What would this be? **Educational Website Content****Question:**Draw the Lewis Structure of the following compounds: SF₄, I₃⁻, BF₃, and NO. Determine which of these compounds have all atoms in the same plane (are flat or planar). Select all that apply.**Options:**- [ ] BF₃- [ ] SF₄- [ ] I₃⁻- [ ] NO**Explanation:**This exercise involves understanding the geometry and Lewis structures of different molecules to identify their planarity. - **BF₃ (Boron Trifluoride):** - Geometry: Trigonal Planar - Planarity: Planar- **SF₄ (Sulfur Tetrafluoride):** - Geometry: Seesaw - Planarity: Not planar due to the presence of a lone pair causing non-planar shape.- **I₃⁻ (Triiodide ion):** - Geometry: Linear - Planarity: Linear and symmetric, thus planar.- **NO (Nitric Oxide):** - Geometry: Linear - Planarity: Mostly planar, though resonance may affect bond angles slightly.**Answer:**Select "BF₃" and "I₃⁻" as these are planar.

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Answered: Draw the Lewis these have all at apply.…

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Draw the Lewis these have all at apply. NO 13 SF4 O BF3

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Answer question d