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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...

Hydrogen Bonds

Hydrogen Bonds

Hydrogen BondsHydrogen 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...

Introduction to Chemical Bonds

Introduction to Chemical Bonds

Chemical Bonds
The electrons of the outermost energy level determine the energetic stability of the atom and its tendency to form chemical bonds with other atoms. The innermost electron shell has a maximum capacity of two electrons, but the next two electron shells can each have a maximum of eight electrons. This is known as the octet rule, which states that, with the exception of the innermost shell, atoms are most stable energetically when they have eight electrons in their valence shell, the...

Cohesion

Cohesion

Cohesion is the attraction between molecules of the same type, such as water molecules. Water molecules have an overall neutral charge but are polar molecule. An oxygen atom in one water molecule has a partial negative charge that can bind to a hydrogen atom with a partial positive charge in a second water molecule, forming a hydrogen bond. Each water molecule can form up to four hydrogen bonds with other water molecules. Hydrogen bonds are responsible for water's cohesive nature.
On a surface,...

Intermolecular Forces

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen bonds, and dispersion...

Intermolecular Forces

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions (attractive or repulsive) between charged species (permanent, partial, or temporary charges) and exist with varying strengths between ions, polar, nonpolar, and neutral molecules. The different types of intermolecular forces are ion–dipole, dipole–dipole, hydrogen bonds, and dispersion; among these, dipole–dipole, hydrogen bonds, and dispersion...

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Related Experiment Video

Updated: Jun 24, 2026

Multiscale Sampling of a Heterogeneous Water/Metal Catalyst Interface using Density Functional Theory and Force-Field Molecular Dynamics

Multiscale Sampling of a Heterogeneous Water/Metal Catalyst Interface using Density Functional Theory and Force-Field Molecular Dynamics

Published on: April 12, 2019

Hydrogen bond dynamics at the water/hydrocarbon interface.

Janamejaya Chowdhary¹, Branka M Ladanyi

¹Department of Chemistry, Colorado State University, Fort Collins, 80523-1872, USA. janamejaya.chowdhary@gmail.com

The Journal of Physical Chemistry. B

|March 27, 2009

Summary

Hydrogen bond dynamics in water near liquid interfaces are minimally affected by hydrocarbon chain length or branching. Water

Area of Science:

Physical Chemistry
Computational Chemistry
Surface Science

Background:

Understanding water behavior at liquid interfaces is crucial for various chemical and biological processes.
The structure and dynamics of interfacial water differ significantly from bulk water.
Hydrocarbon chain length and branching can influence interfacial properties.

Purpose of the Study:

To investigate the dynamics of hydrogen bond formation and breakage in water at water/hydrocarbon interfaces.
To determine the effect of hydrocarbon chain length and branching on interfacial water properties.
To analyze the role of molecular orientation and local coordination on hydrogen bond dynamics.

Main Methods:

Molecular dynamics simulations were employed to study water/alkane liquid interfaces.

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Studying Surfactant Effects on Hydrate Crystallization at Oil-Water Interfaces Using a Low-Cost Integrated Modular Peltier Device

Published on: March 18, 2020

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Last Updated: Jun 24, 2026

Multiscale Sampling of a Heterogeneous Water/Metal Catalyst Interface using Density Functional Theory and Force-Field Molecular Dynamics

Multiscale Sampling of a Heterogeneous Water/Metal Catalyst Interface using Density Functional Theory and Force-Field Molecular Dynamics

Published on: April 12, 2019

Probing the Structure and Dynamics of Interfacial Water with Scanning Tunneling Microscopy and Spectroscopy

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Published on: March 18, 2020

Interface location was defined using density profiles and molecular proximity.

Hydrogen bond time correlations, local coordination, and cooperativity were calculated.

Contributions of translational diffusion and O-H bond reorientation to hydrogen bond dynamics were examined.

Main Results:

Interfacial water hydrogen bond dynamics are weakly influenced by hydrocarbon identity (chain length, branching) and capillary waves.
Hydrogen bond dynamics are sensitive to the initial orientation of water molecules relative to the interface.
Anisotropic rotation of water principal axes and O-H vectors at the interface was confirmed.
Cooperativity in hydrogen bond population relaxation was investigated.

Conclusions:

The hydrocarbon phase has a limited impact on the hydrogen bond dynamics of adjacent interfacial water.
Molecular orientation plays a significant role in the hydrogen bond dynamics at water/hydrocarbon interfaces.
Further studies can explore other types of liquid interfaces and their effects on water dynamics.