In chemistry, a dihydrogen bond is a kind of hydrogen bond, an interaction between a metal hydride bond and an OH or NH group or other proton donor. With a van der Waals radius of 1.2 Å, hydrogen atoms do not usually approach other hydrogen atoms closer than 2.4 Å.

Jun 10, 2016 · The dihydrogen bond—an interaction between a transition-metal or main-group hydride (M—H) and a protic hydrogen moiety (H—X)—is arguably the most intriguing type of hydrogen bond. It was discovered in the mid-1990s and has been intensively explored since then.

In chemistry, a hydrogen bond (H-bond) is a specific type of molecular interaction that exhibits partial covalent character and cannot be described as a purely electrostatic force.

Dihydrogen complexes can “tautomerize” to hydride \(\ce{(H)2}\) isomers through cleavage of the \(\ce{H–H}\) bond to the metal (this is an oxidative addition reaction, as discussed in the chapter on organometallic reactions).

Dec 11, 1998 · Hydrogen bonds are responsible for the strength of materials, such as wood or a spider's web, and molecular binding, such as base pairing in DNA. Recently, however, a whole new world of hydrogen bonding has come to light, in which metals and hydrides can form unusual hydrogen bonds.

In chemistry, a dihydrogen bond is a kind of hydrogen bond, an interaction between a metal hydride bond and an OH or NH group or another proton donor. The first example of this phenomenon is credited to Brown and Heseltine. They observed intense absorption bands in the IR bands at 3300 and 3210 cm-1 for a solution of (CH 3) 2 NHBH 3. The higher ...

Dihydrogen is the homonuclear diatomic molecule formed from two hydrogen atoms. This molecule features a covalent bond between two hydrogen atoms, satisfying each of their required duet configurations.

Jun 8, 2007 · This definitive reference consolidates current knowledge on dihydrogen bonding, emphasizing its role in organizing interactions in different chemical reactions and molecular aggregations. After an overview, it analyzes the differences between dihydrogen bonds, classical hydrogen bonds, and covalent bonds.

Hydrogen bonding principles are at the core of supramolecular design. This overview features a discussion relating molecular structure to hydrogen bond strengths, highlighting the following electronic effects on hydrogen bonding: electronegativity, steric effects, electrostatic effects, π-conjugation, and network cooperativity.

Ancillary ligands play an important role in determining the energetic balance between the dihydrogen and dihydride complexes. For instance, replacement of the 3 COs in the Mo version of Kubas’ original complex with PR3s furnishes the dihydride as the energetically favored complex.