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 XeF_2?

XeF_2 has a bent molecular geometry with two lone pairs on xenon.

XeF_2 has a linear molecular geometry with three lone pairs on xenon.

XeF_2 has a tetrahedral molecular geometry with one lone pair on xenon.

XeF_2 has a trigonal planar molecular geometry with no lone pairs on xenon.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for XeF_2. Xenon (Xe) is a noble gas with 8 valence electrons, and each fluorine (F) atom has 7 valence electrons. Since there are two fluorine atoms, calculate the total valence electrons as: $8 + 2 \times 7 = 22$ electrons.

Step 2: Draw the skeletal structure with xenon as the central atom bonded to two fluorine atoms. Each Xe-F bond uses 2 electrons, so subtract 4 electrons from the total valence electrons, leaving 18 electrons to be placed as lone pairs.

Step 3: Distribute the remaining 18 electrons as lone pairs around the atoms to satisfy the octet rule. Each fluorine needs 6 more electrons (3 lone pairs) to complete its octet, using 12 electrons total. This leaves 6 electrons to be placed as lone pairs on xenon.

Step 4: Count the number of lone pairs on xenon. The 6 leftover electrons correspond to 3 lone pairs on xenon. So xenon has 3 lone pairs and 2 bonding pairs (from the two Xe-F bonds).

Step 5: Use the VSEPR theory to determine the molecular geometry. With 5 regions of electron density (2 bonding pairs + 3 lone pairs), the electron geometry is trigonal bipyramidal. The molecular shape, considering only bonded atoms, is linear because the three lone pairs occupy equatorial positions, minimizing repulsion, and the two fluorine atoms are opposite each other.