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 for a neutral molecule of CO_2?

O–C–O, with each oxygen atom having three lone pairs

O=C=O, with each oxygen atom having two lone pairs

O≡C–O, with one oxygen atom having one lone pair and the other having three

O–C≡O, with the central carbon having two lone pairs

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for the CO_2 molecule. Carbon has 4 valence electrons, and each oxygen has 6 valence electrons, so total valence electrons = 4 + 2 × 6 = 16.

Step 2: Arrange the atoms with carbon as the central atom because it is less electronegative than oxygen. Connect the carbon atom to each oxygen atom with single bonds initially.

Step 3: Distribute the remaining valence electrons as lone pairs to satisfy the octet rule for the outer atoms (oxygen atoms first). Each oxygen should have 8 electrons around it (including bonding electrons).

Step 4: If the octet rule is not satisfied for the central carbon atom, form double bonds by converting lone pairs from oxygen atoms into bonding pairs between carbon and oxygen. This will help carbon achieve an octet.

Step 5: Verify the final Lewis structure by counting all electrons to ensure the total equals 16, and check that each atom (carbon and oxygens) has a complete octet. The correct structure will have carbon double bonded to each oxygen, and each oxygen will have two lone pairs.