Consider just four of the energy levels in a certain atom as shown in the as diagram below, use the diagram for the question How many spectral lines will result from all possible transitions among these levels! Which transition corresponds to the highest-frequency light emitted? Which transition corresponds to the lowest-frequency? 1 three: level 4 to level 3 transition: level 2 to level 1 transition. 2. six: level 4 to level 1 transition; level 4 to level 3 transition. 3. three: level 2 to level 1 transition: level 4 to level 3 transition 4. three: level 4 to level 1 transition: level 4 to level 3 transition An electron de-excites from the fourth quantum level to the third and then directly to the ground state. Two photons are emitted. How does the sum of their frequencies compare to the frequency of the single photon that would be emitted by de-excitation from the fourth level directly to the ground state? 1. None of these 2. The sum is larger than the frequency of the single photon. 3. The sum is smaller than the frequency of the single photon. 4. The sum is equal to the frequency of the single photon. Suppose the four energy levels were somehow evenly spaced. How many spectral lines would result? 1. five 2. six 3. four 4. three
Consider just four of the energy levels in a certain atom as shown in the as diagram below, use the diagram for the question How many spectral lines will result from all possible transitions among these levels! Which transition corresponds to the highest-frequency light emitted? Which transition corresponds to the lowest-frequency? 1 three: level 4 to level 3 transition: level 2 to level 1 transition. 2. six: level 4 to level 1 transition; level 4 to level 3 transition. 3. three: level 2 to level 1 transition: level 4 to level 3 transition 4. three: level 4 to level 1 transition: level 4 to level 3 transition An electron de-excites from the fourth quantum level to the third and then directly to the ground state. Two photons are emitted. How does the sum of their frequencies compare to the frequency of the single photon that would be emitted by de-excitation from the fourth level directly to the ground state? 1. None of these 2. The sum is larger than the frequency of the single photon. 3. The sum is smaller than the frequency of the single photon. 4. The sum is equal to the frequency of the single photon. Suppose the four energy levels were somehow evenly spaced. How many spectral lines would result? 1. five 2. six 3. four 4. three
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Consider just four of the energy levels in a certain atom as shown in the as diagram below, use the diagram for the question
How many spectral lines will result from all possible transitions among these levels!
Which transition corresponds to the highest-frequency light emitted?
Which transition corresponds to the lowest-frequency?
1 three: level 4 to level 3 transition: level 2 to level 1 transition.
2. six: level 4 to level 1 transition; level 4 to level 3 transition.
3. three: level 2 to level 1 transition: level 4 to level 3 transition
4. three: level 4 to level 1 transition: level 4 to level 3 transition
An electron de-excites from the fourth quantum level to the third and then directly to the ground state. Two photons are emitted.
How does the sum of their frequencies compare to the frequency of the single photon
that would be emitted by de-excitation from
the fourth level directly to the ground state?
1. None of these
2. The sum is larger than the frequency of
the single photon.
3. The sum is smaller than the frequency of
the single photon.
4. The sum is equal to the frequency of the
single photon.
Suppose the four energy levels were somehow
evenly spaced.
How many spectral lines would result?
1. five
2. six
3. four
4. three
Transcribed Image Text:n = 4
n = 3
n = 2
n = 1
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