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

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Which of the following best describes the Lewis dot structure of carbon dioxide (CO_2)?

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

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 two double bonds with two oxygen atoms, and each oxygen atom has two lone pairs.

Previous problemNext problem

Verified step by step guidance

Identify the total number of valence electrons available for bonding in CO_2. Carbon has 4 valence electrons, and each oxygen has 6 valence electrons, so total valence electrons = 4 + 2 \times 6 = 16.

Determine the central atom, which is carbon in this case, because it is less electronegative than oxygen and can form multiple bonds.

Start by placing single bonds between the carbon atom and each oxygen atom, using 4 electrons (2 electrons per bond).

Distribute the remaining electrons to satisfy the octet rule for the oxygen atoms first, then place any leftover electrons on the carbon atom if needed.

If the octet rule is not satisfied for carbon, convert lone pairs from oxygen atoms into double bonds with carbon until carbon has a full octet, resulting in two double bonds between carbon and each oxygen, with each oxygen having two lone pairs.