Final answer:
The transition in the visible range for violet light with a wavelength of 450 nm likely correlates to an electron transitioning from a higher energy level to the second energy level (n=2) in the hydrogen atom. However, none of the provided options (A to D) match typical transitions resulting in violet light and thus we cannot definitively select an answer without additional context.
Step-by-step explanation:
You've asked what transition in the visible range corresponds to violet light with a wavelength of 4.5x102 nm (450 nm). First, let's correct the wavelength's representation, which should be 450 nm instead of 4.5x102 nm. Now, we can refer to the Balmer series of the hydrogen emission spectrum to determine which transition matches the given wavelength. The Balmer series represents the transitions of electrons from higher energy levels (n > 2) to the second energy level (n=2) and falls within the visible range.
To determine the specific transition, we would use the Rydberg formula, which is 1/λ = RH(1/n12 - 1/n22), where RH is the Rydberg constant, λ is the wavelength, n1 is the lower energy level, and n2 is the higher energy level. Since we are dealing with the visible spectrum and specifically violet light, this would typically constitute a transition from a higher level to the n=2 level. However, since the provided options do not match typical transitions that result in violet light (which are usually from levels n=6 or higher to n=2), it is challenging to choose an answer from the options A to D without additional information or clarification. Typically, violet light in the hydrogen spectrum results from higher level transitions such as 6 to 2.