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Determine the end (final) value of n in a hydrogen atom transition, if the electron starts in n=4 and the atom emits a photon of light with a wavelength of 486 nm.

Determine the end (final) value of n in a hydrogen atom transition, if the electron starts in n=4 and the atom emits a photon of light with a wavelength of 486 nm.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Question:** Determine the end (final) value of \( n \) in a hydrogen atom transition, if the electron starts in \( n=4 \) and the atom emits a photon of light with a wavelength of 486 nm. --- *Explanation for Educational Content:* In this problem, we are asked to determine the final energy level, \( n \), of an electron in a hydrogen atom after it transitions and emits a photon. The initial energy level is \( n=4 \), and the emitted photon has a wavelength of 486 nm. To solve this, we can use the Rydberg formula for hydrogen spectral lines, which relates the wavelength of light to the energy levels involved in the transition.
Transcribed Image Text:**Question:** Determine the end (final) value of \( n \) in a hydrogen atom transition, if the electron starts in \( n=4 \) and the atom emits a photon of light with a wavelength of 486 nm. --- *Explanation for Educational Content:* In this problem, we are asked to determine the final energy level, \( n \), of an electron in a hydrogen atom after it transitions and emits a photon. The initial energy level is \( n=4 \), and the emitted photon has a wavelength of 486 nm. To solve this, we can use the Rydberg formula for hydrogen spectral lines, which relates the wavelength of light to the energy levels involved in the transition.
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