Which of the following is the correct Lewis dot structure for the neutral compound CF2O?

• A. The central carbon atom is single-bonded to oxygen and single-bonded to each fluorine; oxygen has two lone pairs.
• B. The central carbon atom is triple-bonded to oxygen and single-bonded to each fluorine; oxygen has one lone pair.
• C. The central carbon atom is single-bonded to oxygen and double-bonded to each fluorine; oxygen has three lone pairs.
• D. The central carbon atom is double-bonded to oxygen and single-bonded to each fluorine; all atoms have complete octets.

Answer: (D)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons in CF2O. Carbon has 4 valence electrons, each fluorine has 7, and oxygen has 6. Add these together to find the total electrons available for bonding and lone pairs.
2. Step 2: Identify the central atom, which is carbon in this case, because it is less electronegative than oxygen and fluorine and can form multiple bonds.
3. Step 3: Connect the central carbon atom to the two fluorine atoms and the oxygen atom with single bonds initially. This uses 6 electrons (3 bonds × 2 electrons each).
4. Step 4: Complete the octets of the fluorine atoms by adding three lone pairs (6 electrons) to each fluorine, since fluorine typically forms only one bond and has three lone pairs.
5. Step 5: Use the remaining electrons to complete the octet on oxygen. If oxygen does not have a full octet with a single bond, form a double bond between carbon and oxygen. Adjust lone pairs accordingly so that all atoms have complete octets.