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_4?

XeF_4 has a central xenon atom surrounded by four fluorine atoms and no lone pairs on xenon.

XeF_4 has a central xenon atom surrounded by four fluorine atoms and two lone pairs on xenon.

XeF_4 has a central xenon atom surrounded by four fluorine atoms and one lone pair on xenon.

XeF_4 has a central xenon atom surrounded by six fluorine atoms and no 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 XeF_4. Xenon (Xe) is in group 18 and has 8 valence electrons, while each fluorine (F) atom is in group 17 and has 7 valence electrons. Since there are 4 fluorine atoms, multiply 7 by 4 and add to xenon's 8 electrons.

Step 2: Draw the skeletal structure with xenon as the central atom bonded to four fluorine atoms. Each Xe–F bond represents a pair of shared electrons (2 electrons per bond).

Step 3: Subtract the electrons used in bonding from the total valence electrons to find the number of remaining electrons. These leftover electrons will be placed as lone pairs on the atoms, starting with the outer atoms (fluorines) 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. Since xenon is in period 5, it can expand its octet and accommodate more than 8 electrons.

Step 5: Count the number of lone pairs on xenon after placing all electrons. This will help confirm the correct Lewis structure description, which includes the number of fluorine atoms bonded and the number of lone pairs on xenon.