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 XeCl_4?

XeCl_4 has a central Xe atom with two single bonds to Cl atoms and four lone pairs on Xe.

XeCl_4 has a central Xe atom surrounded by four single bonds to Cl atoms and no lone pairs on Xe.

XeCl_4 has a central Xe atom surrounded by four single bonds to Cl atoms and two lone pairs on Xe.

XeCl_4 has a central Xe atom with four double bonds to Cl atoms and no lone pairs on Xe.

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Verified step by step guidance

Step 1: Identify the central atom and the surrounding atoms in XeCl_4. Xenon (Xe) is the central atom, and it is bonded to four chlorine (Cl) atoms.

Step 2: Determine the total number of valence electrons. Xenon has 8 valence electrons, and each chlorine has 7 valence electrons. For XeCl_4, total valence electrons = 8 (Xe) + 4 × 7 (Cl) = 36 electrons.

Step 3: Draw single bonds between the central Xe atom and each of the four Cl atoms. Each single bond accounts for 2 electrons, so 4 bonds use 8 electrons.

Step 4: Distribute the remaining electrons to satisfy the octet rule for the chlorine atoms first. Each Cl needs 6 more electrons (3 lone pairs) to complete its octet, so 4 × 6 = 24 electrons are used here.

Step 5: Assign the leftover electrons to the central Xe atom as lone pairs. After bonding and filling Cl octets, the remaining electrons form two lone pairs on Xe, consistent with the expanded octet possible for xenon.