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Related Concept Videos

Hydrogen Bonds00:26

Hydrogen Bonds

133.0K
Hydrogen bonds are weak attractions between atoms that have formed other chemical bonds. One of these atoms is electronegative, like oxygen, and has a partial negative charge. The other is a hydrogen atom that has bonded with another electronegative atom and has a partial positive charge.
Hydrogen Bonds Control the World!
Because hydrogen has very weak electronegativity when it binds with a strongly electronegative atom, such as oxygen or nitrogen, electrons in the bond are unequally shared....
133.0K
Hydrogen Bonds01:04

Hydrogen Bonds

14.0K
A hydrogen bond is formed when a weakly positive hydrogen atom already bonded to one electronegative atom (for example, the oxygen in the water molecule) is attracted to another electronegative atom from another polar molecule, such as water (H2O), hydrogen fluoride (HF), or ammonia (NH3). The huge electronegativity difference between the H atom (2.1) and the atom to which it is bonded (4.0 for an F atom, 3.5 for an O atom, or 3.0 for an N atom), combined with the very small size of an H atom...
14.0K
Halogens03:01

Halogens

23.5K
Group 17 elements, known as halogens, are nonmetals. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine a solid. Astatine is a highly unstable radioactive element, so currently, most of its properties are unknown due to its short half-life. Tennessine is a synthetic element also predicted to be in this group. 
23.5K
IR Spectrum Peak Broadening: Hydrogen Bonding01:23

IR Spectrum Peak Broadening: Hydrogen Bonding

1.8K
The vibrational frequency of a bond is directly proportional to its bond strength. As a result, stronger bonds vibrate at higher frequencies, while weaker bonds vibrate at lower frequencies. The stretching vibration of the strong O–H bond in alcohols and phenols (very dilute solution or gas phase) appears as a sharp peak at 3600–3650 cm−1.
However, the extent of hydrogen bonding influences the observed stretching frequency and band broadening. Intermolecular or intramolecular...
1.8K
Valence Bond Theory02:45

Valence Bond Theory

50.1K
Overview of Valence Bond Theory
50.1K
Covalent Bonds01:29

Covalent Bonds

161.9K
Overview
161.9K

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From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding
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From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding

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Hydrogen and Halogen Bond Interactions with 2,6-Dimethoxypyridine.

Margaret M Stucky1, Ashly Antony1, Jonah W Jurss1

  • 1Department of Chemistry & Biochemistry, University of Mississippi, Oxford, Mississippi 38677, United States.

The Journal of Physical Chemistry. A
|January 29, 2026
PubMed
Summary
This summary is machine-generated.

Investigating noncovalent interactions with 2,6-dimethoxypyridine (DMOP), researchers found hydrogen bonding showed no spectroscopic changes. Halogen bonding, however, demonstrated significant vibrational shifts, indicating resilient binding motifs.

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Area of Science:

  • Physical Chemistry
  • Spectroscopy
  • Computational Chemistry

Background:

  • Noncovalent interactions, including hydrogen and halogen bonding, influence molecular properties.
  • Modifying nitrogen-containing heterocycles with electron-donating or withdrawing groups can tune these interactions.
  • 2,6-dimethoxypyridine (DMOP) serves as a model to study electron withdrawal effects.

Purpose of the Study:

  • To investigate the impact of noncovalent interactions on DMOP using Raman spectroscopy and computational chemistry.
  • To explore how electron-withdrawing methoxy groups affect hydrogen and halogen bonding in DMOP.
  • To compare charge transfer and spectroscopic changes in hydrogen versus halogen bonding.

Main Methods:

  • Raman spectroscopy was employed to analyze experimental spectroscopic changes.
  • Computational chemistry, including Natural Bond Orbital (NBO) calculations, was used for theoretical analysis.
  • Mixtures of DMOP with water and heptafluoro-2-iodopropane (HFIP) were studied.

Main Results:

  • Hydrogen bonding between DMOP and water did not yield discernible spectroscopic changes.
  • Computational results indicated preferential water binding to itself or methoxy oxygen atoms.
  • Halogen bonding with HFIP resulted in experimental vibrational red shifts in HFIP modes.
  • NBO calculations showed greater charge transfer in halogen bonding compared to hydrogen bonding.

Conclusions:

  • Competitive binding sites and steric effects in DMOP can hinder nitrogen lone pair accessibility for hydrogen bonding.
  • Halogen bonding involving iodine is a robust interaction in solution, even with competing sites.
  • This resilient halogen bonding motif holds potential for applications in molecular self-assembly.