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Related Concept Videos

Carbocations02:10

Carbocations

Carbocations are one of the reaction intermediates formed during several nucleophilic substitutions or elimination reactions. A carbocation is an electron-deficient species with the central carbon atom having six electrons and three bonded atoms. The central carbon in a carbocation is sp2 hybridized with trigonal planar geometry. It has an empty p orbital perpendicular to the plane of the structure that can accept electrons. Thus, carbocations act as strong electrophiles and may react with any...
ortho–para-Directing Deactivators: Halogens01:24

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Halogens are ortho–para directors. They are more electronegative than carbon. Therefore, as ring substituents, they can withdraw electrons through the inductive effect and deactivate the aromatic ring towards electrophilic substitution. Halogens also have an electron-donating resonance effect on the ring, which influences the orientation of the incoming electrophile. If an electrophile attacks at the ortho or the para position, the halogen donates electrons and stabilizes the intermediate...
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Valence Bond Theory

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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...
Hybridization of Atomic Orbitals I03:24

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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...

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Updated: Jun 26, 2026

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

Strong interactions between carbones and halogen atomic centers.

Shunhua Li1, Hangyu Zhou1, Qingzhong Li1

  • 1The Laboratory of Theoretical and Computational Chemistry, School of Chemistry and Chemical Engineering, Yantai University Yantai 264005 P. R. China lqz@ytu.edu.cn.

Chemical Science
|June 25, 2026
PubMed
Summary
This summary is machine-generated.

Carbone compounds act as strong electron donors, forming potent bonds with halogen Lewis acids. Binding strength varies, with some interactions showing reversed halogen dependence compared to typical halogen bonds.

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Last Updated: Jun 26, 2026

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Area of Science:

  • Quantum chemistry
  • Inorganic chemistry

Background:

  • Carbone compounds feature a divalent carbon atom with two lone pairs.
  • These compounds exhibit unique electronic properties due to their electronic structure.

Purpose of the Study:

  • To investigate the electron-donating capabilities of carbone centers.
  • To analyze the binding interactions between carbone compounds and halogen-containing Lewis acids.

Main Methods:

  • Density Functional Theory (DFT) calculations were employed.
  • 29 different halogen-containing Lewis acids were paired with carbone compounds.

Main Results:

  • Strong binding interactions were observed, comparable to ammonia Lewis bases.
  • Binding energies ranged significantly, up to 40 kcal mol⁻¹.
  • Weak interactions mirrored conventional halogen bonds (Cl < Br < I), while strong interactions showed reversed halogen dependence (Cl > Br > I) with significant halogen atom transfer.

Conclusions:

  • Carbone centers are effective electron donors, forming strong dative bonds.
  • The nature of the Lewis acid dictates the binding strength and halogen atom transfer.
  • Reversed halogen dependence in strong interactions highlights unique bonding characteristics.