This is the BrF3 Lewis structure.
We have a total of 28 valence electrons for
the BrF3 Lewis structure.
Bromine is the least electronegative, we'll
put that at the center; and then we'll put
the Fluorines around the outside.
We'll put single bonds between the Fluorines
and the Bromine.
That's six valence, 2, 4, 6 valence electrons
we've used.
Then we'll go around the outside: 8, 10, and
24.
So we have two pairs of valence electrons
left over.
Because Bromine is in period 4 of the periodic
table, it can have more than 8 valence electrons.
So let's just put those two pairs right here
on the central Bromine.
So at this point, we've used all 28 valence
electrons.
The Fluorines all have octets.
The Bromine has more than 8, but that's OK.
And if we calculated the formal charges, we'd
see that the formal charges on each of the
atoms in the Lewis structure for BrF3 is zero.
So all the formal charges are zero and this
is the Lewis structure for BrF3, and this
is Dr. B., and thanks for watching.
