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 OF2 (oxygen difluoride)?

The oxygen atom has no lone pairs and forms triple bonds with each fluorine atom.

The oxygen atom has one lone pair and forms double bonds with each fluorine atom.

The oxygen atom has two lone pairs and forms single bonds with each fluorine atom.

Each fluorine atom forms a double bond with oxygen and 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 has 6 valence electrons, and each fluorine has 7 valence electrons, so total valence electrons = 6 + 2 \times 7 = 20 electrons.

Step 2: Draw the skeletal structure with oxygen as the central atom bonded to two fluorine atoms. Connect each fluorine to oxygen with a single bond initially.

Step 3: Distribute the remaining valence electrons to satisfy the octet rule for the fluorine atoms first, placing lone pairs around each fluorine until they have 8 electrons total (including bonding electrons).

Step 4: Assign the remaining electrons to the oxygen atom as lone pairs. Since oxygen started with 6 valence electrons and shares two single bonds (2 electrons each), the leftover electrons will form lone pairs on oxygen.

Step 5: Confirm that all atoms have a complete octet and check the bonding: oxygen will have two lone pairs and form single bonds with each fluorine, while each fluorine will have three lone pairs and a single bond to oxygen.