= m
= eV
= Hz


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UV Light
Beer's Law
Diode Array
Deuterium Discharge Lamp
Low Pressure Zinc Discharge Lamp
High Pressure Mercury Discharge Lamp
Low Pressure Cadmium Lamp
Tungsten Halogen Lamp
Lens and Window Material in Spectrometers
Fluorescence Reagents
Diffraction Grating
Fourier Transform IR Spectrometer
Halide Disks
Mull Samples
Film Samples for IR Spectroscopy
Light Pipes
Attenuated Total Reflectance Spectroscopy
Multiple Internal Reflectance
External Reflectance
Specular Reflectance
Diffuse Reflectance
Photoacoustic Spectroscopy
Beam Splitter
Raman Scattering
Rayleigh Scattering
Raman Spectroscopy
Atomic Spectroscopy
Atomic Emission Spectroscopy
Atomic Absorption Spectroscopy
The Inductively Coupled Plasma Torch
The Helium Plasma Torch
Emission Spectrometer
Atomic Absorption Spectrometry
Flame Atomic Absorption Spectrometer
Flame AA
Hollow Cathode Lamp
Electrothermal Atomization
Graphite Furnace
L’vov Platform
Electron Paramagnetic Resonance
Zeeman Effect
Continuous Wave
Electron Paramagnetic Resonance
Pulsed EPR
Electron Spin Echo
Multple Resonance Spectroscopy
Magnetic Resonance Spectroscopy
Nucleus Spin Decoupling in NMR
Superconducting Magnets
NMR Microcells
Electron Impact Ionisation
Chemical Ionization
Inductively Coupled Plasma Ionization
Secondary Ion Mass Spectrometry
Fast Atom Bombardment
Plasma Desorption Mass Spectrometry
Laser Desorption Mass Spectrometry
Matrix Assisted Desorption mass Spectrometry
Field Desorption Ionization
Thermospray Ionization
Electrospray Ionization
Atmospheric Pressure Ionization
Particle Beam Interface
Permeable Membrane Interface
Sector Mass Spectrometer
Quadrupole Mass Spectrometer
Ion Trap Mass Spectrometer
Time of Flight Mass Spectrometer
Optical RotationCircular Dichroism
Circularly Polarized Light
Verdet Constant
Faraday Effect

The Absorption of UV and Visible Light

In the practical wavelength range for UV/Visible spectroscopy (i.e. between about 180 nm and 700 nm) the range between 180 nm and 400 nm is considered part of the UV Spectrum and between 400 nm to 700 nm the whole of the Visible Spectrum. The range below 180 nm is sometimes called the vacuum ultraviolet region. In general, it is difficult to operate at wavelengths below 180 nm as most substances adsorb in this region and thus, the walls of the vessel in which the UV Light is generated will be opaque to light of such wavelengths or transmission will be very poor. In practice, the lower wavelength limit is, at present, about 150 nm but most UV spectroscopic measurements made for analytical purposes are carried out at wavelengths between 180 nm and 400 nm. The energy carried by an electromagnetic wave is not continuous, but, as already discussed, are propagated in finite parcels called quanta.

Radiation is only adsorbed by a substance when the energy of the radiation corresponds to that needed to increase the potential energy of the substance (in some form) by one or more increments. As already stated the transfer of energy is largely achieved by the interaction of its electric vector with the substance. Absorption of UV/Visible radiation changes the electronic state of a molecule and can, for example, raise an electron from the ground state (situated in its most stable orbit) to one of its excited states (in some higher orbit). The electronic ground state is one in which all of the electrons of the species are in their most stable orbits. An electronic excited state is one in which at least one of the electrons occupies an orbit of higher energy than that of the ground state. It would appear that if the wavelength of the radiation passing through a substance is gradually changed, and the transmitted light is simultaneously monitored by an appropriate sensor, then the curve resulting from the output of the sensor being plotted against wavelength might show a series of sharp adsorption lines. These lines would occur at frequencies where the radiation energy (hν) was equal to that of specific electronic transitions in the molecules of the substance.

In solution, a given molecule may exhibit numerous adsorption levels that have energies very close to one another. The bands are so close that, in most cases, they cannot be observed individually and, as a result, they occur under one envelope giving a broad band in the UV adsorption Spectrum. The breadth of the band may extend from 50 to 300 nm. This type of absorption is shown in the Spectrum for ethyl ethanoate in figure 4A.

Figure 4A, Absorption Spectrum of Ethyl ethanoate

The Spectrum for ethyl ethanoate is a very simple Spectrum containing no fine structure and would be of little use for solute identification. In contrast it is seen that the aromatic structure of benzene gives a fairly complex Spectrum (shown below in figure 4B)) that could easily be used for identification purposes. This type of spectra is typical of aromatic compounds. Unfortunately, most compounds, particularly those containing the ester and acid groups, give very similar spectra to that of the ester example and, thus, can only be identified from their UV Spectrum with considerable difficulty.

Figure 4A, Absorption Spectrum of benzene

As a consequence, UV spectroscopy is, perhaps, the least helpful of all the spectroscopic techniques from the point of view of confirmation of substance identity or structure identification. It is, however, the most sensitive and the easiest to employ and, in addition, the UV spectrometer is relatively inexpensive. Consequently, despite its technical limitations, it is one of the more common spectroscopic techniques to be employed in solute identification and structure elucidation when appropriate. As the eye is often used in colorimetric measurements, its response to Visible light needs to be considered. A diagram representing the response of the eye to different colours is shown in figure 5.
The numbers on the vertical axis of the graph in figure 5 are not absolute, only relative. It is seen that the eye is most sensitive to green and fairly sensitive to orange and yellow. This is why most road warning signs are now in orange and yellow as opposed to the older signs that are in red (green is not employed as it has been traditionally used for signs signifying safety, or permission to pass). Police jackets and road workers jackets are in yellow and orange so that they can be more clearly seen. It is also seen that red and blue light have a poor retina response which makes signs with black or blue letters on a red background (or vise versa) difficult for older people to see,

Figure 5. The Response of the Eye to Light (Daylight Vision)

Although not indicated in figure 5, the response of the retina to light intensity is not linear so that absolute colorimetric measurements made by visual observation may be very approximate. The eye, however, is very sensitive to slight changes in light intensity and so accurate measurements can be made visually for analytical purposes if very similar light intensities are compared (i.e. by comparators, comparing the colour of a sample with that of a standard). From the data shown in figure 5, comparative colour measurements using green, yellow or orange derivatives would probably give the greatest accuracy.
As an aside, the illusion of colour is an interesting aspect of the effect of Visible light on the sensors of the eye retina (presumably also electric in nature) and the subsequent interpretation of the generated signals by the brain. electromagnetic radiation of 555nm wavelength reflected or generated by an object and striking the retina sensor cells of the eye transmit electrical signals to the brain that then creates the illusion of the colour green. The object appears green in colour. However, there is no such thing as the colour green; it is solely an illusion created by the brain when stimulated by electromagnetic waves of 555nm wavelength. In a similar manner, when exactly the same type of electromagnetic radiation but having a wavelength of 650 nm stimulates the brain, the illusion of the colour red is produced. Again there is no such colour as red, it is merely an illusion generated by the brain when it responds to the stimuli of radiation having a wavelength of 650 nm. In addition, to further complicate an already complex set of illusions, due to the established structure of the atom, all the apparently solid objects of the solar system (and certainly the planets and their contents) are more than 98% empty space (not gas, just vacuum). This will include the mountains, trees, people etc. that, although appearing so real and genuine to human perception, are also illusionary as they are 98% empty space and their surfaces merely reflect light of different wavelengths (the reason for this will become more apparent as progress is made through his book). The combination of these illusionary concepts can be strongly thought provoking but such thoughts are more appropriately considered in a book on philosophy than in a book on spectroscopy.



About the Author
RAYMOND PETER WILLIAM SCOTT was born on June 20 1924 in Erith, Kent, UK. He studied at the University of London, obtaining his B.Sc. degree in 1946 and his D.Sc. degree in 1960. After spending more than a decade at Benzole Producers, Ltd. Where he became head of the Physical Chemistry Laboratory, he moved to Unilever Research Laboratories as Manager of their Physical Chemistry department. In 1969 he became Director of Physical Chemistry at Hoffmann-La Roche, Nutley, NJ, U.S.A. and subsequently accepted the position of Director of the Applied Research Department at the Perkin-Elmer Corporation, Norwalk, CT, U.S.A.
In 1986 he became an independent consultant and was appointed Visiting Professor at Georgetown
University, Washington, DC, U.S.A. and at Berkbeck College of the University of London; in 1986 he retired but continues to write technical books dealing with various aspects of physical chemistry and physical chemical techniques. Dr. Scott has authored or co-authored over 200 peer reviewed scientific papers and authored, co-authored or edited over thirty books on various aspects of physical and analytical chemistry. Dr. Scott was a founding member of the British chromatography Society and received the American Chemical society Award in chromatography (1977), the M. S. Tswett chromatography Medal (1978), the Tswett chromatography Medal U.S.S.R., (1979), the A. J. P. Martin chromatography Award (1982) and the Royal Society of Chemistry Award in Analysis and Instrumentation (1988).
Dr. Scott’s activities in gas chromatography started at the inception of the technique, inventing the Heat of Combustion Detector (the precursor of the Flame Ionization Detector), pioneered work on high sensitivity detectors, high efficiency columns and presented fundamental treatments of the relationship between the theory and practice of the technique. He established the viability of the moving bed continuous preparative gas chromatography, examined both theoretically and experimentally those factors that controlled dispersion in packed beds and helped establish the gas chromatograph as a process monitoring instrument. Dr. Scott took and active part in the renaissance of liquid chromatography, was involved in the development of high performance liquid chromatography and invented the wire transport detector. He invented the liquid chromatography mass spectrometry transport interface, introduced micro-bore liquid chromatography columns and used them to provide columns of 750,000 theoretical plates and liquid chromatography separations in less than a second. Dr. Scott has always been a “hands-on” scientist with a remarkable record of accomplishments in chromatography ranging from hardware design to the development of fundamental theory. He has never shied away from questioning “conventional wisdom” and his original approach to problems has often produced significant breakthroughs.

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