Writing formula for ionic compounds

When ions of opposite charge get together, they form ionic bonding. Writing the formula for the ionic compound is pretty straightforward. The critical information you’ll need is the charge that each of the ions will form. If they are provided, then life can’t get any better. If not, you’ll need an extra skill to figure that out. Not tough, but may require slight memory space. I’ll post more about it soon. Meanwhile, here are some commonly used ions:

Back to writing the formula, I find the cross-over method (aka criss-cross method/rule) the best when it comes to writing a foolproof formula. I mean who doesn’t want to get the formula right 100% of the time? So here goes:

1. Write out the ions: Cation on the left, anion on the right. Cross the number in the charge over.
2. Write the crossed over number as subscripts.
3. Simplify if needed.

It might be hard trying to imagine, so here’s how I apply this method on five examples. Notice this method also works on polyatomic ions, just don’t forget to use bracket (parenthesis).

Want to test out your skills? Each practice set consists of 10 questions – 5 on monoatomic ion and 5 on polyatomic ions. (You might want to open the practice in another tab if you need the list of monoatomic and polyatomic ion) Happy crossing!

4 thoughts on “Writing formula for ionic compounds”

1. Your formula for acetate is C2H3O2- but the formula shown in my textbook and on my professor’s slides for acetate is CH3CO2-. Can you explain what is causing the discrepancy?

1. They are both correct. It’s just a different way of representing the formula. C2H3O2- shows the total number of atoms present in the formula for C, H and O. CH3CO2- shows how the atoms are connected.