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Related Concept Videos

Hydrogen Bonds01:04

Hydrogen Bonds

16.6K
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...
16.6K
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
Alkyl Halides02:45

Alkyl Halides

22.9K
Structural Properties
Alkyl halides are halogen-substituted alkanes wherein one or more hydrogen atoms of an alkane is replaced by a halogen atom such as fluorine, chlorine, bromine, or iodine. The carbon atom in an alkyl halide is bonded to the halogen atom, which is sp3-hybridized and exhibits a tetrahedral shape.
Unlike alkyl halides, compounds in which a halogen atom is bonded to an sp2 -hybridized carbon atom of a carbon-carbon double bond (C=C) are called vinyl halides. Whereas aryl...
22.9K
Valence Bond Theory02:45

Valence Bond Theory

52.0K
Overview of Valence Bond Theory
52.0K
Valence Bond Theory02:42

Valence Bond Theory

11.9K
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...
11.9K
Halogens03:01

Halogens

24.4K
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. 
24.4K

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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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Halogen bond: a long overlooked interaction.

Gabriella Cavallo1, Pierangelo Metrangolo, Tullio Pilati

  • 1Laboratory of Nanostructured Fluorinated Materials (NFMLab), Department of Chemistry, Materials, and Chemical Engineering "Giulio Natta", Politecnico di Milano, Via L. Mancinelli 7, 20131, Milano, Italy, gabriella.cavallo@polimi.it.

Topics in Current Chemistry
|December 16, 2014
PubMed
Summary
This summary is machine-generated.

Halogen atoms can act as electron donors or acceptors. The halogen bond (XB) specifically describes interactions where the halogen atom functions as an electrophile, a concept with a developing history.

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Area of Science:

  • Chemistry
  • Crystallography
  • Supramolecular Chemistry

Background:

  • Halogen atoms are typically viewed as electron-rich due to high electronegativity.
  • Covalently bound halogens exhibit anisotropic electron density distribution.
  • This anisotropy creates both electron-rich and electron-poor regions on the halogen atom.

Purpose of the Study:

  • To explore the dual role of halogen atoms in chemical interactions.
  • To define and trace the historical development of the halogen bond (XB).
  • To provide a comprehensive categorization of interactions involving electrophilic halogen atoms.

Main Methods:

  • Literature review of experimental and theoretical contributions.
  • Analysis of the historical development of the halogen bond concept.
  • Recollection of key papers in the field.

Main Results:

  • Halogen atoms possess distinct regions of electron density, enabling diverse interactions.
  • The electron-poor region allows halogens to act as electrophilic sites.
  • The concept of the halogen bond (XB) has evolved to encompass these electrophilic interactions.

Conclusions:

  • Halogen atoms exhibit versatile interaction capabilities beyond acting as electron donors.
  • The halogen bond is a significant attractive interaction where halogens act as electrophiles.
  • A unified understanding of halogen electrophilicity in interactions has emerged.