For a hydrogen atom, calculate the energy of the photon that would be emitted for the orbital transition of n(initial) = 4 to n(final) = 1. The Rydberg constant is 1.09678 x 10' m¹. Report to four significant figures.

For a hydrogen atom, calculate the energy of the photon that would be emitted for the orbital transition of n(initial) = 4 to n(final) = 1. The Rydberg constant is 1.09678 x 10' m¹. Report to four significant figures.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section5.3: The Bohr Model Of The Hydrogen Atom

Problem 5.4PSP: (a) Calculate the frequency and the wavelength of the line for the n = 6 to n = 4 transition. (b) Is...

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For a hydrogen atom, calculate the energy of the photon that would be
emitted for the orbital transition of n(initial) = 4 to n(final) = 1. The
Rydberg constant is 1.09678 x 10' m¹. Report to four significant
figures.

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(a) Calculate the frequency and the wavelength of the line for the n = 6 to n = 4 transition. (b) Is this wavelength longer or shorter than that of the n = 7 to n = 4 transition?