Among the given molecules, the correct answer is IF5.
Explanation:
To determine the polarity of a molecule, we need to consider its symmetry and the electronegativity of its constituent atoms. A polar molecule has a net dipole moment due to an uneven distribution of electron density.
– SF6 (Sulfur hexafluoride): This molecule has an octahedral shape, which is highly symmetrical. The bond dipoles cancel each other out, resulting in a nonpolar molecule.
– IF5 (Iodine pentafluoride): This molecule has a square pyramidal shape, which is asymmetric. The bond dipoles do not cancel out, making IF5 a polar molecule.
– PCl5 (Phosphorus pentachloride): Similar to SF6, PCl5 has a trigonal bipyramidal shape and is symmetric, leading to a nonpolar molecule.
– XeF4 (Xenon tetrafluoride): This molecule has a square planar shape, which is also symmetrical. The bond dipoles cancel each other, resulting in a nonpolar molecule.
Therefore, out of the options provided, IF5 is the only polar molecule.