Which of the following best describes the Lewis dot structure for a neutral O2 molecule?

• A. Each oxygen atom shares no electrons, and all electrons remain as lone pairs.
• B. Each oxygen atom shares three pairs of electrons, forming a triple bond, with one lone pair remaining on each atom.
• C. Each oxygen atom shares one pair of electrons, forming a single bond, with three lone pairs remaining on each atom.
• D. Each oxygen atom shares two pairs of electrons, forming a double bond, with two lone pairs remaining on each atom.

Answer: (D)

Verified step by step guidance

1. Recall that the Lewis dot structure represents valence electrons as dots and shared electron pairs as bonds between atoms.
2. Determine the total number of valence electrons for the O2 molecule: each oxygen atom has 6 valence electrons, so total electrons = 6 \times 2 = 12.
3. Arrange the two oxygen atoms with a bond between them and distribute the electrons to satisfy the octet rule for each atom, aiming for 8 electrons around each oxygen.
4. Test different bonding scenarios: single bond (1 pair shared), double bond (2 pairs shared), and triple bond (3 pairs shared), and count lone pairs to see which satisfies the octet rule for both atoms.
5. Identify that sharing two pairs of electrons (a double bond) allows each oxygen atom to have two lone pairs remaining, fulfilling the octet rule and matching the correct Lewis structure for neutral O2.