Which of the following best describes the Lewis dot structure of carbon dioxide (CO_2)?

• A. The central carbon atom forms a triple bond with one oxygen atom and a single bond with the other oxygen atom.
• B. The central carbon atom forms a single bond with each oxygen atom, and each oxygen atom has three lone pairs.
• C. The central carbon atom forms two single bonds with two oxygen atoms, and each oxygen atom has two lone pairs.
• D. The central carbon atom forms two double bonds with two oxygen atoms, and each oxygen atom has two lone pairs.

Answer: (D)

Verified step by step guidance

1. Identify the total number of valence electrons available for bonding in CO_2. Carbon has 4 valence electrons, and each oxygen has 6 valence electrons, so total valence electrons = 4 + 2 \times 6 = 16.
2. Determine the central atom, which is carbon in this case, because it is less electronegative than oxygen and can form multiple bonds.
3. Start by placing single bonds between the carbon atom and each oxygen atom, using 4 electrons (2 electrons per bond).
4. Distribute the remaining electrons to satisfy the octet rule for the oxygen atoms first, then place any leftover electrons on the carbon atom if needed.
5. If the octet rule is not satisfied for carbon, convert lone pairs from oxygen atoms into double bonds with carbon until carbon has a full octet, resulting in two double bonds between carbon and each oxygen, with each oxygen having two lone pairs.