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Molar mass: 117.17 g/mol Appearance Colorless gas, fumes in air Density: 1.326 g/cm 3: ... Boron trichloride is the inorganic compound with the formula BCl 3.
It can also be formed by the electrical discharge procedure of boron trichloride at low temperatures: [1] [3] BCl 3 → BCl 2 + Cl Cl + Hg → HgCl or HgCl 2 2 BCl 2 → B 2 Cl 4. The most efficient synthesis technique uses no dechlorinating metal, instead passing radio-frequency AC current through gaseous boron trichloride. [4]
As a pyrophoric substance, diborane reacts exothermically with oxygen to form boron trioxide and water: 2 B 2 H 6 + 6 O 2 → 2 B 2 O 3 + 6 H 2 O (ΔH r = −2035 kJ/mol = −73.47 kJ/g) Diborane reacts violently with water to form hydrogen and boric acid: B 2 H 6 + 6 H 2 O → 2 B(OH) 3 + 6 H 2 (ΔH r = −466 kJ/mol = −16.82 kJ/g) Diborane ...
Boron trifluoride is the inorganic compound with the formula BF 3. This pungent, colourless, and toxic gas forms white fumes in moist air. It is a useful Lewis acid and a versatile building block for other boron compounds.
Other methods to form methyldiboranes include treating hydrogen with trimethylborane between 80 and 200 °C under pressure, or treating a metal borohydride with trimethylborane in the presence of hydrogen chloride, aluminium chloride or boron trichloride. If the borohydride is sodium borohydride, then methane is a side product. If the metal is ...
It can be purified by bulb to bulb vacuum transfer. Although a structure of BMS has not been determined crystallographically, (pentafluorophenyl)-borane dimethylsulfide (C 6 F 5 BH 2 ·S(CH 3) 2), has been examined by X-ray crystallography. [4] The boron atom adopts a tetrahedral molecular geometry.
Chlorine trifluoride is an interhalogen compound with the formula ClF 3.It is a colorless, poisonous, corrosive, and extremely reactive gas that condenses to a pale-greenish yellow liquid, the form in which it is most often sold (pressurized at room temperature).
The reaction of boron trichloride with alcohols was reported in 1931, and was used to prepare dimethoxyboron chloride, B(OCH 3) 2 Cl. [3] Egon Wiberg and Wilhelm Ruschmann used it to prepare tetrahydroxydiboron by first introducing the boron–boron bond by reduction with sodium and then hydrolysing the resulting tetramethoxydiboron, B 2 (OCH 3) 4, to produce what they termed sub-boric acid. [4]