sp3d2,
this accounts for all 6 electron domains found around the central Br atom.
Verify by checking the Lewis dot configuration. Br has 4 bonded electron domains and 2 lone pairs.
Therefore the hybridization of the central atom in BrF4 is sp3d2
The structure of BrF4- ion is square planar. VSEPR theory predicts this structure as there are 6 electron pairs (4 bonding and 2 lone pairs). The electron pairs are octahedrallly disposed around the Br atomwith the lone pairs are as far apart as possible.
hybridization = sp3d2
By symmetry considerations, orbitals taking part in the hybridization of the Br are s, d and a p orbital. [Symmetries 2A1+B1]. Most likely orbitals are then a dx2-y2 and a px along the s.
Knowing that it has a trigonal planar shape, then it should be sp^2.
The hybridization of Br atom is sp2d.
sp^3d^2
sp3d
sp3d2
sp2
Br +3, balanced by 3 fluorines each with -1.
sp3d2 Br hybridizes 4s, 4p and 4d If I'm not mistaken. Seems kind of strange for a hybridization since it involves two 4d orbital when you'd expect it to hybridize with only one 4d orbital, but that's what I found on a few websites.
PBr2 is also known as Phosphorous Bromide. The P is the Phosphorous element and the Br is the Bromine element. The 2 beside the Br means that there are 2 Bromine elements.... There, PBr2 is one phosphorous and 2 bromine elements. hope this helps....
There are none
Bromine is an element and has the symbol Br.
1
Br +3, balanced by 3 fluorines each with -1.
sp3d2 Br hybridizes 4s, 4p and 4d If I'm not mistaken. Seems kind of strange for a hybridization since it involves two 4d orbital when you'd expect it to hybridize with only one 4d orbital, but that's what I found on a few websites.
PBr2 is also known as Phosphorous Bromide. The P is the Phosphorous element and the Br is the Bromine element. The 2 beside the Br means that there are 2 Bromine elements.... There, PBr2 is one phosphorous and 2 bromine elements. hope this helps....
BrF3
Formula: BrF3
Formula: BrF3
There are none
It is hard to say, because BrF is readily disproportioning into Br2,(l) and BrF3,(l) according to:3 BrF → BrF3 + Br2Bromine trifluoride, BrF3, is boiling at 125.72 °CCompared with Chlorine fluoride: this, ClF, is an (also) unstable brownish yellow gas (with boiling point 5°C)
The hybridization of PH3 is sp3
The preferred geometry of molecule BrF3 or bromine trifluoride is a planar "T-shaped" molecule. This is due to the two lone pairs of electrons on bromine, which cause a repulsion from the fluorine atoms.
Bromine is an element and has the symbol Br.