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 H2CO (formaldehyde)?

The carbon atom forms a triple bond with oxygen and single bonds with each hydrogen; oxygen has one lone pair.

The carbon atom forms a double bond with oxygen and single bonds with each hydrogen; oxygen has two lone pairs.

The carbon atom forms single bonds with both oxygen and hydrogen atoms; oxygen has three lone pairs.

The carbon atom forms single bonds with each hydrogen and no bond with oxygen; oxygen has four lone pairs.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons in the molecule H2CO. Hydrogen has 1 valence electron each, carbon has 4, and oxygen has 6. Add these together to find the total valence electrons available for bonding.

Step 2: Identify the central atom, which is usually the least electronegative atom that can form multiple bonds. In H2CO, carbon is the central atom, with hydrogen and oxygen bonded to it.

Step 3: Arrange the atoms with carbon in the center, single bonds connecting carbon to each hydrogen, and a bond between carbon and oxygen. Then, distribute the remaining valence electrons to satisfy the octet rule for carbon and oxygen, placing lone pairs on oxygen as needed.

Step 4: Consider the bonding between carbon and oxygen. Since carbon needs to complete its octet and oxygen also prefers an octet, a double bond between carbon and oxygen is typically formed. This allows carbon to have four bonds total (two single bonds to hydrogens and one double bond to oxygen).

Step 5: Confirm the number of lone pairs on oxygen. After forming a double bond with carbon, oxygen will have two lone pairs to complete its octet. This matches the correct Lewis structure where carbon forms a double bond with oxygen and single bonds with each hydrogen, and oxygen has two lone pairs.