Answer
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Step 1:I'll solve this step-by-step using molecular geometry and electronegativity principles:
Step 2:: Determine the Lewis Structure
- Total electron count: $$8 + (4 \times 7) = 36$$ valence electrons
- Xenon (Xe) is the central atom - Four fluorine (F) atoms are bonded to Xe - Xe has 8 valence electrons - Each F contributes 7 valence electrons - Xe forms single bonds with each F atom - Xe has two lone pairs of electrons
Step 3:: Identify Molecular Geometry
- Electron geometry is octahedral due to 6 electron domains (4 bonds + 2 lone pairs) - Molecular geometry is square planar - All F atoms are arranged symmetrically around Xe in a square
Step 4:: Analyze Bond Polarity
- Fluorine ($$4.0$$) is much more electronegative than Xenon ($$2.6$$)
- Xe-F bonds are polar due to electronegativity difference - Individual Xe-F bonds have dipole moments
Step 5:: Determine Overall Molecular Polarity
- Despite polar bonds, the square planar geometry results in dipole moment cancellation - Symmetrical arrangement means net dipole moment is zero
Final Answer
XeF^4 is NON-POLAR.
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