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

Answer:

$E=4.847\times 10^{-19}\ J$ is the difference in the energy levels.

Explanation:

Given:

• wavelength of the light emitted for transition of energy levels, $\lambda=4.101\times 10^{-7}\ m$

• initial energy level, $n_i=5$

• final energy level, $n_f=3$

Now as we know that energy can be given by:

$E=\frac{h.c}{\lambda}$

where:

$h= 6.626\times 10^{-34}\ J.s^{-1}$ Planck's Constant

$E=\frac{6.626\times 10^{-34}\times 3\times 10^8}{4.101\times 10^{-7}}$

$E=4.847\times 10^{-19}\ J$ is the difference in the energy levels.