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The UV region typically refers to electromagnetic radiation with wavelengths between 10 nm and 400 nm, encompassing the ultraviolet A (UVA), ultraviolet B (UVB), and ultraviolet C (UVC) regions. This range is just beyond the violet end of the visible spectrum. UV radiation is commonly categorized as UVA (315-400 nm), UVB (280-315 nm), and UVC (100-280 nm) based on the wavelengths involved.
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Why you are use monochromator in uv spectroscopy?
A monochromator in UV spectroscopy is used to isolate a specific wavelength (or range of wavelengths) of light from the UV region of the spectrum. This helps in achieving better wavelength selectivity and accuracy in UV spectroscopic measurements by allowing only the desired wavelengths to pass through to the sample.
What is red solution in uv spectroscopy?
In UV spectroscopy, a red solution could indicate the presence of a compound that absorbs light more in the visible range rather than in the UV range. This could be due to the presence of colored impurities in the sample or the compound itself having strong absorbance in the visible region. Further analysis, such as UV-Vis spectroscopy, can provide more information on the specific properties of the red solution.
Which has the lowest frequency uv- b uv- a uv- c?
UV-C has the lowest frequency among UV wavelengths. UV-C rays range from 100 to 280 nm, while UV-A and UV-B have longer wavelengths and higher frequencies. UV-A ranges from 315 to 400 nm, and UV-B ranges from 280 to 315 nm.
Where does the UV ray get absorbed?
UV rays are mainly absorbed by the ozone layer in the Earth's stratosphere. The ozone layer acts as a protective barrier, absorbing most of the UV radiation before it reaches the Earth's surface. Some UV rays still penetrate the atmosphere and reach the Earth's surface, where they can be absorbed by air, water, and land.
How do hetero cyclic compounds absorb UV light?
Heterocyclic compounds absorb UV light due to the presence of conjugated pi electron systems within their ring structures, which allows for the absorption of light energy. The electrons in the pi system can be excited to higher energy levels by the UV light, resulting in absorption and subsequent electronic transitions.
