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Inorganic Chemistry
- Which of the following statements is/are true? Correct the false statements. a. The molecules SeS3. SeS2, PCl5, TeCl4, ICl3, and XeCl2 all exhibit at least one bond angle which is approximately 120. b. The bond angle in SO2 should be similar to the bond angle in CS2 or SCI2. c. Of the compounds CF4, KrF4, and SeF4, only SeF4 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.arrow_forwardWhat are the bond angles predicted by the VSEPR model about the carbon atom in the formate ion, HCO2? Considering that the bonds to this atom are not identical, would you expect the experimental values to agree precisely with the VSEPR values? How might they differ?arrow_forwardA compound of chlorine and fluorine, CIFx, reacts at about 75C with uranium to produce uranium hexafluoride and chlorine fluoride, CIF. A certain amount of uranium produced 5.63 g of uranium hexafluoride and 457 mL of chlorine fluoride at 75C and 3.00 atm. What is x? Describe the geometry, polarity, and bond angles of the compound and the hybridization of chlorine. How many sigma and pi bonds are there?arrow_forward
- What are the relationships among bond order, bond energy, and bond length? Which of these quantities can be measured?arrow_forwardExplain in terms of bonding theory why all atoms of H2CCCCH2 must lie in the same plane.arrow_forwardTwo variations of the octahedral geometry (see Table 4-1) are illustrated below. Which of the compounds/ions Br3, ClF3, XeF4, SF4, PF5, ClF5, and SF6 have these molecular structures?arrow_forward
- Which of the following statements is(are) true? Correct the false statements. a.The molecules SeS3, SeS2, PCl5, TeCl4, ICl3, and XeCl2 all exhibit at least one bond angle, which is approximately 120. b.The bond angle in SO2 should be similar to the bond angle in CS2 or SCl2. c.Of the compounds CF4, KrF4, and SeF4, only SeF4 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.arrow_forwardSketch the resonance structures for the nitrite ion, NO2. Describe the electron-pair and molecular geometries of the ion. From these geometries, decide on the OMO bond angle, the average NO bond order, and the N atom hybridization.arrow_forwardWhat hybridization is required for central atoms exhibiting trigonal bipyramidal geometry? Octahedral geometry? Describe the bonding of PF5, SF4, SF6, and IF5, using the localized electron model.arrow_forward
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