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Related Concept Videos

Hydrogen Bonds01:04

Hydrogen Bonds

11.5K
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...
11.5K
Hydrogen Bonds00:26

Hydrogen Bonds

128.2K
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....
128.2K
Halogens03:01

Halogens

21.7K
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. 
21.7K
Covalent Bonding and Lewis Structures02:46

Covalent Bonding and Lewis Structures

57.2K
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.
57.2K
Valence Bond Theory02:45

Valence Bond Theory

41.6K
Overview of Valence Bond Theory
41.6K
Valence Bond Theory02:42

Valence Bond Theory

10.0K
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...
10.0K

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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 Bonding: An Odd Chemistry?

Lotta Turunen1, Jørn H Hansen2, Máté Erdélyi1

  • 1Department of Chemistry - BMC, Uppsala University, SE 751 23, Uppsala, Sweden.

Chemical Record (New York, N.Y.)
|May 3, 2021
PubMed
Summary
This summary is machine-generated.

Odd Hassel pioneered halogen bonding research, observing unique atomic interactions. His foundational work, initially overlooked, is now crucial in modern chemistry and molecular interactions.

Keywords:
Odd HasselX-raycharge-transferhalogen bondhalonium

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Area of Science:

  • Chemistry
  • Crystallography
  • Supramolecular Chemistry

Background:

  • Halogen bonding is a significant area of chemical research.
  • Odd Hassel's early crystallographic observations laid the groundwork for understanding these interactions.
  • Hassel's contributions were foundational but historically underappreciated.

Purpose of the Study:

  • To revive the legacy of Odd Hassel.
  • To highlight the impact of his pioneering discoveries in halogen bonding.
  • To underscore the importance of his work in contemporary chemistry.

Main Methods:

  • Crystallographic analysis of interatomic distances.
  • Interpretation of charge-transfer interactions.
  • Historical review of scientific contributions.

Main Results:

  • Observation of interatomic distances shorter than van der Waals radii.
  • Identification of charge-transfer as the mechanism in halogen bonding.
  • Establishment of halogen bonding as a key concept in chemistry.

Conclusions:

  • Odd Hassel's work was ground-breaking and essential for the development of halogen bonding.
  • His research, though initially unrecognized, is now widely applied.
  • There is a need for greater appreciation of Hassel's scientific legacy.