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1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

11. Bonding & Molecular Structure

Lewis Dot Structures: Neutral Compounds

General Chemistry

11. Bonding & Molecular Structure

Lewis Dot Structures: Neutral Compounds

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Multiple Choice

Which of the following best describes the Lewis dot structure of a neutral H2O molecule, including nonbonding electron pairs on the oxygen atom?

Oxygen is bonded to two hydrogen atoms with single bonds and has one pair of nonbonding electrons.

Oxygen is bonded to two hydrogen atoms with double bonds and has no nonbonding electrons.

Oxygen is bonded to two hydrogen atoms with single bonds and has two pairs of nonbonding electrons.

Oxygen is bonded to one hydrogen atom with a single bond and has three pairs of nonbonding electrons.

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Verified step by step guidance

Recall that a Lewis dot structure represents the valence electrons of atoms in a molecule, showing bonding pairs (shared electrons) and nonbonding pairs (lone pairs).

Determine the total number of valence electrons in the H2O molecule: Oxygen has 6 valence electrons, and each Hydrogen has 1 valence electron, so total electrons = 6 + 2(1) = 8 electrons.

Draw the skeleton structure with Oxygen as the central atom bonded to two Hydrogen atoms with single bonds. Each single bond represents 2 shared electrons, so 2 bonds use 4 electrons.

Distribute the remaining electrons as lone pairs on the Oxygen atom. Since 4 electrons are used in bonds, 8 - 4 = 4 electrons remain, which form two lone pairs (each pair has 2 electrons).

Verify that each atom satisfies the octet (or duet for Hydrogen) rule: Oxygen has 2 bonding pairs + 2 lone pairs = 8 electrons, and each Hydrogen has 2 electrons from the single bond.