Which of the following best represents the correct Lewis dot structure for the neutral compound CO_2?

• A. O–C–O, with each oxygen atom having three lone pairs and the carbon atom having two lone pairs
• B. O≡C–O, with one oxygen atom triple-bonded to carbon and the other single-bonded
• C. O=C=O, with each oxygen atom having two lone pairs
• D. O–C≡O, with one oxygen atom single-bonded and the other triple-bonded to carbon

Answer: (C)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons available for the CO_2 molecule. Carbon has 4 valence electrons, and each oxygen has 6 valence electrons, so total valence electrons = 4 + 2 × 6 = 16.
2. Step 2: Arrange the atoms with carbon as the central atom because it is less electronegative than oxygen. Connect each oxygen atom to carbon with a single bond initially.
3. Step 3: Distribute the remaining valence electrons to satisfy the octet rule for the outer atoms (oxygen atoms first), placing lone pairs around them to complete their octets.
4. Step 4: Check if the central atom (carbon) has a complete octet. If not, form double or triple bonds by converting lone pairs from oxygen atoms into bonding pairs between carbon and oxygen until carbon has 8 electrons.
5. Step 5: Verify the final Lewis structure by counting all electrons to ensure the total matches the valence electrons calculated in Step 1, and confirm that each atom (carbon and oxygens) has a complete octet.