Which of the following best describes the correct Lewis dot structure for the neutral compound CH2?

• A. Carbon is bonded to two hydrogen atoms and has two lone pairs.
• B. Carbon is bonded to two hydrogen atoms and has a complete octet with four bonds.
• C. Carbon is bonded to two hydrogen atoms and has two unpaired electrons.
• D. Carbon is bonded to two hydrogen atoms and has one lone pair.

Answer: (C)

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons available for the molecule CH2. Carbon has 4 valence electrons, and each hydrogen has 1 valence electron, so total valence electrons = 4 + 2(1) = 6 electrons.
2. Step 2: Recognize that carbon typically forms four bonds to complete its octet, while hydrogen forms only one bond to fill its duet (2 electrons).
3. Step 3: Since there are only 6 valence electrons total, it is impossible for carbon to form four bonds (which would require 8 electrons) or to have two lone pairs (which would require 4 electrons as lone pairs plus bonding electrons).
4. Step 4: Consider that carbon can form two single bonds with the two hydrogens, using 4 electrons, and the remaining 2 electrons will be unpaired on carbon, resulting in two unpaired electrons rather than lone pairs.
5. Step 5: Conclude that the correct Lewis structure for CH2 is carbon bonded to two hydrogen atoms with two unpaired electrons on carbon, reflecting the molecule's radical nature and incomplete octet.