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?
University Physics Volume 3
17th Edition
ISBN:9781938168185
Author:William Moebs, Jeff Sanny
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Chapter8: Atomic Structure
Section: Chapter Questions
Problem 68P: The ion Li2+ makes ail atomic transition from ail n = 4 state to ail n = 2 state, (a) What is the...
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![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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd272a1c5-7bd8-46f2-af1c-ed5aaeb4fec0%2F2ccae948-056c-4c99-8180-3c48e757b823%2Flj1y0fe_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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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