So in this problem we want to determine the electron pair, and molecular geometries for XeF2. Before we can do that, we actually have to get our Lewis structure first. So that's going to be the first thing we need to worry about. And then in order to find the Lewis structure, I first need to figure out how many valence electrons I have in my molecule. So, for xenon I have 8 electrons plus 2 times 7 from each of the fluorine, and so what I get is a total of 22 electrons in my final structure. So I'm going to draw my skeletal structure, with single bonds. Remembering that fluorine always has a terminal atom. Now I've got, used up four of my electrons. I have 18 left. I'm going to fill in the octet, around each of my terminal fluorine atoms. Now that I've done that, I've used up 16 of my electrons. I see that I still have six additional electrons left. So I'm going to put those on. The central xenon atom, and now I can see what my Lewis structure is for my molecule. Now that I know the Lewis structure, now I can look at the vesper form of the molecule, so I have Xe, which is my central atom, and we'll represent that with an A. Then I have two bonding groups, which we represent with an X. And then around our central atom, we have three non-bonding groups. So remember, that I'm only worried about the non-bonding groups around the central atom. So I see I have a total of 5 groups, and so if I have 5 groups regardless of whether they're bonding or non-bonding, then I know my electron pair geometry will be trigonal. By pyramid or trigonal bipyramidal. Then I can look at my ratio between my bonding and non-bonding groups. And what I see is that, when I have two bonding groups and three non-bonding groups. I see that my molecular geometry, is going to be what we call T-shaped.