Suppose the four energy levels in Exercise 1 were somehow
Chapter 32, Problem 81TAE(choose chapter or problem)
Suppose the four energy levels in question 78 were somehow evenly spaced. How many spectral lines would result?
Consider just four of the energy levels in a certain atom, as shown in the diagram below. How many spectral lines will result from all possible transitions among these levels? Which transition corresponds to the highest-frequency light emitted? To the lowest frequency light emitted?
\(n=4\)
\(n=3\)
\(n=2\)
\(n=1\)
Equation Transcription:
Text Transcription:
78
n=4
n=3
n=2
n=1
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