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 neutral compound ClO$^-$?

Chlorine is bonded to oxygen with a single bond, and the structure has three lone pairs on chlorine and three lone pairs on oxygen, with one extra electron giving a negative charge.

Chlorine is bonded to oxygen with a triple bond, and the structure has one lone pair on each atom.

Chlorine and oxygen are not bonded; each atom has a full octet and no formal charge.

Chlorine is bonded to oxygen with a double bond, and both atoms have two lone pairs, with no extra electrons.

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Verified step by step guidance

Identify the atoms involved: chlorine (Cl) and oxygen (O), and note the overall charge of the ion is -1, indicating one extra electron in the system.

Determine the total number of valence electrons: chlorine has 7 valence electrons, oxygen has 6, and add 1 extra electron for the negative charge, giving a total of 7 + 6 + 1 = 14 valence electrons.

Draw a single bond between chlorine and oxygen, which uses 2 electrons, then distribute the remaining electrons as lone pairs to satisfy the octet rule for both atoms.

Assign lone pairs so that chlorine has three lone pairs (6 electrons) and oxygen has three lone pairs (6 electrons), ensuring both atoms have a full octet (8 electrons each including bonding electrons).

Check the formal charges: chlorine and oxygen should have formal charges that sum to -1, consistent with the extra electron, confirming the structure with a single bond, three lone pairs on each atom, and an overall negative charge.