A hydrogen atom is in the second excited state (n = 3). To what state %3D should it jump to emit light with the shortest possible wavelength, n = 1 n = 4 n = n = 2 Question 8 If you observe an emission spectrum with two lines, line A with 600 nm wavelength and line B with 300 nm wavelength, what can you say about the difference between the electron transitions emitting those two lines? Line B transitions have twice the energy of Line A transitions Line A trancitions haye twice th onerg of Line R trancition

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A hydrogen atom is in the second excited state (n = 3). To what state
should it jump to emit light with the shortest possible wavelength,
n = 1
n = 4
n = 5
O n = 2
Question 8
If you observe an emission spectrum with two lines, line A with 600 nm
wavelength and line B with 300 nm wavelength, what can you say about
the difference between the electron transitions emitting those two lines?
Line B transitions have twice the energy of Line A transitions
Line A transitions have twice the energy of Line B transition
Transcribed Image Text:A hydrogen atom is in the second excited state (n = 3). To what state should it jump to emit light with the shortest possible wavelength, n = 1 n = 4 n = 5 O n = 2 Question 8 If you observe an emission spectrum with two lines, line A with 600 nm wavelength and line B with 300 nm wavelength, what can you say about the difference between the electron transitions emitting those two lines? Line B transitions have twice the energy of Line A transitions Line A transitions have twice the energy of Line B transition
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