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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. [22] 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] −.
Pure H[BF 4] has not been described. The same holds true for the superacids that are known by the simplified formulas H[PF 6] and H[SbF 6]. [4] [5] However, a solution of BF 3 in HF is highly acidic, having an approximate speciation of [H 2 F] + [BF 4] − (fluoronium tetrafluoroborate) and a Hammett acidity function of −16.6 at 7 mol % BF 3, easily qualifying as a superacid. [6]
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.
The mean oxidation number for the boron atoms is then simply the ratio of hydrogen to boron in the molecule. For example, in diborane B 2 H 6, the boron oxidation state is +3, but in decaborane B 10 H 14, it is 7 / 5 or +1.4. In these compounds the oxidation state of boron is often not a whole number.
Structure of boron trifluoride, an example of a molecule with trigonal planar geometry.. In chemistry, trigonal planar is a molecular geometry model with one atom at the center and three atoms at the corners of an equilateral triangle, called peripheral atoms, all in one plane. [1]
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For many substances, the formation reaction may be considered as the sum of a number of simpler reactions, either real or fictitious. The enthalpy of reaction can then be analyzed by applying Hess' law, which states that the sum of the enthalpy changes for a number of individual reaction steps equals the enthalpy change of the overall reaction.