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Structure of the conjuncto boron hydride cluster [B 19 H 22] −. [7] Although relatively rare, several multi-cluster boranes have been characterized. For example, reaction of a borane cluster with B 2 H 6 (as a source of BH 3) can lead to the formation of a conjuncto-borane species in which borane cluster sub-units are joined by the sharing of ...
This family of boron hydrides includes mono- and dialkylboranes. The simplest members readily engage in redistribution reactions: 2 BH 2 (CH 3) → BH(CH 3) 2 + 0.5 B 2 H 6. With bulky substituents, primary and secondary boranes are more readily isolable and even useful. Examples include thexylborane and 9-BBN. Almost all primary and secondary ...
Group 13 hydrides are chemical compounds containing group 13-hydrogen bonds (elements of group 13: boron, aluminium, gallium, indium, thallium, and nihonium). [ 1 ] Trihydrides
Structure of a rare monomeric boron hydride, R = i-Pr. [4] The most-studied class of organoboron compounds has the formula BR n H 3−n. These compounds are catalysts, reagents, and synthetic intermediates. The trialkyl and triaryl derivatives feature a trigonal-planar boron center that is typically only weakly Lewis acidic.
Its structure is that of five atoms of boron arranged in a square pyramid. Each boron has a terminal hydride ligand and four hydrides span the edges of the base of the pyramid. It is classified as a nido cage. It was first prepared by Alfred Stock by pyrolysis of diborane at about 200 °C. [7]
Tetraborane (systematically named arachno-tetraborane(10)) was the first boron hydride compound to be discovered. [2] It was classified by Alfred Stock and Carl Massenez in 1912 and was first isolated by Stock. [3] It has a relatively low boiling point at 18 °C and is a gas at room temperature. Tetraborane gas is foul smelling and toxic.
It is commonly synthesized via the pyrolysis of smaller boron hydride clusters. For example, pyrolysis of B 2 H 6 or B 5 H 9 gives decaborane, with loss of H 2. [4] On a laboratory scale, sodium borohydride is treated with boron trifluoride to give NaB 11 H 14, which is acidified to release borane and hydrogen gas. [3]
The boron atom in BH 3 has 6 valence electrons. Consequently, it is a strong Lewis acid and reacts with any Lewis base ('L' in equation below) to form an adduct: [7] BH 3 + L → L—BH 3. in which the base donates its lone pair, forming a dative covalent bond. Such compounds are thermodynamically stable, but may be easily oxidised in air.