 So, let's do one of these molecular orbital diagrams so we can find the bond order. So, let's do this one, use molecular orbital diagrams to find the bond order and predict whether H2 plus exists and if it exists, right, it's electronic configuration. So, H2 plus is what we're looking at. So, what is that going to be a combination? So, that's going to be a combination of H and H plus, right, because that would be H2 plus. So, would you okay with that? So, when we do molecular orbital theory, recall each of these has its 1s orbital, molecular orbital, the sigma 1s, well, 1s orbital, remember that? So, these should be on the, there's no reason I'm going to look. Okay, so they should be the same size, it's not like I'm trying to draw into it. Okay, so just fill up the orbitals. So, hydrogen's got the 1 electron and H plus has no electrons, right? So, when we take those electrons and fill them up here, we just put the 1 down there. So, in order to determine whether this molecule will exist or not, we have to figure out the bond order, recall that. So, the bond order is going to equal 1 half times the number of bonding electrons minus the antibonding electrons. So, we'll say, we'll do this, we'll write a number of bonding electrons as 1, minus antibonding electrons as 0. So, 1 half times 1, right, 1 minus 0 is 1, so that's equal 1 half, okay? So, the bond order is greater than 1, right? So, this molecule exists, is that going to call that? Are there any questions on this one? Well, let's do one with that, okay? So, any questions on this particular problem?