The minimum frequency of light needed to eject electrons from a metal is called the threshold frequency, vo. Find the minimum energy needed to eject electrons from a metal with a threshold frequency of 4.00 x 1014 s-1. E, = J With what maximum kinetic energy will electrons be ejected when this metal is exposed to light with a wavelength of 235 nm? KEelectron = J

The minimum frequency of light needed to eject electrons from a metal is called the threshold frequency, vo. Find the minimum energy needed to eject electrons from a metal with a threshold frequency of 4.00 x 1014 s-1. E, = J With what maximum kinetic energy will electrons be ejected when this metal is exposed to light with a wavelength of 235 nm? KEelectron = J

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

Chapter4: Introduction To Quantum Mechanics

Section: Chapter Questions

Problem 50AP

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Similar questions

You are an engineer designing a switch that works by the photoelectric effect. The metal you wish to use in your device requires 6.7 1019 J/atom to remove an electron. Will the switch work if the light falling on the metal has a wavelength of 540 nm or greater? Why or why not?
In the photoelectric effect, electrons are ejected from a metal surface when light strikes it. A certain minimum energy, Emin, is required to eject an electron. Any energy absorbed beyond that minimum gives kinetic energy to the electron. It is found that when light at a wavelength of 540 nm falls on a cesium surface, an electron is ejected with a kinetic energy of 2.601020J. When the wavelength is 400 nm, the kinetic energy is 1.541019J. (a) Calculate Emin for cesium in joules. (b) Calculate the longest wavelength, in nanometers, that will eject electrons from cesium.
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?
6.14 For photon with the following energies, calculate the wavelength and identify the region of the spectrum they are from. (a) 3.51020 J, (b) 8.71026 J, (c) 7.11017 J, (d) 5.51027 J
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.
An energy of 3.3 1019 J/atom is required to cause a cesium atom on a metal surface to lose an electron. Calculate the longest possible wavelength of light that can ionize a cesium atom. In what region of the electromagnetic spectrum is that radiation found?
The most prominent line in the emission spectrum of magnesium is 285.2 nm. Other lines are found at 383.8 and 518.4 nm. In what region of the electromagnetic spectrum are these lines? What is the energy of 1.00 mol of photons with the wavelength of the most energetic line?
(a) Give the complete electron configuration (1s22s22p) of aluminum in the ground state. (b) The wavelength of the radiation emitted when the outermost electron of aluminum falls from the 4s state to the ground state is about 395 nm. Calculate the energy separation (in joules) between these two states in the Al atom. (c) When the outermost electron in aluminum falls from the 3d state to the ground state, the radiation emitted has a wavelength of about 310 nm. Draw an energylevel diagram of the states and transitions discussed here and in (b). Calculate the separation (in joules) between the 3d and 4s states in aluminum. Indicate clearly which has higher energy.