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Related Concept Videos

Hydrogen Bonds00:26

Hydrogen Bonds

135.0K
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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Hydrogen Bonds01:04

Hydrogen Bonds

15.3K
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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Hybridization of Atomic Orbitals II03:35

Hybridization of Atomic Orbitals II

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sp3d and sp3d 2 Hybridization
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Chemical Bonds02:40

Chemical Bonds

23.0K

Atoms participate in a chemical bond formation to acquire a completed valence-shell electron configuration similar to that of the noble gas nearest to it in atomic number. Ionic, covalent, and metallic bonds are some of the important types of chemical bonds. Bond energy and bond length determine the strength of a chemical bond.
Types of Chemical Bonds
An ionic bond is formed due to electrostatic attraction between cations and anions. Often, the ions are formed by the transfer of electrons...
23.0K
Hybridization of Atomic Orbitals I03:24

Hybridization of Atomic Orbitals I

68.0K
The mathematical expression known as the wave function, ψ, contains information about each orbital and the wavelike properties of electrons in an isolated atom. When atoms are bound together in a molecule, the wave functions combine to produce new mathematical descriptions that have different shapes. This process of combining the wave functions for atomic orbitals is called hybridization and is mathematically accomplished by the linear combination of atomic orbitals. The new orbitals that...
68.0K
Intermolecular Forces03:13

Intermolecular Forces

72.9K
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...
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In Situ High Pressure Hydrogen Tribological Testing of Common Polymer Materials Used in the Hydrogen Delivery Infrastructure
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In Situ High Pressure Hydrogen Tribological Testing of Common Polymer Materials Used in the Hydrogen Delivery Infrastructure

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Beryllium and strong hydrogen bonds.

T Mark McCleskey1, Brian L Scott

  • 1Los Alamos National Laboratory, Los Alamos, New Mexico 87545, USA. tmark@lanl.gov

Journal of Occupational and Environmental Hygiene
|November 7, 2009
PubMed
Summary
This summary is machine-generated.

Beryllium (Be) can replace hydrogen ions (H+) in strong hydrogen bonds, forming stable tetrahedral complexes. This discovery enables new beryllium-binding ligands for imaging and therapeutic applications.

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Area of Science:

  • Biochemistry
  • Inorganic Chemistry
  • Computational Chemistry

Background:

  • Strong hydrogen bonds play crucial roles in biological systems.
  • Beryllium's interaction with biological molecules is not fully understood.
  • Proton transfer mechanisms are key to understanding chemical reactions.

Purpose of the Study:

  • To compare beryllium's binding affinity to hydrogen ions in strong hydrogen bonds.
  • To investigate the thermodynamic and kinetic factors governing beryllium binding.
  • To explore the design of novel beryllium-binding ligands for biomedical applications.

Main Methods:

  • Computational modeling to compare Be and H+ interactions.
  • Analysis of O-X distances and binding site geometry.
  • Thermodynamic and kinetic barrier assessments for proton transfer.
  • Design and evaluation of new beryllium-chelating ligands.

Main Results:

  • Beryllium thermodynamically prefers to displace H+ in strong hydrogen bonds, forming tetrahedral structures.
  • Strong hydrogen bonds offer optimal O-X distances (2.4-2.8 Å) for beryllium chelation.
  • Low energy barriers facilitate rapid beryllium binding via proton transfer.
  • Binding strength correlates with the basicity (pKa) of the oxygen sites.
  • Designed ligands effectively solubilize beryllium and enable fluorescent imaging.

Conclusions:

  • Beryllium's unique binding properties in strong hydrogen bonds offer new avenues for its application.
  • The developed ligands demonstrate potential for beryllium detection and chelation in biological systems.
  • Understanding beryllium-protein interactions, like with transferrin, is crucial for its biological role.