We are asked to **calculate the energy (J) change** associated with an **electron transition from n = 2 to n = 5 **in a Bohr hydrogen atom.

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:**

Calculate the energy (J) change associated with an electron transition from n = 2 to

n = 5 in a Bohr hydrogen atom.

A) 6.5 x 10^{-19}

B) 5.5 x 10^{-19}

C) 8.7 x 10^{-20}

D) 4.6 x 10^{-19}

E) 5.8 x 10^{-53}

Frequently Asked Questions

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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Calzoni's class at MDC.