Question

7. In the past two sections, you have now examined to different types of spectroscopy: UV-Vis and PES.

a. Sketch a typical atomic energy level diagram (only considering principle quantum number, n) and draw the excitation accomplished by UV-vis spectroscopy (Ground state -> First excited state)

b. In the typical energy level structure above, draw the ionization accomplished by Photoelectron spectroscopy (Ground state -> Ionization)

Answer 1

For the answer please see the below image

nax n=5 NE4 Ionisation n=3 (Excited States n=2- 4 first k Transition Excited state n=1 - •Ground State

a. An electron in an atom stays at its ground state at normal condition but when the atom gets energy as a form of a UV photon or a photon of visible light that photon excites atom’s electrons to a higher energy level this is known as transition. For a transition to occur, the energy absorbed by the electron of the atom must be higher than or equal to the difference in energy between the two energy levels. But once the electron is in the excited, higher energy level, it is in a more unstable on than it was when it was in the ground state. That is why the electron will quickly come back to the ground energy level and during this, it emits a photon with energy the same as the difference in energy levels.

b. When an electron of an atom gets excited by high-energy radiation, such as UV or x-rays then the electron ejected from the atom as the electron reaches the ionization level and the energy which gets by/excited the electron is the ionization energy of the atom/the element.