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:
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.
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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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Bohr and Balmer Equations concept. If you need more Bohr and Balmer Equations practice, you can also practice Bohr and Balmer Equations practice problems.