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 represents the Lewis dot structure of the neutral compound carbon monoxide (CO)?

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

C single bond O, with three lone pairs on C and three 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 no 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 the CO molecule. Carbon has 4 valence electrons, and oxygen has 6 valence electrons, so the total is $4 + 6 = 10$ valence electrons.

Step 2: Arrange the atoms with carbon and oxygen connected by a bond. Since CO is a diatomic molecule, the atoms are connected directly to each other.

Step 3: Use the valence electrons to form bonds and complete octets. Start by placing a single bond (2 electrons) between C and O, then distribute the remaining electrons as lone pairs to satisfy the octet rule for both atoms.

Step 4: If the octet rule is not satisfied for both atoms, try forming double or triple bonds by converting lone pairs into bonding pairs. Remember that carbon and oxygen can form multiple bonds to achieve stable octets.

Step 5: After forming the bonds, count the lone pairs on each atom and verify the total number of electrons equals 10. The correct Lewis structure for CO has a triple bond between C and O, with one lone pair on carbon and one lone pair on oxygen.