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Related Concept Videos

Hydrogen Bonds01:04

Hydrogen Bonds

16.5K
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...
16.5K
Hydrogen Bonds00:26

Hydrogen Bonds

136.6K
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....
136.6K
Halogenation of Alkenes02:46

Halogenation of Alkenes

21.5K
Halogenation is the addition of chlorine or bromine across the double bond in an alkene to yield a vicinal dihalide. The reaction occurs in the presence of inert and non-nucleophilic solvents, such as methylene chloride, chloroform, or carbon tetrachloride.
Consider the bromination of cyclopentene. Molecular bromine is polarized in the proximity of the π electrons of cyclopentene. An electrophilic bromine atom adds across the double bond, forming a cyclic bromonium ion intermediate.
21.5K
Halogens03:01

Halogens

24.3K
Group 17 elements, known as halogens, are nonmetals. At room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine a solid. Astatine is a highly unstable radioactive element, so currently, most of its properties are unknown due to its short half-life. Tennessine is a synthetic element also predicted to be in this group. 
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VSEPR Theory and the Effect of Lone Pairs04:01

VSEPR Theory and the Effect of Lone Pairs

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Effect of Lone Pairs of Electrons on Molecule Geometry
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Hybridization of Atomic Orbitals II03:35

Hybridization of Atomic Orbitals II

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sp3d and sp3d 2 Hybridization
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From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding
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From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding

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Double Hole-Lump Interaction between Halogen Atoms.

Darío J R Duarte1, Nélida M Peruchena1, Ibon Alkorta2

  • 1†Laboratorio de Estructura Molecular y Propiedades, Área de Química Física-Departamento de Química, Facultad de Ciencias Exactas y Naturales y Agrimensura, Universidad Nacional del Nordeste, Avenida Libertad 5460, 3400 Corrientes, Argentina.

The Journal of Physical Chemistry. A
|April 1, 2015
PubMed
Summary
This summary is machine-generated.

This study reveals that unusual halogen-halogen contacts are stabilized by electrostatic interactions and charge transfer, similar to conventional halogen bonds. These interactions significantly increase electron density between halogen atoms, influencing complex geometry.

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Area of Science:

  • Computational Chemistry
  • Quantum Chemistry
  • Chemical Physics

Background:

  • Halogen bonding (X···Y) is a well-established non-covalent interaction.
  • Unusual halogen-halogen contacts (X···X) present unique bonding characteristics.
  • Understanding these interactions is crucial for predicting molecular assembly and reactivity.

Purpose of the Study:

  • To theoretically investigate the nature of unusual halogen-halogen contacts in R-X···X-R complexes.
  • To characterize the electronic and geometric factors governing X···X interactions.
  • To compare the stabilizing forces in X···X contacts with conventional halogen bonds.

Main Methods:

  • Theoretical study employing Atoms in Molecules (AIM) analysis.
  • Natural Bond Orbital (NBO) analysis to probe charge transfer.
  • Molecular Electrostatic Potential (MEP) analysis to evaluate electrostatic contributions.

Main Results:

  • X···X interactions lead to increased electron charge density in the inter-halogen bonding region.
  • Complex stability and geometry are primarily governed by electrostatic interactions (lump-to-hole) and charge transfers (lone pair to antibonding orbital).
  • Dispersion forces are the dominant attractive term for most studied complexes.

Conclusions:

  • Electrostatic interactions and charge transfer play a significant role in stabilizing unusual X···X contacts.
  • These findings highlight similarities between X···X contacts and conventional halogen bonds.
  • The study provides insights into the fundamental nature of non-covalent interactions involving halogens.