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Related Concept Videos

Lewis Acids and Bases02:33

Lewis Acids and Bases

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In 1923, G. N. Lewis proposed a generalized definition of acid-base behavior in which acids and bases are identified by their ability to accept or to donate a pair of electrons and form a coordinate covalent bond.
A coordinate covalent bond (or dative bond) occurs when one of the atoms in the bond provides both bonding electrons. For example, a coordinate covalent bond occurs when a water molecule combines with a hydrogen ion to form a hydronium ion. A coordinate covalent bond also results when...
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Lewis Acids and Bases02:16

Lewis Acids and Bases

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This lesson delves into Lewis acids and bases in the context of the octet rule for electron-deficient compounds. Here, the concept is discussed, emphasizing the group 13 elements like boron or aluminium. Since group 13 elements possess three valence electrons, they form trivalent compounds with a sextet of electrons and a vacant orbital for the central atom. Consequently, these electron-deficient compounds accept electrons from other species to complete their octet in a chemical reaction. They...
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Brønsted-Lowry acid-base chemistry is the transfer of protons; thus, logic suggests a relation between the relative strengths of conjugate acid-base pairs. The strength of an acid or base is quantified in its ionization constant, Ka or Kb, which represents the extent of the acid or base ionization reaction. For the conjugate acid-base pair HA / A−, the ionization equilibrium equations and ionization constant expressions are
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DNA Base Pairing

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Erwin Chargaff’s rules on DNA equivalence paved the way for the discovery of base pairing in DNA. Chargaff’s rules state that in a double-stranded DNA molecule,
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Covalent Bonding and Lewis Structures02:46

Covalent Bonding and Lewis Structures

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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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Characterizing Lewis Pairs Using Titration Coupled with In Situ Infrared Spectroscopy
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Characterizing Lewis Pairs Using Titration Coupled with In Situ Infrared Spectroscopy

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Radicals derived from Lewis acid/base pairs.

Liu Leo Liu1, Douglas W Stephan

  • 1Department of Chemistry, University of Toronto, 80 St. George St., Toronto, Ontario M5S3H6, Canada. dstephan@chem.utoronto.ca.

Chemical Society Reviews
|February 7, 2019
PubMed
Summary
This summary is machine-generated.

This review explores novel methods for stabilizing main group radicals using donor-acceptor molecules. It examines reactions involving Lewis acid-base adducts and frustrated Lewis pairs for radical stabilization.

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Area of Science:

  • Chemistry
  • Organic Chemistry
  • Main Group Chemistry

Background:

  • Conventional stabilization of main group radicals often relies on Lewis acids or bases.
  • New strategies are needed to expand the accessibility and utility of main group radicals.

Purpose of the Study:

  • To review emerging strategies for stabilizing main group radicals.
  • To highlight the role of donor-acceptor molecule combinations in radical stabilization.
  • To discuss the reactivity of these novel radical systems.

Main Methods:

  • Literature review of recent advancements in main group radical chemistry.
  • Analysis of reactions involving Lewis acid-base adducts.
  • Examination of frustrated Lewis pair systems for radical generation and stabilization.

Main Results:

  • Donor-acceptor combinations offer a promising new route to main group radicals.
  • Both classical Lewis acid-base adducts and frustrated Lewis pairs can be employed.
  • Understanding the reactivity of these systems is crucial for synthetic applications.

Conclusions:

  • Stabilization of main group radicals can be achieved through innovative donor-acceptor strategies.
  • Frustrated Lewis pairs represent a powerful tool in this area.
  • These advancements open new possibilities in main group chemistry and catalysis.