there is only 1 lone pair present in BrF5
there are 7 electrons in Br valence shell from which 5 electrons went to make bond with F, while the remaining two makes a lone pair.
and thus anly 1 lone pair exist in BrF5
There will be two lone (unbonded) pairs of electrons. This will result in a "t-shaped," weakly polar molecule. The central bromine atom will experience an expanded valence level of electrons, due to its ability to access the 4d energy sublevel. This particle-level property is called hypervalency.
There are 2 lone pairs
2 :)
2
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.
angular with 109.5 degree
one can find the bond pairs by finding the oxidation state on the central atom
4
0
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.
It is five because there is a total of five electron pairs around the bromine atom.
The lone pairs are on the bromine atom- 3 in all.
Every pair of electrons on the central atom (S) of the Lewis structure of SF6 is shared by an F atom, so therefore there are no lone pairs on the central atom.
Consider: Number of bonding domains on the central atom Number of non-bonding electron pairs (lone pairs) on the central atom
angular with 109.5 degree
Consider: Number of bonding domains on the central atom Number of non-bonding electron pairs (lone pairs) on the central atom
No lone pairs
One on each side (at 180º) of the central atom.
Bromine atom= [Br]
one can find the bond pairs by finding the oxidation state on the central atom
4