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 is the correct Lewis dot structure for the neutral compound HCNO?

H–C=N=O with a lone pair on C

H–C≡N–O with a lone pair on O

H–C–N=O with a lone pair on N

H–C=N–O with a lone pair on N

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for the molecule HCNO. Add the valence electrons from each atom: H (1 electron), C (4 electrons), N (5 electrons), and O (6 electrons).

Step 2: Arrange the atoms in a plausible connectivity. Since hydrogen typically forms only one bond, it will be bonded to carbon. The remaining atoms (C, N, O) will be connected in a way that satisfies their bonding preferences and the octet rule.

Step 3: Draw single bonds between the atoms according to the chosen connectivity (H–C–N–O or H–C=N=O, etc.) and distribute the remaining valence electrons as lone pairs to satisfy the octet rule for each atom (except hydrogen, which only needs 2 electrons).

Step 4: Adjust the bonding by adding double or triple bonds where necessary to ensure that each atom (especially C, N, and O) has a complete octet and the total number of electrons matches the valence count from Step 1.

Step 5: Verify the formal charges on each atom to find the most stable Lewis structure. The best Lewis structure will have formal charges closest to zero and place negative charges on the more electronegative atoms (like oxygen).