00:01
First we need to draw the lewis structure for xef2.
00:05
Xe has eight valence electrons.
00:09
Fluorine has seven.
00:11
There are two of them.
00:13
This gives us a total of 22 valence electrons.
00:19
So if we put xe in the middle and we bond our two fluorines, giving each fluorine an octet with three lone pairs, we would have used up 16 of our total 22 valence electrons.
00:35
Giving us another six.
00:40
So six corresponds to three lone pairs that we can put on xenon.
00:47
That gives us five electron groups surrounding xenon.
00:52
Five electron groups gives us an electron group geometry of trigonal bipramidal, but with two of them, only two of them being bonding, three of them being non -bonding, the molecular geometry is going to be linear.
01:18
So the answer is linear with five total electron groups...