Multiple Choice
Which of the following best describes the molecular polarity of iodine pentafluoride (IF_5)?
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13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Which of the following best describes the molecular polarity of XeF_4?
A
XeF_4 is a nonpolar molecule because its molecular geometry is square planar and the dipoles cancel out.
B
XeF_4 is a polar molecule because its shape is tetrahedral.
C
XeF_4 is a nonpolar molecule because all the atoms are identical.
D
XeF_4 is a polar molecule because it contains polar bonds and lone pairs on the central atom.
Verified step by step guidance1
Identify the central atom and the surrounding atoms in XeF_4. Xenon (Xe) is the central atom bonded to four fluorine (F) atoms.
Determine the number of bonding pairs and lone pairs on the central atom. XeF_4 has 4 bonding pairs and 2 lone pairs on xenon.
Use VSEPR theory to predict the molecular geometry. With 4 bonding pairs and 2 lone pairs, the electron geometry is octahedral, but the molecular shape is square planar because the lone pairs occupy opposite positions.
Analyze the polarity of the bonds and the overall molecule. Each Xe-F bond is polar due to the difference in electronegativity, but the square planar shape causes the dipole moments to cancel out symmetrically.
Conclude that XeF_4 is a nonpolar molecule because its square planar geometry allows the bond dipoles to cancel, resulting in no net dipole moment.
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