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 HCP (hydrogen cyanophosphide)?

H–C=P with two lone pairs on phosphorus

H–C–P with three lone pairs on phosphorus

H=C=P with a lone pair on carbon

H–C≡P with a lone pair on phosphorus

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Verified step by step guidance

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

Step 2: Arrange the atoms in a reasonable skeletal structure. Since hydrogen typically forms only one bond, it will be bonded to carbon. Carbon and phosphorus will be connected to each other. So the skeleton is H–C–P.

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 P. Each single bond accounts for 2 electrons. Then distribute the remaining electrons to satisfy the octet rule for carbon and phosphorus, placing lone pairs as needed.

Step 4: Consider multiple bonds to satisfy the octet rule and minimize formal charges. Carbon and phosphorus can form double or triple bonds. Check the formal charges for each atom with different bonding arrangements to find the most stable structure. The correct structure will have minimal formal charges and satisfy the octet rule where possible.

Step 5: Confirm the final Lewis structure by verifying that the total number of electrons used equals the total valence electrons, that hydrogen has only one bond, and that carbon and phosphorus have appropriate bonds and lone pairs. The correct structure is H–C≡P with a lone pair on phosphorus.