Atomic Spectra Post Module

[Amy Luu 2G]

The transition from n = 4 to n = 2 emits radiation of longer wavelength than the transition from n = 5 to n = 1. This statement is true, however, I am confused as to why this is true. I thought the wavelength of the transition from n=5 to n=1 would be a longer wavelength. Are there any calculations or can you use the model to figure this out?

[Angus Wu_4G]

You would expect the transition from n=5 to n=1 to release more energy than the transition from n=4 to n=2 because going from 5 to 1 is going through more levels.

Using the equation E=(hc)/(wavelength), we can see that the longer the wavelength, the lower the energy is. Therefore, the transition from 5 to 1 because it releases more energy, it should have a smaller wavelength.

[Karyn How 1J]

When electrons jump down levels, they emit energy based on how many levels they are jumping. Since jumping from n=5 to n=1 is farther, the elctron would emit more energy. If the energy is greater, that means the frequency will be a lot higher than the transition from n = 4 to n = 2 (based off the E = hv equation). Higher frequency means a shorter wavelength since they are indirectly proportional as c is a constant (c = λν).

[aishwarya_atmakuri]

The energy transition from n=5 to n=1 requires more energy than the energy transition from n=4 to n=2. More energy means shorter wavelength (E=hv), so the electron going from n=5 to n=1 would emit more energy.

[AmyL_3L]

The transition from n=5 to n=1 emits radiation of shorter wavelength because it requires more energy. Therefore, the frequency is higher than the frequency given off by the transition from n=4 to n=2. Since higher frequencies mean shorter wavelengths, this means the transition from n=5 to n=1 has a shorter wavelength, despite emitting more energy.