**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:**

$\overline{){\mathbf{\u2206}}{\mathbf{E}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{-}}{{\mathbf{R}}}_{{\mathbf{H}}}\mathbf{(}\frac{\mathbf{1}}{{{\mathbf{n}}_{\mathbf{final}}}^{\mathbf{2}}}\mathbf{-}\frac{\mathbf{1}}{{{\mathbf{n}}_{\mathbf{initial}}}^{\mathbf{2}}}\mathbf{)}}$

ΔE = energy related to the transition, J/atom

R_{H} = Rydberg constant, 2.178x10^{-18} J

n_{i} = initial principal energy level

n_{f} = 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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