🤓 Based on our data, we think this question is relevant for Professor Lapeyrouse's class at UCF.

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

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, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level.

a. 2.07 x 10^{-29} J

b. 2.19 x 10^{5} J

c. 2.04 x 10^{-18} J

d. 3.27 x 10^{-1}^{7} J

e. 2.25 x 10^{-18} J

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