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I would be sure to check and make sure you have the correct number of valence electrons when you draw the structure. If not already indicated, you also have to account for the electron that is gained. You will most likely place that electron around the central atom. Then, you can place the brackets and negative charge around the molecule.
For example is we had Br03- and we were adding up the electrons why would we add one instead of subtract one?
A charge of -1 means that the compound has 1 extra electron (more electrons than protons means a negative charge). The Lewis structure would show an amount of electrons equal to the total of the atoms' valence electrons plus one.
For BrO3-, that would be 7+6+6+6+1=26 valence electrons.
For a molecule with a +1 charge such as ammonium, NH4+, you would subtract one e- from the valence e- so the total valence e- would 8. For a molecule with a -1 share like sulfate, SO4^2-, you would add 2 extra valence e-. The result is 32. To draw the lewis structure, just be sure to satisfy the amount of valence electrons and try to keep formal charge as close to 0 as possible.
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