 Okay, so let's try this problem. Shown is the shorthand notation for the cell diagram of the Daniel cell. Label all the parts, show the two half reactions, and show the balanced redox equation. So why do we write things in the shorthand notation? So we can write it all on one line, and it's very descriptive, even though it looks kind of weird. So the things at the ends, you see this is zinc solid, this is copper solid, those are the two electrodes. The one on the left side, that's where the electrons are flowing from, so that's going to be the anode. The electrons are going away, it's losing electrons. So this is the other electrode, what is it called? The cathode. So what you find, right, so when you lose electrons, you're oxidized, so this zinc is becoming zinc 2 plus. So zinc atoms are losing electrons to become zinc 2 plus. In fact, the solution that this electrode, the anode is in, is a zinc 2 plus solution at concentration 1 molar there. So remember, the cathode is this copper, so, well, at the cathode, reduction happens. The Cu2 plus is actually being reduced, because the electrons are flowing onto this copper 2 plus, and the Cu2 plus is becoming Cu. So it's Cu2 plus plus 2 electrons to become Cu. So at the cathode, that reaction, that reduction reaction is occurring. And of course, this is the solution that the cathode's in, and this is the concentration of that solution. So this line just is saying there's an anode in this solution. This line is saying there's a cathode in this solution. This double line, that indicates the break between the two solutions. And remember, we put a salt bridge in between those to kind of counterbalance the loss of electrons from one side and the gain of electrons to the other. So this actually is just indicating that this is a salt bridge. So that's all of the pieces of the shorthand notation. Now let's go ahead and write out the two half reactions. And we described them earlier, so this shouldn't be too difficult for us to try to write them out. But let's do it anyway. So the oxidation half reaction happens at the anode. So what's happening? In oxidation, you're losing electrons. Remember, Leo loses electrons. This is oxidation. So zinc solid is losing electrons to become zinc 2 plus eggless, like that. So how many electrons did it lose? Two. So that's the oxidation half reaction. The reduction half reaction is going to be the opposite. So reduction is gaining electrons. Remember, gr, right? So what is gaining electrons? It's the Cu2 plus eggless. That's going to copper solid like that. But how many electrons do we need to do that? Two. Two, right? So that's the reduction half reaction. This one's really convenient because both of them are two. So the electrons are already balanced for us. So we can just add these two reactions up, cancelling out our electrons there. When we add those up, we're going to get the balanced redox reaction. So the balanced redox reaction is going to be zinc solid plus Cu2 plus eggless goes to zinc 2 plus eggless plus Cu2. So are there any questions on that particular one? Okay, hopefully it makes sense.