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Related Concept Videos

Hydrogen Bonds00:26

Hydrogen Bonds

133.9K
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....
133.9K
Hydrogen Bonds01:04

Hydrogen Bonds

14.8K
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...
14.8K
IR Spectrum Peak Broadening: Hydrogen Bonding01:23

IR Spectrum Peak Broadening: Hydrogen Bonding

1.8K
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...
1.8K
Metal-Ligand Bonds02:51

Metal-Ligand Bonds

24.4K
The hemoglobin in the blood, the chlorophyll in green plants, vitamin B-12, and the catalyst used in the manufacture of polyethylene all contain coordination compounds. Ions of the metals, especially the transition metals, are likely to form complexes.
In these complexes, transition metals form coordinate covalent bonds, a kind of Lewis acid-base interaction in which both of the electrons in the bond are contributed by a donor (Lewis base) to an electron acceptor (Lewis acid). The Lewis acid in...
24.4K
Valence Bond Theory02:45

Valence Bond Theory

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

Covalent Bonds

163.2K
Overview
163.2K

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Updated: Feb 7, 2026

Quantification of Hydrogen Concentrations in Surface and Interface Layers and Bulk Materials through Depth Profiling with Nuclear Reaction Analysis
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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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Hydrogen-Bonded Donor-Acceptor Arrays at the Solution-Graphite Interface.

Gangamallaiah Velpula1, Mengmeng Li2,3, Yunbin Hu2

  • 1KU Leuven, Division of Molecular Imaging and Photonics, Department of Chemistry, Celestijnenlaan 200F, B-3001, Leuven, Belgium.

Chemistry (Weinheim an Der Bergstrasse, Germany)
|July 18, 2018
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Summary

Researchers precisely controlled the nanoscale structure of organic thin films by designing molecular building blocks. This breakthrough enables tailored supramolecular assembly for advanced organic electronics.

Keywords:
STMdonor-acceptorhydrogen-bondingorganic electronicsself-assembly

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A Simple, Low-cost, and Robust System to Measure the Volume of Hydrogen Evolved by Chemical Reactions with Aqueous Solutions
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18F-Labeling of Radiotracers Functionalized with a Silicon Fluoride Acceptor SiFA for Positron Emission Tomography
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18F-Labeling of Radiotracers Functionalized with a Silicon Fluoride Acceptor SiFA for Positron Emission Tomography
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Area of Science:

  • Materials Science
  • Organic Electronics
  • Supramolecular Chemistry

Background:

  • Controlling nanoscale morphology is crucial for organic (opto)electronic devices.
  • Thin film morphology depends on molecular orientation and surface packing.
  • Co-assembly of electron-donating and -accepting molecules is key.

Purpose of the Study:

  • To demonstrate control over surface co-assembly of organic building blocks via supramolecular design.
  • To investigate the co-assembly of hexa-peri-hexabenzocoronene (HBC) derivatives with perylene tetracarboxy diimide (PDI).
  • To explore the role of hydrogen bonding in directing molecular assembly.

Main Methods:

  • Synthesis of hexa-peri-hexabenzocoronene (HBC) derivatives with hydrogen-bonding sites.
  • Studying co-assembly using scanning tunneling microscopy (STM) at the solution-graphite interface.
  • Analyzing the lateral co-assembly of electron-rich HBCs and electron-deficient PDIs.

Main Results:

  • Electron-rich HBCs and electron-deficient PDIs co-assemble laterally with high fidelity via preprogrammed hydrogen bonds.
  • Surface stoichiometry was tunable by altering the number of hydrogen-bonding sites on HBC derivatives.
  • Successful demonstration of controlled co-assembly through molecular design.

Conclusions:

  • Supramolecular design is a powerful strategy for controlling the co-assembly of organic building blocks.
  • This approach is relevant for fabricating organic electronic materials with desired morphologies.
  • The study provides a model for rational design of multicomponent organic thin films.