 Okay, so let's do one of these balancing redox equations. Well, this one's already balanced, but it asks how many electrons are transferred in the following reaction, and that reaction is pictured up there. So it's already been balanced for us, so it wants us to go backwards from the balanced equation. Okay? So what we're going to do is take this equation and break it back up into its reduction in oxidation equations, okay? So hopefully you can see that one of the equations is here, 10i minuses go to 5i2s, right? So let's write that one down. And the other one then would be everything else, so 12h plus goes to, remember when we're doing this, after we balance all of our atoms, we want to balance our charges, okay? So on this side of the equation, we've got 10 negative signs, right? And on this side we have 0 negative signs, so to balance it to get a minus 10 on both sides, we're going to have to add 10 electrons to that side, okay? So now if we look at our charge balance here, we got minus 2, so 2 times negative 1, so it's going to be overall minus 2, and then 12 times positive 1, so that's going to be overall plus 12, right? So minus 2 plus 12 is going to be minus 10, right? Or plus 10. So we're going to have to add 10 electrons to balance the charges out, because this side is 0 over here. Does that make sense? Okay, so what's happening? So losing electrons here, so that's the oxidation half reaction, and this is the reduction, not that that matters, but it asks you how many electrons are being transferred? Well, any questions on that one? Okay, pretty straightforward, but you've got to go backwards.