N-heterocyclic carbone: computational prediction of a divalent carbon (0) compound

Abstract:

Theoretical evidence of a new five-membered divalent carbon (0) compound has been proposed. Calculations at different levels of density functional theory indicate that this compound is highly stable and a suitable candidate for synthesis. The proposed compound is highly basic and its basicity is almost equal or higher than that of related divalent carbon (0) compounds such as carbodicarbene and carbodiphosphorane.

Keywords::

• divalent carbon (0)
• carbodicarbene
• carbodiphosphorane

Introduction

The seminal computational prediction of carbodicarbenes, C(NHC)₂ (1) (Figure 1), a compound with a central C (0) atom stabilized by two N-heterocyclic carbene (NHC) ligand by Tonner and Frenking¹ and subsequent synthesis of its benzannulated derivative by Dyker et al,² has opened a new chapter in the knowledge book of carbon compounds.^3–5 Early on, Ramirez et al synthesized the first carbodiphosphorane (CDP, 2) – C(PPh₃)₂ – in 1961,^6,7 which was later on structurally characterized by an X-ray analysis in 1978.^6,7 However, its carbon (0) character was not recognized at that time. It was only in 2006, when Tonner et al made an in-depth electronic structure analysis of this compound and established the carbon (0) character of the central carbon atom of this compound.⁸ Recently, the bonding situation of carbon (0) compounds has received much theoretical attention and believed to take place through donor–acceptor interactions L→C←L.^9–13 This bonding situation results in the retention of the four valence electrons of carbon as two lone pairs, one of σ symmetry and another of π symmetry.

Figure 1 Schematic representation of carbodicarbene, (1) C(NHC)₂ and (2) CDP.

Abbreviations: NHC, N-heterocyclic carbene; CDP, carbodiphosphoranes.

Hence, the name “carbone” was coined for these types of compounds. Various carbones have now been synthesized and structurally characterized.^2,14–16

In continuation of the search for suitable ligands to stabilize divalent carbon (0) compounds, we recently come across an interesting ligand viz, bis(imidazolin-2-iminium) dication (Figure 2A), which has been used to isolate a three-coordinate boron cation with boron–sulfur double bond, Figure 2B for the first time.¹⁷ The use of this ligand in main-group element chemistry^18–24 and transition metal chemistry^25–32 has been recently reviewed.³³

Figure 2 Schematic representation of bis(imidazolin-2-iminium) cation (A) and the boron cation compound (B).

The central N–B bond in B is actually a donor–acceptor bond (Figure 3), which resembles exactly the same as that of carbones, ie, L→C←L.¹

Figure 3 Donor–acceptor interaction in B.

This has prompted us to investigate whether the ligand framework Figure 2A may stabilize a carbon atom to form a donor–acceptor complex. Quantum chemical calculations predict that the proposed compound (3) should be a synthetically accessible species. It is a neutral five-membered cyclic carbone (3) that contains a central divalent carbon (0) atom within the familiar N-heterocyclic framework. Moreover, the compound shows high basicity as that of other divalent carbon (0) compounds.^1–16

Computational details

All the structures were fully optimized without any symmetry constraints at BP86/TZVP^34–37 level of theory. This level of theory has been widely used for this class of compounds.^1–24 For Au atom, the relativistic small-core effective core potential basis set of Stuttgart/Dresden was used.³⁸ Stationary points were characterized as minima by calculating their Hessian matrix analytically at this level of theory. For the sake of analysis, the planar conformer of 3 is optimized using symmetry constraint. Proton affinities are calculated employing L + H⁺ → L–H⁺ equation. Zero-point corrections are also added in proton affinity calculations. For proton affinity calculations, single-point energies are calculated at MP2/aug-cc-PVDZ^39,40 level of theory on the BP86/TZVP optimized geometries. Solution phase model chemistry has been performed using the polarized continuum model (PCM)⁴¹ employing water as a solvent (dielectric constant, ε =78.39). We have used the PCM calculation using integral equation formalism model with radii of the sphere defined by united atom topological model. The overlap index between two overlapping spheres is taken to be 0.89 (OFAC =0.89), and the minimum radii of the added sphere is 0.2 Å (RMIN =0.2 Å). All the calculations are performed using NWChem 6.1⁴² and Orca⁴³ suite of program.

Results and discussions

Figure 4 shows the optimized geometries of different conformers of 3 with H atom as the substituent at N atoms at BP86/TZVP level of theory. The equilibrium geometry 3H(a) has the two NHC units in the cis conformation with respect to the planar central five-membered ring. The C–N bond of the central five-membered ring in 3H(a) is 1.395 Å, which is very close to the exocyclic C–N bond (1.393 Å). This implies that the central C–N bond is as strong as the exocyclic one. The equilibrium conformer 3H(a) has an acute N–C–N angle of 101.4°. The trans conformer 3H(b) is 10.4 kcal/mol higher in energy with one imaginary frequency. The planar conformers 3H(c) and the 3H(d), where both the NHC units are perpendicular to the central ring, are higher in energy by 19.8 kcal/mol and 96.1 kcal/mol, respectively (Figure 4). The C–C backbone length of the central ring in 3H(a), 3H(b), and 3H(c) is almost the same. It should be noted that the central C–N bond in 3H(a) (bond length 1.395 Å) may not reveal a donor–acceptor interaction. However, this donor–acceptor interaction becomes prominent when their reactivity is concerned.^9–13 Moreover, the singlet–triplet energy separation of 3H(a) is 121.3 kcal/mol, a value quite higher than generally observed for carbenes.⁴⁴ The Mulliken atomic charge on the central carbon atom is −0.389e compared to −0.187e for the adjacent N atoms – suggesting a possible donor–acceptor interaction in 3. We would also like to emphasize here that the donor–acceptor bonding situation in 3 may not have any physical reality, however, they are quite useful while discussing their reactivity.^9–13

Figure 4 Optimized geometries at BP86/TZVP level of theory and relative energies (kcal/mol at MP2/aug-cc-pVDZ//BP86/TZVP) of different conformers of 3H.

Notes: Bond lengths are in Å and angles are in degrees. Number of imaginary frequencies (i) is also provided.

Figure 5 shows the frontier Kohn–Sham orbitals of 3H calculated at BP86/TZVP level of theory. The HOMO (highest occupied molecular orbital) is of π symmetry with an energy of −2.27 eV, whereas the HOMO-1 is of σ symmetry with an energy of −4.91 eV. These orbitals are of similar symmetry to that of C(NHC)₂.¹ However, there is a contrasting feature. In C(NHC)₂, the first protonation takes place at the σ symmetric orbital (HOMO-1) due to the smaller energy gap between the σ- and π-type molecular orbital. However, in case of 3, the first protonation takes place at the π symmetric lone pair orbital (Figure 6).

Figure 5 Shape of frontier Kohn–Sham orbitals of 3H and orbital energies ε in eV at the BP86/TZVP level of theory.

Abbreviation: HOMO, highest occupied molecular orbital.

Figure 6 BP86/TZVP optimized first and second protonated derivatives of 3H.

Visual inspection of these highest lying frontier molecular orbitals of 3 reveals that the largest coefficient is always at the central carbon atom (atomic orbital coefficient for the central carbon in HOMO is 0.73), which suggests that 3 may be considered as carbones.^9–13 Thus, these two molecular orbitals may be considered as two lone pairs at the central carbon atom, and it should behave as double Lewis base. Hence, its first and second proton affinity has been calculated. Table 1 contains the first and second proton affinities of 1–3. While the first proton affinity of 3 is close to 1 but higher than 2, the second proton affinity of 3 is much higher than 1 and 2. This indicates that the proposed compound is highly basic that might have wide application in transition metal catalysis.⁴⁴ Moreover, the calculated bond dissociation energies for the dissociation of one molecule of AuCl from 3 and 3-AuCl are very high (Figure 7), further supporting their divalent carbon (0) character.^9–13

Table 1 MP2/aug-cc-pVDZ//BP86/TZVP calculated proton affinities (in gas phase); PAs (kcal/mol) of 1–3

Molecule	PA1	PA2
1H	283.2 (292.3)	151.2 (155.3)
2Me	278.3 (278.4)	158.9 (156.2)
3H	287.5	192.1

Note: Data from Tonner R, Frenking G. C(NHC)2: divalent carbon(0) compounds with N-heterocyclic carbene ligands-theoretical evidence for a class of molecules with promising chemical properties. Angew Chem Int Ed Engl. 2007;46:8695.¹

Abbreviation: PA, proton affinity.

Figure 7 BP86/BSI (BSI = TZVP for H, C, N, Cl and SDD for Au) optimized protonated derivatives of 3H.

Note: The Au–Au distance in 3H-(AuCl)₂ is 3.351 Å, which is longer than the typical Au–Au distance of ~3.0 Å. Data from Schmidbaur H. The aurophilicity phenomenon: a decade of experimental findings, theoretical concepts and emerging applications. Gold Bull. 2000;33:3.⁵⁰
Abbreviation: SDD, Stuttgart/Dresden.

Calculations (The reaction energetics [including zero-point corrections] of reactions 1 and 2 are further calculated using the hybrid density functionals B3LYP [it is Becke’s three-parameter hybrid method using the Lee, Yang and Parr {LYP} correlation functional]^45–47 and B3PW91^48,49 using the TZVP basis sets. The calculated value of the reaction energetics are qualitatively similar to those obtained at BP86/TZVP level of theory) suggest that the reactions (1–2) are highly exergonic (Table 2) suggesting the spontaneity of their formation. However, these equations may not be realistic as the reaction energetics is calculated in gas phase. To mimic the more realistic situation, we have calculated the reaction energetics in aqueous medium. In aqueous medium, both these reactions are exergonic albeit to a lesser extent than in gas phase – implying that the proposed compound may be a likely candidate for experimental realization.

Table 2 Calculated reaction Gibbs free energies (kcal/mol) of reactions 1 and 2 at T=298.15 K and P=1 atm

Reaction	∆G
	BP86		B3LYP		B3PW91
	Gas	Solution	Gas	Solution	Gas	Solution
1	−194.6	−14.7	−192.3	−15.2	−188.4	−13.6
2	−232.4	−11.6	−229.5	−12.4	−224.2	−10.8

Note: Values are zero-point corrected.

Conclusion

In summary, quantum chemical calculations provide a hint toward possible isolation of new five-membered neutral divalent carbon (0) compound within the familiar N-heterocyclic framework. The proposed compound contains two other NHC units whose electronic character can be modified in many ways,⁵¹ and thus, the proposed compound may serve as an important perspective for transition metal catalysis.⁴⁴

Acknowledgments

The computational facility of Cotton College State University is greatly acknowledged. The authors declare no competing financial interest. Dedicated to my mentors Dr Ashwini K Phukan, Tezpur University, India, and Professor Shridhar R Gadre, IIT Kanpur, India.

Disclosure

The author reports no conflicts of interest in this work.