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 correctly describes the Lewis dot structure for the neutral compound CHClO?

Carbon is the central atom, single-bonded to hydrogen and chlorine, and double-bonded to oxygen.

Carbon is the central atom, single-bonded to hydrogen, chlorine, and oxygen, with no double bonds.

Chlorine is the central atom, single-bonded to carbon, hydrogen, and oxygen.

Oxygen is the central atom, single-bonded to carbon, hydrogen, and chlorine.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for the molecule CHClO. Carbon has 4 valence electrons, hydrogen has 1, chlorine has 7, and oxygen has 6. Add these together to find the total valence electrons available for bonding.

Step 2: Identify the central atom. Generally, the least electronegative atom (excluding hydrogen) is the central atom. Between carbon, chlorine, and oxygen, carbon is the least electronegative and typically serves as the central atom in organic molecules.

Step 3: Arrange the atoms with carbon in the center, and connect it to hydrogen, chlorine, and oxygen with single bonds initially. This accounts for some of the valence electrons used in bonding.

Step 4: Complete the octets of the outer atoms (hydrogen only needs 2 electrons, chlorine and oxygen need 8). After placing lone pairs on chlorine and oxygen, check if carbon has a complete octet. If not, form double bonds as needed, typically between carbon and oxygen, to satisfy the octet rule.

Step 5: Verify the Lewis structure by counting all valence electrons used in bonds and lone pairs to ensure it matches the total valence electrons calculated in Step 1, confirming the structure is correct and neutral.