We are asked to **calculate the energy (J)** **required to ionize hydrogen from the ground state.**

To calculate the energy required for the electronic transition, we will use the **Bohr Equation** shown below which relates electronic transition to the energy:

$\overline{){\mathit{\Delta}}{\mathit{E}}{\mathbf{=}}{\mathbf{}}{\mathbf{-}}{{\mathit{R}}}_{{\mathbf{H}}}\left(\frac{\mathbf{1}}{{{\mathbf{n}}_{\mathbf{f}}}^{\mathbf{2}}\mathbf{}}\mathbf{-}\frac{\mathbf{1}}{{{\mathbf{n}}_{\mathbf{i}}}^{\mathbf{2}}\mathbf{}}\mathbf{}\right)}$

ΔE = energy related to the transition

R_{H} = Rydberg constant

n_{i} = initial principal energy level

n_{f} = final principal energy level

**Given values:**

How much energy is required to ionize hydrogen in each of the following states?

a. ground state

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