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 for XeF_4?

Xe is surrounded by four F atoms and two lone pairs, resulting in a square planar geometry.

Xe is surrounded by four F atoms and no lone pairs, resulting in a tetrahedral geometry.

Xe is surrounded by four F atoms and one lone pair, resulting in a seesaw geometry.

Xe is surrounded by four F atoms and three lone pairs, resulting in a linear geometry.

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Verified step by step guidance

Step 1: Determine the total number of valence electrons for the molecule XeF_4. Xenon (Xe) is a noble gas with 8 valence electrons, and each fluorine (F) atom has 7 valence electrons. Since there are 4 fluorine atoms, multiply 7 by 4 and add to the 8 from xenon: total valence electrons = 8 + (4 \times 7).

Step 2: Draw the skeletal structure with xenon as the central atom bonded to four fluorine atoms. Each Xe-F bond represents 2 electrons.

Step 3: Subtract the electrons used in bonding from the total valence electrons to find the number of remaining electrons. These remaining electrons will be placed as lone pairs on the central atom (Xe) and the fluorine atoms to satisfy the octet rule.

Step 4: Assign lone pairs to the fluorine atoms first to complete their octets (each fluorine needs 3 lone pairs). Then place any remaining lone pairs on the xenon atom.

Step 5: Use the VSEPR theory to determine the molecular geometry. Count the number of bonding pairs (4) and lone pairs on xenon (2) to predict the shape. According to VSEPR, 4 bonding pairs and 2 lone pairs on the central atom result in a square planar geometry.