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 the neutral compound fulminic acid (HCNO)?

The central carbon atom forms a single bond with nitrogen and a triple bond with oxygen.

The central carbon atom forms a triple bond with nitrogen and a single bond with oxygen.

The central carbon atom forms a double bond with nitrogen and a double bond with oxygen.

The central carbon atom forms a triple bond with nitrogen and a single bond with oxygen, with a lone pair on oxygen.

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Verified step by step guidance

Step 1: Identify the atoms involved in fulminic acid (HCNO) and their typical valence electrons: Hydrogen (1 valence electron), Carbon (4 valence electrons), Nitrogen (5 valence electrons), and Oxygen (6 valence electrons).

Step 2: Determine the central atom, which is usually the least electronegative atom that can form multiple bonds; here, carbon is the central atom connecting nitrogen and oxygen.

Step 3: Draw possible Lewis structures by connecting carbon to nitrogen and oxygen with single, double, or triple bonds, ensuring the total number of valence electrons equals the sum from all atoms (1 + 4 + 5 + 6 = 16 electrons).

Step 4: Assign lone pairs to complete the octets of nitrogen and oxygen, and check formal charges to find the most stable structure. The correct structure will minimize formal charges and satisfy the octet rule where possible.

Step 5: Confirm that the correct Lewis structure has carbon forming a triple bond with nitrogen and a single bond with oxygen, with a lone pair on oxygen, consistent with the given correct answer.