Which of the following best represents the correct Lewis dot structure for a neutral water (H2O) molecule?

• A. O atom in the center with two single bonds to H atoms and no lone pairs on O
• B. O atom in the center with one double bond to one H atom and one single bond to the other H atom
• C. O atom in the center with two single bonds to H atoms and one lone pair on O
• D. O atom in the center with two single bonds to H atoms and two lone pairs on O

Answer: (D)

Verified step by step guidance

1. Recall that the Lewis dot structure represents the valence electrons of atoms in a molecule, showing bonds and lone pairs explicitly.
2. Determine the total number of valence electrons: Oxygen has 6 valence electrons, and each hydrogen has 1, so for H2O, total valence electrons = 6 + 2(1) = 8 electrons.
3. Place the oxygen atom in the center because it is less electronegative than hydrogen and can form multiple bonds; then connect each hydrogen atom to oxygen with a single bond, using 2 electrons per bond.
4. After forming two single bonds (4 electrons used), distribute the remaining 4 electrons as lone pairs on the oxygen atom to satisfy the octet rule for oxygen.
5. Verify that each hydrogen has 2 electrons (a full shell for hydrogen) and oxygen has 8 electrons around it (including bonding and lone pairs), confirming the correct Lewis structure has two single bonds and two lone pairs on oxygen.