Electronic transition level

 

It was earlier stated that σ, π, and n electrons are present in molecule and can be excited from the ground state to excited state by the absorption of UV radiation. The various transitions are n→*, *, n→σ*, & σ →σ*

Fig 1: Energy levels of electronic transitions

Fig. 1 shows the energy requirements for different electronic transitions.
The energy requirement order for excitation for different transitions is as follows.
n→*< *< n→σ*< σ→σ*
n→* transition requires lowest energy while σ→σ* requires highest amount of energy.

 

1. n→* transition
n→π* transition requires lowest energy due to longer wavelength. So they are forbidden and corresponding bands are characterized by low molar absorptivity. εmax < 100. It is also known as R- band. They are further characterized by hypsochromic shift or blue shift observed with an increase in solvent polarity.

2. * transition
It is due to the promotion of an electron from a bonding π orbital to an anti-bonding * orbital. Energy requirement is between n→ * and n→σ*. But the extended conjugation and alkyl substituents shifts the λmax towards longer wavelength (Bathochromic shift). It is also called K band.

3. n→σ* transition
Saturated compounds with lone pair of electrons undergo n→σ* transition in addition to σ→σ* transition. Corresponding absorption bands appear at longer wavelengths in near UV region.

4. σ→σ* transition
These transitions can occur in such compounds in which all the electrons are involved in single bonds and there are no lone pair of electrons.
Energy required for σ→σ* transition is very large so the absorption band occurs in the far UV region. So this transition cant normally be observed.

FIND MORE :-

Theory of Spectroscopy EMR Spectra
Beer-Lambert's Law Instrumentation
Effect of Solvent Applications