3. Refer to the illustration on the right. In a set of experiments on a hypothetical one-electron atom, you measure the wavelengths of the photons emitted from transitions ending in the ground state (n=1). You also observe that it takes 15 eV to ionize this atom. (a) What is the energy of the atom in each of the levels (i.e. n=1, n=2, n33, n=4, n=5)? (b) If an electron made a transition from the n=4 to the n=2 level, what wavelength of light would it emit?

3. Refer to the illustration on the right. In a set of experiments on a hypothetical one-electron atom, you measure the wavelengths of the photons emitted from transitions ending in the ground state (n=1). You also observe that it takes 15 eV to ionize this atom. (a) What is the energy of the atom in each of the levels (i.e. n=1, n=2, n33, n=4, n=5)? (b) If an electron made a transition from the n=4 to the n=2 level, what wavelength of light would it emit?

Modern Physics

3rd Edition

ISBN:9781111794378

Author:Raymond A. Serway, Clement J. Moses, Curt A. Moyer

Publisher:Raymond A. Serway, Clement J. Moses, Curt A. Moyer

Chapter4: The Particle Nature Of Matter

Section: Chapter Questions

Problem 31P

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Concept explainers

The Bohr model

Students often get confused between Rutherford’s model and Bohr model of an atom. They interpret the postulates of both these models to be the same, which is incorrect. Rutherford’s model differs from Bohr’s model in the following ways:

Question

100%

n = 5
n = 4
3. Refer to the illustration on the right. In a set of
experiments on a hypothetical one-electron atom,
you measure the wavelengths of the photons
emitted from transitions ending in the ground state
(n=1). You also observe that it takes 15 eV to
ionize this atom. (a) What is the energy of the
atom in each of the levels (i.e. n=1, n=2, n=3, n=4,
n=5)? (b) If an electron made a transition from the
n=4 to the n=2 level, what wavelength of light
n = 3
n = 2
would it emit?
n = 1
A = 73.86 nm
A = 75.63 nm
A=79.76 nm
A = 94.54 nm

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