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Related Concept Videos

Hydrogen Bonds00:26

Hydrogen Bonds

135.4K
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....
135.4K
Hydrogen Bonds01:04

Hydrogen Bonds

15.4K
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...
15.4K
Intermolecular Forces03:13

Intermolecular Forces

73.6K
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...
73.6K
Intermolecular vs Intramolecular Forces03:00

Intermolecular vs Intramolecular Forces

98.9K
Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular force is influenced by the distance of separation between molecules. The forces significantly affect the interactions in solids and liquids, where the molecules are close together. In gases, IMFs become important only under high-pressure conditions (due to the proximity of gas molecules). Intermolecular forces dictate the physical properties of...
98.9K
IR Spectrum Peak Broadening: Hydrogen Bonding01:23

IR Spectrum Peak Broadening: Hydrogen Bonding

1.9K
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...
1.9K
Noncovalent Attractions in Biomolecules02:35

Noncovalent Attractions in Biomolecules

65.6K
Noncovalent attractions are associations within and between molecules that influence the shape and structural stability of complexes. These interactions differ from covalent bonding in that they do not involve sharing of electrons.
Four types of noncovalent interactions are hydrogen bonds, van der Waals forces, ionic bonds, and hydrophobic interactions.
Hydrogen bonding results from the electrostatic attraction of a hydrogen atom covalently bonded to a strong-electronegative atom like oxygen,...
65.6K

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Related Experiment Video

Updated: Feb 23, 2026

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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Special Issue: Intramolecular Hydrogen Bonding 2017.

Steve Scheiner1

  • 1Department of Chemistry and Biochemistry, Utah State University, Logan, UT 84322-0300, USA. steve.scheiner@usu.edu.

Molecules (Basel, Switzerland)
|September 12, 2017
PubMed
Summary

Hydrogen bonds remain fascinating despite over a century of research. Their enduring complexity continues to captivate scientists across various fields.

Area of Science:

  • Chemistry
  • Biophysics
  • Materials Science

Background:

  • The hydrogen bond (H-bond) has been a subject of intense scientific inquiry for over 100 years.
  • Despite extensive study, the H-bond continues to present complex and intriguing characteristics.

Discussion:

  • The H-bond's unique properties contribute to its pervasive influence in chemical and biological systems.
  • Ongoing research aims to further elucidate the nuanced interactions and energetic contributions of H-bonds.

Key Insights:

  • The H-bond's fundamental nature is still a source of fascination and discovery.
  • Its role in molecular interactions is critical across diverse scientific disciplines.

Outlook:

  • Future research will likely uncover new facets of H-bond behavior and applications.

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  • Continued exploration promises deeper understanding and novel technological advancements driven by H-bond phenomena.