Here we have to draw the Lewis dot structure for xenon dibromide molecule. So xenon is in Group 8A. It's a noble gas, so it has 8 valence electrons. Bromines in Group 7A, so it has seven, and there's two of them, so we have 22 total valence electrons. Now Xenon will go in the center and here we're going to be connected to our two bromines.

Now remember, your surrounding elements need to follow the octet rule. So we're going to put our electrons around bromines so that they each have 8 total valence electrons, 3 lone pairs around them, totaling 6 electrons. But remember, they're also sharing electrons from the single bond, so that's eight each one has. So that's using up 16 of my total 22 valence electrons. So we have 6 remaining here.

The remaining 6 electrons, we have no choice but to put them around Xenon. So 6 electrons and we separate them evenly as lone pairs and this would be the structure of xenon dibromide molecule. We can see here that xenon has 246810 electrons around it. It's breaking the octet rule because it is an exception.

Now it's ideal non octet number would have been 16, but again that's when it's ideal. Here we just don't have enough electrons to get to that number of 16. Instead, xenon is OK with having 10 electrons around it. But here we're seeing that our central elements are breaking the octet rule, and it's still OK.