Question

In a hydrogen atom an electron jumps from 3rd orbit to 1st orbit. During this jump energy is emitted in the form of a photon of light of a definite wave length and frequency. What is the energy associated with the electron before jumping?

Answer 1

If the element is Hydrogen then definitely its atomic no. 1

Answer 2

Answer: $-0.24\times 10^{-18}J$

Explanation:-

Energy of electron given by Bohr is:

$E=-R_H\times {\frac{Z^2}{n^2}$

where : $R_H$ = Rydberg's constant = $2.18\times 10^{-18}J$

Z = atomic number = 1 ( for hydrogen )

n = 3 ( electron before jumping)

Putting the values we get:

$E=-2.18\times 10^{-18}J\times {\frac{1^2}{3^2}$

$E=-0.24\times 10^{-18}J$

Thus the energy associated with the electron before jumping is $-0.24\times 10^{-18}J$