Final answer:
Lewis structures depict the arrangement of electrons in molecules. Carbon monoxide (CO) has a triple bond and a lone electron on carbon, while carbon dioxide (CO2) features two double bonds, fulfilling the octet rule.
Step-by-step explanation:
Both carbon monoxide (CO) and carbon dioxide (CO2) are significant in discussions of air pollution and combustion reactions. Carbon monoxide, with its colorless and odorless properties, is a byproduct of the incomplete combustion of carbon-containing materials. It's particularly hazardous to human health, as it can interfere with the oxygen transport in the blood. On the other hand, carbon dioxide is a known greenhouse gas contributing to global climate change.
The Lewis structure for CO shows a triple bond between the carbon and oxygen atoms with a single lone electron on carbon. This reflects the molecule's 10 total valence electrons. As for CO2, its Lewis structure depicts carbon in the center with two double bonds connecting to two oxygen atoms, illustrating a total of 16 valence electrons. These double bonds satisfy the octet rule for all the involved atoms.