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Related Concept Videos

Hydrogen Bonds01:04

Hydrogen Bonds

7.7K
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...
7.7K
Introduction to Chemical Bonds01:01

Introduction to Chemical Bonds

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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...
7.6K
IR Spectrum Peak Broadening: Hydrogen Bonding01:23

IR Spectrum Peak Broadening: Hydrogen Bonding

764
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...
764
Intermolecular Forces03:13

Intermolecular Forces

56.0K
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...
56.0K
Water: A Bronsted-Lowry Acid and Base02:30

Water: A Bronsted-Lowry Acid and Base

49.1K
The reaction between a Brønsted-Lowry acid and water is called acid ionization. For example, when hydrogen fluoride dissolves in water and ionizes, protons are transferred from hydrogen fluoride molecules to water molecules, yielding hydronium ions and fluoride ions:
 
Base ionization of a species occurs when it accepts protons from water molecules. In the example below, pyridine molecules, C5NH5, undergo base ionization when dissolved in water, yielding hydroxide and pyridinium ions:
49.1K
Bond Polarity, Dipole Moment, and Percent Ionic Character02:48

Bond Polarity, Dipole Moment, and Percent Ionic Character

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Bond Polarity
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Related Experiment Video

Updated: May 13, 2025

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

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Quantifying hydrogen bonding using electrically tunable nanoconfined water.

Ziwei Wang1,2, Anupam Bhattacharya3, Mehmet Yagmurcukardes4

  • 1Department of Physics and Astronomy, University of Manchester, Manchester, UK. ziwei.wang@manchester.ac.uk.

Nature Communications
|April 15, 2025
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Summary

This study redefines hydrogen bonds as elastic dipoles, enabling precise quantification of their strength and properties in water systems. This new model, validated with gypsum, opens doors for advanced materials with tunable hydrogen bonding.

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Quantification of Hydrogen Concentrations in Surface and Interface Layers and Bulk Materials through Depth Profiling with Nuclear Reaction Analysis
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Area of Science:

  • Materials Science
  • Physical Chemistry
  • Spectroscopy

Background:

  • Hydrogen bonds are fundamental to biology and technology but poorly understood and quantified.
  • Existing models fail to capture essential hydrogen bond characteristics like strength, directionality, and cooperativity.
  • This limits the prediction and design of complex hydrogen-bonded materials.

Purpose of the Study:

  • To introduce a new conceptual framework for understanding hydrogen bonds as elastic dipoles in electric fields.
  • To develop a method for quantitatively measuring hydrogen bond strength using spectroscopic data.
  • To explore the potential of hydrogen bond heterostructures as novel tunable materials.

Main Methods:

  • Conceptualized hydrogen bonds as elastic dipoles responding to electric fields.
  • Utilized gypsum, a hydrogen bond heterostructure, to calibrate hydrogen bond strength via an applied electric field.
  • Employed spectroscopic measurements, specifically the stretching vibration frequency of confined water, for quantification.

Main Results:

  • The elastic dipole model successfully explains various hydrogen bonding phenomena in water systems.
  • Hydrogen bond strength was quantitatively determined from spectroscopic measurements.
  • The model accurately reproduced key properties of confined water, including O-H bond length and dipole moment.

Conclusions:

  • The elastic dipole concept provides a robust framework for quantifying hydrogen bonds.
  • Hydrogen bond heterostructures represent a new class of tunable materials with enhanced bonding properties.
  • These materials hold promise for applications in catalysis, separation, and energy storage.