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 the molecule OF2?

F:O:F, where O has two lone pairs and each F has three lone pairs

F-O-F, where O has one lone pair and each F has three lone pairs

F=O=F, where O has one lone pair and each F has two lone pairs

F-O-F, where O has three lone pairs and 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 the molecule OF2. Oxygen (O) has 6 valence electrons, and each fluorine (F) has 7 valence electrons. Since there are two fluorines, calculate the total as $6 + 2 \times 7$.

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

Step 3: Distribute the remaining valence electrons as lone pairs to satisfy the octet rule for each atom. Remember that fluorine atoms typically have three lone pairs, and oxygen should have enough lone pairs to complete its octet after bonding.

Step 4: Check the formal charges on each atom to ensure the most stable Lewis structure. The formal charge is calculated by $\text{Formal charge} = \text{Valence electrons} - \text{Nonbonding electrons} - \frac{1}{2} \times \text{Bonding electrons}$.

Step 5: Compare the possible Lewis structures based on the octet rule and formal charges. The correct structure will have all atoms with full octets and minimal formal charges, which corresponds to oxygen having two lone pairs and each fluorine having three lone pairs.