 Okay. So it says, the next problem says you are in the chemistry lab and you mix an aqueous solution of silver 1 nitrate. Remember nitrate. You know, that's the polyatomic ion that I wanted you to remember, right? So silver 1, that means, well, if you look on the periodic table, silver is a G, right? And it's a transition metal, so it's written silver 1 nitrate, right? So silver 1 means a G plus, like that, okay? Nitrate, you have to remember what the polyatomic, the charges for these polyatomic ions, unless you can build them like what we did in the last, the last, or in the last problem. But anyways, nitrate is NO3 minus, okay? So that's just something you want to remember, okay? So silver 1 nitrate, the molecular formula, or the unit formula for that would just be AG NO3, like that, okay? Together with an aqueous solution of calcium bromide, okay? So calcium bromide, you know calcium, it's got always going to have that same charge, right? And if you look on the periodic table, it's plus 2, it's in the group 2, right? Plus 2. So you know bromine always has the same charge 2, and what is that? It's a halogen, so minus 1, right? Minus 1. So does plus 2 and minus 1 equal 0? So how many more minuses do we need? Yeah, we need 2, right? Or we need 2 total, right? So calcium bromide is going to be consisting of a unit formula of 1 calcium for every 2 bromides. Does that make sense? Or 2 bromide ions? So we would write it CABR2, like that. Does that make sense? So let's just erase all that, okay? So we've got these two things. And remember what we did in lab? Like a number of times in lab where we mix silver and halogens, whenever we would mix silver and halogens, that precipitate would form. We did it with iodine, bromine, and chlorine in the lab three weeks ago, and then we did it again with that when we were writing the total net molecular ion. Kind of what we're about to do right here. So anyways, this is called calcium bromide. What is because it's not a transition metal, but yeah, no bromine. Okay, so we've got the formulas. Now it says, so you mixed a solution of silver 1 nitrate together with an aqueous solution of calcium bromide forming a white precipitate. Write the molecular total ionic and net ionic equations for this precipitation reaction. Clearly indicate the spectator ion. So the molecular equation is going to be the reaction between this compound and this compound here. Remember, I told you they were aqueous solutions. So already you know, we're going to put this because just to remind ourselves that we're going to have to balance this equation. White precipitate that forms, remember, is going to be silver bromide. But what is this? This is silver 1, right? And bromine, what's its charge? It's negative 1, right? So it doesn't need two bromines to counter with that one. So what's going to be the formula of silver bromide? AGVR. So already that's going to give us a clue as to how we're going to balance that because there's not enough bromine. And this says it's precipitated, right? So the state of matter here is going to be what? Solid. Solid, right? And then, of course, the other is going to be calcium and nitrate, okay? And remember, the nitrates are a dynamic charge is what? Negative 1, right? Silver 1 nitrate, right? And so how many nitrates does it take to counter that calcium? Two, right? Because calcium is plus two, right? Calcium is plus two and nitrate is what? Minus one. Minus one, right? So that's the molecular equation, unbalanced. And now all we've got to do is balance it, okay? So we've got two bromines here, not there. So two, right? Now we've got two silvers there, not there, right? But we've got two nitrates over here and not here, right? So all we've got to do is put two there and one calcium, one calcium, we're cool, right? Okay, so that's the molecular equation right there, okay? So now it asks the total ionic equation. So you just break up everything into its ions that has a Q behind it, okay? So you've effectively done the whole problem. Now it's just, you know, kind of the rigmarole of doing everything else, right? So that's the molecular. The total ionic is to break it all up and you've got to remember to keep those coefficients, right? So it's going to be two AG plus and aqueous, okay? Two, right? Plus two NO3 minus aqueous. You can help me out. Plus CA2 plus, right? Aqueous plus two VR, right? Remember it's two VRs when you break that thing up. It's not VR2, right? Very important. That's like a very common mistake that people do. Very bad. That doesn't make sense. Those two, does this thing break apart? Yeah, it stays. You've got two plus, right? You need to know that. That's, remember that's like chapter three, okay? So that's the total ionic equation, right? And then the net ionic equation is just everything that didn't change or that changed, okay? So did AG plus change to something else or is AG plus in this side of the equation? So you've got to keep it. Is two NO3 minus in that side of the equation? So you can cancel it out. What we're cancelling now to recall the spectator, right? Is CA2 plus on both sides of the equation? Cancel it out. What about two VR minuses? Okay. So that's the total ionic. The net ionic is going to be, well this is the beginning of the net ionic. And since all the coefficients are two, we're going to raise them. Because so two to two to two is the same as one to one, okay? So that's the net ionic equation, okay? You cool with that? Yeah. So I think, so a lot of people have felt this, the TIE and then the spectator ions are going to be the things that you crossed out, right? Don't need to put the two, right? NO3 minus and we'll go with that. Are there any questions on that one? So I think the real trick to these is to remember your poly atomics, you know.