Chapter 5, Problem 65A

Interpretation Introduction

Interpretation:

According to the Bohr model, the type of electron-orbit transitions produces the ultraviolet lines in hydrogen’s Lyman series needs to be explained.

Concept introduction:

Bohr suggested that the H-atom contained only such acceptable states of energy. An atom's lowest acceptable energy state is called its ground state. It's said that when an atom absorbs energy it's in an excited state. Bohr relates the energy states of the hydrogen atom to the electron in the atom.

Answer to Problem 65A

The electron-orbit transition is because of the higher energy electrons $n=2$ orbital to the $n=1$ orbit.

Explanation of Solution

According to Bohr, the H-atom is in the first energy level that is in the ground state and its single electrons is in the orbit. H atom does not radiate energy in their ground state. The electron is transferred to the higher energy orbit that is in $n=2$ orbit if energy is applied from an external source.

Conclusion

Lyman series is the hydrogen spectral line of transitions, which occurs due to the ultraviolet emission lines of the hydrogen atom when an electron moves from $n\ge 2$ to $n=1$ orbit.