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 best describes the correct Lewis dot structure for the neutral compound HCN?

H–C–N, with single bonds between all atoms and three lone pairs on N

H–C=N, with a single bond between H and C, a double bond between C and N, and two lone pairs on N

H–C≡N, with a single bond between H and C, a triple bond between C and N, and a lone pair on N

H=C=N, with a double bond between H and C, a single bond between C and N, and one lone pair on N

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Verified step by step guidance

Step 1: Determine the total number of valence electrons in 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 with Carbon as the central atom because it can form multiple bonds, placing Hydrogen on one side and Nitrogen on the other.

Step 3: Connect the atoms with single bonds initially: H–C–N. Each single bond represents 2 electrons. Subtract these bonding electrons from the total valence electrons to find how many electrons remain for lone pairs or multiple bonds.

Step 4: Distribute the remaining electrons to satisfy the octet rule for Carbon and Nitrogen. Since Hydrogen only needs 2 electrons, focus on completing octets for C and N. Consider forming double or triple bonds between C and N if needed to complete their octets.

Step 5: Evaluate the formal charges on each atom to ensure the most stable Lewis structure. The best Lewis structure will have formal charges closest to zero and satisfy the octet rule, which leads to a triple bond between C and N, a single bond between H and C, and one lone pair on Nitrogen.