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The reaction commences with the formation of the aquo adduct, H 2 O−BF 3, which then loses HF that gives fluoroboric acid with boron trifluoride. [21] 4 BF 3 + 3 H 2 O → 3 H[BF 4] + B(OH) 3. The heavier trihalides do not undergo analogous reactions, possibly due to the lower stability of the tetrahedral ions [BCl 4] − and [BBr 4] −.
Fluoroboric acid or tetrafluoroboric acid (archaically, fluoboric acid) is an inorganic compound with the simplified chemical formula H +[B F 4]−. Solvent-free tetrafluoroboric acid (H [BF4]) has not been reported. The term "fluoroboric acid" usually refers to a range of compounds including hydronium tetrafluoroborate ([H3O]+[BF4]−), which ...
Boron trifluoride etherate, strictly boron trifluoride diethyl etherate, or boron trifluoride–ether complex, is the chemical compound with the formula BF 3 O (C 2 H 5) 2, often abbreviated BF 3 OEt 2. It is a colorless liquid, although older samples can appear brown. The compound is used as a source of boron trifluoride in many chemical ...
Boranes are chemical compounds of boron and hydrogen, with the generic formula of B x H y. These compounds do not occur in nature. Many of the boranes readily oxidise on contact with air, some violently. The parent member BH 3 is called borane, but it is known only in the gaseous state, and dimerises to form diborane, B 2 H 6.
Lithium tetrafluoroborate is an inorganic compound with the formula Li BF 4. It is a white crystalline powder. It has been extensively tested for use in commercial secondary batteries, an application that exploits its high solubility in nonpolar solvents. [2]
Organotrifluoroborate. Organotrifluoroborates are organoboron compounds that contain an anion with the general formula [RBF 3] −. They can be thought of as protected boronic acids, or as adducts of carbanions and boron trifluoride. Organotrifluoroborates are tolerant of air and moisture [1] and are easy to handle and purify. [2]
Phosphorus trifluoride (formula P F 3), is a colorless and odorless gas.It is highly toxic and reacts slowly with water. Its main use is as a ligand in metal complexes.As a ligand, it parallels carbon monoxide in metal carbonyls, [1] and indeed its toxicity is due to its binding with the iron in blood hemoglobin in a similar way to carbon monoxide.
The standard Gibbs free energy of formation (G f °) of a compound is the change of Gibbs free energy that accompanies the formation of 1 mole of a substance in its standard state from its constituent elements in their standard states (the most stable form of the element at 1 bar of pressure and the specified temperature, usually 298.15 K or 25 °C).