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12 Dec 2019

In the following, use Bohr’s model to describe the emission of a photon of wavelength 4,048 nm from an excited hydrogen atom.

a) What is the energy of this photo in Joules? Rydbergs? Electron‐volts? What part of the electromagnetic spectrum is this light in?

b) Assuming that the emission came from a transition between consecutive energy levels, what was the initial energy level of this emission (ni)?

c) What is the distance of the initial level from the nucleus (ri) in Bohr radii and in meters?

d) How much closer to the nucleus is the electron in its final energy excited state than the initial state? What percent closer?

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Bunny Greenfelder
Bunny GreenfelderLv2
13 Dec 2019

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1) Calculate λ (in nm) for a photon with E = 2.38x10-14 J?

2)A highly excited atom of hydrogen makes a transition from the n = 13 to the n = 12 state and emits a photon. What is the energy of this photon in joules?

3)What is the wavelength in meters of the photon emitted when this highly excited hydrogen atom of hydrogen makes its transition from the n = 13 to the n = 12 state?

1. An atom, X, has a ground state binding energy(energy necessary to eject electron from the ground state) of 2.179e-18 J. The line(emission) spectrum for atom X is shown with n=2 to n=1(121.57 nm), n=3 to n=1(102.57 nm), n=4 to n=1(97.254 nm), n=5 to n=1(94.974 nm),and n=6 to n=1(93.780 nm). For each of the emission lines(given as wavelengths in nm), the final state is the ground state, or lowest energy state, of the atom.

a. What is the energy of the third excited state of X?

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e. Is it possible for X to absorb light of energy 2.5e-18 J? Why or why not?

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