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Related Concept Videos

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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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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Overview of Valence Bond Theory
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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...
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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.
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Catalytic Reactions at Amine-Stabilized and Ligand-Free Platinum Nanoparticles Supported on Titania During Hydrogenation of Alkenes and Aldehydes
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n→π* Interactions Are Competitive with Hydrogen Bonds.

Robert W Newberry1, Samuel J Orke1, Ronald T Raines1

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The study reveals that enhancing n→π* interactions in carbonyl groups weakens their hydrogen bonding capacity. This finding impacts understanding of molecular interactions and chemical behavior in β-keto amides.

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Area of Science:

  • Organic Chemistry
  • Supramolecular Chemistry
  • Chemical Physics

Background:

  • Carbonyl groups are crucial functional groups involved in various chemical interactions.
  • Hydrogen bonds and n→π* interactions are known to influence molecular structure and reactivity.
  • The interplay between these two specific interactions at the carbonyl group requires further investigation.

Purpose of the Study:

  • To investigate the effect of enhanced n→π* interactions on the hydrogen-bonding capacity of carbonyl groups.
  • To explore the consequences of this interplay on the tautomerization of β-keto amides.
  • To elucidate the relationship between n→π* interactions and hydrogen bond strength in amides.

Main Methods:

  • Computational chemistry methods were employed to model and analyze the interactions.
  • Spectroscopic techniques were used to probe hydrogen bonding and tautomeric equilibria.
  • Synthesis of specifically designed β-keto amide derivatives to study n→π* interaction strength.

Main Results:

  • Enhancement of the amidic n→π* interaction was observed to decrease the hydrogen-bonding ability of the amide carbonyl.
  • A reduction in the capacity of β-keto amides to tautomerize to their enol forms was demonstrated.
  • This indicates a direct correlation between the strength of n→π* interactions and the hydrogen-bonding strength of the carbonyl group.

Conclusions:

  • n→π* interactions significantly modulate the hydrogen-bonding properties of carbonyl groups.
  • The findings provide new insights into the factors governing tautomeric equilibria in β-keto amides.
  • Understanding this interplay is crucial for designing molecules with specific chemical and physical properties.