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Draw the Lewis structures for carbon monoxide, carbon dioxide, and the carbonate ion. Identify the species with the longest carbon-oxygen bond and explain your answer.

User Pugz
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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.

User London
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