Multiple Choice
Which of the following best describes the polarity of the molecule BF_3?
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13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
Multiple Choice
Which of the following best describes the molecular polarity of iodine pentafluoride (IF_5)?
A
IF_5 is amphiprotic and can act as both an acid and a base.
B
IF_5 is ionic and therefore does not have molecular polarity.
C
IF_5 is a polar molecule.
D
IF_5 is a nonpolar molecule.
Verified step by step guidance1
Step 1: Determine the molecular geometry of iodine pentafluoride (IF_5). Iodine (I) is the central atom bonded to five fluorine (F) atoms, and there is one lone pair on iodine. This gives IF_5 a square pyramidal shape according to VSEPR theory.
Step 2: Recall that molecular polarity depends on both the polarity of individual bonds and the overall shape of the molecule. Each I-F bond is polar because fluorine is more electronegative than iodine.
Step 3: Analyze the symmetry of the molecule. The square pyramidal shape is asymmetrical due to the lone pair, which means the dipole moments of the I-F bonds do not cancel out completely.
Step 4: Conclude that because the dipole moments do not cancel, IF_5 has a net dipole moment, making it a polar molecule.
Step 5: Understand that the other options are incorrect because IF_5 is not amphiprotic (it does not donate or accept protons), it is a covalent molecule (not ionic), and it is not nonpolar due to its asymmetrical shape and polar bonds.
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