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- 1. Multiple Choice
Which electron transition between the energy
levels of hydrogen causes the emission of a photon of
visible light?
𝑛 = 6 to 𝑛 = 5
𝑛 = 5 to 𝑛 = 6
𝑛 = 5 to 𝑛 = 2
𝑛 = 2 to 𝑛 = 5
- 2. Multiple Choice
Which of the following transitions is the result of
the atom absorbing a photon of the shortest
wavelength?
A
B
C
D
- 3. Multiple Choice
The diagram below shows the Balmer series electron
transitions in a hydrogen atom.
A. 𝐸2 𝑡𝑜 𝐸5
𝐸3 𝑡𝑜 𝐸6
𝐸3 𝑡𝑜 𝐸2
𝐸6 𝑡𝑜 𝐸2
- 4. Multiple Choice
What is the wavelength and color of the emitted
photon, due to a transition in a hydrogen atom from
the 𝑛 = 3 state to the 𝑛 = 2 state?
486 nm Green
656 nm Red
486 nm Blue
434 nm Violet
- 5. Multiple Choice
Which of the transitions below for a hydrogen
atom involves the least energy?
𝑛= 5 𝑡𝑜 𝑛 = 3
𝑛 = 5 𝑡𝑜 𝑛 = 4
𝑛 = 2 𝑡𝑜 𝑛 = 5
𝑛I= 4 𝑡𝑜 𝑛 = 7
- 6. Multiple Choice
A photon having an energy of 9.40 electron volts
strikes a hydrogen atom in the ground state. Why is
the photon not absorbed by the hydrogen atom?
The atom’s orbital electron is moving too
fast
The photon striking the atom is moving
too fast
The photon’s energy is too small
The photon is being repelled by
electrostatic force
- 7. Multiple Choice
What is the minimum energy required to ionize a
hydrogen atom in the n=3 state?
0.66 eV
1.51 eV
12.09 eV
13.6 eV
- 8. Multiple Choice
The energy level diagram for a hypothetical atom
is shown in the figure below. Which of the labeled
transitions in the diagram would produce a photon
with the shortest wavelength?
A
B
C
D
- 9. Multiple Choice
Which type of photon is emitted when an electron
in a hydrogen atom drops from the n=2 to the n=1
energy level?
Ultraviolet
Visible light
Infrared
Radio wave
- 10. Multiple Choice
The visible lines from hydrogen are all members
of the ____.
Lyman series
Balmer series
Paschen series
Lyman and Paschen series
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