Identifying the Correct Sketch for a Spectrum of Light Emitted by Transitions in a Bohr-like Atom of Specified Energy Levels

 AP Physics 2 Skills Practice
  • 1.

    The emission spectrum of Hydrogen is shown below.

    Identify the band formed by an electron transitioning from the third to the second energy level.

    Answers:

    • The third band from the right

    • The second band from the right

    • The first band from the right

    • The fourth band from the right

  • 2.

    The following is the emission spectrum of Hydrogen.

    Which band is formed by the electron jumping from the fourth energy level to the second energy level?

    Answers:

    • The second band from the right

    • The fourth band from the right

    • The third band from the right

    • The first band from the right

  • 3.

    The emission spectrum of Hydrogen is given below.

    Identify the third line of the Balmer series, i.e. the line formed the electron jumping from the fifth to the second energy level.

    Answers:

    • The third line from the left

    • The fourth line from the left

    • The first line from the left

    • The second line from the left

  • 4.

    The following image shows the emission spectrum of hydrogen.

    Identify the band formed by the electron jumping from the sixth to the second energy level.

    Answers:

    • The second band from the left

    • The fourth band from the left

    • The third band from the left

    • The first band from the left

  • 5.

    The emission spectra of two unknown substances are given below.

    A:

    B:

    Which one of them contains the band for the electron jumping from the fourth to the third energy level in singly ionized Helium?

    Answers:

    • Both A and B

    • A

    • Neither

    • B

  • 6.

    Two unknown substances A and B have the following emission spectra.

    A:

    B:

    Which one of them contains the band for the transition from the third to the second energy level of Hydrogen?

    Answers:

    • Both

    • B

    • Neither

    • A

  • 7.

    Two unknown emission spectra are provided below.

    A:

    B:

    Which of these emission spectra contain the band corresponding to the transition from the fourth to the third energy level in a singly ionized helium?

    Answers:

    • Both

    • B

    • Neither

    • A

  • 8.

    Following are four unknown emission spectra.

    A:

    B:

    C:

    D:

    Identify the one that contains the band for the electron jumping from the third to the second energy level in Hydrgen.

    Answers:

    • C

    • A

    • B

    • D

  • 9.

    Take a look at the two unknown emission spectra below.

    1.

    2.

    By looking for the emission line corresponding to the transition from the fourth to the second energy level in Hydrogen, find out which one of these substances is Hydrogen.

    Answers:

    • Substance 1

    • Both substances

    • Neither substance

    • Substance 2

  • 10.

    Four unknown emission spectra are given below.

    1.

    2.

    3.

    4.

    By looking for the emission band corresponding to the transition from the fourth energy level to the third, find out which one of these substances is singly ionized Helium.

    Answers:

    • Substance 3

    • Substance 4

    • Substance 1

    • Substance 2

  • 11.

    An electron jumps from the fifth to the third energy level inside a lithium atom. Identify the spectrum containing the emission band of the electron described above.

    Lithium atomic number: 3

    Answers:

    • Graph 4
      Sketch for a Spectrum of Ligh

    • Graph 3
      Sketch for a Spectrum of Ligh

    • Graph 1
      Sketch for a Spectrum of Ligh

    • Graph 2
      Sketch for a Spectrum of Ligh

  • 12.

    An electron jumps from the sixth to the third energy level inside a boron atom. Identify the spectrum containing the emission band of the electron described above.

    Atomic number of Boron: 5

    Answers:

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

  • 13.

    An electron jumps from the fourth to the second energy level inside an oxygen atom. Identify the spectrum containing the emission band of the electron described above.

    Atomic number of Oxygen: 8

    Answers:

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

  • 14.

    An electron jumps from the fifth to the seventh energy level inside a fluorine atom. Identify the spectrum containing the emission band of the electron described above.

    Atomic number of Fluorine: 9

    Answers:

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

  • 15.

    An electron jumps from the fourth to the sixth energy level inside a sodium atom. Identify the spectrum containing the emission band of the electron described above.

    Atomic number of Sodium: 11

    Answers:

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

  • 16.

    An electron jumps from the first to the fourth energy level inside a nitrogen atom. Identify the spectrum containing the emission band of the electron described above.

    Atomic number of Nitrogen: 7

    Answers:

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

  • 17.

    An electron jumps from the second to the fifth energy level inside a hydrogen atom. Identify the spectrum containing the emission band of the electron described above.

    Atomic number of Hydrogen: 1

    Answers:

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

  • 18.

    An electron jumps from the fourth to the seventh energy level inside a silica atom. Identify the spectrum containing the emission band of the electron described above.

    Atomic number of Silica: 14

    Answers:

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

  • 19.

    An electron jumps from the third to the sixth energy level inside a chlorine atom. Identify the spectrum containing the emission band of the electron described above.

    Chlorine atomic number: 17

    Answers:

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

  • 20.

    An electron jumps from the fourth to the second energy level inside a helium atom. Identify the spectrum containing the emission band of the electron described above.

    Atomic number of Helium: 2

    Answers:

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

    • Sketch for a Spectrum of Ligh

  • 21.

    A Bohr-like atom has the following energy levels:

    {eq}E_1 = -667.00 \, \textrm{eV} \\ E_2 = -166.76 \, \textrm{eV} \\ E_3 = -74.11 \, \textrm{eV} {/eq}

    Which of the following spectra show the correct emission lines if transition between all three levels are allowed?

    Answers:

    • Black and white image of spectra with emission lines at 2.09 nm, 2.48 nm, and 13.38 nm

    • Black and white image of spectra with emission lines at 2.09 nm, 2.48 nm, and 92.65 nm

    • Black and white image of spectra with emission lines at 92.65 nm, 500.24 nm, and 592.89 nm

    • Black and white image of spectra with emission lines at 74.11 nm, 166.76 nm, and 667.00 nm

  • 22.

    A Bohr-like atom has the following energy levels:

    {eq}E_1 = -54.45 \, \textrm{eV} \\ E_2 = -13.61 \, \textrm{eV} \\ E_3 = -6.05 \, \textrm{eV} {/eq}

    Which of the following spectra show the correct emission lines if transition between all three levels are allowed?

    Answers:

    • Black and white image of spectra with emission lines at 30.36 nm, 40.84 nm, and 48.40 nm

    • Black and white image of spectra with emission lines at 7.56 nm, 25.62 nm, and 30.36 nm

    • Black and white image of spectra with emission lines at 6.05 nm, 13.61 nm, and 54.45 nm

    • Black and white image of spectra with emission lines at 25.62 nm, 30.36 nm, and 163.96 nm

  • 23.

    A Bohr-like atom has the following energy levels:

    {eq}E_2 = -13.61 \, \textrm{eV} \\ E_3 = -6.05 \, \textrm{eV} \\ E_4 = -3.40 \, \textrm{eV} {/eq}

    Which of the following spectra show the correct emission lines if transition between all three levels are allowed?

    Answers:

    • Black and white image of spectra with emission lines at 60.73 nm, 82.00 nm, and 234.23 nm

    • Black and white image of spectra with emission lines at 121.45 nm, 164.00 nm, and 468.45 nm

    • Black and white image of spectra with emission lines at 2.65 nm, 7.56 nm, and 10.21 nm

    • Black and white image of spectra with emission lines at 2.65 nm, 3.40 nm, and 6.05 nm

  • 24.

    A Bohr-like atom has the following energy levels:

    {eq}E_3 = -6.05 \, \textrm{eV} \\ E_4 = -3.40 \, \textrm{eV} \\ E_5 = -2.18 \, \textrm{eV} {/eq}

    Which of the following spectra show the correct emission lines if transition between all three levels are allowed?

    Answers:

    • Black and white image of spectra with emission lines at 320.25 nm, 468.45 nm, and 506.12 nm

    • Black and white image of spectra with emission lines at 320.25 nm, 468.45 nm, and 1012.24 nm

    • Black and white image of spectra with emission lines at 506.12 nm, 1012.24 nm, and 1519.00 nm

    • Black and white image of spectra with emission lines at 1519.00 nm, 3282.28 nm, and 4801.28 nm

  • 25.

    A Bohr-like atom has the following energy levels:

    {eq}E_3 = -13.61 \, \textrm{eV} \\ E_4 = -7.66 \, \textrm{eV} \\ E_5 = -4.90 \, \textrm{eV} {/eq}

    Which of the following spectra show the correct emission lines if transition between all three levels are allowed?

    Answers:

    • Black and white image of spectra with emission lines at 142.33 nm, 208.19 nm, and 224.97 nm

    • Black and white image of spectra with emission lines at 142.33 nm, 208.19 nm, and 449.93 nm

    • Black and white image of spectra with emission lines at 284.66 nm, 416.38 nm, and 449.93 nm

    • Black and white image of spectra with emission lines at 224.97 nm, 284.66.38 nm, and 416.38 nm

  • 26.

    A Bohr-like atom has the following energy levels:

    {eq}E_5 = -4.90 \, \textrm{eV} \\ E_6 = -3.40 \, \textrm{eV} \\ E_7 = -2.50 \, \textrm{eV} {/eq}

    Which of the following spectra show the correct emission lines if transition between all three levels are allowed?

    Answers:

    • Black and white image of spectra with emission lines at 1033.04 nm, 1373.66 nm, and 1654.76 nm

    • Black and white image of spectra with emission lines at 516.52 nm, 827.38 nm, and 1373.66 nm

    • Black and white image of spectra with emission lines at 516.52 nm, 686.83 nm, and 827.38 nm

    • Black and white image of spectra with emission lines at 827.38 nm, 1033.04 nm, and 1373.66 nm

  • 27.

    A Bohr-like atom has the following energy levels:

    {eq}E_2 = -54.45 \, \textrm{eV} \\ E_3 = -24.20 \, \textrm{eV} \\ E_4 = -13.61 \, \textrm{eV} {/eq}

    Which of the following spectra show the correct emission lines if transition between all three levels are allowed?

    Answers:

    • Black and white image of spectra with emission lines at 30.36 nm, 40.99 nm, and 58.56 nm

    • Black and white image of spectra with emission lines at 58.56 nm, 60.72 nm, and 81.98 nm

    • Black and white image of spectra with emission lines at 30.36 nm, 40.99 nm, and 117.12 nm

    • Black and white image of spectra with emission lines at 60.72 nm, 81.98 nm, and 117.12 nm

  • 28.

    A Bohr-like atom has the following energy levels:

    {eq}E_4 = -13.61 \, \textrm{eV} \\ E_5 = -8.71 \, \textrm{eV}\\ E_6 = -6.05 \, \textrm{eV} {/eq}

    Which of the following spectra show the correct emission lines if transition between all three levels are allowed?

    Answers:

    • Black and white image of spectra with emission lines at 253.06 nm, 328.04 nm, and 466.17 nm

    • Black and white image of spectra with emission lines at 164.02 nm, 253.06 nm, and 466.17 nm

    • Black and white image of spectra with emission lines at 164.02 nm, 233.09 nm, and 253.06 nm

    • Black and white image of spectra with emission lines at 328.04 nm, 466.17 nm, and 506.12 nm

  • 29.

    A Bohr-like atom has the following energy levels:

    {eq}E_4 = -21.27 \, \textrm{eV} \\ E_5 = -13.61 \, \textrm{eV} \\ E_6 = -9.45 \, \textrm{eV} {/eq}

    Which of the following spectra show the correct emission lines if transition between all three levels are allowed?

    Answers:

    • Black and white image of spectra with emission lines at 104.93 nm, 161.94 nm, and 298.08 nm

    • Black and white image of spectra with emission lines at 149.04 nm, 161.94 nm, and 209.86 nm

    • Black and white image of spectra with emission lines at 104.93 nm, 149.04 nm, and 161.94 nm

    • Black and white image of spectra with emission lines at 104.93 nm, 161.94 nm, and 209.86 nm

  • 30.

    A Bohr-like atom has the following energy levels:

    {eq}E_5 = -19.60 \, \textrm{eV} \\ E_6 = -13.61 \, \textrm{eV}\\ E_7 = -10.00 \, \textrm{eV} {/eq}

    Which of the following spectra show the correct emission lines if transition between all three levels are allowed?

    Answers:

    • Black and white image of spectra with emission lines at 129.15 nm, 171.65 nm, and 207.05 nm

    • Black and white image of spectra with emission lines at 103.53 nm, 129.15 nm, and 207.05 nm

    • Black and white image of spectra with emission lines at 129.15 nm, 207.05 nm, and 343.30 nm

    • Black and white image of spectra with emission lines at 103.53 nm, 129.15 nm, and 171.65 nm

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