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 correctly represents the Lewis dot structure for the neutral compound HCN?

H–C–N with no lone pairs on nitrogen

H–C≡N with a lone pair on nitrogen

H–C=N with two lone pairs on nitrogen

H=C=N with a lone pair on carbon

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for the molecule HCN. Hydrogen (H) has 1 valence electron, carbon (C) has 4, and nitrogen (N) has 5. Add these together to get the total valence electrons available for bonding.

Step 2: Arrange the atoms in a reasonable skeletal structure. Since hydrogen can only form one bond, it is typically placed at the end. Carbon is usually the central atom, so the structure is H–C–N.

Step 3: Use the total valence electrons to form bonds between atoms. Start by placing single bonds between H and C, and between C and N. Each single bond accounts for 2 electrons.

Step 4: Complete the octet for the atoms (except hydrogen, which only needs 2 electrons). Add lone pairs to nitrogen and carbon as needed, and consider forming double or triple bonds to satisfy the octet rule and use all valence electrons.

Step 5: Verify the formal charges on each atom to ensure the most stable Lewis structure. The best Lewis structure will have formal charges closest to zero, with negative charges on the more electronegative atoms (like nitrogen). This leads to the structure H–C≡N with a lone pair on nitrogen.