Draw the Lewis dot structure for the molecule BrF3.
Type of Paper: Question-Answer
Academic Level: Undergrad. (yrs 3-4)
Paper Format: APA
Here is what is needed: Draw the Lewis dot structure for the molecule BrF3.
I beleive it should look like this:
BrF3 does not follow the octet rule. Both Br and F have seven valence electrons, so the lewis structure will have a total of 28 electrons, or 14 electron pairs. Br is the central atom, connected to each F atom by a single bond. 3 lone electron pairs will surround each F atom, and 2 lone electron pairs will be on the Br atom.
What is the electron pair geometry, molecular geometry, and what hybrid orbital on Br is used? Please show how to calculate, and calculate the formal charge on the Br atom in this molecule.
The structure is shown below:
There are 5 electron pairs (10 electrons - 7 from Br and 1 each from the three F) around the central Br atom.
The electron pair have a trigonal bipyramidal geometry (from VSEPR rules).
The molecular geometry is T-shaped (as can be seen).
Hybrid orbitals on Br are dsp3 (total of 5 orbitals 1 x d + 1 x s + 3 x p for 5 electron pairs).
Formal charge on Br = 0 (formal charge = valence electrons - nonbonding electrons - covalently bonded electrons/2 = 7 - 4 - 6/2 = 0).