Final answer:Out of the four given molecules, assuming SF3 should be SF4, SF4 is considered a polar molecule due to its seesaw shape causing a dipole moment, while BF3, SiF4, and XeF4 are nonpolar molecules.Explanation:The question is asking which among the given options is apolar molecule. A molecule is considered polar if it has a net dipole moment, meaning there's an imbalance of electron cloud density that leads to a region of slight positive charge and a region of slight negative charge.Looking at the options, we see that BF3, Boron trihalides, is anon-polar moleculewith a trigonal planar molecular geometry. Hence option A is not a polar molecule.Option B, SF3 is not a typical molecule as sulfur usually forms molecules with an even number of atoms (like SF2, SF4, etc). Interpreting as SF4, it has a see-saw shape and is polar.SiF4, Silicon tetrafluoride (option C) is a nonpolar molecule due to its symmetric tetrahedral shape, so it's not a polar molecule either.Finally, XeF4, Xenon Hexafluoride (option D), is nonpolar as the molecule's structure is square planar resulting in no net dipole moment.Therefore, among the given choices, assuming SF3 as SF4,SF4is the polar molecule.Learn more about Polarity of Molecules here:brainly.com/question/15173422#SPJ11...

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