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Related Concept Videos

Hydrogen Bonds01:04

Hydrogen Bonds

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...
Hydrogen Bonds00:26

Hydrogen Bonds

Hydrogen BondsHydrogen 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...
Valence Bond Theory02:45

Valence Bond Theory

Overview of Valence Bond Theory
Valence Bond Theory02:42

Valence Bond Theory

Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
Introduction to Chemical Bonds01:01

Introduction to Chemical Bonds

Chemical Bonds
The electrons of the outermost energy level determine the energetic stability of the atom and its tendency to form chemical bonds with other atoms. The innermost electron shell has a maximum capacity of two electrons, but the next two electron shells can each have a maximum of eight electrons. This is known as the octet rule, which states that, with the exception of the innermost shell, atoms are most stable energetically when they have eight electrons in their valence shell, the...
Covalent Bonding and Lewis Structures02:46

Covalent Bonding and Lewis Structures

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.

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From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding
06:44

From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding

Published on: March 24, 2018

Mixed valency across hydrogen bonds.

John C Goeltz1, Clifford P Kubiak

  • 1Department of Chemistry and Biochemistry, University of California-San Diego, 9500 Gilman Drive, M/C 0358, La Jolla, California 92093-0358, USA.

Journal of the American Chemical Society
|November 20, 2010
PubMed
Summary
This summary is machine-generated.

A reduced ruthenium cluster forms a dimer stabilized by hydrogen bonds and mixed valency. This electronic effect, observed via spectroscopy, significantly lowers the ground state energy of the complex.

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Area of Science:

  • Inorganic Chemistry
  • Materials Science
  • Spectroscopy

Background:

  • Oxo-centered triruthenium clusters are versatile coordination compounds.
  • Mixed valence complexes exhibit unique electronic properties.
  • Hydrogen bonding plays a crucial role in molecular assembly and stabilization.

Purpose of the Study:

  • To investigate the dimerization of a specific triruthenium cluster upon reduction.
  • To characterize the electronic structure and stability of the resulting dimer.
  • To elucidate the interplay between mixed valency, hydrogen bonding, and electronic coupling.

Main Methods:

  • Synthesis and partial reduction of an oxo-centered triruthenium cluster with pyridine-4-carboxylic acid ligand.
  • Infrared (IR) spectroscopy to probe charge localization.
  • UV/vis/NIR spectroscopy to determine electronic stabilization energies.

Main Results:

  • Formation of a mixed valence monoanionic dicarboxylic acid dimer upon partial reduction.
  • Dimerization was not observed in dimethyl sulfoxide (DMSO) or with the deprotonated carboxylate.
  • Spectroscopic data indicated charge localization and significant ground state stabilization (approx. 7 kcal/mol) due to mixed valency across hydrogen bonds.

Conclusions:

  • The mixed valence dimer is a charge-localized species.
  • A substantial stabilization energy arises from the synergistic effects of hydrogen bonding and electronic coupling.
  • This study highlights the importance of ligand choice and protonation state in controlling cluster assembly and electronic properties.