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

After drawing the Lewis structure of SF6, what are the electron domain geometry and molecular geometry around the sulfur atom?

Electron domain geometry: trigonal bipyramidal; Molecular geometry: trigonal bipyramidal

Electron domain geometry: octahedral; Molecular geometry: octahedral

Electron domain geometry: tetrahedral; Molecular geometry: square planar

Electron domain geometry: octahedral; Molecular geometry: square pyramidal

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Verified step by step guidance

Step 1: Draw the Lewis structure of SF6 by counting the total valence electrons. Sulfur (S) has 6 valence electrons, and each fluorine (F) has 7 valence electrons. Since there are 6 fluorines, total valence electrons = 6 (S) + 6 × 7 (F) = 48 electrons.

Step 2: Arrange the sulfur atom in the center and place six fluorine atoms around it. Connect each fluorine to sulfur with a single bond. Each bond accounts for 2 electrons, so 6 bonds use 12 electrons, leaving 36 electrons to be placed as lone pairs on the fluorines.

Step 3: Complete the octets of the fluorine atoms by placing three lone pairs (6 electrons) on each fluorine. This uses all remaining electrons and satisfies the octet rule for fluorine atoms.

Step 4: Determine the electron domain geometry by counting the regions of electron density around the sulfur atom. Since sulfur forms six single bonds and has no lone pairs, there are six electron domains, which corresponds to an octahedral electron domain geometry.

Step 5: Determine the molecular geometry by considering the positions of atoms only (ignoring lone pairs on the central atom). Since there are no lone pairs on sulfur, the molecular geometry is the same as the electron domain geometry, which is octahedral.