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 statements correctly describes the Lewis dot structure of the carbonate ion, CO_3^{2-}?

It contains three equivalent resonance structures, each with one double bond and two single bonds between carbon and oxygen.

All three oxygen atoms are bonded to carbon with single bonds only.

There are no lone pairs on any of the oxygen atoms in the structure.

It has a single structure with two double bonds and one single bond between carbon and oxygen.

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Verified step by step guidance

Recall that the carbonate ion, CO_3^{2-}, has a total of 24 valence electrons: 4 from carbon, 6 from each oxygen (3 oxygens × 6 = 18), plus 2 extra electrons due to the 2- charge, giving 4 + 18 + 2 = 24 electrons.

Draw a skeletal structure with carbon in the center bonded to three oxygen atoms. Initially, connect each oxygen to carbon with a single bond.

Distribute the remaining valence electrons to satisfy the octet rule for each oxygen atom by adding lone pairs, then check if carbon has a complete octet. If not, form double bonds by converting lone pairs on oxygen atoms into bonding pairs with carbon.

Recognize that the carbonate ion exhibits resonance: there are three equivalent Lewis structures where the double bond is placed between carbon and a different oxygen atom in each structure, while the other two oxygens have single bonds.

Understand that the resonance structures imply that all C–O bonds are equivalent and have bond order between a single and double bond, and that each oxygen atom has lone pairs to complete its octet.