Draw the Lewis structures for \(\mathrm{TeCl}_{4}, \mathrm{ICl}_{5}, \mathrm{PCl}_{5}, \mathrm{KrCl}_{4},\) and \(\mathrm{XeCl}_{2} .\) Which of the compounds exhibit at least one bond angle that is approximately 120 degrees? Which of the compounds exhibit \(d^{2} s p^{3}\) hybridization? Which of the compounds have a square planar molecular structure? Which of the compounds are polar?

First, let's draw the Lewis structure for each compound: - \(\mathrm{TeCl}_{4}\): Te has 6 valence electrons and each Cl has 7 valence electrons. - \(\mathrm{ICl}_{5}\): I has 7 valence electrons and each Cl has 7 valence electrons. - \(\mathrm{PCl}_{5}\): P has 5 valence electrons and each Cl has 7 valence electrons. - \(\mathrm{KrCl}_{4}\): Kr has 8 valence electrons and each Cl has 7 valence electrons. - \(\mathrm{XeCl}_{2}\): Xe has 8 valence electrons and each Cl has 7 valence electrons. After drawing the structures, we can analyze each one in terms of bond angles, hybridization, molecular structure and polarity.

We will now analyze the bond angles and hybridization of each compound: - \(\mathrm{TeCl}_{4}\): Tetrahedral (\(sp^3\) hybridization) with bond angles of approximately 109.5 degrees. - \(\mathrm{ICl}_{5}\): Square pyramid (\(sp^3d\) hybridization) with bond angles of approximately 90 and 180 degrees. - \(\mathrm{PCl}_{5}\): Trigonal bipyramid (\(sp^3d\) hybridization) with bond angles of approximately 90 and 120 degrees. - \(\mathrm{KrCl}_{4}\): Square planar (\(d^2sp^3\) hybridization) with bond angles of approximately 90 and 180 degrees. - \(\mathrm{XeCl}_{2}\): Linear (\(d^2sp^3\) hybridization) with bond angles of approximately 180 degrees.

Here, we list the molecular structure of each compound based on our analysis in step 2: - \(\mathrm{TeCl}_{4}\): Tetrahedral - \(\mathrm{ICl}_{5}\): Square pyramid - \(\mathrm{PCl}_{5}\): Trigonal bipyramid - \(\mathrm{KrCl}_{4}\): Square planar - \(\mathrm{XeCl}_{2}\): Linear

Lastly, let's identify which compounds are polar: - \(\mathrm{TeCl}_{4}\): Polar, due to the presence of lone pairs on Te. - \(\mathrm{ICl}_{5}\): Nonpolar, symmetrical structure that cancels out the polarity of individual I-Cl bonds. - \(\mathrm{PCl}_{5}\): Nonpolar, symmetrical structure that cancels out the polarity of individual P-Cl bonds. - \(\mathrm{KrCl}_{4}\): Nonpolar, symmetrical structure that cancels out the polarity of individual Kr-Cl bonds. - \(\mathrm{XeCl}_{2}\): Nonpolar, symmetrical structure with the polarity of individual Xe-Cl bonds canceling each other out. #Answers# - Compounds with at least one bond angle of approximately 120 degrees: \(\mathrm{PCl}_{5}\). - Compounds with \(d^2sp^3\) hybridization: \(\mathrm{KrCl}_{4}\) and \(\mathrm{XeCl}_{2}\). - Compounds with a square planar molecular structure: \(\mathrm{KrCl}_{4}\). - Polar compounds: \(\mathrm{TeCl}_{4}\).