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 best describes the Lewis dot structure of XeBr2Cl2?

Xe is the central atom with two Br and two Cl atoms bonded to it, and one lone pair on Xe, resulting in a trigonal bipyramidal geometry.

Xe is the central atom with one Br and three Cl atoms bonded to it, and one lone pair on Xe, resulting in a seesaw geometry.

Xe is the central atom with two Br and two Cl atoms bonded to it, and no lone pairs on Xe, resulting in a tetrahedral geometry.

Xe is the central atom with two Br and two Cl atoms bonded to it, and two lone pairs on Xe, resulting in a square planar geometry.

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Verified step by step guidance

Identify the central atom in the molecule, which is Xenon (Xe) because it is the least electronegative and can expand its octet due to being a noble gas in period 5.

Count the total number of valence electrons: Xe has 8 valence electrons, each Br has 7, and each Cl has 7. For XeBr2Cl2, calculate total valence electrons as 8 + 2×7 + 2×7.

Determine the number of electron pairs around Xe by dividing the total valence electrons by 2, then subtract the bonding pairs (4 bonds to halogens) to find the number of lone pairs on Xe.

Use the VSEPR theory to predict the molecular geometry: with 4 bonded atoms and 2 lone pairs, the electron pair geometry is octahedral, but the molecular shape (considering only atoms) is square planar.

Confirm that the Lewis structure has Xe at the center bonded to two Br and two Cl atoms, with two lone pairs on Xe, resulting in a square planar geometry.