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 best Lewis dot structure for XeI_2 (xenon diiodide), a neutral compound?

Xe atom in the center with two single bonds to I atoms, and no lone pairs on Xe

Xe atom in the center with two single bonds to I atoms, and one lone pair on Xe

Xe atom in the center with two single bonds to I atoms, and three lone pairs on Xe

Xe atom in the center with two double bonds to I atoms, and two lone pairs on Xe

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for bonding in XeI_2. Xenon (Xe) is in group 18 and has 8 valence electrons, and each iodine (I) atom is in group 17 with 7 valence electrons. Calculate the total by adding these together: $8 + 2 \times 7$.

Step 2: Draw a skeletal structure with the xenon atom in the center bonded to two iodine atoms. Each bond represents 2 electrons shared between atoms.

Step 3: Subtract the electrons used in bonding from the total valence electrons to find the number of electrons remaining to be placed as lone pairs on the atoms.

Step 4: Assign lone pairs to the iodine atoms first to complete their octets (each iodine needs 8 electrons total, including bonding electrons). Then place any remaining electrons as lone pairs on the xenon atom.

Step 5: Verify that the xenon atom follows the expanded octet rule (it can have more than 8 electrons) and that the total number of electrons used in bonds and lone pairs equals the total valence electrons calculated in Step 1. The best Lewis structure will have xenon with two single bonds to iodine atoms and three lone pairs on xenon.