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Chapter 28 (Quantum Theory)
1. The Bohr model of the hydrogen atom accounts for which quantum number?
a. principal b. orbital c. orbital magnetic d. all of the above
2. The restriction that no more than one electron may occupy a given quantum state in an atom was first stated by which of the following scientists?
a. Bohr b. de Broglie c. Heisenberg d. Pauli
3. The quantum mechanical model of the hydrogen atom requires that if the principal quantum number is 4, there will be how many different permitted orbital quantum number(s)?
a. one b. two c. four d. five
4. The quantum mechanical model of the hydrogen atom requires that if the orbital quantum number of the hydrogen atom is 4, there will be how many permitted orbital magnetic quantum numbers?
a. three b. four c. seven d. nine
5. The quantum mechanical model of the hydrogen atom requires that if the orbital magnetic quantum number is 3, there will be how many permitted spin magnetic quantum numbers?
a. two b. three c. four d. seven
6. How many possible substates are available in a hydrogen atom where the principal quantum number is 3?
a. 6 b. 9 c. 18 d. 36
7. The quantum mechanical model of the hydrogen atom suggests a visual picture of the electron as which of the following?
a. raisin in pudding b. probability cloud c. planetary orbiting body d. light quantum
8. How many electrons are in bromine’s (atomic number 35) next to outer shell (n = 3)?
a. 2 b. 4 c. 8 d. 18
9. The X‑rays that occur when a high energy electron beam is incident on a metal target will show what type of spectrum?
a. continuous b. line c. continuous spectrum superimposed on a line d. absorption
10. The Lyman series of hydrogen is made up of those transitions made from higher levels to n = 1. If the first line in this series has a wavelength of 122 nm, what is the wavelength of the second line?
a. 49 nm b. 103 nm c. 364 nm d. 486 nm
11. The ionization energy for the hydrogen atom is 13.6 eV. What is the energy of a photon that is emitted as a hydrogen atom makes a transition between the n = 5 and n = 3 states?
a. 0.544 eV b. 0.97 eV c. 1.51 eV d. 10.2 eV
12. A hologram is most dependent on which of the following light related phenomenon?
a. reflection b. polarization c. refraction d. interference
13. When a wire carries high current causing it to glow, it will emit which type of spectrum?
a. line emission b. line absorption c. continuous d. monochromatic
14. When a high voltage is applied to a low pressure gas causing it to glow, it will emit which type of spectrum?
a. line emission b. line absorption c. continuous d. monochromatic
15. When a cool gas is placed between a glowing wire filament source and a diffraction grating, the resultant spectrum from the grating is which one of the following?
a. line emission b. line absorption c. continuous d. monochromatic
16. Of the various wavelengths emitted from a hydrogen gas discharge tube, those that‑are associated with transitions from higher levels down to the n = 1 level produce which of the following?
a. infrared b. visible c. mixture of infrared and visible d. ultraviolet
17. Of the various wavelengths emitted from a hydrogen gas discharge tube, those associated with transitions from higher levels down to the n = 2 level produce which of the following?
a. infrared b. visible c. mixture of visible and ultraviolet d. ultraviolet
18. The stimulated emission of photons from the excited atoms in a gas laser is prompted by which of the following?
a. high voltage b. high flux of electrons c. nearby presence of photons of same wavelength as those emitted d. high temperature 19. What is the wavelength of the line in the Paschen series of hydrogen that is comprised of transitions from the n = 4 to the n = 3 levels? (R = 1.097 ´ 107 and 1 nm = 10‑9 m)
a. 1282 nm b. 1875 nm c. 1923 nm d. 2251 nm
20. What is the wavelength of the line in the Balmer series of hydrogen that is comprised of transitions from the n = 4 to the n = 2 level? (R = 1.097 ´ 107 and 1 nm = 10‑9 m)
a. 380 nm b. 486 nm c. 523 nm d. 630 nm
21. The ionization energy of the hydrogen atom is 13.6 eV. What is the energy of the n = 5 state?
a. 2.72 eV b. ‑2.72 eV c. 0.544 eV d. ‑0.544 eV
22. This ionization energy of the hydrogen atom is 13.6 eV. What is the energy of a photon emitted corresponding to a transition from the n = 5 to n = 2 state.
a. 2.86 eV b. 3.5 eV c. 4.0 eV d. 7.9 eV
23. If the radius of the electron orbit in the n = 1 level of the hydrogen atoms is 0.053 nm, what is its radius for the n = 4 level? (Assume the Bohr model is valid.)
a. 0.11 nm b. 0.21 nm c. 0.48 nm d. 0.85 nm
24. The Paschen series of hydrogen corresponds to electron transitions from higher levels to n = 3. What is the shortest wavelength in that series? (R = 1.097 ´ 107 m-1 and 1 nm = 10‑9 m)
a. 365 nm b. 820 nm c. 1094 nm d. 313 nm 25. The Lyman series of hydrogen corresponds to electron transitions from higher levels to n = 1. What is the shortest wavelength in that series? (R = 1.097 ´ 107 m-1 and 1 nm = 10‑9 m)
a. 71 nm b. 91 nm c. 273 nm d. 456 nm
26. The ionization energy of the hydrogen atom is 13.6 eV. What is the wavelength of a photon having this much energy? (h = 6.63 ´ 10‑34 J‑s, c = 3 ´ 108 m/s, 1 eV = 1.6 ´ 10‑19 J and 1 nm = 10‑9 m)
a. 91 nm b. 136 nm c. 273 nm d. 360 nm
27. The quantum mechanical model of the hydrogen atom requires that if the principal quantum number = 5, there will be how many permitted orbital quantum numbers?
a. 3 b. 5 c. 10 d. 25
28. The quantum mechanical model of the hydrogen atom requires that if the orbital quantum number = 7, there will be how many permitted orbital magnetic quantum numbers allowed?
a. 6 b. 7 c. 11 d. 13
29. The quantum mechanical model of the hydrogen atom requires that if the principal quantum number = 4, there will be permitted how many orbital magnetic quantum numbers?
a. 4 b. 6 c. 8 d. 7
30. The quantum mechanical model of the hydrogen atom requires that if the orbital quantum number = 4, there are permitted how many possible substates?
a. 4 b. 8 c. 16 d. 18 31. If the principal quantum number for hydrogen is 5, which one of the following is not a permitted orbital magnetic quantum number for that atom?
a. 6 b. ‑2 c. 0 d. 3
32. If the energy for the ground state level (n = 1) of hydrogen is ‑13.6 eV, which of the following gives an approximate value for the energy of an electron of the K shell (n = 1) of the element oxygen for which the atomic number = 8?
a. ‑95 eV b. ‑109 eV c. ‑666 eV d. ‑1100 eV
33. Which of the following demonstrated the relation between the atomic number of a given element and the wavelength of the K‑alpha X‑ray photon emitted by that element?
a. Bohr b. Compton c. Moseley d. Pauli
34. If a target element with atomic number Z used in the production of X‑rays is replaced by another element for which the atomic number = 3Z, by what factor is the wavelength of the K‑alpha X‑ray line changed?
a. 1/9 b. 1/3 c. 3.0 d. 9.0
35. Atoms which absorb ultraviolet photons and in turn emit photons in the visible range are used in which type of device?
a. incandescent lamp b. radar c. fluorescent lamp d. electron microscope
36. Using quantum theories to study the hydrogen atom allows the prediction and experimental verification of many data about atoms such as He+ and Li2+. Some quantities that can successfully be predicted about He+ and Li2+ in this manner are:
a. the color of the light they will emit. b. their mass. c. their abundance in nature. d. all of the above 37. An alpha particle is:
a. a neutral helium atom. b. any positively charged nucleus. c. an X‑ray. d. none of the above
38. According to the Rutherford model of the atom, most of the volume of an atom:
a. is empty space. b. was occupied by the nucleus. c. contained positive charges. d. excluded electrons.
39. The four visible colors emitted by hydrogen atoms are produced by electrons:
a. that start in the ground state. b. that end up in the ground state. c. that start in the level with n = 2. d. that end up in the level with n = 2.
40. The visible lines from hydrogen are all members of the:
a. Lyman series. b. Balmer series. c. Paschen series. d. Brackett series.
41. The emission of a line from the Balmer series is followed almost immediately by the emission of a line from the Lyman series. This will be true for:
a. only the first line of the Balmer series and the first line of the Lyman series. b. all the lines of the Balmer series followed by only the first line of the Lyman series. c. only the first line of the Balmer series followed by any of the lines of the Lyman series. d. all the lines of the Balmer series followed by any of the lines of the Lyman series.
42. The Bohr theory does not predict that:
a. hydrogen atoms will give off the lines from the Balmer series. b. the ground state of hydrogen is spherically symmetric. c. it requires 13.6 eV to ionize hydrogen. d. the approximate radius of a hydrogen atom is 5.1 ´ 10-11 m
43. In the Bohr model of the atom, the orbits where electrons move fastest
a. have the least energy. b. have the most energy. c. have the biggest radius. d. have the greatest angular momentum.
44. In the hydrogen atom the potential energy is negative but the absolute value of the potential energy:
a. is equal to the kinetic energy of the electron. b. is twice the kinetic energy of the electron. c. is half the kinetic energy of the electron. d. is equal to n2 times the kinetic energy of the electron.
45. When an electron moves from the n = 1 to the n = 2 orbit:
a. both the radius and the angular momentum double. b. both the radius and the angular momentum increase by a factor of 4. c. the radius doubles and the angular momentum increases by a factor of 4. d. radius increases by a factor of 4 and the angular momentum doubles.
46. In an analysis relating Bohr’s theory to the de Broglie wavelength of electrons, when an electron moves from the n = 1 level to the n = 2 level, the circumference for its orbit becomes 4 times greater. This occurs because:
a. there are four times as many wavelengths in the new orbit. b. the wavelength of the electron becomes four times as long. c. there are twice as many wavelengths and each wavelength is twice as long. d. the electron is moving four times as fast.
47. Imagine that an electron had a spin of 5/2 so that its spin quantum number, ms, could have the following six values: ms = +5/2, +3/2, +1/2, ‑1/2, ‑3/2, and -5/2. If this were true, the first element with a filled shell would be the first of the noble gasses and it would be:
a. He with 2 electrons. b. Be with 4 electrons. c. C with 6 electrons. d. O with 8 electrons.
48. In an X‑ray machine, electrons are accelerated and then fired so that they are incident on a metal target. Which part of the process produces the characteristic X‑ray spectra?
a. The incident electron loses energy. b. The incident electron knocks an electron out of one of the metal atoms. c. A vacancy in an energy level in a metal atom is filled. d. The incident electron emits an X‑ray.
49. The familiar yellow light from a sodium vapor street lamp results from the 3p ® as transition in Na. Determine the wavelength of the light given off if the energy difference E3p ‑ E3S = 2.1 eV.
a. 560 nm b. 575 nm c. 590 nm d. 600 nm 50. The wavelength of coherent ruby laser light is 688.3 nm. What energy difference (in eV) exists between the upper excited state and the lower unexcited ground state?
a. 1.746 eV b. 1.804 eV c. 1.862 eV d. 1.936 eV
51. A ruby laser delivers a 10 ns pulse of 1 MW average power. If all the photons are of wavelength 694.3 nm, how many photons are contained in the pulse? (h = 6.626 ´ 10‑34 J‑s)
a. 5.0 ´ 1015 b. 2.0 ´ 1016 c. 3.5 ´ 1016 d. 5.0 ´ 1016
52. The energy needed to change an He+ ion into an He++ ion:
a. 13.6 eV. b. 54.4 eV. c. 92.9 eV. d. 112.4 ev.
53. A hydrogen atom in the ground state absorbs a 12.1 eV photon. To what level is the electron promoted? (The ionization energy of hydrogen is 13.6 eV)
a. n = 2 b. n = 3 c. n = 4 d. n = 5
54. A photon is emitted from a hydrogen atom that undergoes a transition from n = 3 to n = 2. Calculate the energy and wavelength of the photon.
a. Eg = 1.89 eV, l = 658 nm b. Eg = 2.21 eV, l = 563 nm c. Eg = 2.70 eV, l = 460 nm d. Eg = 3.19 eV, l = 390 nm
55. An energy of 13.6 eV is needed to ionize an electron. From the ground state of a hydrogen atom, what wavelength is needed if a photon accomplishes this task?
a. 60 nm b. 70 nm c. 80 nm d. 90 nm
56. A ruby laser can deliver an 8.57 J pulse in approximately 50 nanoseconds. The wavelength of the light is 694.4 nm. How many atoms within the ruby rod had to be excited to allow this high‑energy laser pulse? (h = 6.626 ´ 10‑34 J‑S)
a. 4 ´ 1018 b. 8 ´ 1018 c. 3 ´ 1019 d. 6 ´ 1020
Notes:
# Ans Difficulty # Ans Difficulty
1. 1 A 29. 3 D 2. 1 D 30. 3 D 3. 2 C 31. 2 A 4. 2 C 32. 2 C 5. 2 A 33. 1 C 6. 3 C 34. 1 A 7. 1 B 35. 2 C 8. 2 D 36. 1 A 9. 1 C 37. 1 D 10. 2 B 38. 1 A 11. 2 B 39. 2 D 12. 1 D 40. 2 B 13. 1 C 41. 2 B 14. 2 A 42. 2 B 15. 2 B 43. 2 A 16. 2 D 44. 2 B 17. 2 C 45. 2 D 18. 1 C 46. 2 C 19. 2 B 47. 3 C 20. 2 B 48. 2 C 21. 2 D 49. 2 C 22. 2 A 50. 2 D 23. 2 D 51. 2 C 24. 3 B 52. 2 B 25. 2 B 53. 2 B 26. 2 A 54. 2 A 27. 3 B 55. 2 D 28. 3 D 56. 2 C
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