### The Bohr Equation and Rydberg ConstantThe Bohr equation applies to any 1-electron atom or ion, though the Rydberg constant changes depending on nuclear charge, reduced mass, and other factors. For an He⁺ ion, the Rydberg constant is \( R_{4He} = 2.19176 \times 10^{-18} \, \text{J} \). If a He⁺ ion with an electron in the \( n = 4 \) level **absorbs** a photon of wavelength \( 2153 \, \text{nm} \), in what energy level does the electron end?**Options:**- \( \bigcirc \ 6 \)- \( \bigcirc \ 2 \)- \( \bigcirc \ 3 \)- \( \bigcirc \ 7 \)- \( \bigcirc \ 1 \)

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The Bohr equation applies to any 1 electron atom or ion, though the Rydberg constant changes depending on nuclear charge, reduced mass and other factors. For an He* ion the Rydberg constant is R4He = 2.19176x10 18J. If a He+ ion with an electron in the n=4 level absorbs a photon of wavelength 2153 nm, in what energy level %3D does the electron end? 2 07 1

The Bohr equation applies to any 1 electron atom or ion, though the Rydberg constant changes depending on nuclear charge, reduced mass and other factors. For an He* ion the Rydberg constant is R4He = 2.19176x10 18J. If a He+ ion with an electron in the n=4 level absorbs a photon of wavelength 2153 nm, in what energy level %3D does the electron end? 2 07 1

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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