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 CH2NH (methylenimine)?

The nitrogen atom forms a double bond with the carbon atom, and all atoms have complete octets.

The nitrogen atom forms a triple bond with the carbon atom, and the hydrogen atoms are bonded to nitrogen.

The nitrogen atom forms a single bond with the carbon atom, and the carbon atom has an incomplete octet.

The carbon atom forms double bonds with both hydrogen atoms, and nitrogen is left with a lone pair.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons in CH2NH. Carbon has 4 valence electrons, each hydrogen has 1, nitrogen has 5, so sum them up: $4 + (2 \times 1) + 5 + 1 = 12$ valence electrons.

Step 2: Arrange the atoms with carbon as the central atom bonded to two hydrogens and nitrogen. Hydrogen atoms can only form single bonds, so connect each hydrogen to carbon with a single bond, and connect carbon to nitrogen with a bond.

Step 3: Distribute the remaining valence electrons to satisfy the octet rule for carbon and nitrogen. Remember that hydrogen only needs 2 electrons (a single bond). Adjust bonding between carbon and nitrogen to achieve full octets, considering single, double, or triple bonds.

Step 4: Evaluate the possible bonding scenarios: a single bond between C and N may leave carbon with an incomplete octet; a triple bond may leave nitrogen with no lone pairs; a double bond can allow both atoms to have complete octets and nitrogen to retain a lone pair.

Step 5: Confirm that the final Lewis structure has all atoms with complete octets (except hydrogen), and that the bonding matches the valence electron count and typical bonding patterns (e.g., nitrogen usually has one lone pair). This will help identify the correct description among the options.