Which of the following Lewis dot structures correctly represents a neutral molecule of water (H_2O)?

• 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 two single bonds to H atoms and three lone pairs on O
• C. O atom in the center with one double bond to one H atom and one single bond to the other H atom, 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 a Lewis dot structure represents the valence electrons of atoms in a molecule, showing bonds and lone pairs.
2. Determine the total number of valence electrons in the water molecule: Oxygen has 6 valence electrons, and each Hydrogen has 1, so total electrons = 6 + 2(1) = 8.
3. Place the oxygen atom in the center because it is less electronegative than hydrogen and can form multiple bonds; then connect two hydrogen atoms to oxygen with single bonds, using 4 electrons (2 bonds × 2 electrons each).
4. Distribute the remaining electrons as lone pairs on the oxygen atom to complete its octet; since 4 electrons are used in bonds, 4 electrons remain, which form two lone pairs on oxygen.
5. Verify that each hydrogen has 2 electrons (a full shell for hydrogen) and oxygen has 8 electrons around it (octet rule), confirming the correct Lewis structure is oxygen with two single bonds to hydrogen and two lone pairs on oxygen.