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The Balmer series for the hydrogen atom corresponds to electronic transitions that terminate in the state with quantum number n = 2 as shown in Figure P41.7 (page 1140). Consider the photon of longest wavelength corresponding to a transition shown in the figure. Determine (a) its energy and (b) its wavelength. Consider the spectral line of shortest wavelength corresponding to a transition shown in the figure. Find (c) its photon energy and (d) its wavelength. (e) What is the shortest possible wavelength in the Balmer series?

Chapter 41, Problem 7P, The Balmer series for the hydrogen atom corresponds to electronic transitions that terminate in the

Figure P41.7

 

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Ankit Lal
Ankit LalLv10
7 Mar 2021

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Related textbook solutions

Physics: Principles with Applications
7th Edition, 2013
Giancoli
ISBN: 9780321625922

Related questions

For this question consider the figure to the right that shows an energy level diagram for a certain atom (not hydrogen). Several transitions are shown and labeled by letters. Note the diagram is not drawn to scale.

(A) Which transition corresponds to the emission of the photon with the longest wavelength?

(B) Which transition corresponds to the emission of the photon with the shortest wavelength?

(C) Which transition corresponds to the emission of the photon with 177 nm wavelength?

(D) Which transition corresponds to the emission of the photon with 124 nm wavelength?

For this question consider the figure to the right shows an energy level diagram fora certain atom(not hydrogen). Several transitions are shown and are labeled by letters.  Note: The diagram is not drawn to scale

a) Which transition corresponds to the emission of the photon with the longest wavelength?

b) Which transition corresponds to the emission of the photon with the shortest wavelength?

c) Which transition corresponds to the emission of 177 nm photon?

d) Which transition corresponds to the absorption of a 124 nm Photons?

 

Part A:

Use the energy levels of hydrogen, given by the equation:[En = (-13.606/n2)eV] to calculate theenergy, ΔE, of the visible Balmer series photons: ΔE = 13.606eV(1/4 - l/n2), where n=3 for the red line, n=4 for theblue-green, and n=5 for the violet; your text shows how to computethe wavelength (in Angstroms) of a photon if its energy is known ineV (electron volts): λ = 12398/ΔE. Use this formula to compute thewavelenths of the three Balmer lines that you observed; show eachstep of your work

Part B:

At what angle would you expect to see the second order line forλ=6562Angstroms in this experiment?

Please any help would be very much appreciated. Thank you.!!

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