Using the Rydberg calculate the emission wavelengths and state the region of the electromagnetic spectrum of those wavelengths (UV, visible, or infrared) for electron transitions going from a. n-6 to n=3 b. n-3 ton=1
Electronic Transitions and Spectroscopy
The term “electronic” connotes electron, and the term “transition” implies transformation. In a molecule, the electrons move from a lower to a higher energy state due to excitation. The two energy states, the ground state and the excited state are the lowest and the highest energy states, respectively. An energy change is observed with this transition, which depicts the various data related to the molecule.
Photoelectron Spectroscopy
Photoelectron spectroscopy (PES) is a part of experimental chemistry. It is a technique used in laboratories that involves projecting intense beams of radiation on a sample element. In response, the element ejects electrons for which the relative energies are measured.
For the hydrogen like atom the electronic transition occurs between n2 and n1. If the corresponding wavelength for this transition is , then
1/ =
a) for n= 6 to n= 3
here n1=3 n2=6 n1 - final orbital n2- initial orbital
RH - Rydberg constant for H atom = 109677cm-1
1/ =
=109677
=9139.75cm-1
= 1/ 9139.75 = 1.09x10-4 cm
The region corresponding to this particular wavelength is Infrared (IR zone)
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