QQuestionChemistry
QuestionChemistry
Of the two compounds, SiF^4 and SF^4, which is polar and which is nonpolar?
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Answer
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Step 1:I'll solve this problem step by step, focusing on molecular geometry and polarity.
Step 2:: Determine the Lewis structure and electron geometry for SiF^4
- Total valence electrons: $$4 + (4 \times 7) = 32$$ electrons
- Silicon (Si) is the central atom - Silicon has 4 valence electrons - Fluorine (F) has 7 valence electrons - Arrangement will be tetrahedral with 4 identical Si-F bonds
Step 3:: Analyze the molecular geometry of SiF^4
- Bond angles are $$109.5^\circ
- Central Si atom has 4 identical F atoms - Molecular geometry is tetrahedral
Step 4:: Analyze bond polarity in SiF^4
- Si-F bonds are polar due to electronegativity difference - Fluorine is much more electronegative than silicon - However, the tetrahedral symmetry causes dipoles to cancel
Step 5:: Determine polarity of SiF^4
- Despite polar bonds, the overall molecule is nonpolar - Symmetrical tetrahedral structure results in net zero dipole moment
Step 6:: Repeat analysis for SF^4
- Total valence electrons: $$6 + (4 \times 7) = 34$$ electrons
- Sulfur (S) is the central atom - Sulfur has 6 valence electrons - Fluorine has 7 valence electrons
Step 7:: Analyze SF^4 molecular geometry
- Central S atom has 4 F atoms - Molecular geometry is see-saw (distorted tetrahedral) - Asymmetric arrangement means unequal dipole cancellation
Step 8:: Determine polarity of SF^4
- S-F bonds are polar - Asymmetric molecular geometry - Net dipole moment exists - SF^4 is polar
Final Answer
- SiF^4: Nonpolar - SF^4: Polar
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