Periodic Trend: Ionization Energy Video Lessons

Concept: Ionization Energy (IE)

# Problem: Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from the energy state characterized by n = 1, by n = 2.

###### FREE Expert Solution

We can determine Δ E first using the Bohr Equation shown below:

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

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

Calculate ΔE:

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###### Problem Details

Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from the energy state characterized by n = 1, by n = 2.