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Halogens03:01

Halogens

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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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Valence Bond Theory02:45

Valence Bond Theory

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Overview of Valence Bond Theory
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Valence Bond Theory02:42

Valence Bond Theory

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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...
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Electron Affinity03:07

Electron Affinity

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The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).
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Alkyl Halides02:45

Alkyl Halides

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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...
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Hydrogen Bonds01:04

Hydrogen Bonds

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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...
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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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Does fluorine participate in halogen bonding?

Kiamars Eskandari1, Mina Lesani

  • 1Department of Chemistry, Isfahan University of Technology, Isfahan, 84156-83111 (Iran). k.eskandari@cc.iut.ac.ir.

Chemistry (Weinheim an Der Bergstrasse, Germany)
|February 6, 2015
PubMed
Summary
This summary is machine-generated.

Fluorine bonds, distinct from halogen bonds, involve electron-withdrawing groups and spherical charge distribution around fluorine. These interactions, where fluorine acts as an electron sink, warrant a new classification.

Keywords:
ab initio calculationsbond theoryfluorinehalogen bondsquantum chemistry

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Area of Science:

  • * Quantum Chemistry
  • * Supramolecular Chemistry
  • * Chemical Bonding Theory

Background:

  • * Noncovalent interactions are crucial in chemistry and biology.
  • * Halogen bonding, a type of noncovalent interaction, involves electron-deficient regions on halogens.
  • * The role of fluorine in similar interactions has been less understood.

Purpose of the Study:

  • * To investigate the nature of noncovalent interactions involving fluorine (R-F) and electron donors.
  • * To differentiate these interactions from classical halogen bonds.
  • * To propose a new classification for these fluorine-mediated interactions.

Main Methods:

  • * Computational chemistry methods, including source function analysis and Interacting Quantum Atoms (IQA) analysis.
  • * Analysis of charge distribution, atomic multipoles, and atomic energies.
  • * Comparison with established halogen bond systems (e.g., involving Cl and Br).

Main Results:

  • * Fluorine in R-F molecules exhibits spherical electron distribution, unlike anisotropic halogens.
  • * Fluorine acts as an electron density sink, not a source, in F⋅⋅⋅N interactions.
  • * These interactions lack the characteristic σ-holes of halogen bonds and involve atomic dipole moments.

Conclusions:

  • * F⋅⋅⋅N interactions differ fundamentally from halogen bonds in electronic structure and interaction mechanisms.
  • * The attractive nature of halogen bonds is replaced by repulsion in F⋅⋅⋅N interactions.
  • * These interactions should be termed "fluorine bonds" to distinguish them from halogen bonds.