scholarly journals Synthesis, structure and reactivity of a terminal magnesium fluoride compound, [TpBut,Me]MgF: hydrogen bonding, halogen bonding and C–F bond formation

2016 ◽  
Vol 7 (1) ◽  
pp. 142-149 ◽  
Author(s):  
Michael Rauch ◽  
Serge Ruccolo ◽  
John Paul Mester ◽  
Yi Rong ◽  
Gerard Parkin
Keyword(s):  
Hydrogen Bond ◽  
Hydrogen Bonding ◽  
Halogen Bond ◽  
Bond Formation ◽  
Halogen Bonding ◽  
Magnesium Fluoride ◽  
Fluoride Compound

The terminal magnesium fluoride compound, [TpBut,Me]MgF, serves as a hydrogen bond and halogen bond acceptor for indole and C6F5I, and also reacts with Ph3CCl to form a C–F bond.

scholarly journals Halogen-Bonding-Driven Self-Assembly of Solvates of Tetrabromoterephthalic Acid

Crystals ◽  
2021 ◽  
Vol 11 (2) ◽  
pp. 198
Author(s):  
Nucharee Chongboriboon ◽  
Kodchakorn Samakun ◽  
Winya Dungkaew ◽  
Filip Kielar ◽  
Mongkol Sukwattanasinitt ◽  
...  
Keyword(s):  
Hydrogen Bond ◽  
Hydrogen Bonding ◽  
Phase Transitions ◽  
Self Assembly ◽  
Solid Phase ◽  
Halogen Bond ◽  
Halogen Bonding ◽  
Cooperative Effect ◽  
Hydrogen Bonding Interactions ◽  
Solvent Molecules

Halogen bonding is one of the most interesting noncovalent attractions capable of self-assembly and recognition processes in both solution and solid phase. In this contribution, we report on the formation of two solvates of tetrabromoterephthalic acid (H2Br4tp) with acetonitrile (MeCN) and methanol (MeOH) viz. H2Br4tp·2MeCN (1MeCN) and H2Br4tp·2MeOH (2MeOH). The host structures of both 1MeCN and 2MeOH are assembled via the occurrence of simultaneous Br···Br, Br···O, and Br···π halogen bonding interactions, existing between the H2Br4tp molecular tectons. Among them, the cooperative effect of the dominant halogen bond in combination with hydrogen bonding interactions gave rise to different supramolecular assemblies, whereas the strength of the halogen bond depends on the type of hydrogen bond between the molecules of H2Br4tp and the solvents. These materials show a reversible release/resorption of solvent molecules accompanied by evident crystallographic phase transitions.

Halogen bonding controlled 2D self-assembled polymorphism of regioisomeric thienophenanthrene derivatives by coadsorption

2021 ◽  
Author(s):  
Peng Pang ◽  
Yi Wang ◽  
Xinrui Miao ◽  
Bang Li ◽  
Wenli Deng
Keyword(s):  
Hydrogen Bonding ◽  
Formation Mechanism ◽  
Self Assembly ◽  
Halogen Bond ◽  
Bond Formation ◽  
Halogen Bonding ◽  
Supramolecular Assemblies ◽  
The Self ◽  
Self Assembled

Deeply understanding the halogen-bond formation mechanism in surface-supported supramolecular assemblies is under explored compared with the existing knowledge of hydrogen bonding. Here we report the self-assembly of regioisomeric bromine substituted...

Competition between the hydrogen bond and the halogen bond in a [CH3OH–CCl4] complex: a matrix isolation IR spectroscopy and computational study

2020 ◽  
Vol 22 (39) ◽  
pp. 22465-22476
Author(s):  
Dhritabrata Pal ◽  
Sumit Kumar Agrawal ◽  
Amrita Chakraborty ◽  
Shamik Chakraborty
Keyword(s):  
Hydrogen Bond ◽  
Hydrogen Bonding ◽  
Ir Spectroscopy ◽  
Computational Study ◽  
Halogen Bond ◽  
Matrix Isolation ◽  
Halogen Bonding ◽  
Bond Interaction ◽  
Bonding Interaction ◽  
Polar Mixtures

Halogen bonding interaction (X-Bond) is prevalent over hydrogen bonding (H-Bond) interaction in [CH3OH–CCl4] mixtures/clusters: consequence in polar/non-polar mixtures and/or corresponding complexes in atmosphere needs to be investigated.

Halogen Bonding Organocatalysis Enhanced through Intramolecular Hydrogen Bonds

2022 ◽  
Author(s):  
Asia Marie S Riel ◽  
Daniel Adam Decato ◽  
Jiyu Sun ◽  
Orion Berryman
Keyword(s):  
Hydrogen Bond ◽  
Hydrogen Bonds ◽  
Halogen Bond ◽  
Direct Interaction ◽  
Halogen Bonding ◽  
Intramolecular Hydrogen Bonds ◽  
Intramolecular Hydrogen

Recent results indicate a halogen bond donor is strengthened through direct interaction with a hydrogen bond to the electron-rich belt of the halogen. Here, this Hydrogen Bond enhanced Halogen Bond...

scholarly journals Superior anion induced shuttling behaviour exhibited by a halogen bonding two station rotaxane

2016 ◽  
Vol 7 (8) ◽  
pp. 5171-5180 ◽  
Author(s):  
Timothy A. Barendt ◽  
Sean W. Robinson ◽  
Paul D. Beer
Keyword(s):  
Hydrogen Bonding ◽  
Halogen Bond ◽  
Translational Motion ◽  
Anion Recognition ◽  
Halogen Bonding ◽  
Recognition Site ◽  
Naphthalene Diimide

Two bistable halogen and hydrogen bonding-naphthalene diimide [2]rotaxanes have been prepared and the system incorporating a halogen bond donor anion recognition site is demonstrated to exhibit superior anion induced translational motion of the macrocyclic wheel component relative to the hydrogen bonding analogue.

Enthalpies of hydrogen bond formation of 1-octanol with aprotic organic solvents. A comparison of the solvation enthalpy, pure base, and non-hydrogen-bonding baseline methods

1985 ◽  
Vol 63 (2) ◽  
pp. 342-348 ◽  
Author(s):  
W. Kirk Stephenson ◽  
Richard Fuchs
Keyword(s):  
Hydrogen Bond ◽  
Hydrogen Bonding ◽  
Bond Formation ◽  
Enthalpies Of Solution ◽  
Dispersion Interactions ◽  
Butyl Ether ◽  
Hydrogen Bond Formation ◽  
Solvation Enthalpy ◽  
Benzene Toluene ◽  
Good Agreement

Enthalpies of solution (ΔHs) of 1-octanol and five model compounds (di-n-butyl ether, n-heptyl methyl ether, 1-fluoro-octane, 1-chlorooctane, and n-octane) have been determined in 13 solvents (heptane, cyclohexane, CCl4, 1,1,1-trichloro-ethane, 1,2-dichloroethane, triethylamine, butyl ether, ethyl acetate, DMF, DMSO, benzene, toluene, mesitylene), and combined with heats of vaporization to give enthalpies of transfer from vapor to solvent (ΔH(v → S)). These values have been used to calculate the enthalpy of hydrogen bond formation (ΔHh) of 1-octanol with each solvent, using the pure base (PB), solvation enthalpy (SE), and non-hydrogen-bonding baseline (NHBB) methods. Evidence is presented suggesting that (a) the SE method is susceptible to mismatches of the 1-octanol vs. model polar and dispersion interactions, (b) the PB method is sensitive to polar interaction mismatches, whereas (c) the NHBB method compensates for both polar and dispersion interactions mismatches. The (apparent) ΔHh values determined by the SE and PB methods may be as much as several kcal/mol (nearly 50%) too large, because of the inclusion of other polar and dispersion interactions. The NHBB method is therefore preferred for determining enthalpies of H-bond formation from calorimetric data. However, apparent ΔHh values from the SE and PB methods can be incorporated into total solvatochromic equations using Taft–Kamiet π*, β, and ξ parameters, to provide enthalpies of H-bond formation in good agreement with ΔHh (NHBB).

Anharmonicity, solvent effects, and hydrogen bonding: NH stretching vibrations

1970 ◽  
Vol 48 (14) ◽  
pp. 2197-2203 ◽  
Author(s):  
A. Foldes ◽  
C. Sandorfy
Keyword(s):  
Hydrogen Bond ◽  
Hydrogen Bonding ◽  
Solvent Effects ◽  
Bond Formation ◽  
Hydrogen Bond Formation ◽  
Stretching Vibration ◽  
Solvent Shifts ◽  
Stretching Vibrations ◽  
Secondary Amides ◽  
Influence Of Solvent

The influence of solvent effects and hydrogen bond formation on the anharmonicity of the NH stretching vibration of simple secondary amides, lactams, anilides, indole, pyrrole, and imidazole have been studied; and the frequencies of the first and second overtones, their half widths and solvent shifts measured. The validity of Buckingham's theory is established in the case of inert solvents; whereas the second order perturbation treatments are shown to be inapplicable to the case of hydrogen bonding solvents. All NH stretching modes seem to exhibit the same anharmonic behavior which is very different from that of OH vibrations.

Dynamics of the chemical bond: inter- and intra-molecular hydrogen bond

2015 ◽  
Vol 177 ◽  
pp. 51-64 ◽  
Author(s):  
Elangannan Arunan ◽  
Devendra Mani
Keyword(s):  
Hydrogen Bond ◽  
Hydrogen Bonding ◽  
Molecular Hydrogen ◽  
Theoretical Calculations ◽  
Bond Formation ◽  
Chem Phys ◽  
Equilibrium Structure ◽  
Molecular Hydrogen Bond ◽  
Mode Vibration ◽  
Definition Of

In this discussion, we show that a static definition of a ‘bond’ is not viable by looking at a few examples for both inter- and intra-molecular hydrogen bonding. This follows from our earlier work (Goswami and Arunan,Phys. Chem. Chem. Phys.2009,11, 8974) which showed a practical way to differentiate ‘hydrogen bonding’ from ‘van der Waals interaction’. We report results fromab initioand atoms in molecules theoretical calculations for a series of Rg⋯HX complexes (Rg = He/Ne/Ar and X = F/Cl/Br) and ethane-1,2-diol. Results for the Rg⋯HX/DX complexes show that Rg⋯DX could have a ‘deuterium bond’ even when Rg⋯HX is not ‘hydrogen bonded’, according to the practical criterion given by Goswami and Arunan. Results for ethane-1,2-diol show that an ‘intra-molecular hydrogen bond’ can appear during a normal mode vibration which is dominated by the O⋯O stretching, though a ‘bond’ is not found in the equilibrium structure. This dynamical ‘bond’ formation may nevertheless be important in ensuring the continuity of electron density across a molecule. In the former case, a vibration ‘breaks’ an existing bond and in the later case, a vibration leads to ‘bond’ formation. In both cases, the molecule/complex stays bound irrespective of what happens to this ‘hydrogen bond’. Both these cases push the borders on the recent IUPAC recommendation on hydrogen bonding (Arunanet al. Pure. Appl. Chem.2011,831637) and justify the inclusive nature of the definition.

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