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Hydrogen Bonds

Hydrogen Bonds

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....

Hydrogen Bonds

Hydrogen Bonds

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...

Halogens

Halogens

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.

IR Spectrum Peak Broadening: Hydrogen Bonding

IR Spectrum Peak Broadening: Hydrogen Bonding

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...

Molecular and Ionic Solids

Molecular and Ionic Solids

Crystalline solids are divided into four types: molecular, ionic, metallic, and covalent network based on the type of constituent units and their interparticle interactions.
Molecular Solids
Molecular crystalline solids, such as ice, sucrose (table sugar), and iodine, are solids that are composed of neutral molecules as their constituent units. These molecules are held together by weak intermolecular forces such as London dispersion forces, dipole-dipole interactions, or hydrogen bonds, which...

Valence Bond Theory

Valence Bond Theory

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Related Experiment Video

Updated: Jan 25, 2026

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

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

Published on: March 24, 2018

Halogenated building blocks for 2D crystal engineering on solid surfaces: lessons from hydrogen bonding.

Arijit Mukherjee¹, Ana Sanz-Matias², Gangamallaiah Velpula¹

¹Division of Molecular Imaging and Photonics , Department of Chemistry , KU Leuven , Celestijnenlaan, 200F , B-3001 Leuven , Belgium . Email: kunal.mali@kuleuven.be ;

Chemical Science

|April 25, 2019

Summary

This summary is machine-generated.

Crystal engineering using halogen bonds shows promise, but a direct analogy with hydrogen bonds leads to fractured networks. Modified molecular designs are needed for predictable 2D structures.

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

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Area of Science:

Supramolecular chemistry
Materials science
Crystal engineering

Background:

Halogen bonding is a key interaction in crystal engineering, analogous to hydrogen bonding.
Predictive design of 2D networks is crucial for materials applications.

Purpose of the Study:

To evaluate a retrosynthetic approach for designing 2D halogen-bonded networks based on hydrogen bond topology.
To investigate the self-assembly of 1,3-dibromo-5-alkoxybenzene derivatives.

Main Methods:

Scanning tunneling microscopy (STM) for experimental characterization.
Density functional theory (DFT) calculations with natural bonding orbitals (NBO) and perturbation analysis.
Modified force field development for energy calculations.

Main Results:

The retrosynthetic approach successfully formed small halogen-bonded clusters but not continuous lamellar structures.
Observed networks consisted of fractured rows of molecular modules.
DFT calculations elucidated the interactions stabilizing halogen-bonded dimers.

Conclusions:

The direct analogy between hydrogen and halogen bonds is insufficient for predicting large-scale 2D network structures.
Molecular design modifications are necessary for successful application of this analogy.
Further research is needed to refine predictive models for halogen-bonded materials.