Question

which of the following statement(s) applies to the carbonate ion, illustrated here? select all correct options. carbonate ion exhibits resonance; all the carbon - oxygen bond lengths in carbonate are the same; the double bond in carbonate alternates between different oxygen atoms; the carbonate ion has two longer single bonds and one shorter double bond

Explanation:

1. Resonance in Carbonate Ion: The carbonate ion ($\ce{CO_3^{2-}}$) exhibits resonance. Resonance structures are different Lewis structures that can be drawn for a molecule or ion where the electrons are delocalized. The given diagram shows multiple resonance structures for the carbonate ion, so this statement is correct.
2. Carbon - Oxygen Bond Lengths: Due to resonance, the electrons in the carbon - oxygen bonds are delocalized. This means that all the carbon - oxygen bonds in the carbonate ion are equivalent (a hybrid between single and double bonds). So, all the carbon - oxygen bond lengths are the same. This statement is correct.
3. Alternating Double Bond: In reality, because of resonance, the double bond is not localized between a specific pair of carbon and oxygen atoms. It is delocalized over all three carbon - oxygen bonds. So, the double bond does not alternate between different oxygen atoms. This statement is incorrect.
4. Bond Lengths in Carbonate Ion: As a result of resonance, the carbonate ion does not have two longer single bonds and one shorter double bond. Instead, all the bonds are of the same length (a hybrid bond length between single and double bonds). This statement is incorrect.

Answer:

• carbonate ion exhibits resonance
• all the carbon - oxygen bond lengths in carbonate are the same