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 the neutral compound O2F2 (dioxygen difluoride)?

Each oxygen atom is bonded to two fluorine atoms, with no O–O bond present.

Each oxygen atom has three lone pairs and is not bonded to any other atom.

The two fluorine atoms are bonded directly to each other, with each also bonded to an oxygen atom.

Each oxygen atom is bonded to one fluorine atom and to the other oxygen atom, with each oxygen having one lone pair.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for O2F2. Oxygen has 6 valence electrons and fluorine has 7 valence electrons. Since there are 2 oxygen atoms and 2 fluorine atoms, calculate the total as: $2 \times 6 + 2 \times 7$.

Step 2: Arrange the atoms to reflect the most likely bonding pattern. Since fluorine typically forms only one bond and oxygen can form two bonds, consider connecting the two oxygen atoms together and bonding each oxygen to one fluorine atom.

Step 3: Draw single bonds between the atoms: O–O and each O–F. Each single bond represents 2 shared electrons. Subtract these bonding electrons from the total valence electrons calculated in Step 1.

Step 4: Distribute the remaining electrons as lone pairs to satisfy the octet rule for each atom. Start by completing the octets on the fluorine atoms (which usually have three lone pairs) and then place the remaining electrons on the oxygen atoms, ensuring each oxygen has one lone pair after bonding.

Step 5: Verify the Lewis structure by checking that each atom has a complete octet (8 electrons around it) and that the total number of electrons used equals the total valence electrons calculated initially. This confirms that each oxygen atom is bonded to one fluorine atom and to the other oxygen atom, with each oxygen having one lone pair.