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# Writing an ionic equation Watch

1. I'm not sure if I understand this properly.

Would I need to write multiple ionic equations and then combine them?
Explanations are appreciated
2. (Original post by jamesthelam)
I'm not sure if I understand this properly.

Would I need to write multiple ionic equations and then combine them?
Explanations are appreciated
If I remember...
Ionic equations are equations without the spectator ions. They're the ions that remain unchanged in the reaction.

Rewrite the equation and break up each ionic compound into it's ions. These are the ones that are aqueous only as the ions are free in solution.
Spoiler:
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i.e. 3Cl2 + 6Na+ + 6OH- ---> 5Na+ + 5Cl- + Na+ + ClO3- + 3H2O

Notice that the ClO3 is a 1- ion. That's a polyatomic you need to learn. You can also work it out from the fact that the oxidation state of Na is +1 and the overall oxidation state of the compound is 0.
Notice that I didn't break up Chlorine or Water.

Then cancel the ions you see on both sides because they didn't change, they spectated the reaction.
Spoiler:
Show
3Cl2 + 6OH- ---> + 5Cl- + ClO3- + 3H2O

I may be wrong so I appreciate if someone else verifies the answer.

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