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 neutral COF_2 (carbonyl fluoride)?

The central carbon atom forms a double bond with each fluorine atom and a single bond with oxygen.

The central carbon atom forms a double bond with oxygen and single bonds with each fluorine atom, with no lone pairs on carbon.

The central carbon atom forms a triple bond with oxygen and single bonds with each fluorine atom.

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

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Verified step by step guidance

Identify the total number of valence electrons available for COF_2 by adding the valence electrons of each atom: carbon (C), oxygen (O), and two fluorine (F) atoms.

Determine the central atom, which is typically the least electronegative element; in this case, carbon is the central atom.

Arrange the atoms with carbon in the center, oxygen and fluorines bonded to carbon, and start by placing single bonds between carbon and each attached atom.

Distribute the remaining valence electrons to satisfy the octet rule for the outer atoms (fluorine and oxygen) first, then adjust bonding by forming double or triple bonds if necessary to complete the octet of the central carbon atom.

Analyze the resulting structure to confirm that carbon has no lone pairs, forms a double bond with oxygen, and single bonds with each fluorine atom, which matches the correct Lewis structure description.