Question

The wavelength of the violet light emitted from a hydrogen atom is 410.1 nm. This light is a result of electronic transitions between the n = 5 and n = 2 energy levels. How much higher in energy is the n = 5 energy level than the n = 2 energy level?

Answer 1

`E=4.847* 10^(-19)\ J` is the difference in the energy levels.

Step-by-step explanation:

Given:

• wavelength of the light emitted for transition of energy levels,
  `\lambda=4.101* 10^(-7)\ m`

• initial energy level,
  `n_i=5`

• final energy level,
  `n_f=3`

Now as we know that energy can be given by:

`E=(h.c)/(\lambda)`

where:

`h= 6.626* 10^(-34)\ J.s^(-1)` Planck's Constant

`E=(6.626* 10^(-34)* 3* 10^8)/(4.101* 10^(-7))`

`E=4.847* 10^(-19)\ J` is the difference in the energy levels.