Question

The energy of the electron in a hydrogen atom can be calculated from the Bohr formula: In this equation stands for the Rydberg energy, and stands for the principal quantum number of the orbital that holds the electron. (You can find the value of the Rydberg energy using the Data button on the ALEKS toolbar.) Calculate the wavelength of the line in the absorption line spectrum of hydrogen caused by the transition of the electron from an orbital with to an orbital with . Round your answer to significant digits.

Answer 1

Answer:

Wavelength,$\lambda=657\ nm$

Explanation:

The energy of the electron in a hydrogen atom can be calculated from the Bohr formula as :

$E=\dfrac{-R}{n^2}$.............(1)

Where

R is the Rydberg constant

n is the number of orbit

We need to find the wavelength of the line in the absorption line spectrum of hydrogen caused by the transition of the electron from an orbital with to an orbital with n₁ = 2 to an orbital with n₂ = 3.

Equation (1) can be re framed as :

$\dfrac{1}{\lambda}=R(\dfrac{1}{n_1^2}-\dfrac{1}{n_2^2})$

$\dfrac{1}{\lambda}=1.096\times 10^7\times (\dfrac{1}{2^2}-\dfrac{1}{3^2})$

$\lambda=6.569\times 10^{-7}\ m$

or

$\lambda=657\ nm$

So, the the wavelength of the line in the absorption line spectrum is 657 nm. Hence, this is the required solution.