{"id":7541,"date":"2021-06-08T21:56:42","date_gmt":"2021-06-08T21:56:42","guid":{"rendered":"https:\/\/opentextbc.ca\/introductorychemistry\/chapter\/end-of-chapter-9-material\/"},"modified":"2021-10-04T16:20:21","modified_gmt":"2021-10-04T16:20:21","slug":"end-of-chapter-9-material","status":"publish","type":"chapter","link":"https:\/\/opentextbc.ca\/introductorychemistry\/chapter\/end-of-chapter-9-material\/","title":{"raw":"End-of-Chapter Material","rendered":"End-of-Chapter Material"},"content":{"raw":"[latexpage]\r\n
\r\n

Additional Exercises<\/p>\r\n\r\n<\/header>\r\n

\r\n
    \r\n \t
  1. Explain why iron and copper have the same Lewis electron dot diagram when they have different numbers of electrons.<\/li>\r\n \t
  2. Name two ions with the same Lewis electron dot diagram as the Cl\u2212<\/sup> ion.<\/li>\r\n \t
  3. Based on the known trends, what ionic compound from the first column of the periodic table and the next-to-last column of the periodic table should have the highest lattice energy?<\/li>\r\n \t
  4. Based on the known trends, what ionic compound from the first column of the periodic table and the next-to-last column of the periodic table should have the lowest lattice energy?<\/li>\r\n \t
  5. P2<\/sub> is not a stable form of phosphorus, but if it were, what would be its likely Lewis electron dot diagram?<\/li>\r\n \t
  6. Se2<\/sub> is not a stable form of selenium, but if it were, what would be its likely Lewis electron dot diagram?<\/li>\r\n \t
  7. What are the Lewis electron dot diagrams of SO2<\/sub>, SO3<\/sub>, and SO4<\/sub>2\u2212<\/sup>?<\/li>\r\n \t
  8. What are the Lewis electron dot diagrams of PO3<\/sub>3\u2212<\/sup> and PO4<\/sub>3\u2212<\/sup>?<\/li>\r\n \t
  9. Which bond do you expect to be more polar: an O\u2013H bond or an N\u2013H bond?<\/li>\r\n \t
  10. Which bond do you expect to be more polar: an O\u2013F bond or an S\u2013O bond?<\/li>\r\n \t
  11. Use bond energies to estimate the energy change of this reaction.\r\n

    C3<\/sub>H8<\/sub> + 5O2<\/sub> \u2192 3CO2<\/sub> + 4H2<\/sub>O<\/p>\r\n<\/li>\r\n \t

  12. Use bond energies to estimate the energy change of this reaction.\r\n

    N2<\/sub>H4<\/sub> +\u00a0O2<\/sub> \u2192\u00a0N2<\/sub> + 2H2<\/sub>O<\/p>\r\n<\/li>\r\n \t

  13. Ethylene (C2<\/sub>H4<\/sub>) has two central atoms. Determine the geometry around each central atom and the shape of the overall molecule.<\/li>\r\n \t
  14. Hydrogen peroxide (H2<\/sub>O2<\/sub>) has two central atoms. Determine the geometry around each central atom and the shape of the overall molecule.<\/li>\r\n \t
  15. Determine the molecular dipole moments for the following molecules:\r\n

    \"dipole_moment_questions\"<\/p>\r\n<\/li>\r\n \t

  16. What is the hybridization in the central atom of:\r\n
      \r\n \t
    1. HCN<\/li>\r\n \t
    2. NH4<\/sub><\/li>\r\n \t
    3. TeBr2<\/sub><\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
    4. Draw the molecular orbital electron configuration energy diagram of He2<\/sub>\u00a0and determine the bond order.<\/li>\r\n \t
    5. Draw the molecular orbital electron configuration energy diagram of O2<\/sub>\u00a0and determine the bond order.<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n
      \r\n

      Answers<\/p>\r\n\r\n<\/header>\r\n

      \r\n
        \r\n \t
      1. Iron has d<\/em> electrons that typically are not shown on Lewis electron dot diagrams.<\/li>\r\n<\/ol>\r\n
          \r\n \t
        1. LiF<\/li>\r\n<\/ol>\r\n
            \r\n \t
          1. It would be like N2<\/sub>:\r\n

            [latex]\\chemfig{\\Lewis{4:,P}~\\Lewis{0:,P}}[\/latex]<\/p>\r\n<\/li>\r\n<\/ol>\r\n

              \r\n \t
            1. [latex]\\chemfig{\\Lewis{2:4:,O}=\\Lewis{6:,S}=\\Lewis{0:6:,O}}, \\chemfig{\\Lewis{4:6:,O}=[:30]S(=[:90]\\Lewis{0:2:,O})=[:-30]\\Lewis{0:6:,O}},\\text{ and }\\chemfig{\\Lewis{2:4:6:,O}-\\ce{S^{2-}}(=[:90]\\Lewis{0:4:,O})(=[:-90]\\Lewis{0:4:,O})-\\Lewis{0:2:6:,O}}[\/latex]<\/li>\r\n<\/ol>\r\n
                \r\n \t
              1. an O\u2013H bond<\/li>\r\n<\/ol>\r\n
                  \r\n \t
                1. \u22122,000 kJ<\/li>\r\n<\/ol>\r\n
                    \r\n \t
                  1. trigonal planar about both central C atoms<\/li>\r\n<\/ol>\r\n
                      \r\n \t
                    1. \"dipole_moment_solutions\"<\/li>\r\n<\/ol>\r\n
                        \r\n \t
                      1. \"He2_MO_config_001\"\r\nbond order = 0<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>","rendered":"
                        \n
                        \n

                        Additional Exercises<\/p>\n<\/header>\n

                        \n
                          \n
                        1. Explain why iron and copper have the same Lewis electron dot diagram when they have different numbers of electrons.<\/li>\n
                        2. Name two ions with the same Lewis electron dot diagram as the Cl\u2212<\/sup> ion.<\/li>\n
                        3. Based on the known trends, what ionic compound from the first column of the periodic table and the next-to-last column of the periodic table should have the highest lattice energy?<\/li>\n
                        4. Based on the known trends, what ionic compound from the first column of the periodic table and the next-to-last column of the periodic table should have the lowest lattice energy?<\/li>\n
                        5. P2<\/sub> is not a stable form of phosphorus, but if it were, what would be its likely Lewis electron dot diagram?<\/li>\n
                        6. Se2<\/sub> is not a stable form of selenium, but if it were, what would be its likely Lewis electron dot diagram?<\/li>\n
                        7. What are the Lewis electron dot diagrams of SO2<\/sub>, SO3<\/sub>, and SO4<\/sub>2\u2212<\/sup>?<\/li>\n
                        8. What are the Lewis electron dot diagrams of PO3<\/sub>3\u2212<\/sup> and PO4<\/sub>3\u2212<\/sup>?<\/li>\n
                        9. Which bond do you expect to be more polar: an O\u2013H bond or an N\u2013H bond?<\/li>\n
                        10. Which bond do you expect to be more polar: an O\u2013F bond or an S\u2013O bond?<\/li>\n
                        11. Use bond energies to estimate the energy change of this reaction.\n

                          C3<\/sub>H8<\/sub> + 5O2<\/sub> \u2192 3CO2<\/sub> + 4H2<\/sub>O<\/p>\n<\/li>\n

                        12. Use bond energies to estimate the energy change of this reaction.\n

                          N2<\/sub>H4<\/sub> +\u00a0O2<\/sub> \u2192\u00a0N2<\/sub> + 2H2<\/sub>O<\/p>\n<\/li>\n

                        13. Ethylene (C2<\/sub>H4<\/sub>) has two central atoms. Determine the geometry around each central atom and the shape of the overall molecule.<\/li>\n
                        14. Hydrogen peroxide (H2<\/sub>O2<\/sub>) has two central atoms. Determine the geometry around each central atom and the shape of the overall molecule.<\/li>\n
                        15. Determine the molecular dipole moments for the following molecules:\n

                          \"dipole_moment_questions\"<\/p>\n<\/li>\n

                        16. What is the hybridization in the central atom of:\n
                            \n
                          1. HCN<\/li>\n
                          2. NH4<\/sub><\/li>\n
                          3. TeBr2<\/sub><\/li>\n<\/ol>\n<\/li>\n
                          4. Draw the molecular orbital electron configuration energy diagram of He2<\/sub>\u00a0and determine the bond order.<\/li>\n
                          5. Draw the molecular orbital electron configuration energy diagram of O2<\/sub>\u00a0and determine the bond order.<\/li>\n<\/ol>\n<\/div>\n<\/div>\n
                            \n
                            \n

                            Answers<\/p>\n<\/header>\n

                            \n
                              \n
                            1. Iron has d<\/em> electrons that typically are not shown on Lewis electron dot diagrams.<\/li>\n<\/ol>\n
                                \n
                              1. LiF<\/li>\n<\/ol>\n
                                  \n
                                1. It would be like N2<\/sub>:\n

                                  \"\chemfig{\Lewis{4:,P}~\Lewis{0:,P}}\"<\/p>\n<\/li>\n<\/ol>\n

                                    \n
                                  1. \"\chemfig{\Lewis{2:4:,O}=\Lewis{6:,S}=\Lewis{0:6:,O}}, \chemfig{\Lewis{4:6:,O}=[:30]S(=[:90]\Lewis{0:2:,O})=[:-30]\Lewis{0:6:,O}},\text{ and }\chemfig{\Lewis{2:4:6:,O}-\ce{S^{2-}}(=[:90]\Lewis{0:4:,O})(=[:-90]\Lewis{0:4:,O})-\Lewis{0:2:6:,O}}\"<\/li>\n<\/ol>\n
                                      \n
                                    1. an O\u2013H bond<\/li>\n<\/ol>\n
                                        \n
                                      1. \u22122,000 kJ<\/li>\n<\/ol>\n
                                          \n
                                        1. trigonal planar about both central C atoms<\/li>\n<\/ol>\n
                                            \n
                                          1. \"dipole_moment_solutions\"<\/li>\n<\/ol>\n
                                              \n
                                            1. \"He2_MO_config_001\"
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