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 XeO_4?

XeO_4 has xenon as the central atom, surrounded by four oxygen atoms, each connected by a single bond, with one lone pair on xenon.

XeO_4 has xenon as the central atom, surrounded by four oxygen atoms, each connected by a double bond, with two lone pairs on xenon.

XeO_4 has xenon as the central atom, surrounded by four oxygen atoms, each connected by a double bond, with no lone pairs on xenon.

XeO_4 has xenon as the central atom, surrounded by four oxygen atoms, each connected by a single bond, with two lone pairs on xenon.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons available for bonding in XeO_4. Xenon (Xe) is in group 18 and has 8 valence electrons, and each oxygen (O) atom is in group 16 with 6 valence electrons. Calculate total valence electrons as: $8 + 4 \times 6$.

Step 2: Identify the central atom, which is xenon (Xe), because it is less electronegative and can expand its octet due to available d-orbitals.

Step 3: Connect the four oxygen atoms to xenon with single bonds initially, using 2 electrons per bond. Subtract these bonding electrons from the total valence electrons to find remaining electrons.

Step 4: Distribute the remaining electrons to satisfy the octet rule for oxygen atoms first, then place any leftover electrons on xenon. Check if xenon has an expanded octet and if lone pairs remain on xenon.

Step 5: Consider the possibility of forming double bonds between xenon and oxygen atoms to reduce formal charges and achieve a more stable Lewis structure. Calculate formal charges to confirm the most stable arrangement, which typically results in xenon bonded to four oxygens with double bonds and no lone pairs on xenon.