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 best describes the Lewis dot structure for OF_2 (oxygen difluoride)?

Fluorine is the central atom with two single bonds to oxygen and two lone pairs on fluorine.

Oxygen is the central atom with two single bonds to fluorine atoms and two lone pairs on oxygen.

Oxygen is the central atom with two single bonds to fluorine atoms and no lone pairs on oxygen.

Oxygen is the central atom with one double bond to one fluorine and one single bond to the other fluorine, with one lone pair on oxygen.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for OF_2. Oxygen has 6 valence electrons, and each fluorine has 7 valence electrons, so 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 two fluorine atoms bonded to it.

Step 3: Draw single bonds between the central oxygen atom and each fluorine atom. Each single bond uses 2 electrons, so 4 electrons are used in bonding.

Step 4: Distribute the remaining electrons as lone pairs to satisfy the octet rule. Place lone pairs on fluorine atoms first to complete their octets, then place any remaining electrons on oxygen.

Step 5: Verify that all atoms have a complete octet (8 electrons around each atom) and that the total number of electrons used equals the total valence electrons calculated in Step 1.