Which of the following best describes the Lewis dot structure of a neutral CO_2 molecule?

• 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 two single bonds with two oxygen atoms, and each oxygen atom has two lone pairs.
• C. The central carbon atom forms a single bond with each oxygen atom, and each oxygen atom has three 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. Recall that the Lewis dot structure represents the valence electrons of atoms and how they are shared or paired in bonds to satisfy the octet rule (or duet for hydrogen).
2. Determine the total number of valence electrons in CO_2: Carbon has 4 valence electrons, and each oxygen has 6 valence electrons, so total valence electrons = 4 + 2 × 6 = 16 electrons.
3. Place the carbon atom in the center because it is less electronegative than oxygen, and connect it to each oxygen atom with single bonds initially.
4. Distribute the remaining electrons to satisfy the octet rule for each atom, starting by completing the octets of the oxygen atoms with lone pairs, then adjust bonding by forming double bonds if necessary to ensure carbon also has a full octet.
5. Recognize that the most stable Lewis structure for CO_2 has carbon forming two double bonds (one with each oxygen), and each oxygen atom having two lone pairs, which satisfies the octet rule for all atoms and uses all 16 valence electrons.