carried out using the Gaussian 09 package (Frisch, 2009).

Results

Global Minimum Structure and Alternative Low-Lying Isomers

Our computational structural searches lead to the GM structure 1 (C_2v, ¹A₁) for anion B₅O₆⁻ cluster; see Figure 1. Alternative low-lying isomeric structures are presented in Figure 2 along with their relative energies at four levels of theory: PBE0/6-311+G(d), PBE0-D3/6-311+G(d), and B3LYP-D3/6-311+G(d) levels, as well as the single-point CCSD(T)/6-311+G(d) level on the basis of PBE0-D3/6-311+G(d) geometries. The four sets of independent energetics data are highly consistent (Figure 2), firmly establishing cluster 1 as the GM structure. It is relatively well-defined on the potential energy surface, being at least 12 kcal mol⁻¹ more stable than any alternative geometry. It is noted that the PBE0 functional has been widely tested for boron clusters (Zhai et al., 2014b; Fagiani et al., 2017; Guo et al., 2017), which is a popular and reliable choice for boron-based systems.

FIGURE 1

FIGURE 1. Global minimum (GM) structure of B₅O₆⁻ (1, C_2v, ¹A₁) cluster and a representative 2 (C_s, ¹A′) isomer. They feature a heterocyclic hexagonal B₃O₃ ring and a tetrahedral B center, respectively. Relevant structures 3/4 of B₅O₅⁻ cluster (left panels) show a distinctly reversed energy order. The relative energies are shown in kcal mol⁻¹ at the PBE0/6-311+G(d) level.

FIGURE 2

FIGURE 2. Alternative optimized low-lying isomeric structures of B₅O₆⁻ cluster at the PBE0/6-311+G(d) level along with their relative energies (in kcal mol⁻¹), including zero-point energy (ZPE) corrections. The energetics data are also presented at the PBE0-D3/6-311+G(d) (in brackets, with ZPE corrections) and B3LYP-D3/6-311+G(d) (in square brackets, with ZPE corrections) levels, as well as at single-point CCSD(T)/6-311+G(d) level based on their PBE0-D3/6-311+G(d) geometries (in curly brackets).

Cluster 1 is closed-shell. The lowest-energy triplet structure is 54.85 kcal mol⁻¹ higher in energy at the single-point CCSD(T) level (Figure 2). Among the low-lying isomers is a tetrahedral 2 (C_s, ¹A′) structure, which is 22.10 kcal mol⁻¹ above GM cluster 1 at PBE0 [20.85 kcal mol⁻¹ at single-point CCSD(T)]. Its geometry can be traced back to the GM structure 3 (C_s, ¹A′) of anion B₅O₅⁻ cluster (Figure 1) (Tian et al., 2015b), upon substitution of one terminal boronyl by an OBO unit. For the latter cluster, hexagonal isomer 4 (C_s, ¹A′) is substantially higher in energy than GM cluster 3, by as much as 33.31 kcal mol⁻¹ at PBE0. Structures 1–4 have an intriguing energetics relationship; see Figure 1. A clear structural transition occurs from B₅O₅⁻ to B₅O₆⁻. The optimized Cartesian coordinates of structures 1 and 2 are presented in Supplementary Table S1 (ESI†).

Bond Distances, Wiberg Bond Indices, and Natural Atomic Charges

As shown in Figure 3, the perfectly planar GM B₅O₆⁻ (1, C_2v, ¹A₁) cluster contains a heteroatomic hexagonal B₃O₃ ring, two-terminal BO ligands, and one terminal O unit. The BO or O units are attached to three B sites on the periphery. The structure is relatively straightforward to elucidate based on interatomic distances. Typical triple B≡O, double B=O, single B−O, and single B−B bonds are around 1.21, 1.28, 1.37, and 1.66 Å, respectively (Yao et al., 2009; Zhai et al., 2014a; Tian et al., 2015b; Pyykkö and Atsumi, 2009). The bond distances for BO links in hexagonal ring of cluster 1 are slightly uneven (1.33–1.48 Å; Figure 3, left panel) due to asymmetric coordination of B sites. Their average value is in line with single B−O bonds. The terminal BO groups (1.21 Å) are assigned as boronyls with triple B≡O bonds. In contrast, the upper BO unit (1.26 Å) is close to a double B=O bond.

FIGURE 3

FIGURE 3. Optimized bond distances (in Å; black color) of GM structure 1 and isomer 2 of the B₅O₆⁻ cluster at the PBE0/6-311+G(d) level. Also shown are their Wiberg bond indices (WBIs; blue color) from the natural bond orbital (NBO) analysis. The B atoms are illustrated in blue and O in red.

The calculated WBIs generally confirm the abovementioned assignments (Figure 3, left panel). The inner BO links have WBI values of 0.64–1.10, in line with (uneven) single bonds. The boronyl groups have WBIs of 1.87 owing to their polar nature (Zhai et al., 2014a). The upper BO unit has a smaller WBI value of 1.56, in line with a double bond. The calculated natural atomic charges for cluster 1 are shown in Figure 4. There are moderate intramolecular B−O charge transfers within the B₃O₃ core, within boronyl groups, and in between the core and terminals. The charge transfers are relatively local processes, suggesting polar and yet covalent BO chemical bonding.

FIGURE 4

FIGURE 4. Calculated natural atomic charges (in |e|) for structures 1 and 2 of the B₅O₆⁻ cluster from the NBO analysis at PBE0/6-311+G(d), as compared to those of B₅O₅⁻ (3, C_s, ¹A′), B₅O₅⁻ (4, C_s, ¹A′), and B₅O₄⁻ (5, T_d, ¹A₁) clusters. The B atoms are shown in blue and O in red.

Likewise, the isomeric tetrahedral B₅O₆⁻ (2, C_s, ¹A′) structure can be easily understood (Figures 3, 4). It consists of a central B site, two BO groups, and two OBO groups. The components are held together in a tetrahedral fashion. Approximately, in anion cluster, the B center forms four B−B or B−O single bonds with terminal ligands, whose B−B (1.72 Å) and B−O (1.49–1.50 Å) links are somewhat elongated with respect to the abovementioned reference values for single bonds. However, their WBIs are 0.97 and 0.67, respectively, and even the latter seems reasonable (for a polar bond). Such a bonding situation around the B center is less than ideal, which is partly the reason why this structure is a higher-energy isomer (vide infra). For the terminal ligands, two BO groups (1.21 Å) are boronyls with WBIs of 1.84. The two OBO units are asymmetric in terms of B−O distances: 1.22 versus 1.29 Å. Their average is close to a double B=O bond. The calculated natural atomic charges of cluster 2 are presented in Figure 4. The central B site is practically neutral (+0.12 |e|) despite the fact that other B atoms each carry a larger positive charge (+0.85 and +1.21 |e|). This situation again hints that the central B site struggles severely in order to maintain four-fold bonding.

To aid the understanding of GM C_2v B₅O₆⁻ (1) and isomeric C_s B₅O₆⁻ (2) clusters, three prior species (Yao et al., 2009; Tian et al., 2015b) are also analyzed: tetrahedral GM C_s B₅O₅⁻ (3), hexagonal isomeric C_s B₅O₅⁻ (4), and tetrahedral GM T_d B₅O₄⁻ (5). Their calculated bond distances and WBIs (Supplementary Figure S1, ESI†) and natural atomic charges (Figure 4) are well behaved, providing support to our assessment with regard to clusters 1 and 2 (as described above).

Superhalogen Anion

The electronic properties of GM B₅O₆⁻ (1) cluster are predicted here to aid its future experimental characterization in the gas phase. The calculated ground-state VDE of B₅O₆⁻ (1) cluster and those of a few relevant species are presented in Supplementary Table S2 (ESI†) at three levels of theory: PBE0, single-point CCSD(T), and OVGF. Using the experimentally known B₄O₃⁻ cluster (Zhai et al., 2007a) as a calibration, it is shown that the PBE0 and single-point CCSD(T) data are superior to those of OVGF; see a note in Supplementary Table S2 (ESI†). The VDE of GM B₅O₆⁻ (1) cluster amounts to 5.26 eV at PBE0 and 5.14 eV at CCSD(T), which is quite high, markedly surpassing the electron affinities of halogens (Cl: 3.61 eV). The ground-state VDEs of the whole B₅O_n⁻ (n = 1–6) series at PBE0/6-311+G(d) are plotted in Figure 5, which show an abrupt increase between n = 3 and 4. All the B₅O_n⁻ (n = 4–6) species have high VDEs. Based on this observation, the GM B₅O₆⁻ (1) cluster clearly belongs to the class of species called superhalogen anions. (Gutsev and Boldyrev, 1984; Srivastava, 2022; Kandalam et al., 2015; A Technical Note)

FIGURE 5

FIGURE 5. Evolution of ground-state vertical detachment energies (VDEs) of B₅O_n⁻ (n = 1–6) series calculated at the PBE0/6-311+G(d) level.

The simulated photoelectron spectrum of GM B₅O₆⁻ (1) cluster is presented in Figure 6, according to the TD-PBE0 calculation, which has three well-separated bands in the 5–7 eV binding energy regime. For comparison, the simulation is also carried out for isomeric structure 2 with a higher ground-state band (Figure 6B). A nature implication is that for their corresponding neutral species, the hexagonal structure has an even greater advantage in terms of energetics (over tetrahedral structure). Indeed, our PBE0 calculations show that the hexagonal neutral B₅O₆ cluster is 54.59 kcal mol⁻¹ below its tetrahedral counterpart, as compared to a relative energy of 22.10 kcal mol⁻¹ between anionic 1/2 structures at the same level (Figure 1). The two neutral structures are analyzed in Supplementary Figures S2, S3 (ESI†). For the hexagonal anion/neutral system, the extra charge goes primarily to the upper O terminal (by as much as 0.66 |e|), which further justifies the assessment of an O⁻ terminal for GM B₅O₆⁻ (1) cluster, as well as its exact analogy to phenolate anion (vide infra). In contrast, the extra charge in the tetrahedral system smears over the entire cluster (with the central B site gaining 0.34 |e| only), thus leading to an even higher ground-state VDE.

FIGURE 6

FIGURE 6. Simulated photoelectron spectra of anionic B₅O₆⁻ (1) and B₅O₆⁻ (2) clusters at the time-dependent PBE0/6-311+G(d) (TD-PBE0) level.

Discussion

Heterocyclic Hexagonal Global-Minimum C_2v B₅O₆⁻ Cluster: A Boronyl-Based Inorganic Analog of Phenolate Anion

The GM C_2v B₅O₆⁻ (1) cluster marks the exact onset of a heteroatomic hexagonal B₃O₃ ring along the whole B₅O_n⁻ (n = 0–6) series (Zhai et al., 2002; Yao et al., 2009; Zhai et al., 2011; Chen et al., 2012; Chen et al., 2013; Tian et al., 2015b). A simple valence electron counting suggests that the available number of electrons for direct B−B bonding diminishes gradually from 16 electrons in B₅⁻ down to 4 in B₅O₆⁻, two electrons for each additional O atom. Indeed, both GM B₅O₆⁻ cluster 1 and isomeric structure 2 have four electrons for direct B−B bonding, that is, two B−B single bonds (see Figure 1).

To fully understand GM B₅O₆⁻ (1) cluster, it is essential to conduct an in-depth analysis of chemical bonding. We choose to focus on the CMO analysis, which is fundamental for a molecular system. Cluster 1 is a closed-shell structure with 52 valence electrons. The 26 occupied CMOs are presented in Figure 7, which are sorted into five subsets according to their components of atomic orbitals (AOs). The seven CMOs in subset (a) are classified as O lone-pairs. Among them, HOMO−21/HOMO−24/HOMO−25 are typical bonding/nonbonding/antibonding combination of O 2s AOs from three O sites in the hexagonal ring owing to pseudo-three-fold symmetry of the cluster. According to the CMO building principles, they are readily recombined as three O 2s lone pairs. HOMO−20 is an O 2s lone-pair on the upper O site, whereas HOMO−22/HOMO−23 recombine as two O 2s lone-pairs on terminal boronyls. The HOMO approximately represents an O 2p lone-pair on the upper O site with 88% contribution from tangential O 2p AO. Thus, the upper O site has two lone pairs, and the remaining O sites each have one lone pair.

FIGURE 7

FIGURE 7. Pictures of occupied canonical molecular orbitals (CMOs) of B₅O₆⁻ (1) cluster. (A) Seven lone pairs for the O atoms, including two for the upper O site. (B) Nine σ CMOs for Lewis-type skeleton and terminal B−O σ bonds. (C) Two σ CMOs for Lewis-type B−B σ single bonds. (D) Five CMOs for both in-plane and out-of-plane π bonds relevant to terminal B−O units. (E) Three delocalized π CMOs over the B₃O₃ ring.

In subset (b), nine B−O σ single bonds are presented. Specifically, HOMO−3 is a σ bond for terminal B−O unit at the top. HOMO−13/HOMO−14 recombine as two σ bonds on the bottom boronyl groups. These are primarily contributed by radial O 2p AOs from three terminal O sites. The next six CMOs are responsible for skeleton B−O σ bonds along the hexagonal ring, which are evenly contributed by the B/O sites: radial O 2p AOs versus tangential B 2p AOs.

The CMOs in subset (c) are two B−B σ bonds, which link hexagonal rings and two boronyl ligands. The subset (d) shows the terminal B−O π bonds, including two in-plane π bonds on boronyls. Overall, the three-terminal B−O links each have one σ bond (Figure 7B) and one out-of-plane π bond (Figure 7D). Furthermore, the boronyl groups each have one in-plane π bond. The boronyls show triple bonds, whereas the upper B−O terminal has a double bond.

All the abovementioned CMOs are Lewis-type bonding elements: seven O 2s/2p lone-pairs, six B−O σ single bonds along the hexagon, two B−B σ bonds, one B=O double bond for the upper terminal, and two B≡O triple bonds for boronyls. These Lewis elements collectively consume 23 pairs of electrons, leaving the remaining six electrons for a π framework over the hexagonal ring (Figure 7E). Of the three π CMOs, HOMO−4 recombines partially with HOMO−10 to get “purified,” which has a B versus O ratio of roughly 1/11 in the hexagon. HOMO−6 has a ratio of 1/11 for B/O contributions. For HOMO−15, the ratio of B/O contributions in the ring boosts greatly to about 1/1. Overall, the B components in the π framework cannot be ignored, and the π sextet should be viewed as six-centered (at least formally). This π pattern is closely similar to that in boroxine and boronyl boroxine (Li et al., 2013), thus rendering GM B₅O₆⁻ (1) cluster a new member of the “inorganic benzene” family. The 6π electron-counting conforms to the (4n + 2) Hückel rule for aromaticity. The bonding picture is elegantly borne out from the AdNDP analysis (Zubarev and Boldyrev, 2008), as shown in Figure 8. All the occupation numbers (ONs) are close to ideal.

FIGURE 8

FIGURE 8. Chemical bonding pattern of B₅O₆⁻ (1) cluster according to the adaptive natural density partitioning (AdNDP) analysis. The occupation numbers (ONs) are indicated.

Based on the bonding picture, we should propose that GM B₅O₆⁻ (1) cluster is an exact boronyl-based analog of phenolate anion. They share the same characteristic structural and bonding features. First, they both have a hexagonal core: heteroatomic B₃O₃ ring versus C₆ ring. The two kinds of rings are actually isoelectronic in terms of hexagonal bonding, once lone-pairs or terminal Lewis-type bonds are accounted for. Indeed, each ring consumes 18 electrons for chemical bonding within the ring. Second, both species possess a π sextet. Third, both species have an O⁻ terminal, which is attached to the hexagon via a double bond (B=O⁻ versus C=O⁻). It is appropriate to state that the current finding of chemical analogy between GM B₅O₆⁻ (1) cluster and phenolate anion parallels that between boronyl boroxine (Li et al., 2013) and benzene.

We shall only briefly mention the tetrahedral isomeric cluster B₅O₆⁻ (2). Its structural characters suggest a relatively classical cluster between a formal B⁻ center and four ligands (two boronyls versus two OBO units), via single bonds in a tetrahedral fashion. The chemical bonding within an OBO unit is presented in Supplementary Figure S4 (ESI†). Here, HOMO−16 and HOMO form a three-center, four-electron (3c-4e) π bond in the vicinity of an OBO unit, that is, “π hyperbond,” which is in a bonding/nonbonding combination due to its three-center nature. The upper CMO has relatively minor bonding or antibonding effect. Thus, a 3c-4e π bond is, in effect, equivalent to a 3c-2e bond or two B−O half bonds. There is a second 3c-4e π bond (HOMO−17 and HOMO−1) on the same OBO unit, which offers two B−O half bonds in the perpendicular direction. In short, the four CMOs in Supplementary Figure S4A (ESI†) can be collectively viewed as two B−O single bonds, similar to the prior tetrahedral C_s B₅O₅⁻ (3) cluster (Tian et al., 2015b) (see Supplementary Figure S4B, ESI†). An OBO unit in cluster 2 also has two B−O σ bonds (not shown). The same ideal works for the other OBO ligand. Overall, the OBO ligands can be formulated as O=B=O, featuring double bonds.

Weak 6π Aromaticity in C_2v B₅O₆⁻ Cluster: Comparison With a Series of Relevant Species

The π sextet in GM B₅O₆⁻ (1) cluster stems primarily from three O 2p_z lone-pairs in the hexagonal ring, taking advantage of the empty B 2p_z AOs from three neighboring B sites for six-centered π delocalization. Consequently, π aromaticity in cluster 1 is expected to be moderate only, despite its ideal 6π electron-counting. To quantitatively probe π aromaticity in cluster 1, we have calculated the color-filled maps of ICSS in the z-direction, that is, ICSS_zz (in ppm) (Guo et al., 2020), as shown in Figure 9A at 1.0 Å above the molecular plane. It noted that a positive ICSS_zz value indicates aromaticity. It turns out that the shielding effect at 1.0 Å above the ring center of cluster 1 is weak and only at a larger distance (such as 1.5 or 2.0 Å) does the shielding become apparent. Specifically, the calculated NICS_zz values for cluster 1 are +2.08 (likely due to disturbance from O lone-pairs), −3.24, and −4.02 ppm at 1.0, 1.5, and 2.0 Å, respectively, a trend in line with weak π aromaticity. For comparison, the corresponding NICS_zz values for boronyl boroxine are −1.97, −6.07, and −5.73 ppm, respectively, indicating slightly stronger π aromaticity.

FIGURE 9

FIGURE 9. Color-filled maps of iso-chemical shielding surfaces (ICSSs) in the z-direction, ICSS_zz (in ppm), for (A) B₅O₆⁻ (1) and (B) boronyl boroxine D_3h B₆O₆ clusters. Positive ICSS_zz values indicate aromaticity. The calculations are carried out on a plane that is 1.0 Å above the molecular plane.

Alternatively, we can also compare the extent of π aromaticity of GM B₅O₆⁻ (1) cluster and relevant species using the ELF data. (Silvi and Savin, 1994), (Wang et al., 2017) The π bifurcation value, ELF_π, of GM B₅O₆⁻ (1) cluster is compared with those of boroxine D_3h B₃O₃H₃, boronyl boroxine D_3h B₆O₆, and benzene D_6h C₆H₆ in Supplementary Figure S5 (ESI†). Not surprisingly, benzene has a π bifurcation value that is close to 1.0. Boroxine and boronyl boroxine (Li et al., 2013) have smaller and yet comparable π bifurcation values (0.64 versus 0.67). The GM B₅O₆⁻ (1) cluster has an even smaller π bifurcation value of 0.53, which is marginally π aromatic. The primary reason is that cluster 1 is asymmetrically coordinated so that its hexagonal ring has uneven B−O bond distances (Figure 3).

A Plausible Mechanism for Structural Transition in the B₅O₆⁻ Cluster: From Tetrahedral Isomer to Hexagonal Global Minimum

A possible mechanism for tetrahedral-to-hexagonal structure transition from 3/2 to 1 is illustrated in Figure 10. This is an oxygen diradical nucleophilic substitution mechanism. Our starting point is tetrahedral GM B₅O₅⁻ (3) cluster, which is substantially more stable than its hexagonal isomer 4 (Figure 1) and inherits the geometry from GM T_d B₅O₄⁻ (5) cluster. Upon insertion of an O atom (assumed as oxygen diradical) between the B⁻ center and one boronyl terminal, the negative charge on central B⁻ site would migrate to its surrounding, thus leading to structure 2 (step 1), which is illustrated approximately only. Next, the negatively charged BO migrates to bind a neighboring positively charged B center in the OBO ligand and the charge further migrates so that the former OBO units are ready to fuse (step 2). In other words, the electron-rich boronyl group acts as a nucleophilic reagent to attack a weaker B–O link. A key structure 6 is present here. Interestingly, structure 6 has been identified as well in our structural searches, which is the 9th isomer in Figure 2.

FIGURE 10

FIGURE 10. Plausible mechanism for the structural evolution between tetrahedral B₅O₅⁻ (3) and hexagonal B₅O₆⁻ (1) clusters.

Once structure 6 is reached, the next are downhill processes. The negative terminal O center binds with the positive B center in the second OBO ligand and a heterocyclic hexagon is formed (structure 1′; step 3). The formation of π sextet from 1′ results in the final structure of cluster 1 (step 4). The abovementioned mechanism is primarily based on regioselectivity and stereoselectivity (Ren et al., 2017).

The proposed mechanism is reasonable also for a different reason, as outlined in Section Bond Distances, Wiberg Bond Indices, and Natural Atomic Charges. Basically, isomer B₅O₆⁻ (2) is not an ideal system, despite its tetrahedral configuration similar to those of B₅O₄⁻ (5) and B₅O₅⁻ (3) (see Figure 4). Ideally, the central site of a tetrahedral molecular system should be valence four so that four Lewis-type single σ bonds can form, such as in CH₄ and BH₄⁻. The central B site in B₅O₄⁻ (5) and B₅O₅⁻ (3) are in the B^−1.63 and B^−0.66 charge states, respectively (Figure 4). In stark contrast, the central B site in B₅O₆⁻ (2) is practically neutral (+0.12 |e|) and inconsistent with a formal B⁻ center. As a consequence, the tetrahedral coordination is not favorable for the B₅O₆⁻ cluster, which is susceptible to structural transformation.

Conclusion

The structural and bonding properties of a boron oxide B₅O₆⁻ cluster has been studied using computer global structure searches and quantum chemical calculations, revealing a perfectly planar C_2v (¹A₁) global minimum geometry. It has a heterocyclic B₃O₃ hexagon as the core, which is terminally bonded to two boronyls and one O⁻ ligand, marking the exact onset of a hexagonal ring in the B₅O_n⁻ (n = 1–6) cluster series. The electronic structure shows a rather high vertical electron affinity of greater than 5 eV, suggesting that the species belongs to superhalogen anions. Chemically, the B₅O₆⁻ C_2v (¹A₁) cluster is a close boronyl-based analog to phenolate anion, in which a boronyl ligand is isovalent to hydrogen and a heteroatomic B₃O₃ ring substitutes a C₆ ring. The two kinds of hexagonal rings are, in effect, isoelectronic with each other in terms of the available number of electrons for bonding within the rings. The B₅O₆⁻ C_2v (¹A₁) cluster features a π sextet, similar to those in boroxine and boronyl boroxine, thus also rendering the cluster a new member of the “inorganic benzene” family. A plausible mechanism is proposed to account for the tetrahedral-to-hexagonal structure transition in the B₅O_n⁻ (n = 1–6) clusters.

Data Availability Statement

The original contributions presented in the study are included in the article/Supplementary Material; further inquiries can be directed to the corresponding authors.

Author Contributions

The topic of this study is discussed and determined by J-CG and H-JZ. S-JG performed the global minimum search; carried out the geometry optimization and frequency calculations of all the isomers; and the calculations of VDEs, molecular orbital chemical bonding analyses, and the AdNDP chemical bonding analyses. The data analyses were carried out by J-CG and H-JZ. The manuscript was written and commented by all the authors.

Funding

This work was supported by the National Natural Science Foundation of China (Nos. 21873058, 21573138, and 22173053), the Natural Science Foundation of Shanxi Province (Nos. 201801D121103 and 20210302123439), the Shanxi “1331” Project, the Scientific and Technological Innovation Programs of Higher Education Institutions in Shanxi (No. STIP 2019L0965), the Key Research and Development Project in High-tech Field of the Lvliang Science and Technology Bureau (No. 2021GXYF-2-62), and the Lvliang Key Laboratory of Optical and Electronic Materials and Devices (No. 2021ZDSY-2-88).

Conflict of Interest

The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.

Publisher’s Note

All claims expressed in this article are solely those of the authors and do not necessarily represent those of their affiliated organizations, or those of the publisher, the editors, and the reviewers. Any product that may be evaluated in this article, or claim that may be made by its manufacturer, is not guaranteed or endorsed by the publisher.

Supplementary Material

The Supplementary Material for this article can be found online at: https://www.frontiersin.org/articles/10.3389/fchem.2022.868782/full#supplementary-material

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