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 is the correct Lewis dot structure for OF2 (oxygen difluoride)?

O atom in the center with double bonds to each F atom; O has one lone pair, each F has two lone pairs.

F atom in the center with single bonds to two O atoms; F has three lone pairs, each O has two lone pairs.

O atom in the center with two single bonds to F atoms; O has two lone pairs, each F has three lone pairs.

O atom in the center with single bonds to F atoms; O has three lone pairs, each F has two lone pairs.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for OF2. Oxygen (O) has 6 valence electrons, and each fluorine (F) has 7 valence electrons. Since there are two fluorine atoms, total valence electrons = 6 + 2 \times 7 = 20 electrons.

Step 2: Identify the central atom. Oxygen is less electronegative than fluorine, so oxygen will be the central atom with the two fluorine atoms bonded to it.

Step 3: Draw single bonds between the central oxygen atom and each fluorine atom. Each single bond represents 2 electrons, so 2 bonds use 4 electrons out of the total 20.

Step 4: Distribute the remaining electrons as lone pairs to satisfy the octet rule. Start by completing the octets of the fluorine atoms first, then place any leftover electrons on the oxygen atom.

Step 5: Count the lone pairs on each atom after distribution. Oxygen should have two lone pairs (4 electrons), and each fluorine should have three lone pairs (6 electrons) to complete their octets.