Problem: Ionization involves completely removing an electron from an atom. How much energy is required to ionize a hydrogen atom in its ground (or lowest energy) state? What wavelength of light contains enough energy in a single photon to ionize a hydrogen atom?

FREE Expert Solution

Ionization energy (I. E.) is the energy required to remove an electron from a gaseous atom or ion.


We can determine the energy for Ionization using the Bohr Equation shown below:

E = -RH(1nfinal2-1ninitial2)

ΔE = energy related to the transition, J/atom
RH = Rydberg constant, 2.178x10-18 J
ni = initial principal energy level
nf = final principal energy level


The final principal energy level would be infinity (∞) because the electron is totally removed. 


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Ionization involves completely removing an electron from an atom. How much energy is required to ionize a hydrogen atom in its ground (or lowest energy) state? What wavelength of light contains enough energy in a single photon to ionize a hydrogen atom?

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