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 describes the Lewis dot structure of a neutral CO_2 molecule?

The central carbon atom forms two double bonds with two oxygen atoms, and each oxygen atom has two lone pairs.

The central carbon atom forms a single bond with each oxygen atom, and each oxygen atom has three lone pairs.

The central carbon atom forms two single bonds with two oxygen atoms, and each oxygen atom has two lone pairs.

The central carbon atom forms a triple bond with one oxygen atom and a single bond with the other oxygen atom.

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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 \times 6 = 16.

Step 2: Identify the central atom, which is carbon in CO_2, and arrange the atoms with carbon in the center and oxygen atoms on either side.

Step 3: Connect the central carbon atom to each oxygen atom with single bonds initially, using 2 electrons per bond, which accounts for 4 electrons.

Step 4: Distribute the remaining electrons to satisfy the octet rule for the oxygen atoms first by adding lone pairs, then place any leftover electrons on the central carbon atom.

Step 5: Check if the octet rule is satisfied for all atoms. If not, convert lone pairs on oxygen atoms into double bonds with carbon to ensure carbon has a full octet, resulting in two double bonds between carbon and oxygen, with each oxygen having two lone pairs.