We are going to take another look at a net ionic equation here. Okay, so for this one we’re going to do our chemical reaction between aluminum and silver nitrate, so here’s aluminum aluminum is a metal.

So it’s solid silver nitrate is aqueous, so we are going to switch the metals liberating silver and it is a solid because it is a metal and aluminum nitrate. Okay, so we’re going to proceed to our total net ionic equation, step 2.

Here now the things that are equus are going to break up, so we only have to aqueous in this question and now things that are solid. It going to remain solid, so first off, this aluminum is solid, got to balance it.

Firstly, we got aluminum end. It is solid, so we will keep it as solid pull us. We’Ve got silver nitrate, let’s break it up into silver and nitrate. Let’S not forget that there are three. There is a three in front of the silver nitrate which gives us three silvers.

There’S our nitrate, and now we have three nitrates and on the other side again, this silver is solid, so we’re just going to rewrite it and let’s break up our aluminum nitrate. We’Ve got aluminum les plus three and we have three nitrates.

Now we’re going to do our spectator, ions, there’s actually in fact only one I on in this equation. That is exactly the same on both sides, and that would be those three nitrates. So let’s cancel them out for things to be common.

Both sides, if be exactly the same, this aluminum here, is a solid over here. It’S an aqueous, so they’re not the same and same thing with the silver. So to rewrite our stuff, that’s not cancelled out.

We put aluminum together with three silver ions in solution, and we make our silver precipitate out and we have an aluminum and our o single spectator ion would be the nitrates. Thank you for watching.

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