In the hydrogen atom, the transition from the 2p state to the 1s state emits a photon with energy 16.2 x10-19 J. In an iron atom, the same transition emits X-rays with wave- length 0.193 nm. Calculate the energy difference between these two states in iron. Explain the difference in the 2p-1s energy level spacing in these two atoms.

In the hydrogen atom, the transition from the 2p state to the 1s state emits a photon with energy 16.2 x10-19 J. In an iron atom, the same transition emits X-rays with wave- length 0.193 nm. Calculate the energy difference between these two states in iron. Explain the difference in the 2p-1s energy level spacing in these two atoms.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter5: Quantum Mechanics And Atomic Structure

Section: Chapter Questions

Problem 43AP: In the hydrogen atom, the transition from the 2p state to the 1s state emits a photon with energy...

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Similar questions

When metallic sodium is dissolved in liquid sodium chloride, electrons are released into the liquid. These dissolved electrons absorb light with a wavelength near 800 nm. Suppose we treat the positive ions surrounding an electron crudely as defining a three-dimensional cubic box of edge L, and we assume that the absorbed light excites the electron from its ground state to the first excited state. Calculate the edge length L in this simple model.
The figure below represents part of the emission spectrum for a one-electron ion in lhe gas phase. All the lines result from electronic transitions from excited states to the n = 3 state. (See Exercise 160.) a. What electronic transitions correspond to lines A and B? b. If the wavelength of line B is 142.5 nm, calculate the wavelength of line A.
What type of relationship (direct or inverse) e xists between wavelength, frequency, and photon energy? What does a photon energy unit of a joule equal?
In a FranckHertz experiment on sodium atoms, the first excitation threshold occurs at 2.103 eV. Calculate the wavelength of emitted light expected just above this threshold. (Note: Sodium vapor lamps used in street lighting emit spectral lines with wavelengths 5891.8 and 5889.9 Å.)
In two-photon ionization spectroscopy, the combined energies carried by two different photons are used to remove an electron from an atom or molecule. In such an experiment, a K atom in the gas phase is to be ionized by two different light beams, one of which has a 650-nm wavelength. What is the maximum wavelength for the second beam that will cause two-photon ionization?
Consider the representations of the p and d atomic orbitals in Figs. 2-15 and 2- 17. What do the + and signs indicate?
6.29 A mercury atom emits light at many wavelengths, two of which are at 435.8 and 546.1 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) lf a transition between the two higher energy states could be observed, what would be the frequency of the light?
Consider an electron for a hydrogen atom in an excited state. The maximum wavelength of electromagnetic radiation that can completely remove (ionize) the electron from the H atom is 1460 nm. What is the initial excited state for the electron (n = ?)?
The figure below represents part of the emission spectrum for a one-electron ion in the gas phase. All the lines result from electronic transitions from excited states to the n 3 state. (See Exercise 174.) a. What electronic transitions correspond to lines A and B? b. If the wavelength of line B is 142.5 nm, calculate the wavelength of line A.
6.28 A neon atom cmi light at many wavelengths, two of which are at 616.4 and 638.3 nm. Both of these transitions are to the same final state. (a) What is the energy difference between the two states for each transition? (b) If a transition between the two higher energy states could be observed, what would be the frequency of the light?
Until recently, it was thought that Ca was unstable, and that the Ca atom therefore had a negative electron affinity. Some new experiments have now measured an electron affinity of +2.0kJmol1 for calcium. What is the longest wavelength of light that could remove an electron from Ca ? In which region of the electromagnetic spectrum does this light fall?
6.71 Several excited states of the neon atom are important in the operation of a helium-neon laser. In these excited states, one electron of the neon atom is promoted from the 2p level to a higher energy orbital. An excited neon atom with a 1s22s22p55s1 electron configuration can emit a photon with a wavelength of 3391 nm as it makes a transition to a lower energy state with a 1s22s22p54p1 electron configuration. Other transitions are also possible. If an excited neon atom with a 1s22s22p53p1 electron configuration makes a transition to a lower energy state with a 1s22s22p53p1 electron configuration, it emits a photon with a wavelength of 632.8 nm. Find the wavelength of the photon that would be emitted in a transition from the 1s22s22p54p1 electron configuration to the 1s22s22p53p1 electron configuration. (It should help if you start by drawing an energy-level diagram.)

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