Two of the emission wavelengths in the hydrogen emission spectrum are 656 nm and 486 nm. One of these is due to the n = 4 to n = 2 transition, and the other is due to the n = 3 to n = 2 transition. Which wavelength corresponds to which transition?
Here, we are going to identify which of the given wavelengths corresponds to the given transitions.
It is already known that, when an electron jumps from a lower orbit to a higher orbit, it absorbs energy whereas when the electron jumps from higher orbit to lower orbit, it emits energy.
Thus, n = 4 to n = 2 transition corresponds to higher emission of energy compared to n = 3 to n = 2 transition.