Which of the following Lewis structures for H2O correctly shows the partial charges and nonbonding electrons?

• A. H:O: with two lone pairs on O, and δ− on O, δ+ on each H
• B. H–O–H with no lone pairs and no partial charges
• C. H–O–H with one lone pair on O, and δ+ on O, δ− on each H
• D. H:O: with two lone pairs on O, and no partial charges

Answer: (A)

Verified step by step guidance

1. Recall that the Lewis structure of water (H\_2O) shows oxygen bonded to two hydrogen atoms with two lone pairs of electrons on oxygen.
2. Draw the Lewis structure with oxygen in the center, single bonds to each hydrogen, and two lone pairs (four electrons) on oxygen, represented as pairs of dots.
3. Understand that oxygen is more electronegative than hydrogen, so it will attract the bonding electrons more strongly, resulting in a partial negative charge (δ\-) on oxygen and partial positive charges (δ\+) on each hydrogen.
4. Check that the structure correctly shows the two lone pairs on oxygen and the partial charges: oxygen with δ\- and hydrogens with δ\+.
5. Eliminate options that either lack lone pairs on oxygen or incorrectly assign partial charges opposite to the electronegativity trend.