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 number of valence electrons for the neutral compound XeF2, and which Lewis structure best represents it?

22 valence electrons; Xe in the center with two single bonds to F atoms and three lone pairs on Xe

18 valence electrons; Xe in the center with two single bonds to F atoms and one lone pair on Xe

16 valence electrons; Xe in the center with two single bonds to F atoms and two lone pairs on Xe

20 valence electrons; Xe in the center with two double bonds to F atoms and two lone pairs on Xe

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Verified step by step guidance

Determine the total number of valence electrons by adding the valence electrons of each atom in the molecule. Xenon (Xe) is a noble gas in group 18, so it has 8 valence electrons. Each fluorine (F) atom is in group 17 and has 7 valence electrons. Since there are two fluorine atoms, multiply 7 by 2 and add to the 8 from xenon: $8 + 2 \times 7$.

Sum the valence electrons to find the total number available for bonding and lone pairs in the molecule: $8 + 14 = 22$ valence electrons.

Draw the Lewis structure by placing xenon in the center (since it is less electronegative and can expand its octet) and connect it to each fluorine atom with a single bond. Each single bond accounts for 2 electrons.

Distribute the remaining electrons as lone pairs to satisfy the octet rule for the fluorine atoms first (each fluorine needs 6 more electrons to complete its octet after the single bond).

Place the remaining electrons as lone pairs on the xenon atom. Since xenon can have an expanded octet, it can accommodate more than 8 electrons. Count the lone pairs on xenon to confirm the structure matches the one with three lone pairs on xenon and two single bonds to fluorine atoms.