Which statement best describes the Lewis dot structure of a neutral water molecule (H2O)?

• A. The oxygen atom has one lone pair and forms three single bonds with hydrogen atoms.
• B. The oxygen atom has no lone pairs and forms two double bonds with hydrogen atoms.
• C. The oxygen atom has three lone pairs and forms one single bond with a hydrogen atom.
• D. The oxygen atom has two lone pairs and forms two single bonds with hydrogen atoms.

Answer: (D)

Verified step by step guidance

1. Recall that a Lewis dot structure represents the valence electrons of atoms in a molecule, showing bonds and lone pairs explicitly.
2. Identify the valence electrons for each atom: oxygen has 6 valence electrons, and each hydrogen has 1 valence electron.
3. Determine the total number of valence electrons in the water molecule: 6 (from O) + 2 × 1 (from 2 H) = 8 electrons.
4. Arrange the atoms with oxygen as the central atom bonded to two hydrogens, then distribute the electrons to satisfy the octet rule for oxygen and duet rule for hydrogen.
5. Assign two single bonds between oxygen and each hydrogen (using 4 electrons), and place the remaining 4 electrons as two lone pairs on the oxygen atom, resulting in oxygen having two lone pairs and two single bonds.