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 XeO2F2?

Xe is the central atom, bonded to two F atoms and two O atoms, with no lone pairs on Xe.

Xe is the central atom, bonded to four O atoms, with no lone pairs on Xe.

Xe is the central atom, bonded to two O atoms and two F atoms, with one lone pair on Xe.

Xe is the central atom, bonded to two O atoms and two F atoms, with two lone pairs on Xe.

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Verified step by step guidance

Step 1: Identify the central atom in XeO2F2. Xenon (Xe) is a noble gas but can form compounds by expanding its octet, so it will be the central atom bonded to oxygen (O) and fluorine (F) atoms.

Step 2: Count the total valence electrons. Xe has 8 valence electrons, each O has 6, and each F has 7. Calculate the total number of valence electrons for the molecule: $8 + 2 \times 6 + 2 \times 7$.

Step 3: Draw single bonds from Xe to each of the four atoms (2 O and 2 F). Each bond uses 2 electrons, so subtract $4 \times 2 = 8$ electrons from the total valence electrons.

Step 4: Distribute the remaining electrons to satisfy the octet rule for the outer atoms (O and F). Oxygen and fluorine typically complete their octets with lone pairs. After placing lone pairs on O and F, assign any leftover electrons as lone pairs on Xe.

Step 5: Determine the number of lone pairs on Xe by subtracting the bonding electrons and the electrons assigned to outer atoms from the total valence electrons. This will help confirm whether Xe has one or two lone pairs, which clarifies the correct Lewis structure description.