Chapter 9 1. Which of the following are correct statements about the valence–shell electron–pair repulsion (VSEPR) model of bonding? 1. Electron pairs orient themselves to give the smallest angles possible. 2. Only bonding electron pairs are important in the VSEPR model. 3. Electron–pair geometry in all cases describes the spatial geometry of the atoms in the molecule. A. 1 only B. 2 only C. 3 only D. 1, 2, and 3 E. None of the above 2. Which of the following is non–planar? A. SO2 B. SO3 C. SO42− D. NO3− E. BF3 3. The number of bonding pairs of electrons, non–bonding pairs of electrons and molecular shape of the H3O+ ion are Bonding Pairs Non–bonding Pairs Molecular Shape A. 4 0 tetrahedral B. 3 1 tetrahedral C. 2 2 bent D. 3 1 trigonal pyramidal E. 3 0 trigonal planar4. Among the following gaseous molecules BeF2 BF3 CF4 NF3 OF2 What is the correct trend in FMF bond angle? LARGEST SMALLEST A. BeF2 > BF3 > CF4 > NF3 > OF2 B. BeF2 = OF2 > CF4 > BF3 = NF3 C. BeF2 = OF2 > BF3 = NF3 > CF4 D. BeF2 > BF3 > OF2 > NF3 > CF4 E. CF4 > BF3 = NF3 > BeF2 = OF2 5. Which of the following molecules has a trigonal planar structure? 1. CO32− 2. SOCl2 3. H3O+ 4. SO32− A. 1 only B. 1, 2 and 3 C. 1 and 3 D. 1, 3 and 4 E. 3 and 4 6. Which of the following molecules and ions possesses a tetrahedral molecular structure? A. TeI4 B. SeBr4 C. XeCl4 D. NH3 E. AlF4− 7. The bond angles in H2O2 are approximately: A. 90° B. 105° C. 109.5° D. 120° E. 180°8. Identify which of the following bonds is(are) polar and which element in each is the more electronegative. HCl NO Si2 Now consider these five statements about your conclusions. 1. HCl is polar, with H the more electronegative. 2. HCl is polar, with the Cl the more electronegative. 3. NO is polar, with the N the more electronegative. 4. NO is polar, with O the more electronegative. 5. Si2 is polar. The correct statement(s) above is(are) A. 2 only B. 2 and 3 only C. 2 and 4 only D. 2, 3 and 5 only E. 1 and 4 only 9. Consider the following molecules. 1. BF3 2. NH3 3. SOCl2 4. SiF4 Which of these should have a dipole moment? A. 2 only B. 2, 3 and 4 only C. 1, 2 and 3 ony D. 1 and 4 only E. 2 and 3 only 10. Which of the following molecules has the largest dipole moment? A. XeF2 B. XeF4 C. PF5 D. SF4 E. SF611. Which of the following benzene–like molecules do you expect to have the largest dipole moment? A. FFFFClCl B. FHFHHF C. ClClHHHH D. HHHFHF E. HFHFHH 12. Which of the following statements is true? A. There are two π bonds in B. The H–N–H angle in NH3 is slightly larger than the H–C–H angle in CH4. C. In CO2, the carbon is sp2 hybridized. D. The molecule below possesses a dipole moment. E. None of the above statements is true. C CHHH H C C HClC l H13. Which of the following is a correct set of electron–pair geometry, hybridization, and bond angle(s)? Geometry Hybridization Bond Angle(s) A. linear sp2 180° B. trigonal planar sp2 120° C. octahedral d2sp3 60° D. tetrahedral dsp3 109.5° E. trigonal bipyramidal d2sp3 120°, 90° 14. Of the following statements about delocalized bonds, which are true? 1. They occur in molecules with alternating single and double bonds. 2. They can be made from sp2 hybrid σ bonds. 3. They are most often found in bonds involving heavy atoms. 4. They can be made from πbonds. 5. They rarely, if ever, involve bonds with fluorine. A. 1, 4, and 5 only B. 4 and 5 only C. 1, 3, and 4 only D. 1, 2, and 3 only E. All of the above 15. Which of the following statements is incorrect? A. Hybridization accounts for the experimental observation that all F−C−F bond angles in CF4 are the same. B. All C−C bond distances in benzene, C6H6, are the same. C. The energy required to break a carbon–carbon triple bond is greater than that needed to break a carbon–carbon double bond. D. The bonding in benzene, C6H6, includes 12 sigma (σ) bonds and 3 localized pi (π) bonds. E. The π electrons in NO3− are delocalized.BNBNBNHHHHHH16. The following molecule should be used HC1HC2HCC3H The hybridizations of C1, C2 and C3 respectively are C1 C2 C3 A. sp3 sp3 sp2 B. sp3 sp sp2 C. sp3 sp3 sp3 D. dsp3 sp sp2 E. None of the above. 17. Borazine B3N3H6 has been called inorganic benzene. What is the hybridization of the boron atoms? A. sp B. sp2 C. sp3 D. sp4 E.
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