Use Coulomb’s law to calculate the ionization energy in kJ>mol of an atom composed of a proton and an electron separated by 100.00 pm. What wavelength of light would have sufficient energy to ionize the atom?

Chemistry by OpenStax (2015-05-04)
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Chapter6: Electronic Structure And Periodic Properties Of Elements
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Problem 83E: Of the five elements Sn, Si, Sb, O, Te, which has the most endothermic reaction? (E represents an...
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Use Coulomb’s law to calculate the ionization energy in kJ>mol of an atom composed of a proton and an electron separated by 100.00 pm. What wavelength of light would have sufficient energy to ionize the atom?

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