00:01
All right.
00:01
So for part a, we have brf5.
00:04
So we have seven electrons from the bromine, and then the five florins and each have seven electrons.
00:09
So that's a total of five times seven plus seven, 42.
00:15
Correct? yes, six times seven, 42.
00:18
So if you were to put five fluorines around the bromine and form five bonds, and then each fluorine has an octet, then that's going to have eight times five or 40 electrons.
00:33
And to get to the bromine and form five bonds.
00:34
And to get a lot of one, and then each fluorine has an octet, then that's going to have eight times five or 40 electrons.
00:34
And to get to get to to 42, we'd also need to include a lone pair.
00:37
So this is going to be an octahedral species because it has six electron domains around it.
00:44
And then, of course, florines all have three lone pairs to satisfy their octets like so.
00:57
For part b, we have scl6.
01:00
There's six groups around the central atoms so we can already predict that it's going to be octahedral.
01:05
But just to verify, let's count the number of electrons and make sure that we should indeed have six groups.
01:11
Electron domains.
01:12
So we have six electrons from the sulfur and then six chlorines each have seven electrons.
01:18
So this is equal to 48, which is six groups of eight electrons.
01:26
So indeed, if we form one bond to each of the chlorines and then each of those chlorines has a complete octet, we will have the right number of electrons without any other loan pairs on the central atom.
01:41
Not that there can be more than six electron domains around the central atom as far as we know.
01:45
For any species, but i always want to be sure...