QQuestionChemistry
QuestionChemistry
Draw the Lewis structure for the SF₄ and SF₆ molecules and determine if each molecule is polar or nonpolar.
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Answer
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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Determine the number of valence electrons for SF₄
- Total valence electrons for SF₆: $$6 + (7 \times 6) = 48$$ electrons
- Sulfur (S): 6 valence electrons - Fluorine (F): 7 valence electrons × 4 (for SF₄) or 6 (for SF₆)
Step 3:: Lewis Structure for SF₄
- Central sulfur atom - Place 4 fluorine atoms around sulfur - Distribute remaining electrons as lone pairs - Sulfur will have 2 lone pairs - Lewis structure arrangement: \begin{array}{c} \text{F} \ \text{F-S-F} \ \text{F} \end{array}
Step 4:: Molecular Geometry for SF₄
- Electron domain geometry: Trigonal bipyramidal - Molecular geometry: See-saw - Two lone pairs occupy equatorial positions
Step 5:: Polarity Analysis for SF₄
- Asymmetric molecular geometry - Unequal distribution of electron density - Molecular is POLAR
Step 6:: Lewis Structure for SF₆
- Central sulfur atom - 6 fluorine atoms surrounding sulfur - Distribute remaining electrons - No lone pairs on central sulfur - Symmetric octahedral structure \begin{array}{c} \text{Symmetric SF}_6 \text{ structure} \end{array}
Step 7:: Molecular Geometry for SF₆
- Electron domain geometry: Octahedral - Molecular geometry: Octahedral - Perfectly symmetric arrangement
Step 8:: Polarity Analysis for SF₆
- Symmetric molecular geometry - Uniform electron distribution - Molecular is NONPOLAR
Final Answer
- SF₄: Polar molecule - SF₆: Nonpolar molecule
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