Multiple Choice
Which of the following molecules is polar?
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13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
Multiple Choice
Which of the following best describes the molecular polarity of xenon tetrafluoride (XeF_4)?
A
XeF_4 is a nonpolar molecule because its molecular geometry is square planar, resulting in the cancellation of dipole moments.
B
XeF_4 is a polar molecule due to the presence of lone pairs on xenon.
C
XeF_4 is a polar molecule because the fluorine atoms create a net dipole moment.
D
XeF_4 is nonpolar because it contains only nonpolar bonds.
Verified step by step guidance1
Identify the central atom and the surrounding atoms in the molecule XeF_4. Xenon (Xe) is the central atom bonded to four fluorine (F) atoms.
Determine the number of valence electrons for xenon and fluorine, then draw the Lewis structure of XeF_4, including any lone pairs on the central atom.
Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the molecular geometry of XeF_4. Consider both bonding pairs and lone pairs on xenon to find the shape.
Analyze the molecular geometry to see how the bond dipoles from the Xe-F bonds are arranged. Check if the dipole moments cancel out due to symmetry.
Conclude the overall polarity of XeF_4 based on the geometry and dipole moment analysis, explaining why the molecule is polar or nonpolar.
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