Explain the wavelength of light would have sufficient energy

Reference no: EM13490191

-Use Coulomb's law to calculate the ionization energy in of an atom composed of a proton and an electron separated by 234.00pm

-What wavelength of light would have sufficient energy to ionize the atom?

For the first one I got 3.7*10^24 kJ/mol but that was wrong

Reference no: EM13490191

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