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 structure of the neutral compound CO (carbon monoxide)?

CO has a triple bond between C and O, with one lone pair on C, two lone pairs on O, and a formal charge of -1 on C and +1 on O.

CO has a single bond between C and O, with three lone pairs on O and two lone pairs on C, and no formal charges.

CO has a triple bond between C and O, with no lone pairs on either atom, and no formal charges.

CO has a double bond between C and O, with two lone pairs on each atom, and no formal charges.

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Verified step by step guidance

Determine the total number of valence electrons available for the CO molecule by adding the valence electrons of carbon (4 electrons) and oxygen (6 electrons), giving a total of 10 valence electrons.

Draw a skeletal structure with carbon and oxygen connected by a bond. Since CO is a diatomic molecule, start with a single bond between C and O, which uses 2 electrons.

Distribute the remaining electrons to satisfy the octet rule for both atoms. Add lone pairs to oxygen and carbon as needed, and consider multiple bonds (double or triple) to achieve full octets.

Calculate the formal charges on carbon and oxygen for each possible Lewis structure using the formula: Formal charge = (Valence electrons) - (Nonbonding electrons) - (Bonding electrons / 2). This helps identify the most stable structure with the lowest formal charges.

Compare the structures and select the one where carbon and oxygen have formal charges of -1 and +1 respectively, a triple bond between them, one lone pair on carbon, and two lone pairs on oxygen, as this best represents the actual Lewis structure of CO.