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The adduct with diethyl ether, boron trifluoride diethyl etherate, or just boron trifluoride etherate, (BF 3 ·O(CH 2 CH 3) 2) is a conveniently handled liquid and consequently is widely encountered as a laboratory source of BF 3. [16] Another common adduct is the adduct with dimethyl sulfide (BF 3 ·S(CH 3) 2), which can be handled as a neat ...
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 trihalides adopt a planar trigonal structure. These compounds are Lewis acids in that they readily form adducts with electron-pair donors, which are called Lewis bases. For example, fluoride (F −) and boron trifluoride (BF 3) combined to give the tetrafluoroborate anion, BF 4 −. Boron trifluoride is used in the petrochemical industry as ...
The most common Lewis bases are anions. The strength of Lewis basicity correlates with the pK a of the parent acid: acids with high pK a 's give good Lewis bases. As usual, a weaker acid has a stronger conjugate base. Examples of Lewis bases based on the general definition of electron pair donor include: simple anions, such as H − and F −
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]
Boron trifluoride, BF 3, a pungent colourless toxic gas; Bromotrifluoromethane, CBrF 3, (carbon monobromide trifluoride) Bromine trifluoride, BrF 3;
For example, boron trifluoride (BF 3) and ammonia (NH 3) form an adduct or coordination complex F 3 B←NH 3 with a B–N bond in which a lone pair of electrons on N is shared with an empty atomic orbital on B. BF 3 with an empty orbital is described as an electron pair acceptor or Lewis acid, while NH 3 with a lone pair that can be shared is ...
As discussed above (see § Structure), BF has a much lower bond order, so that the valence shell around boron is unfilled. Consequently, BF as a ligand is much more Lewis acidic; it tends to form higher-order bonds to metal centers, and can also bridge between two or three metal atoms (μ 2 and μ 3). [11]