?A series of lines in the spectrum of neutral Li atoms rise from transitions between \(1

Chapter 8, Problem P8C.5

(choose chapter or problem)

A series of lines in the spectrum of neutral Li atoms rise from transitions between \(1 s^{2} 2 p^{1}\) \({ }^{2} \mathrm{P}\) and \(1 \mathrm{~s}^{2} n \mathrm{~d}^{1}\) \({ }^{2} \mathrm{D}\) and occur at 610.36nm, 460.29nm, and 413.23nm. The d orbitals are hydrogenic. It is known that the transition from the \({ }^{2} \mathrm{P}\) to the \({ }^{2} \mathrm{S}\) term (which arises from the ground-state configuration \(1 s^{2} 2 s^{1}\)) occurs at 670.78nm. Calculate the ionization energy of the ground state atom.

Text Transcription:

1 s^22p^1

^2P

1s^2nd^1

^2D

^2P

^2S

1s^22s^1