Table of contents

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 species is correctly represented by a valid Lewis dot structure for a neutral compound?

NH3

H2O2 with each oxygen having only one lone pair

NaCl (as Na and Cl atoms, not ions)

CO2 with a single bond between C and each O

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Verified step by step guidance

Recall that a valid Lewis dot structure for a neutral compound must satisfy the octet rule (or duet for hydrogen) for each atom, and the total number of valence electrons must be correctly represented.

Analyze NH3 (ammonia): Nitrogen has 5 valence electrons and forms three single bonds with hydrogen atoms (each contributing 1 electron), and it has one lone pair. This satisfies the octet rule for nitrogen and duet for hydrogen, making NH3 a valid Lewis structure.

Examine H2O2 (hydrogen peroxide) with each oxygen having only one lone pair: Oxygen typically has two lone pairs in peroxides to satisfy the octet rule. Having only one lone pair on each oxygen means the octet is incomplete, so this is not a valid Lewis structure.

Consider NaCl as neutral atoms (Na and Cl atoms, not ions): Sodium (Na) and chlorine (Cl) do not form a stable neutral molecule by sharing electrons; Na tends to lose one electron to become Na⁺, and Cl gains one to become Cl⁻. Therefore, representing NaCl as neutral atoms bonded together is incorrect.

Look at CO2 with single bonds between carbon and each oxygen: Carbon needs to form double bonds with oxygen to satisfy the octet rule. Single bonds would leave carbon electron-deficient, so this is not a valid Lewis structure.