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Related Concept Videos

Hydrogen Bonds00:26

Hydrogen Bonds

134.3K
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....
134.3K
Hydrogen Bonds01:04

Hydrogen Bonds

15.0K
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...
15.0K
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
Valence Bond Theory02:45

Valence Bond Theory

50.3K
Overview of Valence Bond Theory
50.3K
Covalent Bonds01:29

Covalent Bonds

163.7K
Overview
163.7K
Covalent Bonding and Lewis Structures02:46

Covalent Bonding and Lewis Structures

62.0K
Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual attraction of atoms for a “shared” pair of electrons.
62.0K

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Related Experiment Video

Updated: Feb 10, 2026

Fabrication and Characterization of Superconducting Resonators
10:26

Fabrication and Characterization of Superconducting Resonators

Published on: May 21, 2016

11.9K

High-temperature superconductivity using a model of hydrogen bonds.

Daniel Kaplan1, Yoseph Imry1

  • 1Department of Condensed Matter Physics, Faculty of Physics, Weizmann Institute of Science, Rehovot 76100, Israel yoseph.imry@weizmann.ac.il daniel.kaplan@weizmann.ac.il.

Proceedings of the National Academy of Sciences of the United States of America
|May 16, 2018
PubMed
Summary

This study presents a simple model explaining superconducting gap behavior in hydrogen-based superconductors using Bardeen-Cooper-Schrieffer theory. The model successfully reproduces experimental effects like the isotope effect and pressure-dependent enhancement.

Keywords:
BCS theoryhigh-temperature superconductivityhydrogen bondshydrogen sulfidephysical chemistry

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Area of Science:

  • Condensed Matter Physics
  • Materials Science

Background:

  • Growing interest in high-temperature and hydrogen-based superconductors.
  • Understanding the superconducting gap is crucial for material applications.

Purpose of the Study:

  • To develop a simple model for the superconducting gap behavior.
  • To explain experimental observations in hydrogen-based superconductors.

Main Methods:

  • Application of naive Bardeen-Cooper-Schrieffer (BCS) theory.
  • Analysis of factors within the BCS gap equation.

Main Results:

  • The model reproduces key experimental findings, including the isotope effect.
  • It explains the enhancement of the superconducting gap under pressure.
  • Identified proton state matrix elements and level splitting as key factors.

Conclusions:

  • A simplified BCS model effectively describes superconducting gap phenomena in hydrogen-based materials.
  • Proton-specific interactions significantly influence superconductivity under pressure.