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 best describes the Lewis dot structure for XeF_4 (xenon tetrafluoride)?

Xe at the center with two F atoms bonded to it, and three lone pairs on Xe.

Xe at the center with four F atoms bonded to it, and no lone pairs on Xe.

Xe at the center with four F atoms bonded to it, and one lone pair on Xe.

Xe at the center with four F atoms bonded to it, and two lone pairs on Xe.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for XeF_4. Xenon (Xe) is in group 18 and has 8 valence electrons, and each fluorine (F) atom has 7 valence electrons. Since there are 4 fluorine atoms, calculate the total valence electrons as: $8 + 4 \times 7$.

Step 2: Draw the skeletal structure with xenon (Xe) at the center and four fluorine (F) atoms bonded to it. Each Xe-F bond represents 2 electrons.

Step 3: Subtract the electrons used in bonding from the total valence electrons to find the remaining electrons. These remaining electrons will be placed as lone pairs on the atoms, starting with fluorine atoms to complete their octets.

Step 4: After completing the octets of the fluorine atoms, place any remaining electrons as lone pairs on the central xenon atom. Remember that xenon can have an expanded octet because it is in period 5.

Step 5: Count the lone pairs on xenon after placing all electrons. For XeF_4, xenon will have two lone pairs, which along with the four bonding pairs, gives the correct Lewis structure.