 OK, let's try this one. So recall, well, what is the question? Which one of these compounds has the stronger ionic bond between it, between the two ions? And you can determine this by determining the melting point. And we'll write that down after we figure out the problem, answer the problem. But anyways, remember we said that attraction increases in such a way as we've got a big plus minus. They're not going to be as attracted to each other as a small plus minus. But two plus and two minus are going to be more attracted to each other than a plus minus, like small, small. So this is size here, and this is charge. So this is attraction increases in this way. And of course, this one's going to have more attractive forces than the ones with only one. So attraction increases like that. OK, so in other words, if we recall what the common ions for this are, it's La plus 1 and f minus. So this is both little, but it doesn't matter because we're comparing. If you've got the same atom, it's really easy to compare. So we've got Li plus and O2 minus here. So you can see what we're really doing is comparing a lot of charge. And here, one charge, so this is going to be, here we've got a plus 1 and a minus 2. So it would be somewhere in the middle for, OK, so. And in other words, if we were to qualitatively assign which one of these compounds has the stronger ionic oxide because we've got this negative 2 and positive 1, as opposed to here, we've got just a negative 1. And if we melting points of these two compounds, it does for this is 1570 degrees Celsius. And for the employer, it is eight of these. We'll leave that chart up there, and we'll see if you guys can pick it up. Similar principle, but.