What do each of the following sets of compounds/ions have in common with each other? See your Lewis structures for Exercises 113 through 116 . a. \(\mathrm{XeCl}_{4}, \mathrm{XeCl}_{2}\) b. \(\mathrm{ICl}_{5}, \mathrm{TeF}_{4}, \mathrm{ICl}_{3}, \mathrm{PCl}_{3}, \mathrm{SCl}_{2}, \mathrm{SeO}_{2}\)

First, we need to draw the Lewis structures for the compounds in each set. The Lewis structures are representations of molecules that show how the valence electrons are arranged around the atoms. a. For the first set, the compounds are \(\mathrm{XeCl}_{4}\) and \(\mathrm{XeCl}_{2}\). Their Lewis structures are: \(\rm{XeCl_4}\): The Xe atom is the central atom, surrounded by four Cl atoms with single bonds. The Xe atom has two lone pairs of electrons as well. \(\rm{XeCl_2}\): The Xe atom is the central atom, surrounded by two Cl atoms with single bonds. The Xe atom has three lone pairs of electrons. b. For the second set, the compounds are \(\mathrm{ICl}_{5}, \mathrm{TeF}_{4}, \mathrm{ICl}_{3}, \mathrm{PCl}_{3}, \mathrm{SCl}_{2},\) and \( \mathrm{SeO}_{2}\). Their Lewis structure is as follows: \(\mathrm{ICl}_{5}\): The I atom is the central atom, surrounded by five Cl atoms with single bonds. The I atom has one lone pair of electrons. \(\mathrm{TeF}_{4}\): The Te atom is the central atom, surrounded by four F atoms with single bonds. The Te atom has one lone pair of electrons. \(\mathrm{ICl}_{3}\): The I atom is the central atom, surrounded by three Cl atoms with single bonds. The I atom has two lone pairs of electrons. \(\mathrm{PCl}_{3}\): The P atom is the central atom, surrounded by three Cl atoms with single bonds. No lone pairs on the P atom. \(\mathrm{SCl}_{2}\): The S atom is the central atom, surrounded by two Cl atoms with single bonds. The S atom has two lone pairs of electrons. \(\mathrm{SeO}_{2}\): The Se atom is the central atom, surrounded by two O atoms with double bonds. The Se atom has two lone pairs of electrons.

Now that we have the Lewis structures, we need to examine them and find any common properties between the compounds in each set. a. In the first set, both \(\mathrm{XeCl}_{4}\) and \(\mathrm{XeCl}_{2}\) have xenon (Xe) as their central atoms, and both have chlorine (Cl) atoms bonded to the central atom. The common property they have is that they are both examples of Xenon-chlorine compounds. b. For the second set, we can see that all of the compounds contain a central atom and bonded atoms around it. In addition, all of these central atoms have lone pairs of electrons. We can also observe that all these molecules have polar bonds, making them polar through dipole parameters.

Now that we have identified the common properties, we can write them down for each set: a. Both \(\mathrm{XeCl}_{4}\) and \(\mathrm{XeCl}_{2}\) are Xenon-chlorine compounds. b. All of the compounds in the second set (\(\mathrm{ICl}_{5}, \mathrm{TeF}_{4}, \mathrm{ICl}_{3}, \mathrm{PCl}_{3}, \mathrm{SCl}_{2}, \mathrm{SeO}_{2}\)) have central atoms with lone pairs of electrons and are polar molecules.