Lewis Structure of CO Molecule Steps:

• Calculate total valence electrons: carbon (4) + oxygen (6) = 10 electrons.
• Form a triple bond between C and O, accounting for 6 shared electrons.
• Distribute remaining 4 electrons as one lone pair on C and one lone pair on O.
• Confirm structure: :C≡O: with two lone pairs total.

Why A is correct:

• The Lewis structure of CO shows exactly two lone pairs (one on each atom), satisfying the octet rule with 10 valence electrons.

Why the others are wrong:

• B: No coordinate bond from O to C in the primary Lewis structure; triple bond is covalent, though resonance forms exist.
• C: Triple bond has one σ bond and two π bonds, not two σ bonds from O to C.
• D: Option incomplete, provides no valid feature.

Final answer: A