Final answer:
The resonance forms of the carbonate ion (CO32-) involve three equivalent structures with one of the oxygen atoms double-bonded to the carbon atom and carrying no charge, while the other two oxygens are single-bonded and carry a -1 charge each.
Step-by-step explanation:
The question asks to write resonance forms that describe the distribution of electrons in various molecules and ions. Specifically, we can discuss the carbonate ion (CO32-) as it is one of the ions mentioned multiple times.
The carbonate ion has three equivalent resonance forms that can be drawn. Each of these forms has the carbon atom at the center with a double bond to one oxygen atom and single bonds to the other two oxygens, each of which carry a -1 charge.
Resonance forms are a way to represent structures that cannot be adequately depicted by a single Lewis structure. These forms illustrate the delocalization of electrons within a molecule.
For the carbonate ion, all three oxygen atoms are equivalent and capable of forming a double bond with the carbon, which leads to three possible arrangements.