Search research articles

ABOUT JoVE

Overview Leadership Blog JoVE Help Center

AUTHORS

Publishing Process Editorial Board Scope & Policies Peer Review FAQ Submit

LIBRARIANS

Testimonials Subscriptions Access Resources Library Advisory Board FAQ

RESEARCH

JoVE Journal Methods Collections JoVE Encyclopedia of Experiments Archive

EDUCATION

JoVE Core JoVE Business JoVE Science Education JoVE Lab Manual Faculty Resource Center Faculty Site

Terms & Conditions of Use

Related Concept Videos

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 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....

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...

Valence Bond Theory

Valence Bond Theory

Overview of Valence Bond Theory

Valence Bond Theory

Valence Bond Theory

Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...

Hybridization of Atomic Orbitals II

Hybridization of Atomic Orbitals II

sp3d and sp3d 2 Hybridization

You might also read

Related Articles

Articles linked to this work by shared authors, journal, and citation graph.

Sort by

Same author

Mode-Selective Dual-Level Vibrational Perturbation Theory Assisted by Machine Learning for Rotational and Vibrational Spectra of Benzoic Acid and Aspirin.

The journal of physical chemistry. A·2026

Same author

Correlating picosecond electron transfer and confined water dynamics in Prussian Blue using electrochemical two-dimensional infrared spectroscopy.

Proceedings of the National Academy of Sciences of the United States of America·2026

Same author

VPT2 Calculations of Vibrational Energies of CH<sub>3</sub>COOC<sub>6</sub>H<sub>4</sub>COOH Done in Seconds on a Laptop Using a Machine Learned Potential.

The journal of physical chemistry letters·2026

Same author

Strong Proper C-H Hydrogen Bonds: Experimental Evidence across Spectral Ranges.

JACS Au·2026

Same author

Roaming dynamics in highly excited-state unimolecular and complex bimolecular reactions.

Physical chemistry chemical physics : PCCP·2026

Same author

Monomeric Neural Network Potential for General Covalent Molecules: Linear Alkanes as an Example.

Journal of chemical theory and computation·2026

Search research articles

Related Experiment Video

Updated: Nov 22, 2025

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

Crossover from hydrogen to chemical bonding.

Bogdan Dereka¹, Qi Yu², Nicholas H C Lewis¹

¹Department of Chemistry, Institute for Biophysical Dynamics, and James Franck Institute, The University of Chicago, Chicago, IL 60637, USA.

Science (New York, N.Y.)

|January 8, 2021

Summary

Short strong hydrogen bonds (H-bonds) blur the line between electrostatic and covalent interactions. This study reveals their unique vibrational behavior in water, identifying the transition from hydrogen bonding to chemical bonding.

More Related Videos

Synthesis and Characterization of Supramolecular Colloids

Synthesis and Characterization of Supramolecular Colloids

Published on: April 22, 2016

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

Related Experiment Videos

Last Updated: Nov 22, 2025

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

Synthesis and Characterization of Supramolecular Colloids

Synthesis and Characterization of Supramolecular Colloids

Published on: April 22, 2016

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

Area of Science:

Chemical Physics
Spectroscopy
Quantum Chemistry

Background:

Hydrogen bonds (H-bonds) present a duality, interpretable as electrostatic or covalent interactions.
Distinguishing between these descriptions, especially for short, strong H-bonds, is challenging due to limited experimental techniques.

Purpose of the Study:

To investigate the nature of short strong hydrogen bonds (H-bonds).
To explore the transition point where hydrogen bonding becomes chemical bonding.
To characterize the vibrational dynamics of the [F-H-F]⁻ ion in water.

Main Methods:

Femtosecond two-dimensional infrared (2D IR) spectroscopy to probe vibrational potentials.
High-level quantum-chemical calculations for theoretical analysis.

Main Results:

Observed superharmonic behavior in proton motion within the [F-H-F]⁻ ion.
Proton motion strongly couples to donor-acceptor stretching.
This coupling diminishes upon H-bond bending, indicating a distinct spectroscopic signature.

Conclusions:

Demonstrated a clear spectroscopic crossover from conventional to short strong H-bonds.
Provided experimental evidence for the transition from hydrogen bonding to chemical bonding.
Highlighted the utility of 2D IR spectroscopy and quantum chemistry in understanding complex bonding phenomena.