= 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 Light

The absorption of light energy can result in the increase in energy of the atom or molecule in a number of different ways. If the light is in the UV/Visible region it can produce an electronic change whereby an electron is moved to an orbit of higher energy. If the light is in the infrared range then it can result in an increase in vibrational or rotational energy. It is not intended here to deal extensively with the wave theory of light but some basic concepts must be introduced to understand the basic mechanics of UV spectrometry.From equation (1) and (2)he energy (E) in a quantum of light of frequency(ν) is given by,


where (c) is the velocity of light, (λ) is the wavelength of the light,

and (h) is Planks constant = 6.62 x 10-27 ergs/sec.
The size of a single quantum of light energy is inconveniently small and so the energy associated with the transition of (N) quanta is used (where (N) is Avogadro’s number 6.02 x 1023, the number of molecules in a gram molecule of the substance). The energy associated with the transition of a gram molecule is called an einstein. Thus, the number of einsteins required to effect a given transition will vary with the frequency of the radiation. Consider first the Bohr atom, which is depicted in figure 6 as a hydrogen atom.

Figure 6. The Bohr Atom

Although now considered obsolete, the Bohr atom serves as a useful introduction to the phenomena of light absorption and light emission and, thus, will briefly be discussed. Bohr depicted the hydrogen atom as a central positively charged nucleus (in the case of hydrogen , a single proton) orbited by a negatively charged electron held in equilibrium by the balanced outward centrifugal force and the inward electrical attractive force. This likens the electron and atom to a planet revolving round a star. The electron could spin round a number of different orbits having different energies in each, the actual energy increasing as the orbit becomes larger. Three such orbits are depicted in figure 6, labelled (n=1), (n=2), and (n=3). The innermost orbit has the lowest energy (n=1).
If light of 656 nm wavelength strikes a hydrogen atom and is absorbed (E= hν) and this can result in an electron in the orbit where n=2 being transferred to the orbit where n=3. In a similar manner if an electron in orbit n=3 falls back to the obit where n=2 then light of 656 nm will be emitted. Thus, the basic mechanics of UV/visible light absorption and fluorescent emission can be accounted for. However, although the energy difference of the electrons between orbits could be understood, an explanation of the factors that control the value of (n) requires a more sophisticated model to be considered. The star-planet model must be significantly modified.
In 1924 the concept was introduced that all electromagnetic radiation could be considered as either waves or particles and furthermore very small particles (i.e. electrons) travelling at high speed could also exhibit wave properties. This was confirmed by experiments that demonstrated the diffraction of electrons (in the manner of light) and ultimately the development of the electron microscope.
In 1924, Broglie produced equations that reconcile, in a relatively simply way, this particle-wave nature as follows.
If(λ) is the wavelength of the wave and (p) the momentum of the particle,
()And for an electron, mass (me) traveling in a straight line at a velocity (v)

Then (5)
The wave nature of the electron easily explains the restricted nature of the different orbits. The electron can only exist in orbits in which the wave is a standing wave.
Such a condition is depicted in figure 7. It follows that if the orbit radius is (r), for a standing wave the circumference of the orbit.
And for an electron, mass (me) travelling in a straight line at a velocity (v)
The integer (n) is known as the principal quantum number introduced by Bohr and can take values of 1.2.3………n

Figure 7. An Electron in Orbit Presented as a Standing Wave

The orbital depicted in figure 7 is for n =12.
The behaviour of an electron as a wave rather than as a particle provoked a quite different approach to the theory called Quantum Mechanics or Wave mechanics. The subject of wave mechanics is outside the scope of this book and for those readers who wish to study the subject further they are recommended to read Basic Atomic and Molecular Spectroscopy by J. Michael Hollas published by the Royal Society of Chemistry.


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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