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 a correct Lewis dot structure for hydrogen cyanide (HCN)?

H–C=N with two lone pairs on nitrogen

H=C=N with one lone pair on nitrogen

H–C–N with three lone pairs on nitrogen

H–C≡N with a lone pair on nitrogen

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for bonding 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.

Step 2: Arrange the atoms in a reasonable skeletal structure. Since carbon is less electronegative than nitrogen and can form multiple bonds, place carbon between hydrogen and nitrogen: H–C–N.

Step 3: Use the total valence electrons to form bonds between atoms. Start by placing single bonds between H–C and C–N, then add multiple bonds as needed to satisfy the octet rule for carbon and nitrogen.

Step 4: Assign lone pairs to the atoms to complete their octets. Hydrogen only needs 2 electrons (a single bond), carbon needs 8 electrons total, and nitrogen also needs 8 electrons. Place lone pairs on nitrogen after bonding to complete its octet.

Step 5: Verify the Lewis structure by checking that the total number of electrons used (bonding and lone pairs) equals the total valence electrons calculated in Step 1, and that each atom (except hydrogen) satisfies the octet rule. The correct structure for HCN is H–C≡N with a lone pair on nitrogen.