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Related Concept Videos

Hydrogen Bonds01:04

Hydrogen Bonds

15.5K
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...
15.5K
Hydrogen Bonds00:26

Hydrogen Bonds

135.7K
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....
135.7K
Noncovalent Attractions in Biomolecules02:35

Noncovalent Attractions in Biomolecules

65.7K
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,...
65.7K
Noncovalent Attractions in Biomolecules02:35

Noncovalent Attractions in Biomolecules

19.7K
19.7K
¹H NMR: Long-Range Coupling01:27

¹H NMR: Long-Range Coupling

2.8K
The coupling interactions of nuclei across four or more bonds are usually weak, with J values less than 1 Hz. While these are usually not observed in spectra, the presence of multiple bonds along the coupling pathway can result in observable long-range coupling.
In alkenes, spin information is communicated via σ–π overlap, as seen in allylic (four-bond) and homoallylic (five-bond) couplings. These coupling interactions are stronger when the σ bond is parallel to the alkene...
2.8K
Spin–Spin Coupling: One-Bond Coupling01:17

Spin–Spin Coupling: One-Bond Coupling

1.5K
Coupling interactions are strongest between NMR-active nuclei bonded to each other, where spin information can be transmitted directly through the pair of bonding electrons. While nuclei polarize their electrons to the opposite spins, the bonding electron pair has opposite spins. Configurations with antiparallel nuclear spins are expected to be lower in energy. When coupling makes antiparallel states more favorable, J is considered to have a positive value. The one-bond coupling constant, 1J,...
1.5K

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Related Experiment Video

Updated: Mar 2, 2026

Construction and Systematical Symmetric Studies of a Series of Supramolecular Clusters with Binary or Ternary Ammonium Triphenylacetates
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Construction and Systematical Symmetric Studies of a Series of Supramolecular Clusters with Binary or Ternary Ammonium Triphenylacetates

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Strong Short-Range Cooperativity in Hydrogen-Bond Chains.

Nicholas Dominelli-Whiteley1, James J Brown1, Kamila B Muchowska1

  • 1EaStCHEM School of Chemistry, University of Edinburgh, Joseph Black Building, David Brewster Road, Edinburgh, EH9 3FJ, UK.

Angewandte Chemie (International Ed. in English)
|May 12, 2017
PubMed
Summary
This summary is machine-generated.

Hydrogen bond chains in water and proteins show surprising energetic cooperativity. Adding a second donor nearly doubles terminal bond strength, with further additions having minimal impact.

Keywords:
cooperativityhydrogen bondsnoncovalent interactionssupramolecular chemistry

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Area of Science:

  • Chemical Physics
  • Biophysics
  • Supramolecular Chemistry

Background:

  • Hydrogen bonds are crucial in biological systems like water and proteins.
  • Cooperativity in hydrogen bond chains is often inferred theoretically due to experimental challenges.
  • Previous studies suggest enhanced stability in hydrogen bond chains, but direct evidence is limited.

Purpose of the Study:

  • To directly measure the energetic cooperativity of hydrogen bond chains.
  • To investigate how chain length and geometry influence hydrogen bond strength.
  • To provide experimental validation for theoretical models of hydrogen bond cooperativity.

Main Methods:

  • Development of an experimental system to precisely control hydrogen bond chain geometry and length.
  • Direct measurement of the energetics of individual hydrogen bonds within controlled chains.
  • Systematic variation of the number of hydrogen bond donors in the chain.

Main Results:

  • The addition of a second hydrogen bond donor almost doubles the strength of the terminal hydrogen bond.
  • Extending the hydrogen bond chain beyond two donors yields diminishing returns on terminal bond strength.
  • Observed cooperativity effects are significant but primarily short-range.

Conclusions:

  • Direct experimental evidence confirms significant energetic cooperativity in hydrogen bond chains.
  • The strength enhancement is most pronounced when forming a dimer, with limited additional benefit from longer chains.
  • Findings support computational predictions of strong, short-range cooperative effects in hydrogen-bonded systems.