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 statements correctly describes the Lewis dot structure of the neutral compound CH3NO?

The carbon atom forms a double bond with the oxygen atom, and the nitrogen atom is bonded to three hydrogens.

The nitrogen atom is bonded to three hydrogens and the oxygen atom is bonded to the carbon atom with a single bond.

The nitrogen atom forms a double bond with the oxygen atom, and the carbon atom is bonded to three hydrogens and the nitrogen.

The oxygen atom is bonded to three hydrogens, and the carbon atom is bonded to the nitrogen atom with a triple bond.

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Verified step by step guidance

Identify the total number of valence electrons available in the molecule CH3NO by summing the valence electrons of each atom: Carbon (C), Hydrogen (H), Nitrogen (N), and Oxygen (O).

Determine the central atom, which is usually the least electronegative atom that can form multiple bonds; in this case, carbon is typically the central atom bonded to hydrogens and nitrogen.

Arrange the atoms to satisfy the typical bonding patterns: carbon forms four bonds, hydrogen forms one bond, nitrogen typically forms three bonds, and oxygen typically forms two bonds with possible double bonds.

Draw single bonds between carbon and the three hydrogens, and between carbon and nitrogen. Then, consider the bonding between nitrogen and oxygen, checking if a double bond is needed to satisfy the octet rule for nitrogen and oxygen.

Assign lone pairs to oxygen and nitrogen to complete their octets, and verify that the total number of electrons used matches the total valence electrons calculated initially, ensuring the Lewis structure is neutral and follows the octet rule.