{"id":4816,"date":"2015-08-21T20:23:22","date_gmt":"2015-08-21T20:23:22","guid":{"rendered":"https:\/\/courses.candelalearning.com\/chemistryformajorsxmaster\/?post_type=chapter&p=4816"},"modified":"2016-10-27T17:20:30","modified_gmt":"2016-10-27T17:20:30","slug":"assignment-atomic-structure-and-the-periodic-table","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-fmcc-chem-atoms-first\/chapter\/assignment-atomic-structure-and-the-periodic-table\/","title":{"raw":"Assignment\u2014Atomic Structure and the Periodic Table","rendered":"Assignment\u2014Atomic Structure and the Periodic Table"},"content":{"raw":"To download a copy of the assignment, please click on the link Sample Questions<\/a>.\r\n\r\nAs you work these matter and measurement problems, consider and explain:\r\n
    \r\n \t
  1. What type of question is it?<\/li>\r\n \t
  2. How do you know what type of question it is?<\/li>\r\n \t
  3. What information are you looking for?<\/li>\r\n \t
  4. What information do they give?<\/li>\r\n \t
  5. How will you go about solving this?<\/li>\r\n \t
  6. Show how to solve the problem.<\/li>\r\n \t
  7. Be able to answer for a different reaction, number, set of conditions, etc.<\/li>\r\n<\/ol>\r\n

    Sample Questions<\/h2>\r\n
      \r\n \t
    1. Which form of electromagnetic radiation has the longest wavelengths?<\/li>\r\n \t
    2. A line in the spectrum of atomic mercury has a wavelength of 254 nm. When mercury emits a photon of light at this wavelength, what is the frequency of the light?<\/li>\r\n \t
    3. Consider an atom traveling at 1% of the speed of light. The de Broglie wavelength is found to be 1.46 \u00d7\u00a010\u20133<\/sup> pm. Which element is this?<\/li>\r\n \t
    4. What is the energy of a photon of blue light that has a wavelength of 453 nm?<\/li>\r\n \t
    5. The four lines observed in the visible emission spectrum of hydrogen tell us that:\r\n
        \r\n \t
      1. The hydrogen molecules they came from have the formula H4<\/sub>.<\/li>\r\n \t
      2. We could observe more lines if we had a stronger prism.<\/li>\r\n \t
      3. There are four electrons in an excited hydrogen atom.<\/li>\r\n \t
      4. Only certain energies are allowed for the electron in a hydrogen atom.<\/li>\r\n \t
      5. The spectrum is continuous.For questions 6\u20138, consider the following portion of the energy-level diagram for hydrogen:\r\n\r\n\r\n\r\n\r\n\r\n\r\n
        n<\/i> = 4<\/td>\r\n\u20130.1361 \u00d7 10\u201318<\/sup> J<\/td>\r\n<\/tr>\r\n
        n<\/i> = 3<\/td>\r\n\u20130.2420 \u00d7 10\u201318<\/sup> J<\/td>\r\n<\/tr>\r\n
        n<\/i> = 2<\/td>\r\n\u20130.5445 \u00d7 10\u201318<\/sup> J<\/td>\r\n<\/tr>\r\n
        n<\/i> = 1<\/td>\r\n\u20132.178 \u00d7 10\u201318<\/sup> J<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
      6. For which of the following transitions does the light emitted have the longest wavelength?\r\n
          \r\n \t
        1. n<\/i> = 4 to n<\/i> = 3<\/li>\r\n \t
        2. n<\/i> = 4 to n<\/i> = 2<\/li>\r\n \t
        3. n<\/i> = 4 to n<\/i> = 1<\/li>\r\n \t
        4. n<\/i> = 3 to n<\/i> = 2<\/li>\r\n \t
        5. n<\/i> = 2 to n<\/i> = 1<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
        6. In the hydrogen spectrum, what is the wavelength of light associated with the n<\/i> = 3 to n<\/i> = 1 electron transition?<\/li>\r\n \t
        7. When a hydrogen electron makes a transition from n<\/i> = 3 to n<\/i> = 1, which of the following statements is true<\/em>?\r\n
            \r\n \t
          1. Energy is emitted.<\/li>\r\n \t
          2. Energy is absorbed.<\/li>\r\n \t
          3. The electron loses energy.<\/li>\r\n \t
          4. The electron gains energy.<\/li>\r\n \t
          5. The electron cannot make this transition.<\/li>\r\n<\/ol>\r\n
              \r\n \t
            1. I, IV<\/li>\r\n \t
            2. I, III<\/li>\r\n \t
            3. II, III<\/li>\r\n \t
            4. II, IV<\/li>\r\n \t
            5. V<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
            6. Which of the following is a reasonable criticism of the Bohr model of the atom?\r\n
                \r\n \t
              1. It makes no attempt to explain why the negative electron does not eventually fall into the positive nucleus.<\/li>\r\n \t
              2. It does not adequately predict the line spectrum of hydrogen.<\/li>\r\n \t
              3. It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen.<\/li>\r\n \t
              4. It does not adequately predict the ionization energy of the first energy level electrons for one-electron species for elements other than hydrogen.<\/li>\r\n \t
              5. It shows the electrons to exist outside of the nucleus.<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
              6. The energy of the light emitted when a hydrogen electron goes from n<\/i> = 2 to n<\/i> = 1 is what fraction of its ground-state ionization energy?<\/li>\r\n \t
              7. Which of the following is incorrect<\/em>?\r\n
                  \r\n \t
                1. The emission spectrum of hydrogen contains a continuum of colors.<\/li>\r\n \t
                2. Diffraction produces both constructive and destructive interference.<\/li>\r\n \t
                3. All matter displays both particle and wavelike characteristics.<\/li>\r\n \t
                4. Niels Bohr developed a quantum model for the hydrogen atom.<\/li>\r\n \t
                5. The lowest possible energy state of a molecule or atom is called its ground state.<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
                6. A gamma ray of wavelength 1.00 \u00d7 10\u20138<\/sup> cm has enough energy to remove an electron from a\u00a0hydrogen atom.<\/li>\r\n \t
                7. Which of the following best describes an orbital?\r\n
                    \r\n \t
                  1. space where electrons are unlikely to be found in an atom<\/li>\r\n \t
                  2. space which may contain electrons, protons, and\/or neutrons<\/li>\r\n \t
                  3. the space in an atom where an electron is most likely to be found<\/li>\r\n \t
                  4. small, walled spheres that contain electrons<\/li>\r\n \t
                  5. a single space within an atom that contains all electrons of that atom<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
                  6. How many f<\/i> orbitals have the value n<\/i> = 3?<\/li>\r\n \t
                  7. If n<\/i> = 2, how many orbitals are possible?<\/li>\r\n \t
                  8. Consider the following representation of a 2p<\/i>-orbital:\"Two\r\nWhich of the following statements best describes the movement of electrons in a p<\/i>-orbital?\r\n
                      \r\n \t
                    1. The electrons move along the outer surface of the p<\/i>-orbital, similar to a \u201cfigure 8\u201d type of movement.<\/li>\r\n \t
                    2. The electrons move within the two lobes of the p<\/i>-orbital, but never beyond the outside surface of the orbital.<\/li>\r\n \t
                    3. The electrons are concentrated at the center (node) of the two lobes.<\/li>\r\n \t
                    4. The electrons are only moving in one lobe at any given time.<\/li>\r\n \t
                    5. The electron movement cannot be exactly determined.<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
                    6. How many electrons in an atom can have the quantum numbers n<\/i> = 3, l<\/i> = 2?<\/li>\r\n \t
                    7. How many electrons can be contained in all of the orbitals with n<\/i> = 4?<\/li>\r\n \t
                    8. Which of the following combinations of quantum numbers is not allowed?\r\n
                        \r\n \t
                      1. n<\/i> = 1, l<\/i> = 1, ml<\/sub><\/i> = 0, ms<\/sub><\/i> = 1\/2<\/li>\r\n \t
                      2. n<\/i> = 3, l<\/i> = 0, ml<\/sub><\/i> = 0, ms<\/sub><\/i> = -1\/2<\/li>\r\n \t
                      3. n<\/i> = 2, l<\/i> = 1, ml<\/sub><\/i> = -1, ms<\/sub><\/i> = 1\/2<\/li>\r\n \t
                      4. n<\/i> = 4, l<\/i> = 3, ml<\/sub><\/i> = -2, ms<\/sub><\/i> = -1\/2<\/li>\r\n \t
                      5. n<\/i> = 4, l<\/i> = 2, ml<\/sub><\/i> = 0, ms<\/sub><\/i> = 1\/2<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
                      6. Which of the following atoms or ions has three unpaired electrons?\r\n
                          \r\n \t
                        1. N<\/li>\r\n \t
                        2. O<\/li>\r\n \t
                        3. Al<\/li>\r\n \t
                        4. S2\u2013<\/sup><\/li>\r\n \t
                        5. Ti2+<\/sup><\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
                        6. What is the electron configuration for the barium atom?<\/li>\r\n \t
                        7. What is the complete electron configuration of tin?<\/li>\r\n \t
                        8. Which of the following statements is true<\/em>?\r\n
                            \r\n \t
                          1. The exact location of an electron can be determined if we know its energy.<\/li>\r\n \t
                          2. An electron in a 2s<\/i> orbital can have the same n<\/i>, l<\/i>, and ml<\/i> quantum numbers as an electron in a 3s<\/i> orbital.<\/li>\r\n \t
                          3. Ni has two unpaired electrons in its 3d<\/i> orbitals.<\/li>\r\n \t
                          4. In the buildup of atoms, electrons occupy the 4f<\/i> orbitals before the 6s<\/i> orbitals.<\/li>\r\n \t
                          5. Only three quantum numbers are needed to uniquely describe an electron.<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
                          6. What is the statement that \"the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals\"\u00a0known as?<\/li>\r\n \t
                          7. An element with the electron configuration [Xe] 6s<\/i>2<\/sup>4f<\/i>14<\/sup>5d<\/i>7 would belong to which class on the periodic table?<\/li>\r\n \t
                          8. Ti has __________ in its d orbitals.<\/li>\r\n<\/ol>\r\n[reveal-answer q=\"137847\"]Show Sample Answers[\/reveal-answer]\r\n[hidden-answer a=\"137847\"]\r\n
                              \r\n \t
                            1. radio waves<\/li>\r\n \t
                            2. 1.18 \u00d7 1015<\/sup>s-1<\/sup><\/li>\r\n \t
                            3. Zr<\/li>\r\n \t
                            4. 4.39 \u00d7 10<sup-19 J<\/li>\r\n \t
                            5. D<\/li>\r\n \t
                            6. A<\/li>\r\n \t
                            7. 1.03 \u00d7 10-7<\/sup> m<\/li>\r\n \t
                            8. B<\/li>\r\n \t
                            9. C<\/li>\r\n \t
                            10. 3\/4<\/li>\r\n \t
                            11. A<\/li>\r\n \t
                            12. T<\/li>\r\n \t
                            13. C<\/li>\r\n \t
                            14. 0<\/li>\r\n \t
                            15. 4<\/li>\r\n \t
                            16. E<\/li>\r\n \t
                            17. 10<\/li>\r\n \t
                            18. 32<\/li>\r\n \t
                            19. A<\/li>\r\n \t
                            20. A<\/li>\r\n \t
                            21. [Xe]6s<\/i>2<\/sup><\/li>\r\n \t
                            22. 1s<\/i>2<\/sup>2s<\/i>2<\/sup>2p<\/i>6<\/sup>3s<\/i>2<\/sup>3p<\/i>6<\/sup>4s<\/i>2<\/sup>3d<\/i>10<\/sup>4p<\/i>6<\/sup>5s<\/i>2<\/sup>4d<\/i>10<\/sup>5p<\/i>2<\/sup><\/li>\r\n \t
                            23. C<\/li>\r\n \t
                            24. Hund's rule<\/li>\r\n \t
                            25. transition elements<\/li>\r\n \t
                            26. two electrons<\/li>\r\n<\/ol>\r\n[\/hidden-answer]","rendered":"

                              To download a copy of the assignment, please click on the link Sample Questions<\/a>.<\/p>\n

                              As you work these matter and measurement problems, consider and explain:<\/p>\n

                                \n
                              1. What type of question is it?<\/li>\n
                              2. How do you know what type of question it is?<\/li>\n
                              3. What information are you looking for?<\/li>\n
                              4. What information do they give?<\/li>\n
                              5. How will you go about solving this?<\/li>\n
                              6. Show how to solve the problem.<\/li>\n
                              7. Be able to answer for a different reaction, number, set of conditions, etc.<\/li>\n<\/ol>\n

                                Sample Questions<\/h2>\n
                                  \n
                                1. Which form of electromagnetic radiation has the longest wavelengths?<\/li>\n
                                2. A line in the spectrum of atomic mercury has a wavelength of 254 nm. When mercury emits a photon of light at this wavelength, what is the frequency of the light?<\/li>\n
                                3. Consider an atom traveling at 1% of the speed of light. The de Broglie wavelength is found to be 1.46 \u00d7\u00a010\u20133<\/sup> pm. Which element is this?<\/li>\n
                                4. What is the energy of a photon of blue light that has a wavelength of 453 nm?<\/li>\n
                                5. The four lines observed in the visible emission spectrum of hydrogen tell us that:\n
                                    \n
                                  1. The hydrogen molecules they came from have the formula H4<\/sub>.<\/li>\n
                                  2. We could observe more lines if we had a stronger prism.<\/li>\n
                                  3. There are four electrons in an excited hydrogen atom.<\/li>\n
                                  4. Only certain energies are allowed for the electron in a hydrogen atom.<\/li>\n
                                  5. The spectrum is continuous.For questions 6\u20138, consider the following portion of the energy-level diagram for hydrogen:
                                    \n\n\n\n\n\n\n
                                    n<\/i> = 4<\/td>\n\u20130.1361 \u00d7 10\u201318<\/sup> J<\/td>\n<\/tr>\n
                                    n<\/i> = 3<\/td>\n\u20130.2420 \u00d7 10\u201318<\/sup> J<\/td>\n<\/tr>\n
                                    n<\/i> = 2<\/td>\n\u20130.5445 \u00d7 10\u201318<\/sup> J<\/td>\n<\/tr>\n
                                    n<\/i> = 1<\/td>\n\u20132.178 \u00d7 10\u201318<\/sup> J<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/li>\n<\/ol>\n<\/li>\n
                                  6. For which of the following transitions does the light emitted have the longest wavelength?\n
                                      \n
                                    1. n<\/i> = 4 to n<\/i> = 3<\/li>\n
                                    2. n<\/i> = 4 to n<\/i> = 2<\/li>\n
                                    3. n<\/i> = 4 to n<\/i> = 1<\/li>\n
                                    4. n<\/i> = 3 to n<\/i> = 2<\/li>\n
                                    5. n<\/i> = 2 to n<\/i> = 1<\/li>\n<\/ol>\n<\/li>\n
                                    6. In the hydrogen spectrum, what is the wavelength of light associated with the n<\/i> = 3 to n<\/i> = 1 electron transition?<\/li>\n
                                    7. When a hydrogen electron makes a transition from n<\/i> = 3 to n<\/i> = 1, which of the following statements is true<\/em>?\n
                                        \n
                                      1. Energy is emitted.<\/li>\n
                                      2. Energy is absorbed.<\/li>\n
                                      3. The electron loses energy.<\/li>\n
                                      4. The electron gains energy.<\/li>\n
                                      5. The electron cannot make this transition.<\/li>\n<\/ol>\n
                                          \n
                                        1. I, IV<\/li>\n
                                        2. I, III<\/li>\n
                                        3. II, III<\/li>\n
                                        4. II, IV<\/li>\n
                                        5. V<\/li>\n<\/ol>\n<\/li>\n
                                        6. Which of the following is a reasonable criticism of the Bohr model of the atom?\n
                                            \n
                                          1. It makes no attempt to explain why the negative electron does not eventually fall into the positive nucleus.<\/li>\n
                                          2. It does not adequately predict the line spectrum of hydrogen.<\/li>\n
                                          3. It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen.<\/li>\n
                                          4. It does not adequately predict the ionization energy of the first energy level electrons for one-electron species for elements other than hydrogen.<\/li>\n
                                          5. It shows the electrons to exist outside of the nucleus.<\/li>\n<\/ol>\n<\/li>\n
                                          6. The energy of the light emitted when a hydrogen electron goes from n<\/i> = 2 to n<\/i> = 1 is what fraction of its ground-state ionization energy?<\/li>\n
                                          7. Which of the following is incorrect<\/em>?\n
                                              \n
                                            1. The emission spectrum of hydrogen contains a continuum of colors.<\/li>\n
                                            2. Diffraction produces both constructive and destructive interference.<\/li>\n
                                            3. All matter displays both particle and wavelike characteristics.<\/li>\n
                                            4. Niels Bohr developed a quantum model for the hydrogen atom.<\/li>\n
                                            5. The lowest possible energy state of a molecule or atom is called its ground state.<\/li>\n<\/ol>\n<\/li>\n
                                            6. A gamma ray of wavelength 1.00 \u00d7 10\u20138<\/sup> cm has enough energy to remove an electron from a\u00a0hydrogen atom.<\/li>\n
                                            7. Which of the following best describes an orbital?\n
                                                \n
                                              1. space where electrons are unlikely to be found in an atom<\/li>\n
                                              2. space which may contain electrons, protons, and\/or neutrons<\/li>\n
                                              3. the space in an atom where an electron is most likely to be found<\/li>\n
                                              4. small, walled spheres that contain electrons<\/li>\n
                                              5. a single space within an atom that contains all electrons of that atom<\/li>\n<\/ol>\n<\/li>\n
                                              6. How many f<\/i> orbitals have the value n<\/i> = 3?<\/li>\n
                                              7. If n<\/i> = 2, how many orbitals are possible?<\/li>\n
                                              8. Consider the following representation of a 2p<\/i>-orbital:\"Two
                                                \nWhich of the following statements best describes the movement of electrons in a p<\/i>-orbital?<\/p>\n
                                                  \n
                                                1. The electrons move along the outer surface of the p<\/i>-orbital, similar to a \u201cfigure 8\u201d type of movement.<\/li>\n
                                                2. The electrons move within the two lobes of the p<\/i>-orbital, but never beyond the outside surface of the orbital.<\/li>\n
                                                3. The electrons are concentrated at the center (node) of the two lobes.<\/li>\n
                                                4. The electrons are only moving in one lobe at any given time.<\/li>\n
                                                5. The electron movement cannot be exactly determined.<\/li>\n<\/ol>\n<\/li>\n
                                                6. How many electrons in an atom can have the quantum numbers n<\/i> = 3, l<\/i> = 2?<\/li>\n
                                                7. How many electrons can be contained in all of the orbitals with n<\/i> = 4?<\/li>\n
                                                8. Which of the following combinations of quantum numbers is not allowed?\n
                                                    \n
                                                  1. n<\/i> = 1, l<\/i> = 1, ml<\/sub><\/i> = 0, ms<\/sub><\/i> = 1\/2<\/li>\n
                                                  2. n<\/i> = 3, l<\/i> = 0, ml<\/sub><\/i> = 0, ms<\/sub><\/i> = -1\/2<\/li>\n
                                                  3. n<\/i> = 2, l<\/i> = 1, ml<\/sub><\/i> = -1, ms<\/sub><\/i> = 1\/2<\/li>\n
                                                  4. n<\/i> = 4, l<\/i> = 3, ml<\/sub><\/i> = -2, ms<\/sub><\/i> = -1\/2<\/li>\n
                                                  5. n<\/i> = 4, l<\/i> = 2, ml<\/sub><\/i> = 0, ms<\/sub><\/i> = 1\/2<\/li>\n<\/ol>\n<\/li>\n
                                                  6. Which of the following atoms or ions has three unpaired electrons?\n
                                                      \n
                                                    1. N<\/li>\n
                                                    2. O<\/li>\n
                                                    3. Al<\/li>\n
                                                    4. S2\u2013<\/sup><\/li>\n
                                                    5. Ti2+<\/sup><\/li>\n<\/ol>\n<\/li>\n
                                                    6. What is the electron configuration for the barium atom?<\/li>\n
                                                    7. What is the complete electron configuration of tin?<\/li>\n
                                                    8. Which of the following statements is true<\/em>?\n
                                                        \n
                                                      1. The exact location of an electron can be determined if we know its energy.<\/li>\n
                                                      2. An electron in a 2s<\/i> orbital can have the same n<\/i>, l<\/i>, and ml<\/i> quantum numbers as an electron in a 3s<\/i> orbital.<\/li>\n
                                                      3. Ni has two unpaired electrons in its 3d<\/i> orbitals.<\/li>\n
                                                      4. In the buildup of atoms, electrons occupy the 4f<\/i> orbitals before the 6s<\/i> orbitals.<\/li>\n
                                                      5. Only three quantum numbers are needed to uniquely describe an electron.<\/li>\n<\/ol>\n<\/li>\n
                                                      6. What is the statement that “the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli principle in a particular set of degenerate orbitals”\u00a0known as?<\/li>\n
                                                      7. An element with the electron configuration [Xe] 6s<\/i>2<\/sup>4f<\/i>14<\/sup>5d<\/i>7 would belong to which class on the periodic table?<\/li>\n
                                                      8. Ti has __________ in its d orbitals.<\/li>\n<\/ol>\n
                                                        Show Sample Answers<\/span><\/p>\n
                                                        \n
                                                          \n
                                                        1. radio waves<\/li>\n
                                                        2. 1.18 \u00d7 1015<\/sup>s-1<\/sup><\/li>\n
                                                        3. Zr<\/li>\n
                                                        4. 4.39 \u00d7 10<sup-19 J<\/li>\n
                                                        5. D<\/li>\n
                                                        6. A<\/li>\n
                                                        7. 1.03 \u00d7 10-7<\/sup> m<\/li>\n
                                                        8. B<\/li>\n
                                                        9. C<\/li>\n
                                                        10. 3\/4<\/li>\n
                                                        11. A<\/li>\n
                                                        12. T<\/li>\n
                                                        13. C<\/li>\n
                                                        14. 0<\/li>\n
                                                        15. 4<\/li>\n
                                                        16. E<\/li>\n
                                                        17. 10<\/li>\n
                                                        18. 32<\/li>\n
                                                        19. A<\/li>\n
                                                        20. A<\/li>\n
                                                        21. [Xe]6s<\/i>2<\/sup><\/li>\n
                                                        22. 1s<\/i>2<\/sup>2s<\/i>2<\/sup>2p<\/i>6<\/sup>3s<\/i>2<\/sup>3p<\/i>6<\/sup>4s<\/i>2<\/sup>3d<\/i>10<\/sup>4p<\/i>6<\/sup>5s<\/i>2<\/sup>4d<\/i>10<\/sup>5p<\/i>2<\/sup><\/li>\n
                                                        23. C<\/li>\n
                                                        24. Hund’s rule<\/li>\n
                                                        25. transition elements<\/li>\n
                                                        26. two electrons<\/li>\n<\/ol>\n<\/div>\n<\/div>\n\n\t\t\t
                                                          \n\t\t\t

                                                          Candela Citations<\/h3>\n\t\t\t\t\t
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                                                          \n\t\t\t\t\t\t\t
                                                          CC licensed content, Original<\/div>