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We have to classify the given electronic transitions based on whether these take place with absorption of energy or emission of energy. Additionally, we need to find out which one will occur with the greatest change in energy.

The Bohr model for hydrogen atom mentions that the jumping of electrons between orbits is accompanied by absorption or release of electromagnetic radiation (h𝜈).

The amount of energy absorbed or released is given by:

**Where,**

h = Planck’s constant

𝜈 = frequency of photon absorbed or released

For a hydrogen-like atom, classify these electron transitions by whether they result in the absorption or emission of light.

n = 3 to n = 2

n = 3 to n = 5

n = 1 to n = 3

n = 2 to n = 1

Ignoring sign, which transition is associated with the greatest energy change?

a. n = 2 to n = 1

b. n = 1 to n = 3

c. n = 3 to n = 5

d. n = 3 to n = 2

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