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 statements correctly describes the Lewis dot structure of neutral HNO?

HNO has a single bond between H and O, and a double bond between O and N, with one lone pair on N.

HNO has a triple bond between N and O, with H bonded to O, and no lone pairs.

HNO has a single bond between H and N, and a double bond between N and O, with one lone pair on O.

HNO has a single bond between H and N, and a single bond between N and O, with two lone pairs on N.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for HNO. Hydrogen (H) has 1 valence electron, Nitrogen (N) has 5, and Oxygen (O) has 6. Add these together to get the total valence electrons available for bonding.

Step 2: Decide the skeletal structure of the molecule. Since hydrogen can only form one bond, it will be bonded to either nitrogen or oxygen. Consider typical bonding patterns: nitrogen often forms multiple bonds, and oxygen usually forms two bonds with lone pairs.

Step 3: Draw possible Lewis structures by connecting atoms with single, double, or triple bonds, ensuring the total number of electrons used matches the total valence electrons calculated. Remember to place lone pairs to complete the octet for nitrogen and oxygen where applicable.

Step 4: Check the formal charges on each atom in your Lewis structures. The best Lewis structure minimizes formal charges and places negative charges on the more electronegative atoms (oxygen in this case).

Step 5: Compare the given options with your Lewis structures and select the one that matches the correct bonding pattern (single bond between H and N, double bond between N and O, and one lone pair on O) and has the lowest formal charges.