What is the wavelength (in nm) of a photon if theenergy is 7.49 × 1019 J? (h = 6.626 x 1034 J•s)%3Dnm1346.C789.+/-ㅇx 10013SEP35,997étv S824280MacBook Proor tyn e LURI5

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Answered: What is the wavelength (in nm) of a…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter7: Electronic Structure

Section: Chapter Questions

Problem 7.47QE

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Similar questions

A photoemissive material has a threshold energy, Emin = 5 1019 J. Will 300. nm radiation eject electrons from the material? Explain.
A particular microwave oven delivers 750 watts. (A watt is a unit of power, which is the joules of energy delivered, or used, per second.) If the oven uses microwave radiation of wavelength 12.6 cm, how many photons of this radiation are required to heat 1.00 g of water 1.00C, assuming that all of the photons are absorbed?
The colors of the visible spectrum and the wavelengths corresponding to the colors are given in Figure 5.2. (a) Which colors of light involve photons with less energy per photon than yellow light? (b) Which color of visible light has photons of greater energy, green or violet? (c) Which color of light has the greater frequency, blue or green?
Octyl methoxycinoamate and oxybenzone are common ingredients in sunscreen applications. These compounds work by absorbing ultraviolet (UV) B light (wavelength 280-320 nm), the UV light most associated with sunburn symptoms. What frequency range of light do these compounds absorb?
Cobalt-60 is a radioactive isotope used in medicine for the treatment of certain cancers. It produces particles and rays, the latter having energies of 1.173 and 1.332 MeV. (1 MeV = 106 electron-volts and 1 eV = 1.6022 1019 J.) What are the wave-length and frequency of a -ray photon with an energy of 1.173 MeV?
6.85 The visible lines in the hydrogen atom emission spectrum arise from transitions with a final state with n = 2. In what spectral region should we expect to find transitions that have a final state of n = 1 ? Explain your reasoning using an energy level diagram similar to the one in Problem 6.26.
Spectroscopists have observed He+ in outer space. This ion is a one-electron species like a neutral hydrogen atom. Calculate the energy of the photon emitted for the transition from the n = 5 to the n = 3 state in this ion using the equation: En = − Z2/n2 (2.179 × 10−18 J). Z is the positive charge of the nucleus and n is the principal quantum number. In what part of the electromagnetic spectrum does this radiation lie?
6.86 An excited He+ ion returns to the ground state by emitting a series of three photons, with wavelengths of 26 nm, 469 nm, and 1014 nm. The process is represented in the energy level diagram below. Which arrow (A, B, or C) in the diagram represents the 1014-nm light?

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What is the wavelength (in nm) of a photon if the energy is 7.49 x 1019 J? (h = 6.626 x 10 34 J•s)