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THE SPECTRO-PAEDIA

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absorbance
adsorption
Atomization
bandwidth
Beamsplitters
bioluminescence
chemiluminescence
chromatography
electroluminescence
electromagnetic
emission
Emissivity
Fluorescence
luminescence
Michelson
monochromators
photo-multiplier
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photodiodes
photoelectric
photoluminescence
Rayleigh
Raman
spectrofluorometer
spectrometer
spectrophotometer
Spectrum
Transmittance
ultraviolet
Visible
wavelength
Wavenumber
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
Cuvettes
Luminescence
Photoluminescence
Fluorescence
Phosphorescence
Bioluminescence
Radioluminescence
Electroluminescence
Fluorescence Reagents
Spectrum
Diffraction Grating
Interferogram
Fourier Transform IR Spectrometer
FT-IR
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
NMR
Precessing
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
 

Normal Vibration Modes

A molecule can be regarded as an assembly of balls (atomic nuclei) and springs (chemical bonds). The atoms of any molecule with have three coordinates that define its position and potential directions of movement in space and therefore if the molecule has (n) atoms then it will have (3n) translational degrees of freedom. However, if the position of an atom is defined then the bond distance and angle will also be fixed.

Now the molecule as a whole can move in the three coordinate directions and this will utilize three of the degrees of freedom, thus, there will remain (3n-3) degrees of freedom. In the same manner the rotational movement of a non-linear molecule can be resolved into three components and specification of these axis also utilizes three degrees of freedom so the so the total degrees of freedom become (3n-6)

Thus a nonlinear molecule can have (3n – 6) fundamental vibrations.

However, a linear molecule has an exceedingly low energy when rotating about its bond axis and can be considered to only have two rotational degrees of freedom,

Thus, a linear molecule can have (3n – 5) fundamental vibrations

In the case of a diatomic molecule (number of atoms is 2, (i.e.n=2), it can only have one degree of vibrational freedom as the joining bond can only stretch or compress. It will also have three degrees of translational freedom and two degrees of rotational freedom Thus, the diatomic molecule will have six degrees of freedom (i.e.3n = 3x2 = 6, as n=2).

As already considered, there can be two basic forms of a molecule, a non-linear molecule and a linear molecule; a linear and non-linear molecules are typified by carbon dioxide and water and these are shown in figure 3.

Figure 3. Linear and Non-Linear Molecules

Carbon dioxide and water each have three degrees of translational freedom. Water has three degrees of rotational freedom but the linear carbon dioxide molecule has only two degrees of rotational freedom as the molecule rotating about its O-C-O axis involves little or no energy. Thus, the degrees of freedom for vibrational energy will be 3n-5 for carbon dioxide and 3n-6 for water. This relationship is summed up in table 1.

Table 1. The Distribution of Degrees of Freedom for Polyatomic Molecules

Degrees of Freedom Linear Molecules Non-Linear Mol;ecules
Translational 3 3
Rotational 2 3
Vibrational 3n-5 3n-6
Total 3n 3n

The frequency of a vibrational mode will depend on the mass at either end of the bond and the stiffness of the bond. The stiffness of the bond is defined by a proportionality constant called the force constant (k).

The frequency The frequency of the adsorbing wave (ν) is given by,

( 2 )

The constant (μ) is the reduced mass of the system and is calculated from the following equation

(3)


Now, if () is the wave number, (4)

Thus, from (2), (5)

Consequently, a characteristic fundamental frequency and a specific absorption band will be associated with each vibration mode. Vibrations can be due to a change in bond length stretching or alternatively due to a change in the bond angle bending as shown in figure 4. Depending on the molecule (cf. water in figure 3), stretching vibrations can be symmetrical or asymmetrical.

In addition, the stretching process can take place in a number of different ways. Consider now the vibrations possible from bromochloromethane. There are four possible ways the hydrogen -carbon bond can vibrate. These four possibilities are shown diagrammatically in figure 5 and are termed deformation, rock, wags and twists. The two common methods of depicting these processes are included in figure 5.

Figure 4. Example of Stretching and Bending Vibrations

Figure 5. Possible hydrogen carbon Bond Vibrations in bromochloromethane

Fortunately, the analysis of complex molecules is simpler than it might appear. The hydrogen atoms in the molecule can be considered exclusively because they are often attached to more massive and, thus, the more rigid parts of the molecule and, as a consequence, will not have a great effect the hydrogen bond vibrations.

When m1 >>> m2, then, tends to m2, i.e, the mass of the hydrogen atom.

Both UV and IR absorption provide spectra that are characteristic of the molecule and both can be used for compound identification. IR spectra, however, because of the relatively large number of possible absorption bands, show considerable differences between diverse molecules and contain much fine structure. This is in contrast to the majority of UV spectra that are very similar for many compounds even though the structure of the molecules may differ considerably. It follows, that IR spectra can be far more useful for confirming compound identity than UV spectra. Unfortunately, the measurement of an IR Spectrum requires considerably more sample than that required for a UV Spectrum and, thus, although the IR Spectrum is more informative, the technique is not as sensitive.

IR spectra can be presented as curves relating Transmission to, frequency, wavelength or wave numbers; alternatively the curves can relate Absorbance to the same variables. Transmission is obviously the complement of absorption and both methods of presentation are usually available on IR spectrometers. The Spectrum for polystyrene is shown both as a transmission curve and an absorption curve in figure 6.

Figure 6. Two Spectra of polystyrene Presented as an Absorption Spectrum and a Transmission Spectrum

It is seen that the noise on the transmission Spectrum is far greater than the noise on the absorption Spectrum and this is generally true for all spectra. It follows, that it is absorption spectra that are normally used for analytical purposes.

 

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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