Write the relevant information on the table. How many holes will the central atom require to Build the indicated models and sketch a 3-D accommodate the hybridized orbitals? representation of them in the table. Molecule PCl Lewis Structure [6N+ 2] - [VE] = Model VSEPR structure 1) Would you expect phosphorus pentachloride to be a polar molecule? Explain why or why not. If so, indicate its molecular dipole in the table. 2) The structure of sulfur tetrafluoride is different from that of phosphorus pentachloride in that it has a lone pair. Electrons arrange themselves in such a way to minimize repulsion between the electron groups, and lone pairs of electrons experience more repulsion than bonding electron groups. With this in mind, which position should the lone pair of electrons occupy, axial or equatorial? Why? Molecule SF4 Lewis Structure [6N+2]-[VE] = Model VSEPR structure 3) Would you expect sulfur tetrafluoride to be polar? Explain why or why not. If so, indicate its molecular dipole in the table. 4) Draw the hybridization scheme for sulfur tetrafluoride. 5) Chlorine trifluoride has two sets of lone pairs of electrons. Which position should the lone pair of electrons occupy, axial or equatorial? Why? Molecule Lewis Structure [6N+ 2]-[VE] = CIF3 Model VSEPR structure 6) Would you expect chlorine trifluoride to be polar? Explain why or why not. If so, indicate its molecular dipole in the table. 7) Write the bonding scheme for chlorine trifluoride. 8) Xenon difluoride has three sets of lone pairs of electrons. Which position should the lone pair of electrons occupy, axial or equatorial? Why? Molecule XeF2 Lewis Structure [6N+ 2]-[VE] = Model VSEPR structure 9) Would you expect xenon difluoride to be polar? Explain why or why not. If so, indicate its molecular dipole in the table.