Final answer:
Carbon monoxide (CO) is a harmful, colorless, and odorless gas caused by incomplete combustion of fossil fuels, which can lead to possible health issues or death upon exposure. CO2 differs from CO as it is involved in climate change, highlighting the importance of knowing their Lewis structures. CO also has industrial applications, requiring careful management to prevent toxicity.
Step-by-step explanation:
Carbon monoxide (CO) is a colorless, odorless gas that can have both detrimental and beneficial effects. When inhaled in high concentrations, it can be toxic, leading to symptoms like headaches, dizziness, and nausea, and in severe cases, can be fatal due to its binding with hemoglobin in the blood, which prevents oxygen from being transported throughout the body. This is why CO is considered dangerous when it accumulates in indoor environments from sources like unvented heaters, leaking chimneys, and gas stoves. CO emissions primarily originate from the combustion of fossil fuels in vehicles and industrial processes, contributing to outdoor air pollution.
Despite its toxicity, CO has some applications in the industrial sector. For instance, it is utilized as a reducing agent in metallurgical processes and is a key component in the production of chemicals such as methanol. Careful handling and safety protocols are essential when working with CO due to its potential health hazards.
It is important to differentiate CO from carbon dioxide (CO2), which is a normal byproduct of respiration and combustion but is a concern for global climate change. Understanding the Lewis structures of CO and CO2 reveals the differences in their chemical bonding and implications for environmental impact.