Chapter 7, Problem 7.7P

Interpretation Introduction

Interpretation:

The wavelength of the absorbed light is to be calculated.

Concept introduction: if an atom absorbs energy then this atom gets excited from the lower energy orbital to the higher energy orbital. This state of an atom is termed as excited state. The energy absorbed by an atom is calculated by the Planck’s equation. This equation is,
   $E=\frac{hc}{\lambda }$

Where,

• $E$ is the energy absorbed by the atom.
• $\lambda$ is the is the wavelength of light.
• $c$ is the speed of light.
• $h$ is the Planck’s constant.

The value of Planck’s constant $\left(h\right)$ is $6.626\times {10}^{-34}\text{J}$ .

To determine: The wavelength of the light absorbed when an electron in a hydrogen atom makes a transition from an orbital $n=2$ to $n=7$ .