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Related Concept Videos

Exceptions to the Octet Rule02:55

Exceptions to the Octet Rule

Many covalent molecules have central atoms that do not have eight electrons in their Lewis structures. These molecules fall into three categories:
VSEPR Theory and the Effect of Lone Pairs04:01

VSEPR Theory and the Effect of Lone Pairs

Effect of Lone Pairs of Electrons on Molecule Geometry
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.
Resonance02:52

Resonance

The Lewis structure of a nitrite anion (NO2−) may actually be drawn in two different ways, distinguished by the locations of the N-O and N=O bonds.
Lewis Symbols and the Octet Rule02:36

Lewis Symbols and the Octet Rule

Chemical bonds are complex interactions between two or more atoms or ions, which reduce the potential energy of the molecule. Gilbert N. Lewis developed a model called the Lewis model that simplified the depiction of chemical bond formation and provided straightforward explanations for the chemical bonds seen in most common compounds.
Resonance and Hybrid Structures02:16

Resonance and Hybrid Structures

According to the theory of resonance, if two or more Lewis structures with the same arrangement of atoms can be written for a molecule, ion, or radical, the actual distribution of electrons is an average of that shown by the various Lewis structures.
Resonance Structures and Resonance Hybrids
The Lewis structure of a nitrite anion (NO2−) may actually be drawn in two different ways, distinguished by the locations of the N–O and N=O bonds.

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Characterizing Lewis Pairs Using Titration Coupled with In Situ Infrared Spectroscopy
07:49

Characterizing Lewis Pairs Using Titration Coupled with In Situ Infrared Spectroscopy

Published on: February 20, 2020

Carbon-based frustrated Lewis pairs.

Shabana Khan1, Manuel Alcarazo

  • 1Max Planck Institut für Kohlenforschung, Kaiser Wilhelm Platz 1, 45470, Mülheim an der Ruhr, Germany.

Topics in Current Chemistry
|November 10, 2012
PubMed
Summary

Frustrated Lewis pairs (FLPs) provide a versatile strategy for activating small molecules, including H2, CO2, and olefins. Recent advances focus on designing new carbon-based frustrated systems for enhanced reactivity.

Area of Science:

  • * Inorganic Chemistry
  • * Materials Science
  • * Organic Synthesis

Background:

  • * Frustrated Lewis pairs (FLPs) represent a novel class of Lewis acid-base pairs.
  • * FLPs exhibit unique reactivity due to the steric hindrance preventing classical adduct formation.
  • * Activation of small molecules is a key challenge in chemistry.

Purpose of the Study:

  • * To review recent advancements in the design of FLPs.
  • * To explore the reactivity of FLPs with various small molecules.
  • * To highlight the role of carbon-based partners in frustrated systems.

Main Methods:

  • * Literature review of recent studies on FLP design and reactivity.
  • * Analysis of experimental data on small molecule activation by FLPs.

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  • * Focus on systems incorporating at least one carbon-based component.

    • Main Results:

    • * FLPs effectively activate a range of small molecules: H2, CO2, acetylenes, disulfides, olefins, and nitrogen oxides.
    • * New FLP designs incorporating carbon-based partners show promising reactivity.
    • * Steric and electronic factors influencing FLP activity are elucidated.

    Conclusions:

    • * FLPs offer a powerful and adaptable platform for small molecule activation.
    • * Carbon-based frustrated systems are expanding the scope of FLP chemistry.
    • * Continued research promises further applications in catalysis and synthesis.