Planar Tetracoordinate Carbon in 6σ + 2π Double Aromatic CBe42– Derivatives

Bo JIN Jian-Hong BIAN Xue-Feng ZHAO Cai-Xia YUAN Jin-Chang GUO Yan-Bo WU

Citation:  Bo JIN, Jian-Hong BIAN, Xue-Feng ZHAO, Cai-Xia YUAN, Jin-Chang GUO, Yan-Bo WU. Planar Tetracoordinate Carbon in 6σ + 2π Double Aromatic CBe42– Derivatives[J]. Chinese Journal of Structural Chemistry, 2022, 41(3): 2203218-2203226. doi: 10.14102/j.cnki.0254-5861.2011-3332 shu

Planar Tetracoordinate Carbon in 6σ + 2π Double Aromatic CBe42– Derivatives

English

  • As a typical electron deficient element (two electrons in four valence orbitals), beryllium (Be) prefers the multicenter bonding to have the number of its valence shell electrons as much as possible. Such a bonding preference is particularly useful for designing the species with non-classical planar hypercoordinate carbon (phC). In 2008, Wang group first designed a series of planar tetracoordinate carbon (ptC) species involving beryllium[1]. In 2010 and 2016, Wu and Wang groups designed BeH-based ptC species with the carbon skeletons of monocyclic arenes and ethylene, whose structural models were also extended to various types of nanomolecules[2, 3]. In 2018 and 2019, Guo et al. reported a series of global minima ptC species, including CBe4Au4, CBe4Li4, and CBe3X3+ (X = H, Li, Na, Cu, Ag)[46].

    In comparison with the being employed for designing ptC species, beryllium was more frequently and successfully employed in designing species with planar pentacoordinate carbon (ppC) previously. In 2010 and 2012, Wang, Wu, and Merino joint groups reported the global energy minima (GEM) ppC species CAl4Be, CAl3Be2, CAl2Be32–, and CAl2Be3Li by substituting the aluminum atom(s) in milestone CAl5+ with beryllium atom(s)[7, 8]. In 2018, Wu group further found that these GEM ppC species can be further stabilized by introducing H atom on the peripheral edges involving beryllium atom[9]. In 2012, Merino group designed the GEM CBe5E (E = Al, Ga, In, Tl) with a CBe4E ppC core moiety[10]. In 2008, Luo et al. reported the hexatomic species CBe5 and CBe54– with a ppC[11]. Remarkably, though highly negatively charged CBe54– was unstable, it was employed subsequently as a core moiety to design dozens of σ and π double aromatic GEM species with a ppC CBe5Enn–4 (n = 1~5) by introducing various kinds and numbers of monovalent elements (including H, Li, Na, K, F, Cl, Br, Au) to the bridging positions of Be–Be edges[1215].

    Beryllium has also been applied to design the species with planar hexacoordinate carbon or boron (p6C[16] or p6B[17]) as well as the planar heptacoordinate transition metals. Beryllium was utilized to design the monolayer sheets with perfect ptC[18], the zig-zag double chain nanoribbon with ppC and ribbon aromaticity[19], the quasi-ppC-containing monolayer sheet featuring the half metallic property and negative Poisson ratio[20], and the semi-conductive monolayer sheet with quasi-p6C[21].

    In the application of beryllium to design phC species, the most exciting part by far should be the design of ppC, because beryllium was involved in more than half of GEM ppC species. In particular, the ppC-containing CBe54– derivatives were the paragon of such non-classical molecule design. Dozens of species can be designed by stepwise introduction of various mon-valent elements onto the Be-Be edges of CBe54– and the majority of these species were turned out to the GEM. Is there a similar paragon that can be employed in the design of ptC? The answer is positive. We will show in the following that CBe42– species can play the parallel role in designing ptC species to that played by CBe54– in designing ppC species.

    The geometries of designed species were optimized and the subsequent harmonic vibrational frequencies were analyzed at both B3LYP/BS1 and B2PLYP-D/BS1 levels. Herein, BS1 is a mixed basis set used in this work with aug-cc-pVTZ for elements lighter than Cu and aug-cc-pVTZ-PP for Cu and heavier elements; while B2PLYP-D is a double hybrid B2PLYP functional considering the empirical dispersion. The geometries and frequencies obtained using B3LYP functional were not different in essential from those obtained using B2PLYP-D, so the B3LYP functional was employed for further studies, including electronic structure analyses and stability explorations. The chemical bonding in the designed species was interpreted using adaptive natural density partitioning (AdNDP) analyses at the B3LYP/BS2 level, where BS2 denotes a mixed basis sets with 6-31G(d) for elements lighter than Br and LANL2DZ for heavier elements. The potential energy surfaces of the concerned components were explored using the stochastic search algorithm. Both the singlet and triplet surfaces were considered. The generated random structures were initially optimized at the B3LYP/BS2 level, and then ten lowest isomers were optimized and harmonic vibrational frequencies were analyzed at the B3LYP/BS1 level. The energies of these isomer were further improved at the CCSD(T)/BS1 level and the relative energies were compared using the CCSD(T)/BS1 single point energy in combination with the zero-point energy corrections obtained at the B3LYP/BS1 level (abbreviated as CCSD(T)//B3LYP). The dynamic stability of designed species was studied using Born-Oppenheimer molecular dynamic (BOMD)[22, 23] simulations at the B3LYP/BS2 level at 298 K. The structural evolution during simulation was described by the root-mean-square derivation (RMSD, in Å) relative to the B3LYP/BS2-optimized structures. The nucleus-independent chemical shifts (NICS)[24-26] were calculated at the centers of the three-membered rings and the points located 2 Å above the centers of the three-membered rings and above ptCs to assess the aromatic nature of these ptC species. The AdNDP analyses were performed using AdNDP program[27, 28], the stochastic search algorithm[29, 30] was realized using GXYZ 2.0 program[31, 32], the CCSD(T) calculations were carried out using MolPro 2012.1 package[33], and all other calculations were performed using Gaussian 16 package[34].

    We had recently reported the ptC species CBe4Mnn–2 (M = Li, Au, n = 1~3)[35]. In that work, we focused on achieving the 14 valence electrons species with ptC rather than the systematic design of ptC species based on a good template structure. Nevertheless, we found that the similar structural model might be extended to the congeners of Li and Au, including Na, Cu, and Ag, though the potential energy surfaces of corresponding species were not explored. Therefore, consulting the previous excellent works on designing ppC species based on CBe5 core moiety, we speculated that CBe4 might be another excellent core moiety for systematically designing new ptC species by attaching the monovalent atoms on the Be–Be edges. First, we verify the molecular charges of CBe4 cluster, which can be deduced from our previously reported species having the formula of CBe4Mnn–2 (n = 1~3). If the value of n is extended to zero, a dianionic cluster with the formula of CBe42– (0, see Fig. 1) can be obtained. At both B3LYP/BS1 and B2PLYP-D/BS1 levels, such a cluster adopts the planar structure in C2v symmetry and encloses a ptC. As a comparison, neutral CBe4 and the highly negatively charged CBe44– adopt the non-planar structures in D2 and D2d symmetries, respectively, and thus they are disregarded in the following. The C–Be interatomic distances in 0 are 1.60 and 1.68 Å, short enough for each beryllium atom to be counted as a coordination to center carbon, so 0 is an eligible ptC species.

    Figure 1

    Figure 1.  Optimized structure of CBe44–, CBe42– (0), and CBe4 at the B3LYP/aug-cc-pVTZ level (A) and the AdNDP view of chemical bonding in 0 (B)

    The AdNDP analysis revealed that 0 had seven pairs of valence electrons, in which three of them were highly diffused Be–Be two-center two electron (2c-2e) σ bonds with occupation number of 1.97 |e|. The diffusion character of such σ bonds, possibly attributed to the high negative charges of the molecule and the metallic nature of beryllium, is unbeneficial to the stabilization of 0 because the electrons at the position far from the nuclei will be reactive. Therefore, the elimination of such diffused σ bonds is highly desired. In contrast, though the remained four pairs of electrons involve all five atoms, they are less diffused than the Be–Be 2c-2e bonds. Note that such four 5c-2e bonds (ON = 2.00 |e|) supported eight electrons to valence shell of the central carbon, which stabilizes the molecule by making the carbon meet the octet rule. In addition, four pairs of electrons consist of three 5c-2e σ and one 5c-2e π bonds, matching the famous 4n+2 rule with n = 1 and 0, respectively, so the preference of ptC structure in 0 may stem from the novel σ and π double aromaticity. Therefore, retaining such 5c-2e bonds is also highly desired. Remarkably, according to our extensive exploration of CBe42– potential energy surface, 0 is GEM and locates 4.17 kcal·mol–1 lower in energy than the second lowest isomer (0a, see Fig. S4) at the CCSD(T)//B3LYP level. As a comparison, CBe54– ppC structure is a high energy local minimum. The lower molecular charge and the GEM nature of 0 suggest its higher plausibility as a core moiety than CBe54– species for the subsequent design of phC species.

    The systematic design of the ptC species was realized by attaching the monovalent element on the bridging positions of 0, similar to the design of ppC species based on CBe54–. The literature survey had revealed the feasible bridging atoms (E) that had been employed for the ppC design based on CBe54–, including group 1 elements H, Li, Na, group 11 elements Cu, Ag, Au, and group 17 elements F, Cl, Br, I. In this work, the design of ptC species involves the stepwise introduction of these monovalent E elements onto the Be–Be edge(s). As shown in Scheme 1, for the species with one or two E atoms, i.e. CBe4E and CBe4E2, we considered two possible structural models, which are labelled as M1/M1′ and M2/M2′, respectively. Note that a new model can be found for both CBe4E and CBe4E2 species (M1″ and M2″, see Scheme 1) during the isomer search.

    Scheme 1

    Scheme 1.  Stepwise introduction of E atom(s) on the Be–Be of CBe42–

    We have computed the isomers in various model structures. Fig. 2 shows those with lower energies. If E is an alkali or group 11 metal, it tends to bind CBe4 moiety on the top Be–Be edge (M1 model) of CBe42– structure (see CBe4E (E = Li (1), Na (4), Cu (7), Ag (10), and Au (13)) in the first column of Fig. 2) rather than on the side Be–Be edge (M1′ model). If E is H or a halogen, it prefers neither top nor the side Be–Be edges, but prefers the terminal position on a bottom Be atom (M1″ model) (see CBe4E (E = H (16), F (19), Cl (22), Br (25), and I (28)) in the fourth column of Fig. 2). Note that the ground electronic state for 19 is triplet (E = F) and that for other CBe4E species is closed-shell singlet.

    Figure 2

    Figure 2.  Optimized structures of ptC species designed based on 0. The necessary bond lengths regarding molecular symmetries are given in Å

    When two E atoms are anchored on the CBe4 moiety to give CBe4E2 species, the situation is similar in structural preference to CBe4E: If E is an alkali or group 11 metal, two E atoms tend to bind CBe4 moiety with one E atom on top and the other on the side Be–Be edges (M2 model), respectively (see CBe4E2 (E = Li (2), Na (5), Cu (8), Ag (11), and Au (13)) in the second column of Fig. 2) rather than both on the side Be–Be edges (M2′ model). As a comparison, if E is H or a halogen, corresponding CBe4E2 species prefer the M2″ model (see CBe4E2 (E = H (17), F (20), Cl (23), Br (26), and I (29) in the fifth column of Fig. 2) with one E atom on side Be–Be edge and the other E atom on the terminal position of a bottom Be atom. The ground electronic state of all CBe4E2 species is closed-shell singlet.

    Nevertheless, when three E atoms bind the CBe4 moiety, corresponding CBe4E3+ species always prefer the M3 model structure (Scheme 1) despite the type of E atom. The third and sixth columns of Fig. 2 show the structures of these 10 species, i.e. CBe4E3+ (E = Li (3), Na (6), Cu (9), Ag (12), Au (15), H (18), F (21), Cl (24), Br (27), and I (30)).

    As Fig. 2 shows, all these thirty species adopt planar structures with carbon atom surrounded by four Be atoms. The C–Be distances in 1~30 range from 1.568 to 1.736 Å, shorter than the sum of covalent radii of C and Be (1.790 Å), so the carbon atoms in 1~30 are the well-defined ptCs. The Be–Be distances in 1~30 range from 1.869 to 2.208 Å, covering the typical lengths of Be–Be single[36], double, and pseudo-triple bonds[37, 38]. Remarkably, there are three very short Be–Be distances in CBe4H2 (2) and CBe4H3+ (3) (1.893/1.893, 1.891 and 1.869 Å, respectively), within the range of ultrashort metal-metal distances (USMMDs, defined as dM–M < 1.900 Å)[39] and suggesting the strong Be– Be interactions. We further re-optimized the geometries of CBe4H2 (2) and CBe4H3+ (3) to verify the USMMDs at the CCSD(T) level and corresponding geometric parameters are given in Fig. 2 in the parenthesis and red font. As Fig. 2 shows, the above ultrashort Be–Be distances were elongated slightly to 1.935/1.910, 1.911, and 1.888 Å, respectively after the optimization at the CCSD(T) level and only a Be– Be distance (1.888 Å) in 3 was still shorter than 1.900 Å and can be regarded as the USMMD. The USMMD of 1.888 Å can be rationalized by electronic analysis.

    The chemical bonding in these ptC species can be described by the AdNDP analysis. The AdNDP results for CBe4Cunn–2 and CBe4Hnn–2 (n = 1~3) are shown representatively in Fig. 3, while those for other species are similar to E = Cu or E = H, thus they are given in the Supporting Information. As Fig. 3 shows, in CBe4Cunn–2 (n = 1~3) species, a diffused Be–Be 2c-2e σ bond with ON of 1.93 or 1.87 |e| can be found for the Be–Be edges without bridging Cu atom (see the first column in upper part), while a less diffused Be–Cu– Be 3c-2e σ bond with ON of 1.84~1.98 |e| can be found for the Be–Be edges with a Cu atom (see the second column in upper part). As a comparison, the peripheral bonding in CBe4Hnn–2 (n = 1~3) is a little different in that there is a Be–H 2c-2e σ bond with ON of 2.00 |e| covering the terminal Be–H group of CBe4H and CBe4H2. Other peripheral bonding patterns are similar to that in CBe4Cunn–2 (n = 1~3) species, including a diffused Be–Be 2c-2e σ bond (ON = 1.84 or 1.93 |e|) on Be–Be edges without H atom and a less diffused Be–H–Be 3c-2e σ bond (ON = 1.98 or 1.99 |e|) on Be–Be edges with an H atom. Remarkably, the bonding patterns concerning the core CBe4 moieties in CBe4Cunn–2 and CBe4Hnn–2 (n = 1~3) species are similar as they possess three CBe4 5c-2e σ bonds (ON = 1.97~1.99 |e|) and one 5c-2e π bond (ON = 1.97~1.99 |e|). These four orbitals are also similar to that in CBe42– template molecule and provide the basis for adopting the ptC structures. By meeting our initial expectation on the electronic structures of derived species (stepwise eliminating the diffused Be–Be σ bonds but retaining four central 5c-2e bond), the designed species would possess the better and better stability when number of E atoms (n) increases. In addition, the AdNDP results can rationalize the existence of USMMD in 18. As shown in Fig. 3, there are five orbitals contributed positively to shorten the concerned Be–Be distance, including one Be–H–Be 3c-2e σ bond, three CBe4 5c-2e σ bonds and one CBe4 5c-2e π bond. Please note that this does not mean that there is a pseudo-quintuple bond between two beryllium atoms because each of the four 5c-2e bonds only contributes partially for such Be–Be bonding.

    Figure 3

    Figure 3.  AdNDP view of chemical bonding in CBe4Cu (7), CBe4Cu2 (8), and CBe4Cu3+ (9) as well as CBe4H (16), CBe4H2 (17), and CBe4H3+ (18)

    As mentioned above, both the CBe42– template molecule and its derivatives retain three 5c-2e σ bonds and one 5c-2e π bond. Such an electronic structure not only leads to the planarity, but also corresponds to six delocalized σ electrons and two delocalized π electrons, meeting the Huckel's 4n + 2 rule for n = 1 and 0, respectively and suggesting the novel 6σ + 2π double aromaticity. To corroborate the existence of aromaticity, the NICS calculations were performed by using the highly stable CBe4E3 species as the examples. The results for CBe4Cu3+ (9) and CBe4H3+ (18) are shown representatively in Fig. 4, while those for other species are given in Supporting Information. As shown in Fig. 4, the centers of Be–C–Be triangles in 9 possessed the NICS values of –25.5 and –18.8 ppm, while those in 18 showed the values of –24.7 and –21.6 ppm, suggesting the existence of σ aromaticity in both 9 and 18. Simultaneously, the points located 1.0 Å above the molecular plane all possessed the negative NICS values, ranging from –10.1 to –22.4 ppm and suggesting the existence of π aromaticity.

    Figure 4

    Figure 4.  NICS values of CBe4Cu3+ (A) and CBe4H3+ (B). Along the vertical line, the NICS points (red balls) are 0.5 Å apart from their neighbors

    The stabilization effect of bridging E atoms can be verified by the variation of HOMO-LUMO gaps (Gap). The value for CBe42– is only 0.53 eV at the B3LYP/BS1 level. As shown in Fig. 5, the CBe4E and CBe4E2 species possess the obviously enlarged Gaps of 1.37~1.88 eV and 1.30~2.42 eV, respectively. Moreover, when the diffused Be–Be 2c-2e bonds are completely eliminated in CBe4E3+ species, the Gaps increased dramatically to 2.38 to 4.59 eV. Except that E is an alkali metal (Li and Na), other CBe4E3+ species possess the Gaps higher than 3.47 eV. Especially for E = H and halogens, the Gaps are all wider than 4.21 eV, revealing their well-defined electronic structures. The difference between H/ halogens and alkali/group 11 metals mainly lies in their electronegativity. From electronic structure point of view, H can be considered as a halogen because it needs only one electron to have its valence shell occupied fully. When the Be–Be edges of CBe4 core were surrounded by H and halogens (the typical non-metals), the resulted species should possess better electronic structures than the species whose Be–Be edges of CBe4 core were surrounded by the alkali and group 11 metals. Consistently, the HOMO-LUMO gaps of the former are wider than those of the latter.

    Figure 5

    Figure 5.  Variation of HOMO-LUMO gaps (Gap, in eV) with the increasing number of E atom

    To assess the possibility to realize the ptC species designed in this work, the systematic exploration of potential energy surfaces (PESs) was carried out using the stochastic search algorithm. According to the relative energy determination at the final CCSD(T)//B3LYP level, only the GEMs of CBe4E2 (E = H, F, Cl, Br, I) components did not adopt the ptC structure, while those of all other CBe4Enn–2 (E = H, Li, Na, Cu, Ag, Au, F, Cl, Br, I; n = 1~3) components adopted one of the ptC models shown in Scheme 1. As shown in Fig. S4, S5, and S6 in the Supporting Information, these GEMs located 0.6 to 21.8 kcal·mol–1 below their second lowest isomers at the CCSD(T)//B3LYP level, suggesting their good thermodynamic stability.

    The dynamic stability is equally important for the experimental viability of computationally designed species. In this work, the dynamic stability was studied using 100 picoseconds BOMD simulations for 26 GEM ptC species (including 0) at the B3LYP/BS2 level. The results for CBe42– (0), CBe4Cu3+ (9), CBe4F3+ (21), and CBe4H3+ (18) are shown representatively in Fig. 6, while those for other GEMs are given in Figs. S7, S8, and S9 in the Supporting Information. We found that the RMSD plots for many of GEM ptC species showed upward jumps, suggesting the significant changes in the position of atoms. The detailed structural examination revealed that the geometry of CBe42– shows the reversible isomerization to a structure (0c) we located during the PES exploration. As Fig. 6 shows, 0c took up for the larger proportion during the simulation than 0, but the reversible transformation still suggested the high viability of 0 and indicated the high flexibility of Be atoms in 0.

    Figure 6

    Figure 6.  RMSD versus simulation time for the BOMD simulation of CBe42–, CBe4Cu3+, CBe4F3+, and CBe4H3+, respectively at the B3LYP/BS2 level and 298 K

    The RMSD plot for the simulation of CBe4Ag2 (11) shows the irreversible upward jump, which corresponds to the structural evolution to an isomer having a tetrahedral carbon (see 11a in Fig. S5), so it is dynamically unviable. That of CBe4Cu3+ (9) shows some reversible and fleeting upward jumps. However, the detailed structural sampling revealed that the upward jumps corresponded to the flexibility of the molecule as a whole rather than the isomerization. The RMSD plot for CBe4F3+ (21) does not show the upward jump and the fluctuation of RMSD values is small, suggesting the rather rigid structure of 21. Interestingly, the RMSD plot for CBe4H3+ (18) shows two stepwise upward jumps, which correspond to two times of isomerization. In the first isomerization, the structure of 18 is converted to its second lowest isomer (see 18a in Fig. S6), while in the second isomerization, 18a is converted to 18 again. As shown in Fig. 6, if the labels (numbering of the atoms) are considered, we can see a Be–H group rotate around the central ptC during two times of isomerization. In the majority of simulation time, the structure of 18 is adopted, so 18 is also dynamically viable. The plots for CBe4Li2 (2), CBe4Na2 (3), CBe4Cu2 (8), and CBe4I3+ (30) are similar to that of 18, thus though they are not dynamically stable, they are still dynamically viable. The RMSD plots of other ptC GEMs are similar to 9 or 21, thus they are dynamically stable and viable.

    In summary, we had proved that the strategy for designing ppC species based on CBe54– can be transferred to design the ptC species based on CBe42–. The monovalent atoms including group 1 elements H, Li, Na, group 11 elements Cu, Ag, Au, and group 17 elements F, Cl, Br, I are all suitable for further stabilizing CBe42– by anchoring the monovalent atoms on its Be–Be edges to stepwise eliminate the highly diffused Be–Be 2c-2e bonds. In thirty-one designed ptC species (including CBe42– itself), twenty-five of them are dynamically viable global energy minima, which are potentially possible for experimental realization in experiments. Remarkably, the dynamic simulations suggest that the Be and E atoms in some ptC species are highly flexible but the basic ptC geometry can be maintained during the changes of atom positions, thus suggesting the stable but flexible bonding nature.


    1. [1]

      Wang, Z. X.; Zhang, C. G.; Chen, Z.; Schleyer, P. V. R. Planar tetracoordinate carbon species involving beryllium substituents. Inorg. Chem. 2008, 47, 1332‒1336. doi: 10.1021/ic7017709

    2. [2]

      Wu, Y. B.; Jiang, J. L.; Zhang, R. W.; Wang, Z. X. Computationally designed families of flat, tubular, and cage molecules assembled with "starbenzene" building blocks through hydrogen-bridge Bonds. Chem. -Eur. J. 2010, 16, 1271‒1280. doi: 10.1002/chem.200901983

    3. [3]

      Zhao, X. F.; Li, H.; Yuan, C. X.; Li, Y. Q.; Wu, Y. B.; Wang, Z. X. Linear, planar, and tubular molecular structures constructed by double planar tetracoordinate carbon D2h C2(BeH)4 species via hydrogen-bridged -BeH2Be-bonds. J. Comput. Chem. 2016, 37, 261‒269. doi: 10.1002/jcc.24018

    4. [4]

      Guo, J. C.; Feng, L. Y.; Dong, C.; Zhai, H. J. Planar pentacoordinate versus tetracoordinate carbons in ternary CBe4Li4 and CBe4Li42− clusters. J. Phys. Chem. A 2018, 122, 8370‒8376. doi: 10.1021/acs.jpca.8b08573

    5. [5]

      Guo, J. C.; Feng, L. Y.; Dong, C.; Zhai, H. J. Ternary 12-electron CBe3X3+ (X = H, Li, Na, Cu, Ag) clusters: planar tetracoordinate carbons and superalkali cations. Phys. Chem. Chem. Phys. 2019, 21, 22048‒22056. doi: 10.1039/C9CP04437J

    6. [6]

      Guo, J. C.; Feng, L. Y.; Zhai, H. J. Ternary CBe4Au4 cluster: a 16-electron system with quasi-planar tetracoordinate carbon. Phys. Chem. Chem. Phys. 2018, 20, 6299‒6306. doi: 10.1039/C7CP08420J

    7. [7]

      Jimenez Halla, J. O. C.; Wu, Y. B.; Wang, Z. X.; Islas, R.; Heine, T.; Merino, G. CAl4Be and CAl3Be2: global minima with a planar pentacoordinate carbon atom. Chem. Commun. 2010, 46, 8776‒8778. doi: 10.1039/c0cc03479g

    8. [8]

      Wu, Y. B.; Duan, Y.; Lu, H. G.; Li, S. D. CAl2Be32− and its salt complex LiCAl2Be3: anionic global minima with planar pentacoordinate carbon. J. Phys. Chem. A 2012, 116, 3290‒3294. doi: 10.1021/jp300302w

    9. [9]

      Zhao, X. F.; Bian, J. H.; Huang, F.; Yuan, C.; Wang, Q.; Liu, P.; Li, D.; Wang, X.; Wu, Y. B. Stabilization of beryllium-containing planar pentacoordinate carbon species through attaching hydrogen atoms. RSC Adv. 2018, 8, 36521‒36526. doi: 10.1039/C8RA07664B

    10. [10]

      Castro, A. C.; Martinez Guajardo, G.; Johnson, T.; Ugalde, J. M.; Wu, Y. B.; Mercero, J. M.; Heine, T.; Donald, K. J.; Merino, G. CBe5E (E = Al, Ga, In, Tl): planar pentacoordinate carbon in heptaatomic clusters. Phys. Chem. Chem. Phys. 2012, 14, 14764‒14768. doi: 10.1039/c2cp40839b

    11. [11]

      Luo, Q. Theoretical observation of hexaatomic molecules containing pentacoordinate planar carbon. Sci. China Ser. B 2008, 51, 1030‒1035. doi: 10.1007/s11426-008-0121-5

    12. [12]

      Grande Aztatzi, R.; Cabellos, J. L.; Islas, R.; Infante, I.; Mercero, J. M.; Restrepo, A.; Merino, G. Planar pentacoordinate carbons in CBe54− derivatives. Phys. Chem. Chem. Phys. 2015, 17, 4620‒4624. doi: 10.1039/C4CP05659K

    13. [13]

      Guo, J. C.; Feng, L. Y.; Barroso, J.; Merino, G.; Zhai, H. J. Planar or tetrahedral? A ternary 17-electron CBe5H4+ cluster with planar pentacoordinate carbon. Chem. Commun. 2020, 56, 8305‒8308. doi: 10.1039/D0CC02973D

    14. [14]

      Guo, J. C.; Ren, G. M.; Miao, C. Q.; Tian, W. J.; Wu, Y. B.; Wang, X. CBe5Hnn−4 (n = 2~5): hydrogen-stabilized CBe5 pentagons containing planar or quasi-planar pentacoordinate carbons. J. Phys. Chem. A 2015, 119, 13101‒13106. doi: 10.1021/acs.jpca.5b10178

    15. [15]

      Guo, J. C.; Tian, W. J.; Wang, Y. J.; Zhao, X. F.; Wu, Y. B.; Zhai, H. J.; Li, S. D. Star-like superalkali cations featuring planar pentacoordinate carbon. J. Chem. Phys. 2016, 144. 244303‒9.

    16. [16]

      Wu, Y. B.; Duan, Y.; Lu, G.; Lu, H. G.; Yang, P.; Schleyer, P. V. R.; Merino, G.; Islas, R.; Wang, Z. X. D3h CN3Be3+ and CO3Li3+: viable planar hexacoordinate carbonprototypes. Phys. Chem. Chem. Phys. 2012, 14, 14760–14763. doi: 10.1039/c2cp41822c

    17. [17]

      Zhao, X. F.; Li, J. J.; Li, H. R.; Yuan, C.; Tian, X.; Li, S. D.; Wu, Y. B.; Guo, J. C.; Wang, Z. X. Viable aromatic BenHn stars enclosing a planar hypercoordinate boron or late transition metal. Phys. Chem. Chem. Phys. 2018, 20, 7217‒7222. doi: 10.1039/C7CP06955C

    18. [18]

      Xiao, B.; Cheng, J. B.; Liu, Z. B.; Li, Q. Z.; Li, W. Z.; Yang, X.; Yu, X. F. Beryllium decorated armchair BC2N nanoribbons: coexistence of planar tetracoordinate carbon and nitrogen moieties. RSC Adv. 2015, 5, 73945‒73950. doi: 10.1039/C5RA12660F

    19. [19]

      Li, J. J.; Mu, Y.; Tian, X.; Yuan, C.; Wu, Y. B.; Wang, Q.; Li, D.; Wang, Z. X.; Li, S. D. Zigzag double-chain C‒Be nanoribbon featuring planar pentacoordinate carbons and ribbon aromaticity. J. Mater. Chem. C 2017, 5, 408‒414. doi: 10.1039/C6TC04356A

    20. [20]

      Wang, Y.; Li, F.; Li, Y.; Chen, Z. Semi-metallic Be5C2 monolayer global minimum with quasi-planar pentacoordinate carbons and negative Poisson's ratio. Nat. Commun. 2016, 7, 11488. doi: 10.1038/ncomms11488

    21. [21]

      Li, Y.; Liao, Y.; Chen, Z. Be2C Monolayer with quasi-planar hexacoordinate carbons: a global minimum structure. Angew. Chem. Int. Ed. 2014, 53, 7248‒7252. doi: 10.1002/anie.201403833

    22. [22]

      Li, X. S.; Millam, J. M.; Schlegel, H. B. Ab initio molecular dynamics studies of the photodissociation of formaldehyde, H2CO → H2 + CO: direct classical trajectory calculations by MP2 and density functional theory. J. Chem. Phys. 2000, 113, 10062‒10067. doi: 10.1063/1.1323503

    23. [23]

      Millam, J. M.; Bakken, V.; Chen, W.; Hase, W. L.; Schlegel, H. B. Ab initio classical trajectories on the Born-Oppenheimer surface: Hessian-based integrators using fifth-order polynomial and rational function fits. J. Chem. Phys. 1999, 111, 3800‒3805. doi: 10.1063/1.480037

    24. [24]

      Schleyer, P. V. R.; Maerker, C.; Dransfeld, A.; Jiao, H.; Hommes, N. J. R. E. Nucleus-independent chemical shifts: a simple and efficient aromatic-city probe. J. Am. Chem. Soc. 1996, 118, 6317−6318. doi: 10.1021/ja960582d

    25. [25]

      Schleyer, P. V. R.; Jiao, H.; Hommes, N. J. R. E.; Malkin, V. G.; Malkina, O. L. An evaluation of the aromaticity of inorganic rings: refined evidence from magnetic properties. J. Am. Chem. Soc. 1997, 119, 12669−12670. doi: 10.1021/ja9719135

    26. [26]

      Corminboeuf, C.; Heine, T.; Seifert, G.; von Rague Schleyer, P. V. R.; Weber, J. Induced magnetic fields in aromatic [n]-annulenes-interpretation of NICS tensor components. Phys. Chem. Chem. Phys. 2004, 6, 273−276. doi: 10.1039/B313383B

    27. [27]

      Zubarev, D. Y.; Boldyrev, A. I. Developing paradigms of chemical bonding: adaptive natural density partitioning. Phys. Chem. Chem. Phys. 2008, 10, 5207‒5217. doi: 10.1039/b804083d

    28. [28]

      Zubarev, D. Y.; Boldyrev, A. I. Revealing intuitively assessable chemical bonding patterns in organic aromatic molecules via adaptive natural density partitioning. J. Org. Chem. 2008, 73, 9251‒9258. doi: 10.1021/jo801407e

    29. [29]

      Bera, P. P.; Sattelmeyer, K. W.; Saunders, M.; Schaefer, H. F.; Schleyer, P. V. R. Mindless chemistry. J. Phys Chem. A 2006, 110, 4287‒4290. doi: 10.1021/jp057107z

    30. [30]

      Saunders, M. J. Stochastic search for isomers on a quantum mechanical surface. Comput. Chem. 2004, 25, 621‒626. doi: 10.1002/jcc.10407

    31. [31]

      Wu, Y. B.; Lu, H. G.; Li, S. D.; Wang, Z. X. J. Simplest neutral singlet C2E4 (E = Al, Ga, In, and Tl) global minima with double planar tetracoordinate carbons: equivalence of C2 Moieties in C2E4 to carbon centers in CAl42− and CAl5+. Phys. Chem. A 2009, 113, 3395‒3402. doi: 10.1021/jp8099187

    32. [32]

      Lu, H. G., Wu, Y. B. in GXYZ 2.0, A Random Search Program. Shanxi University: Taiyuan 2015.

    33. [33]

      Werner, H. J.; Knowles, P. J.; Knizia, G.; Manby, F. R.; Schütz, M. MolPro 2012.1. University College Cardiff Consultants Limited: Cardiff UK 2012.

    34. [34]

      Frisch, M. J.; Trucks, G. W.; Schlegel, H. B.; Scuseria, G. E.; Robb, M. A.; Cheeseman, J. R.; Scalmani, G.; Barone, V.; Petersson, G. A.; Nakatsuji, H.; Li, X.; Caricato, M.; Marenich, A. V.; Bloino, J.; Janesko, B. G.; Gomperts, R.; Mennucci, B.; Hratchian, H. P.; Ortiz, J. V.; Izmaylov, A. F.; Sonnenberg, J. L.; Williams-Young, D.; Ding, F.; Lipparini, F.; Egidi, F.; Goings, J.; Peng, B.; Petrone, A.; Henderson, T.; Ranasinghe, D.; Zakrzewski, V. G.; Gao, J.; Rega, N.; Zheng, G.; Liang, W.; Hada, M.; Ehara, M.; Toyota, K.; Fukuda, R.; Hasegawa, J.; Ishida, M.; Nakajima, T.; Honda, Y.; Kitao, O.; Nakai, H.; Vreven, T.; Throssell, K.; Montgomery, Jr. J. A.; Peralta, J. E.; Ogliaro, F.; Bearpark, M. J.; Heyd, J. J.; Brothers, E. N.; Kudin, K. N.; Staroverov, V. N.; Keith, T. A.; Kobayashi, R.; Normand, J.; Raghavachari, K.; Rendell, A. P.; Burant, J. C.; Iyengar, S. S.; Tomasi, J.; Cossi, M.; Millam, J. M.; Klene, M.; Adamo, C.; Cammi, R.; Ochterski, J. W.; Martin, R. L.; Morokuma, K.; Farkas, O.; Foresman, J. B.; Fox, D. J. Gaussian 16, Revision A. 03. Gaussian, Inc., Wallingford CT 2016.

    35. [35]

      Guo, J. C.; Feng, L. Y.; Zhai, H. J. Planar tetracoordinate carbon molecules with 14 valence electrons: examples of CBe4Mnn−2 (M = Li, Au; n = 1~3) clusters. New J. Chem. 2020, 44, 18293. doi: 10.1039/D0NJ03944F

    36. [36]

      Pyykkö, P. Additive covalent radii for single-, double-, and triple-bonded molecules and tetrahedrally bonded crystals: a summary. J. Phys. Chem. A 2015, 119, 2326‒2337. doi: 10.1021/jp5065819

    37. [37]

      Yuan, C.; Zhao, X. F.; Wu, Y. B.; Wang, X. Ultrashort beryllium-beryllium distances rivalling those of metal-metal quintuple bonds between transition metals. Angew. Chem. Int. Ed. 2016, 55, 15651‒15655. doi: 10.1002/anie.201609455

    38. [38]

      Zhao, X. F.; Yuan, C.; Li, S. D.; Wu, Y. B.; Wang, X. Simulating the effect of a triple bond to achieve the shortest main group metal-metal distance in diberyllium complexes: a computational study. Dalton Trans. 2018, 47, 14462‒14467. doi: 10.1039/C8DT02683A

    39. [39]

      Wagner, F. R.; Noor, A.; Kempe, R. Ultrashort metal-metal distances and extreme bond orders. Nat. Chem. 2009, 1, 529‒536. doi: 10.1038/nchem.359

  • Figure 1  Optimized structure of CBe44–, CBe42– (0), and CBe4 at the B3LYP/aug-cc-pVTZ level (A) and the AdNDP view of chemical bonding in 0 (B)

    Scheme 1  Stepwise introduction of E atom(s) on the Be–Be of CBe42–

    Figure 2  Optimized structures of ptC species designed based on 0. The necessary bond lengths regarding molecular symmetries are given in Å

    Figure 3  AdNDP view of chemical bonding in CBe4Cu (7), CBe4Cu2 (8), and CBe4Cu3+ (9) as well as CBe4H (16), CBe4H2 (17), and CBe4H3+ (18)

    Figure 4  NICS values of CBe4Cu3+ (A) and CBe4H3+ (B). Along the vertical line, the NICS points (red balls) are 0.5 Å apart from their neighbors

    Figure 5  Variation of HOMO-LUMO gaps (Gap, in eV) with the increasing number of E atom

    Figure 6  RMSD versus simulation time for the BOMD simulation of CBe42–, CBe4Cu3+, CBe4F3+, and CBe4H3+, respectively at the B3LYP/BS2 level and 298 K

  • 加载中
计量
  • PDF下载量:  0
  • 文章访问数:  49
  • HTML全文浏览量:  3
文章相关
  • 发布日期:  2022-03-01
  • 收稿日期:  2021-08-14
  • 接受日期:  2021-10-21
通讯作者: 陈斌, bchen63@163.com
  • 1. 

    沈阳化工大学材料科学与工程学院 沈阳 110142

  1. 本站搜索
  2. 百度学术搜索
  3. 万方数据库搜索
  4. CNKI搜索

/

返回文章