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 a triple bond with one oxygen atom and a single bond with the other oxygen atom.

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 single bond with each oxygen atom, and each oxygen atom has three lone pairs.

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

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Verified step by step guidance

Recall that the Lewis dot structure represents the valence electrons of atoms and how they are shared or paired in bonds to satisfy the octet rule (or duet for hydrogen).

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

Place the carbon atom in the center because it is less electronegative than oxygen, and connect it to each oxygen atom with single bonds initially.

Distribute the remaining electrons to satisfy the octet rule for each atom, starting by completing the octets of the oxygen atoms with lone pairs, then adjust bonding by forming double bonds if necessary to ensure carbon also has a full octet.

Recognize that the most stable Lewis structure for CO_2 has carbon forming two double bonds (one with each oxygen), and each oxygen atom having two lone pairs, which satisfies the octet rule for all atoms and uses all 16 valence electrons.