Abstract:Halogen bonds involving an aromatic moiety as an acceptor, otherwise known as R-X…π interactions, have increasingly been recognized as being important in materials and in protein-ligand complexes. These types of interactions have been the subject of many recent investigations, but little is known about the ways in which the strengths of R-X…π interactions vary as a function of the relative geometries of the interacting pairs. Here we use the accurate CCSD(T) and SAPT2+3δMP2 methods to investigate the potential… Show more
“…R-X···π interactions are generally slightly weaker than their R-X···Y counterparts, with binding energies whose magnitudes are typically 10-25% lower [20,25,29]. The SAPT characteristics of R-X···π interactions are similar to those of R-X···Y interactions, however, the former tend to have larger relative contributions from dispersion, which is to be expected given the large size and polarizabilities of both halogens and phenyl groups [25,29].…”
Section: Introductionmentioning
confidence: 90%
“…The SAPT characteristics of R-X···π interactions are similar to those of R-X···Y interactions, however, the former tend to have larger relative contributions from dispersion, which is to be expected given the large size and polarizabilities of both halogens and phenyl groups [25,29]. The geometric properties of R-X···π interactions are inherently different than those of standard halogen bonds because of the diffuse nature of the region of negative potential in an aromatic system.…”
Section: Introductionmentioning
confidence: 90%
“…Thus, it is observed that a halogen bound to an electron withdrawing group will generally have a larger, more positive, σ-hole than one bound to an electropositive or electroneutral group. The size of a σ-hole correlates strongly with the strength of the halogen bonding, or R-X···π, interaction in which the halogen participates [24,25,34,35].…”
Section: Figurementioning
confidence: 99%
“…Traditionally, electronegative Lewis bases have been considered the primary halogen bond accepting group, as is true in hydrogen bonding [12][13][14][15][16]. More recently, π-bonding and aromatic moieties have been shown to be effective halogen bond acceptors, leading to a subclass of interactions, sometimes called R-X···π (or C-X···π) interactions [19][20][21][22][23][24][25].…”
Section: Introductionmentioning
confidence: 99%
“…In a recent computational study, utilizing the accurate CCSD(T)/aug-cc-pVQZ and SAPT2+3δMP2/aug-cc-pVTZ methods on model complexes involving a benzene R-X···π acceptor, the ways in which the strengths of R-X···π interaction depends on the relative orientation of the interacting pair that were investigated [25]. It was seen that the strength of an R-X···π interaction depends strongly on the distance between the halogen and the benzene ring, a distance that is described by both R(R-X···π) and the α angle (as defined in Figure 2, and first introduced by Glaser et al) [33], while being only mildly dependent on the R-X···π angle (θ).…”
Abstract:Here, we investigate the strengths of R-X···π interactions, involving both chlorine and bromine, in model systems derived from protein-ligand complexes found in the PDB. We find that the strengths of these interactions can vary significantly, with binding energies ranging from −2.01 to −3.60 kcal/mol. Symmetry adapted perturbation theory (SAPT) analysis shows that, as would be expected, dispersion plays the largest role in stabilizing these R-X···π interactions, generally accounting for about 50% to 80% of attraction. R-Br···π interactions are, for the most part, found to be stronger than R-Cl···π interactions, although the relative geometries of the interacting pair and the halogen's chemical environment can also have a strong impact. The two factors that have the strongest impact on the strength of these R-X···π interactions is the distance between the halogen and the phenyl plane as well as the size of the halogen σ-hole.
“…R-X···π interactions are generally slightly weaker than their R-X···Y counterparts, with binding energies whose magnitudes are typically 10-25% lower [20,25,29]. The SAPT characteristics of R-X···π interactions are similar to those of R-X···Y interactions, however, the former tend to have larger relative contributions from dispersion, which is to be expected given the large size and polarizabilities of both halogens and phenyl groups [25,29].…”
Section: Introductionmentioning
confidence: 90%
“…The SAPT characteristics of R-X···π interactions are similar to those of R-X···Y interactions, however, the former tend to have larger relative contributions from dispersion, which is to be expected given the large size and polarizabilities of both halogens and phenyl groups [25,29]. The geometric properties of R-X···π interactions are inherently different than those of standard halogen bonds because of the diffuse nature of the region of negative potential in an aromatic system.…”
Section: Introductionmentioning
confidence: 90%
“…Thus, it is observed that a halogen bound to an electron withdrawing group will generally have a larger, more positive, σ-hole than one bound to an electropositive or electroneutral group. The size of a σ-hole correlates strongly with the strength of the halogen bonding, or R-X···π, interaction in which the halogen participates [24,25,34,35].…”
Section: Figurementioning
confidence: 99%
“…Traditionally, electronegative Lewis bases have been considered the primary halogen bond accepting group, as is true in hydrogen bonding [12][13][14][15][16]. More recently, π-bonding and aromatic moieties have been shown to be effective halogen bond acceptors, leading to a subclass of interactions, sometimes called R-X···π (or C-X···π) interactions [19][20][21][22][23][24][25].…”
Section: Introductionmentioning
confidence: 99%
“…In a recent computational study, utilizing the accurate CCSD(T)/aug-cc-pVQZ and SAPT2+3δMP2/aug-cc-pVTZ methods on model complexes involving a benzene R-X···π acceptor, the ways in which the strengths of R-X···π interaction depends on the relative orientation of the interacting pair that were investigated [25]. It was seen that the strength of an R-X···π interaction depends strongly on the distance between the halogen and the benzene ring, a distance that is described by both R(R-X···π) and the α angle (as defined in Figure 2, and first introduced by Glaser et al) [33], while being only mildly dependent on the R-X···π angle (θ).…”
Abstract:Here, we investigate the strengths of R-X···π interactions, involving both chlorine and bromine, in model systems derived from protein-ligand complexes found in the PDB. We find that the strengths of these interactions can vary significantly, with binding energies ranging from −2.01 to −3.60 kcal/mol. Symmetry adapted perturbation theory (SAPT) analysis shows that, as would be expected, dispersion plays the largest role in stabilizing these R-X···π interactions, generally accounting for about 50% to 80% of attraction. R-Br···π interactions are, for the most part, found to be stronger than R-Cl···π interactions, although the relative geometries of the interacting pair and the halogen's chemical environment can also have a strong impact. The two factors that have the strongest impact on the strength of these R-X···π interactions is the distance between the halogen and the phenyl plane as well as the size of the halogen σ-hole.
The structures and associated functions of biological molecules are driven by noncovalent interactions, which have classically been dominated by the hydrogen bond (H-bond). Introduction of the σ-hole concept to describe the anisotropic distribution of electrostatic potential of covalently bonded elements from across the periodic table has opened a broad range of nonclassical noncovalent (ncNC) interactions for applications in chemistry and biochemistry. Here, we review how halogen bonds, chalcogen bonds and tetrel bonds, as they are found naturally or introduced synthetically, affect the structures, assemblies, and potential functions of peptides and proteins. This review intentionally focuses on examples that introduce or support principles of stability, assembly and catalysis that can potentially guide the design of new functional proteins. These three types of ncNC interactions have energies that are comparable to the Hbond and, therefore, are now significant concepts in molecular recognition and design. However, the recently described H-bond enhanced X-bond shows how synergism among ncNC interactions can be exploited as potential means to broaden the range of their applications to affect protein structures and functions.
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