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Gao CY, Pei BB, Li SD. Fluxional halogen bonds in linear complexes of tetrafluorodiiodobenzene with dinitrobenzene. J Comput Chem 2025; 46:e27483. [PMID: 39350679 DOI: 10.1002/jcc.27483] [Citation(s) in RCA: 0] [Impact Index Per Article: 0] [Reference Citation Analysis] [Abstract] [Key Words] [Grants] [Track Full Text] [Journal Information] [Subscribe] [Scholar Register] [Received: 06/20/2024] [Revised: 07/26/2024] [Accepted: 08/05/2024] [Indexed: 11/26/2024]
Abstract
The fluxional nature of halogen bonds (XBs) in small molecular clusters, supramolecules, and molecular crystals has received considerable attention in recent years. In this work, based on extensive density-functional theory calculations and detailed electrostatic potential (ESP), natural bonding orbital (NBO), non-covalent interactions-reduced density gradient (NCI-RDG), and quantum theory of atoms in molecules (QTAIM) analyses, we unveil the existence of fluxional halogen bonds (FXBs) in a series of linear (IC6F4I)m(OONC6H4NOO)n (m + n = 2-5) complexes of tetrafluorodiiodobenzene with dinitrobenzene which appear to be similar to the previously reported fluxional hydrogen bonds (FHBs) in small water clusters (H2O)n (n = 2-6). The obtained GS ⇌ TS ⇌ GS ' fluxional mechanisms involve one FXB in the systems which fluctuates reversibly between two linear CI···O XBs in the ground states (GS and GS') via a bifurcated CI O2N van der Waals interaction in the transition state (TS). The cohesive energies (Ecoh) of these complexes with up to four XBs exhibit an almost perfect linear relationship with the numbers of XBs in the systems, with the average calculated halogen bond energy of Ecoh/XB = 3.48 kcal·mol-1 in the ground states which appears to be about 55% of the average calculated hydrogen bond energy (Ecoh/HB = 6.28 kcal·mol-1) in small water clusters.
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Affiliation(s)
- Cai-Yue Gao
- Institute of Molecular Science, Shanxi University, Taiyuan, China
| | - Bin-Bin Pei
- Institute of Molecular Science, Shanxi University, Taiyuan, China
| | - Si-Dian Li
- Institute of Molecular Science, Shanxi University, Taiyuan, China
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Schmidt A, Krupp A, Kleinheider J, Binnenbrinkmann TML, Wang R, Englert U, Strohmann C. The Halogen Bond to Ethers - Prototypic Molecules and Experimental Electron Density. ACS OMEGA 2024; 9:35037-35045. [PMID: 39157102 PMCID: PMC11325402 DOI: 10.1021/acsomega.4c05124] [Citation(s) in RCA: 0] [Impact Index Per Article: 0] [Reference Citation Analysis] [Abstract] [Grants] [Track Full Text] [Figures] [Subscribe] [Scholar Register] [Received: 05/31/2024] [Revised: 07/14/2024] [Accepted: 07/16/2024] [Indexed: 08/20/2024]
Abstract
Halogen bonds to dialkyl ether molecules have remained largely unexplored. We here address the synthesis and the structural chemistry of the first halogen-bonded noncyclic alkyl ethers, combining 1,4-diiodotetrafluorobenzene and the prototypic or commonly used ethers dimethyl ether, tetrahydrofuran, and methyl-tert-butyl ether as halogen acceptors. Two different structural motifs based on moderately strong halogen bonds were obtained: Discrete trimolecular aggregates are formed, and unexpected halogen-bonded supramolecular chain adducts feature oxygen-bifurcated halogen bonds with 1:1 donor:acceptor ratio. Both structure types may be selectively obtained even for the same ether by adjusting the stoichiometry in the crystallization experiments. The geometric features of the etheric oxygen center were found to be flexible, in contrast to the almost linear geometry about the halogen donor atom. A high-resolution X-ray diffraction experiment on the extended adduct of dimethyl ether allowed us to study the electronic details of the acceptor-bifurcated I···O···I halogen bonds. The electron density in the bond critical points and derived properties such as the Laplacian indicate essentially electrostatic interactions and explain the geometrical flexibility of ethers in halogen bonds. Our studies demonstrate the great versatility of ethers as halogen bond acceptors, that can occur in many geometrical arrangements and whose contribution to nature's structural designs should not be underestimated.
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Affiliation(s)
- Annika Schmidt
- Inorganic
Chemistry, TU Dortmund University, Otto-Hahn-Straße 6, 44227 Dortmund, Germany
| | - Anna Krupp
- Inorganic
Chemistry, TU Dortmund University, Otto-Hahn-Straße 6, 44227 Dortmund, Germany
| | - Johannes Kleinheider
- Inorganic
Chemistry, TU Dortmund University, Otto-Hahn-Straße 6, 44227 Dortmund, Germany
| | | | - Ruimin Wang
- Institute
of Inorganic Chemistry, RWTH Aachen University, Landoltweg 1, 52056 Aachen, Germany
- Institute
of Molecular Science, Key Laboratory of Chemical Biology and Molecular
Engineering of the Education Ministry, Shanxi
University, Taiyuan, Shanxi 030006, China
| | - Ulli Englert
- Institute
of Inorganic Chemistry, RWTH Aachen University, Landoltweg 1, 52056 Aachen, Germany
- Institute
of Molecular Science, Key Laboratory of Chemical Biology and Molecular
Engineering of the Education Ministry, Shanxi
University, Taiyuan, Shanxi 030006, China
| | - Carsten Strohmann
- Inorganic
Chemistry, TU Dortmund University, Otto-Hahn-Straße 6, 44227 Dortmund, Germany
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Scheiner S. Does a halogen bond require positive potential on the acid and negative potential on the base? Phys Chem Chem Phys 2023; 25:7184-7194. [PMID: 36815530 DOI: 10.1039/d3cp00379e] [Citation(s) in RCA: 4] [Impact Index Per Article: 2.0] [Reference Citation Analysis] [Abstract] [Track Full Text] [Journal Information] [Subscribe] [Scholar Register] [Indexed: 02/22/2023]
Abstract
It is usually expected that formation of a halogen bond (XB) requires that a region of positive electrostatic potential associated with a σ or π-hole on the Lewis acid will interact with the negative potential of the base, either a lone pair or π-bond region. Quantum calculations of model systems suggest this not to be necessary. The placement of electron-withdrawing substituents on the base can reverse the sign of the potential in its lone pair or π-bond region to positive, and this base can nonetheless engage in a XB with the positive σ-hole of a Lewis acid. The reverse scenario is also possible in certain circumstances, as a negatively charged σ-hole can form a XB with the negative lone pair region of a base. Despite these classical Coulombic repulsions, the overall electrostatic interaction is attractive in these XBs, albeit only weakly so. The strengths of these bonds are surprisingly insensitive to changes in the partner molecule. For example, even a wide range in the depth of the σ-hole of the approaching acid yields only a minimal change in the strength of the XB to a base with a positive potential.
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Affiliation(s)
- Steve Scheiner
- Department of Chemistry and Biochemistry Utah State University Logan, Utah, USA, 84322-0300.
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