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1 of 9 /8/0 :40 PM Assignment 3 (468740) Question Question DetailsChang9 7.EOCP.. [70794] An electron in a hydrogen atom is excited from the ground state to the n = 4 state. Comment on the correctness of the following statements (/). (a) n = 4 is the first excited state. (b) It takes more energy to ionize (remove) the electron from n = 4 than from the ground state. (c) The electron is farther from the nucleus (on average) in n = 4 than in the ground state. (d) The wavelength of light emitted when the electron drops from n = 4 to n = is longer than that from n = 4 to n =. (e) The wavelength the atom absorbs in going from n = to n = 4 is the same as that emitted as it goes from n = 4 to n =.. Question DetailsLairdUChem.TB.04. [9473] Which of the following sets of quantum numbers is not possible? (Select all that apply.) n:, l: 0, m l :, m s : -/ n: 3, l: 0, m l :0, ms : +/ n:, l: 0, m l:0, ms: -/ n: 3, l: 0, m l :, m s: -/ n: 4, l: 0, m l :-, ms: +/ 3. Question DetailsLairdUChem.TB.06. [94735] What is the maximum number of electrons in a atom that can have the following set of quantum numbers? n = 4 l = 3 m l = - m s = +/ Question DetailsLairdUChem.TB.07. [9477] A possible set of quantum numbers for the last electron added to complete an atom of gallium Ga in its ground state is: n: 4, l: 0, m l :0, ms: -/ n: 3, l: 0, m l :, ms : +/ n: 3, l:, m l :0, ms : -/ n: 4, l:, m l :0, ms: +/ 5. Question DetailsLairdUChem.TB.03. [94744] How many orbitals are allowed in a subshell if the angular momentum quantum number for electrons in that subshell is 3?
2 of 9 /8/0 :40 PM Question DetailsLairdUChem.EOCP.045. [94700] Calculate the total number of electrons that can occupy the following orbitals. (a) one s orbital (b) three p orbitals (c) five d orbitals (d) seven f orbitals one three five six two six nine seven three nine ten twelve six twelve fifteen fourteen 7. Question DetailsLairdUChem.EOCP.005. [03650] The atomic number of an element is 73. Is this element diamagnetic or paramagnetic? paramagnetic diamagnetic 8. Question DetailsLairdUChem.EOCP.0. [03640] Write the ground-state electron configurations for the following elements. Zn [Ar] 4s Sn [Kr] 5s 4d 5p Na [Ne] 3s Hg [Xe] 4f 4 5d 6s Br [Ar] 4s 4p 5 Ni [Ar] 4s 8 9. Question DetailsLairdUChem.EOCP.0. [03643] Write the ground-state electron configurations for the following elements.
3 3 of 9 /8/0 :40 PM (a) I [Kr] 5s 4d 5p 5 (b) Se [Ar] 4s 4p 4 (c) Cs [Xe] 6s (d) Si [Ne] 3s 3p (e) Fe [Ar] 4s 6 (f) Zr [Kr] 4d 5s. Question DetailsLairdUChem.EOCP.056. [03648] The electron configurations described in this chapter all refer to gaseous atoms in their ground states. An atom may absorb a quantum of energy and promote one of its electrons to a higher-energy orbital. When this happens, we say that the atom is in an excited state. The electron configurations of some excited atoms are given. Identify these atoms and write their ground-state configurations. (a) s s name helium -or- He ground state configuration [He] (b) s s p name nitrogen -or- N ground state configuration [He] s p 3 (c) s s p 6 4s name sodium -or- Na ground state configuration [Ne] 3s (d) [Ar]4s 4p 4 name arsenic -or- As
4 4 of 9 /8/0 :40 PM ground state configuration [Ar] 4s 4p 3. Question DetailsLairdUChem.PracticeEx.07. [6367] Practice Exercise.7 (a) Which of the following atoms should have a larger first ionization energy: O or S? O (b) Which of the following atoms should have a smaller second ionization energy: Fr or Ra? Ra HINTS I'm Stuck. Question DetailsLairdUChem.Supp.3-0. [9546] Which of the following is the electronic configuration for a chlorine atom? s s p 6 3s 3p 6 s s p 6 3s 3p 5 s s p 6 3s 3p 6 4s 4p 5 s s p 6 3s 3p 4 This is the only configuration that has precisely 7 electrons. 3. Question DetailsLairdUChem.Supp [95493] The electronic configurations for a sodium atom is s s p 6 3s 3p 6 4s s s p 6 3s s s p 6 3s s s p 5 3s Both s s p 6 3s 3p 6 4s and s s p 6 3s have single electrons in the outer shell, but only B has electrons. 4. Question DetailsLairdUChem.Supp.4-0. [9563] Select the equation that depicts the first ionization of calcium. Ca (g) Ca + (g) + e - Ca + (g) Ca (g) Ca (g) Ca - + e - Ca (g) + e - Ca - (g) Ionization energy is the amount of energy required to remove one electron from a neutral gaseous atom. 5. Question DetailsLairdUChem.Supp [95338] Select the equation that depicts the second ionization of calcium. Ca + (g) + e - Ca (g) Ca (g) Ca + (g) + e - Ca + (g) + e - Ca + (g) Ca + (g) Ca + (g) + e - The second ionization energy is the energy associated with the loss of an electron by a gaseous + ion. 6. Question DetailsLairdUChem.Supp [9504] Which of the following lists the six elements in order of increasing first ionization energy?
5 5 of 9 /8/0 :40 PM Li < B < Be < C < O < N Li < B < Be < C < N < O Li < Be < B < C < O < N Li < Be < B < C < N < O Ionization energy varies across a period with specfic irregularites due to electron configurations. 7. Question DetailsLairdUChem.Supp [95568] Which of the elements below has the lowest ionization energy? Na Be K Cl Generally, the element that is farthest left and lowest on the table has the lowest ionization energy. 8. Question DetailsLairdUChem.Supp [9575] Which of the elements below has the lowest ionization energy? Na K Li Rb Generally, the element that is farthest left and lowest on the table has the lowest ionization energy. 9. Question DetailsLairdUChem.Supp [9594] Which of the elements below would demonstrate a large jump in ionization energy between the third and fourth ionization energies? Si Mg Rb Al Aluminum likes to lose three electrons; once these are gone, the removal of a fourth electron requires a lot of energy. Sodium and Magnesium would lose one and two electrons, respectively, and would resist losing any more. Silicon can lose up to four electrons, so we would not expect a big jump between four and five. 0. Question DetailsLairdUChem.Supp.4-. [9504] The amount of energy associated with completely removing a single electron from a gaseous atom in its ground state is the electron affinity. first ionization energy. electronic discharge energy. ionic charge. Ionization energy is the energy required to remove an electron from a neutral gaseous atom.. Question DetailsLairdUChem.Supp.4-3. [95869] The energy required to remove the least tightly-held electrons from a mole of gaseous atoms is called the
6 6 of 9 /8/0 :40 PM ionic charge. electron affinity. electronegativity. ionization energy. Ionization energy has units of kj/mol.. Question DetailsLairdUChem.TB.09. [953688] How many valence electrons does a carbon atom have? Question DetailsLairdUChem.TB.00. [9573] How many valence electrons does a tin (Sn) atom have? Question DetailsLairdUChem.TB.0. [95369] How many electrons are in the 4p orbitals of selenium? Question DetailsLairdUChem.TB.055. [95373] Which element will display an unusually large jump in ionization energy values between I 3 and I4, its third and fourth ionization energies? Na Al P Si Mg 6. Question DetailsLairdUChem.TB.058. [95757] Which of the elements listed below has the following pattern for its first six ionization energies? (I = first ionization energy, I = second ionization energy, etc.)
7 7 of 9 /8/0 :40 PM Al Se Si Ca P 7. Question DetailsLairdUChem.TB.083. [953303] For Mg atoms a very large jump in the magnitudes of the ionization energies will occur between the second and the third ionization energies. True False 8. Question DetailsChang9 7.EOCP.4. [7088] Shown below are portions of orbital diagrams representing the ground-state electron configurations of certain elements. Which of them violate the Pauli exclusion principle? Which of them violate Hund's rule? (a) (b) (c) (d) (e)
8 8 of 9 /8/0 :40 PM (f) 9. Question DetailsBurdgeChem 6.EOCP.090. [4604] Use the Aufbau principle to obtain the ground-state electron configuration of cadmium. [Kr] 5s 4d 30. Question DetailsBurdgeChem 6.TB.0. [45558] Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by E n = J(/n ).07-9 J.5-8 J.04-8 J J.9 5 J 3. Question DetailsBurdgeChem 6.TB.0. [4473] Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen E n = J(/n ) /s /s.74 4 /s /s.8-9 /s 3. Question DetailsBurdgeChem 6.TB.05. [4550] The second line of the Balmer series occurs at a wavelength of 486. nm. What is the energy difference between the initial and final levels of the hydrogen atom in this emission process? J.44 8 J J J J 33. Question DetailsBurdgeChem 6.TB.039. [4678] Which element has the following ground-state electron configuration? [Kr]5s 4d 5p 3
9 9 of 9 /8/0 :40 PM Sb Sn Te Pb Bi 34. Question DetailsBurdgeChem 6.TB.06. [45908] Each shell (principal energy level) of quantum number n contains n subshells. True False 35. Question DetailsBurdgeChem 6.TB.06. [4689] A neon atom in its ground state will be diamagnetic. True False Assignment Details Name (AID): Assignment 3 (468740) Submissions Allowed: 5 Category: Homework Code: Locked: Yes Author: Hammond, Nicholas ( hmnd@bu.edu ) Last Saved: Oct 3, 0 0:3 PM EDT Permission: Protected Randomization: Person Which graded: Last Feedback Settings Before due date Question Score Assignment Score Publish Essay Scores Question Part Score Mark Add Practice Button Help/Hints Response Save Work After due date Question Score Assignment Score Publish Essay Scores Key Question Part Score Solution Mark Add Practice Button Help/Hints Response
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