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The central atom of ammonia is nitrogen and it has 3 bonding pairs and a lone pair around, hence it undergoes sp3 hybridization. The central atom of boron trifluoride is the boron atom, and around it has only three bonding pairs. So it hybridizes as sp2.
BF3 is the compound Boron Triflouride
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The central atom B has less than 8 electrons in the valence shell. BF3 has a tendency to accept electron pair.
Boron trifluoride is BF3. So each mole of BF3 contains 1 moles of boron (B) and 3 moles of fluorine (F). Thus, 3 moles of BF3 contains NINE moles of fluorine.
electron back bonding in bf3 due to vacant p orbital so stable and does not react.
Increasing order of Lewis acidity BH3>BBR3>BCl3>BF3
There are three bonding pairs of electrons in BF3. There are 0 nonbinding pairs, but BF3 can accept two more electrons to give it a complete octet
oh yeah
) Boron atom, in BX3, has six electrons in the outermost orbit and thus it can accept a pair of electrons form a donor molecule like NH3 to complete its octet. Hence boron halides act as very efficient Lewis acids. The relative Lewis acid character of boron trihalides is found to obey the order ; BI3>BBr3>BCl3>BF3.However, the above order is just the reverse of normally expected order on the basis relative electronegativities of the halogens. Fluorine, being the most electronegative, should create the greatest electron deficiency on boron and thus B in BF3 should accept electron pair from a donor very rapidly than in other boron trihalides. But this is not true.This anomalous behavior has been explained on the basis of the relative tendency of the halogen atom to back-donate its unutilised electrons to the vacant p orbitals of boron atom. In boron trifluoride, each fluorine has completely filled unutilised 2p orbitals while boron has a vacant 2p orbital. Now since both of these orbitals belong to same energy level (2p) they can overlap effectively as a result of which fluorine electrons are transferred into the vacant 2p orbital of boron resulting in the formation of an additional pπ-pπ bond. This type of bond formation is known as back bonding or back donation. Thus the B- F bond has some double bond character. Back bonding may take place between boron and of the three fluorine atoms and thus boron trifluoride is regarded as a resonance hybrid of some structures.Resonance in boron trifluoride is also evidenced by the fact that the three boron-fluorine bonds are indentical and are shorter than the usual single boron-fluorine bond As a result of back bonding, the electron deficiency of boron is reduced and hence Lewis acid nature is decreased. The tendency for the formation of back bonding (pπ-pπ bond) is maximum in BF3 and decreases very rapidly from BF3 to BI3This is probably due to the fact that overlapping of the vacant 2p orbitals of boron cannot take place easily with the p-orbitals of high energy levels (3p in Cl, 4p in Br and 5p in iodine). Thus BI3Br3 and BCl3are stronger Lewis acids than the BF3.
BF3 is Non-Polar :)
The prefix for "bf3" is "boron trifluoride."
BF3 because i have both and BF3 is very realiastic, has many interactive objects like vehicles, the online is very nice. MW3 is almost cartoony compared to BF3 and MW3 is just like the other COD's and gets boring. its predictable. I like BF3 way more. :)
The central atom of ammonia is nitrogen and it has 3 bonding pairs and a lone pair around, hence it undergoes sp3 hybridization. The central atom of boron trifluoride is the boron atom, and around it has only three bonding pairs. So it hybridizes as sp2.
bf3 all the way Jokes Mw3 is way better
Every time you turn on bf3 it will show up if you denied it.
BF3. It exists as a non-octet molecule with 3 single covalent bonds between each Boron and Fluorine atom. This satisfies the outer shells of each Fluorine atom but Boron exists with only 3 pairs of electrons - 6 in total. This forms a trigonal planar shape as there are no non-bonding electron pairs, rather than pyramidal, such is the case with a compound like ammonia (NH3).