Which of the following statements is(are) true? Correct the false statements. a. The molecules \(\mathrm{SeS}_{3}, \mathrm{SeS}_{2}, \mathrm{PCl}_{5}, \mathrm{TeCl}_{4}, \mathrm{ICl}_{3}\), and \(\mathrm{XeCl}_{2}\) all exhibit at least one bond angle, which is approximately \(120^{\circ}\). b. The bond angle in \(\mathrm{SO}_{2}\) should be similar to the bond angle in \(\mathrm{CS}_{2}\) or \(\mathrm{SCl}_{2}\). c. Of the compounds \(\mathrm{CF}_{4}, \mathrm{KrF}_{4}\), and \(\mathrm{SeF}_{4}\), only \(\mathrm{SeF}_{4}\) exhibits an overall dipole moment (is polar). d. Central atoms in a molecule adopt a geometry of the bonded atoms and lone pairs about the central atom in order to maximize electron repulsions.

First, let's find the molecular geometries and bond angles for each molecule mentioned in statement a: 1. \(\mathrm{SeS}_{3}\): The central atom Se has 3 bonding regions (3 S atoms) and 1 lone pair. Therefore, its molecular geometry is trigonal pyramidal, and it has a bond angle of approximately \(109.5^{\circ}\). 2. \(\mathrm{SeS}_{2}\): The central atom Se has 2 bonding regions (2 S atoms) and 1 lone pair. Therefore, its molecular geometry is bent, and it has a bond angle of less than \(120^{\circ}\). 3. \(\mathrm{PCl}_{5}\): The central atom P has 5 bonding regions (5 Cl atoms) and no lone pairs. Therefore, its molecular geometry is trigonal bipyramidal, and it has a bond angle of \(120^{\circ}\) and \(90^{\circ}\). 4. \(\mathrm{TeCl}_{4}\): The central atom Te has 4 bonding regions (4 Cl atoms) and no lone pairs. Therefore, its molecular geometry is tetrahedral, and it has a bond angle of approximately \(109.5^{\circ}\). 5. \(\mathrm{ICl}_{3}\): The central atom I has 3 bonding regions (3 Cl atoms) and 2 lone pairs. Therefore, its molecular geometry is T-shaped, and it has a bond angle of approximately \(120^{\circ}\). 6. \(\mathrm{XeCl}_{2}\): The central atom Xe has 2 bonding regions (2 Cl atoms) and 3 lone pairs. Therefore, its molecular geometry is linear, and it has a bond angle of \(180^{\circ}\). Among the given molecules, only \(\mathrm{PCl}_{5}\) and \(\mathrm{ICl}_{3}\) exhibit a bond angle of approximately \(120^{\circ}\). So, statement a is false.

Now, let's compare the bond angles of \(\mathrm{SO}_{2}\), \(\mathrm{CS}_{2}\), and \(\mathrm{SCl}_{2}\): 1. \(\mathrm{SO}_{2}\): The central atom S has 2 bonding regions (2 O atoms) and 1 lone pair. Therefore, its molecular geometry is bent, and it has a bond angle of less than \(120^{\circ}\). 2. \(\mathrm{CS}_{2}\): The central atom C has 2 bonding regions (2 S atoms) and no lone pairs. Therefore, its molecular geometry is linear, and it has a bond angle of \(180^{\circ}\). 3. \(\mathrm{SCl}_{2}\): The central atom S has 2 bonding regions (2 Cl atoms) and 1 lone pair. Therefore, its molecular geometry is bent, and it has a bond angle of less than \(120^{\circ}\). The bond angle in \(\mathrm{SO}_{2}\) is similar to the bond angle in \(\mathrm{SCl}_{2}\) but not to the bond angle in \(\mathrm{CS}_{2}\). Therefore, statement b is false.

To analyze the overall dipole moments of \(\mathrm{CF}_{4}\), \(\mathrm{KrF}_{4}\), and \(\mathrm{SeF}_{4}\), we should first analyze their molecular geometries: 1. \(\mathrm{CF}_{4}\): The central atom C has 4 bonding regions (4 F atoms) and no lone pairs. Therefore, its molecular geometry is tetrahedral, and it is a nonpolar molecule. 2. \(\mathrm{KrF}_{4}\): The central atom Kr has 4 bonding regions (4 F atoms) and 2 lone pairs. Therefore, its molecular geometry is square planar, and it is a nonpolar molecule. 3. \(\mathrm{SeF}_{4}\): The central atom Se has 4 bonding regions (4 F atoms) and 1 lone pair. Therefore, its molecular geometry is seesaw, and it is a polar molecule. Statement c is true, as only \(\mathrm{SeF}_{4}\) exhibits an overall dipole moment.

The VSEPR theory is based on the idea that electron pairs around a central atom repel each other and arrange themselves to minimize these repulsions, which determines the molecular geometry. Thus, statement d is true.