Final answer:
The Lewis structure of carbon monoxide (CO) includes a triple bond, carbon dioxide (CO2) has two double bonds, and the carbonate ion (CO3 2-) has three resonance forms, with an equal and average bond order of 1.33. The longest carbon-oxygen bond is found in the carbonate ion due to its average bond being effectively a combination of single and double bonds, while the triple bond in CO is the shortest and strongest.
Step-by-step explanation:
To draw the Lewis structures for carbon monoxide (CO), carbon dioxide (CO2), and the carbonate ion (CO32-), and identify the species with the longest carbon-oxygen bond:
- Carbon monoxide (CO) has a structure with a triple bond between carbon and oxygen, with one bond being a coordinate covalent bond where oxygen donates both electrons.
- Carbon dioxide (CO2) has two double bonds, each linking the carbon atom with an oxygen atom, with a total of two pairs of shared valence electrons forming each bond.
- The carbonate ion (CO32-) has three equivalent resonance forms with a possible double bond between the carbon and any one of the three oxygen atoms. The actual carbonate ion is a resonance hybrid with an average bond order of 1.33, indicating that every C-O bond is identical and effectively a combination of single and double bonds.
The species with the longest carbon-oxygen bond is carbon monoxide because it has a triple bond, which is shorter and stronger than the double bonds in carbon dioxide and the '1.33' bonds in the carbonate ion.