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by BlastRoom
Track electron jumps between hydrogen energy levels and the photons absorbed or emitted.
#physics
30 questions
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In the figure, an electron drops from n=3 to n=2 in hydrogen. What is the energy of the emitted photon?
A hydrogen electron falls from n=2 to n=1 as shown. How much energy does the photon carry away?
The arrow in the figure runs downward from n=4 to n=2. What is the emitted photon's energy?
The figure shows absorption from n=1 to n=3. What photon energy must the atom absorb?
A drawn arrow drops from n=4 to n=3. What is the energy of the emitted photon?
The figure shows an electron at n=2 absorbing energy up to the ionization level at 0 eV. What energy is required?
In the figure, an electron absorbs a photon and jumps from n=1 to n=4. What is the photon's energy?
A downward arrow in the figure goes from n=3 to n=1. What energy is emitted as one photon?
For the shown n=4 to n=2 emission, use J*s and . What is the photon frequency?
For the shown n=3 to n=2 emission, use J*s, m/s, and . What is the wavelength?
The arrow in the figure points upward from n=2 to n=4. Does this transition emit or absorb a photon?
The figure shows an arrow downward from n=4 to n=1. Does this transition emit or absorb a photon?
Use the labeled hydrogen energy-level diagram. Which arrow releases the greatest photon energy?
The figure gives a hydrogen energy-level diagram with labeled transitions. Which absorption needs the most energetic photon?
A hydrogen energy-level diagram shows several labeled transitions. Which arrow represents absorption?
Refer to the labeled hydrogen energy-level diagram. Which arrow has the smallest photon energy?
The figure compares two labeled emissions in a hydrogen energy-level diagram. Which emitted light has the longer wavelength?
The figure shows P: n=3 to n=2 and Q: n=4 to n=2. Which photon has the higher frequency?
In the figure, P is n=4 to n=3 and Q is n=3 to n=2. Which emitted photon has the lower frequency?
The figure compares P: n=3 to n=2 and Q: n=2 to n=1. Which statement about the emitted photons is correct?
For hydrogen in the Bohr model, which level is the ground state?
What is the first excited state of hydrogen in this level model?
Which description best matches an excited state of a hydrogen atom?
What did Bohr's fixed energy levels help explain for hydrogen?
Which result is correctly matched to Rutherford, not Bohr?
Why does a hydrogen emission spectrum contain separated bright lines instead of every color?
Cool hydrogen atoms in the ground state absorb 10.20 eV photons but not 9.00 eV photons. Why are 9.00 eV photons not absorbed?
A hydrogen atom is in n=2. A 2.00 eV photon passes by, but the n=2 to n=3 gap is 1.89 eV and n=2 to n=4 is 2.55 eV. What happens?
A ground-state hydrogen atom meets a 10.30 eV photon. The n=1 to n=2 gap is 10.20 eV, and n=1 to n=3 is 12.09 eV. What is the best prediction?
Why do the absorption and emission lines of hydrogen occur at the same photon energies?
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The Uncertainty Principle and Quantum Technology
40 questions
