Tuesday, November 27, 2018

The Basic Principle of UV Spectroscopy

The ultraviolet-visible spectroscopy (UV) is an important method of analytical chemistry and it is one of the commonly used for the identification of chemicals and qualitative analysis. However, quantitative analysis of various inorganic and organic compounds is the most important use of UV. Principally, UV spectroscopy is associated with the interaction of light with the matter since, the light is absorbed by the substance/matter, the resultant energy content of atoms or molecules increases. The absorption of ultraviolet or visible light by an analyte will generate a specific spectrum, while ultraviolet radiation is absorbed; it results in the electrons excitation in the state of high energy from the ground state. The theory that revolves about this concept suggests that the energy absorbed by ultraviolet radiation is equivalent to the energy difference between the ground and high energy state.
UV spectrophotometer principle adheres to the Beer-Lambert Law; this law expresses that when a beam of monochromatic light is gone through a sample solution an absorbing analyte. The diminishing rate of the radiation power alongside the thickness of the sample solution is really corresponding to the incident radiation and solution concentration.
Beer-Lambert Law is expressed through this equation:
A = log (I0/I) = ECI.
It is clear from the Beer-Lambert law that the number of molecules able to absorb the light of a specified wavelength, the light absorption limit is high. This is the fundamental principle of UV spectroscopy.


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