Chapter 5, Problem 5.137CP

Interpretation Introduction

Interpretation:

‘Energy state’ should be identified.

Concept introduction: The electron jumps from n=1 to n=2 is called the 1^st excitation and n=2 to n=3 is 2^nd excitation and like that. It is seen that as the number of n increases the energy gap between the successive orbitals decreases. The energy required to jump one electron from n=1 to n= infinity is called the ionisation energy of the atom.
The position of the electron on consumption of certain amount of energy is determined by Balmer-Rydberg equation, which is $\overline{\upsilon }=R\left[\frac{1}{n_1^2}-\frac{1}{n_2^2}\right]$.

Given:

The wave length ( $\lambda$ ) of the UV light is $1.03\times {10}^{-7}m$. The initial shell from which the electron jumps i.e. $n_1$ = 1

To determine:

On absorption of ultra violet light at the ground state of wave length $1.03\times {10}^{-7}m$ the position of the electron.