 OK, so not to beat a dead horse, but let's do just one more. So let's do one that's a noble gas. So remember where the noble gases are. They're in the last column on the end, right? So group 8, 8, or 18, or whatever you want to call them. But anyways, they're called the noble gases. Why? Because remember, they don't react with anything. And again, we'll talk about why right now, I guess. It's really because their valence shell is filled. So let's talk about argon. So let's just do the same problem. Let's the total number of electrons, total number of valence electrons, and energy level of the valence electrons for argon. So again, I really like to just go ahead and do the full electron configuration, get it out of the way. So let's just do that. So 1s2, 2s2, 2p6, 3s2. So where's argon? So it's all the way on the end, right? So 1, 2, 3, 4, 5, 6. So it's got that p orbital, or those p orbitals, filled as well, right? So remember, your valence electrons are just your last energy level. So total number of electrons, you can count them up. It gets kind of tedious at this point, or you can just look at the period of table to tell you. So the total number of electrons, valence electrons, it's just the ones that are to the right of that line, in that last period that you're going down. So in this case, it's 8. And the second is that once you've got 8 electrons in one shell, you've got what's called a complete octet. And you can see that when we draw the Lewis structure, the spaces are filled. And of course, in the n-equal time, you'll see people write neon plus all that must.