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Related Concept Videos

Hydrogen Bonds01:04

Hydrogen Bonds

12.7K
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...
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Hydrogen Bonds00:26

Hydrogen Bonds

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

IR Spectrum Peak Broadening: Hydrogen Bonding

1.7K
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...
1.7K
Conformations of Cyclohexane02:11

Conformations of Cyclohexane

14.9K
Cyclohexane does not exist in a planar form due to the high angle and torsional strain it would experience in the planar structure. Instead, it adopts non-planar chair and boat conformations.
The chair form is the most stable and derives its name from its resemblance to the “easy chair.” In the chair conformation, two carbon atoms are arranged out-of-plane — one above and one below, minimizing the torsional strain. In the chair form, the bond angle is very close to the ideal...
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VSEPR Theory and the Effect of Lone Pairs04:01

VSEPR Theory and the Effect of Lone Pairs

51.6K
Effect of Lone Pairs of Electrons on Molecule Geometry
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2D NMR: Heteronuclear Single-Quantum Correlation Spectroscopy (HSQC)01:19

2D NMR: Heteronuclear Single-Quantum Correlation Spectroscopy (HSQC)

1.3K
Heteronuclear single-quantum correlation spectroscopy (HSQC) is a 2D NMR technique that reveals one-bond correlations between hydrogen and a heteronucleus. The HSQC experiment is similar to the heteronuclear correlation experiment (HETCOR) but is more sensitive. In the HSQC spectrum, the proton chemical shift is plotted on the horizontal F2 axis, while the 13C chemical shift is plotted on the vertical F1 axis. The corresponding proton and 13C spectra are also shown. The HSQC contour plot does...
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Fluorescence Anisotropy as a Tool to Study Protein-protein Interactions
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Charting Hydrogen Bond Anisotropy.

Diogo Santos-Martins1, Stefano Forli1

  • 1Department of Integrative Structural and Computational Biology, The Scripps Research Institute, La Jolla, California 92037, United States.

Journal of Chemical Theory and Computation
|February 28, 2020
PubMed
Summary
This summary is machine-generated.

Hydrogen bonds (HBs) are crucial for life's chemistry. This study reveals no correlation between HB strength and directionality, challenging previous assumptions and offering new insights for molecular recognition and drug design.

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Area of Science:

  • Chemistry
  • Biophysics
  • Computational Chemistry

Background:

  • Hydrogen bonds (HBs) are fundamental to biological and chemical processes.
  • Existing methods like X-ray crystallography introduce biases, overemphasizing strong HBs and underrepresenting weak ones.
  • The interplay between HB strength and directionality remains incompletely understood due to environmental influences.

Purpose of the Study:

  • To rigorously quantify the strength and directionality of hydrogen bonds.
  • To investigate the relationship between hydrogen bond strength and directionality.
  • To provide an unbiased perspective on hydrogen bond characteristics free from solid-state packing forces.

Main Methods:

  • Performed 180,000 quantum mechanics (QM) calculations to determine interaction energies.
  • Covered a wide range of hydrogen bond donors and acceptors in defined geometries.
  • Analyzed both single-site and cooperative hydrogen bonding interactions.

Main Results:

  • Quantified hydrogen bond directionality and found no correlation with strength.
  • Identified strong hydrogen bond acceptors with isotropic interactions (e.g., dimethyl sulfoxide).
  • Observed weak hydrogen bond acceptors with sharp directional profiles (e.g., thioacetone).
  • Demonstrated that groups with similar directionality can have vastly different strengths.

Conclusions:

  • Hydrogen bond strength and directionality are independent properties that must be analyzed separately.
  • Findings offer a new framework for understanding hydrogen bond behavior.
  • Implications for molecular recognition, protein engineering, and drug design in chemical biology.