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 is the correct Lewis dot structure for carbon monoxide (CO)?

C triple bond O, with one lone pair on C and two lone pairs on O

C double bond O, with two lone pairs on C and two lone pairs on O

C triple bond O, with two lone pairs on C and one lone pair on O

C single bond O, with three lone pairs on C and three lone pairs on O

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for bonding in CO. Carbon has 4 valence electrons and oxygen has 6 valence electrons, so total valence electrons = 4 + 6 = 10.

Step 2: Connect the carbon and oxygen atoms with a bond. Start with a single bond, which uses 2 electrons, leaving 8 electrons to be distributed as lone pairs or additional bonds.

Step 3: Use the remaining electrons to satisfy the octet rule for both atoms. Add lone pairs and multiple bonds as needed to ensure both carbon and oxygen have 8 electrons around them.

Step 4: Consider the possibility of multiple bonds (double or triple bonds) between carbon and oxygen to achieve full octets and minimize formal charges. Calculate formal charges for each structure to find the most stable arrangement.

Step 5: Identify the Lewis structure with a triple bond between carbon and oxygen, one lone pair on carbon, and two lone pairs on oxygen, as this arrangement satisfies the octet rule and results in the lowest formal charges on both atoms.