Welcome back.! :) My sincere apologies to all my readers for not having posted for a long time.
We were discussing the different types of
spectrophotometers. We have already discussed about the instrumentation and
applications of UV-visible spectrophotometry. In this post, we will have a look
at (infra-red) IR spectrophotometry.
As we have seen earlier that visible light that we are able
to see is just a small part of electromagnetic radiation spectrum. On the
immediate lower side of this visible spectrum lies the infrared and on the
other side lies the ultraviolet. So, in this post, we will be discussing about
the absorption on the lower side of this spectrum. This infrared covers the range of 0.78nm and
1000nm of the electromagnetic spectrum.
We will try to understand the theory of infra-red
absorption. So, to start with, we know that the infra-red radiation is of
higher wavelength as compared to UV-visible region, so the electromagnetic
radiation of this region constantly has low energy. Thus, infra-red radiation is
associated with vibrational transitions of molecules. The atoms in molecules
are in continuous vibration with respect to each other at temperatures above
absolute zero.
Remember that the bond distance between the atoms in a molecule fluctuate to about ±0.5A˚.
Now, there are two kinds of vibrations as:
Remember that the bond distance between the atoms in a molecule fluctuate to about ±0.5A˚.
Now, there are two kinds of vibrations as:
a. Stretching vibrations
b. Bending vibrations
b. Bending vibrations
The stretching vibrations are those where there is an
increase or decrease in the bond length but the atoms remain in the same bond
axis. The bending type of vibrations
involves the changes in the positions of the atoms with respect to bond axis
(here, such variations in bond angles may be about ±0.5˚). These vibrational
transitions are low energy transitions and these energy levels correspond to
the energies of the electromagnetic radiation in the infra-red region of the
spectrum.
So, now we can ask a question as to ‘When does the molecule absorb
radiation?' So, the answer is, when the frequency of a specific vibration equals the frequency of
the IR radiation directed on the molecule, then the molecule absorbs radiation.
Note: Difference in the presentation of IR spectra and UV-visible
spectra:
Firstly, in the IR spectra, wave number is used rather than wavelength. Secondly, IR spectra are typically presented as percent transmission (transmittance x 100) versus wave number.
Firstly, in the IR spectra, wave number is used rather than wavelength. Secondly, IR spectra are typically presented as percent transmission (transmittance x 100) versus wave number.
Modes of Vibration:
Each of the atoms has three degrees of freedom which
corresponds to the motions along any of the three Cartesian coordinate axes (x,
y, z). The theory of molecular vibrations predicts that an asymmetrical molecule
will have 3n – 6 modes of fundamental vibrations where n is the number of atoms
in that molecule. So, by this, the molecule methane (CH4) will have
3 (5) - 6 i.e.; 9 fundamental modes of vibration.
The diagram shown above depicts the vibrational modes
available for AX2 systems (were any atom is joined to two other atoms eg., NO2,
CH2 etc.)
Normally each vibration mode absorbs at a different
frequency. Thus, a CH2 group will give rise to two C - H stretch
bands which maybe symmetric or asymmetric. However, this is not always true. There
will be some vibrations that may absorb at the same frequency and naturally,
their absorption bands will overlap. Such vibrations are said to be degenerate.
Also, there are vibrations whose absorption frequency may lie outside the
normal infrared examined.
Till
now we have seen about the vibrations which are fundamental. There are many
other frequencies at which the bands can appear in an infra-red absorption spectrum.
Some of them are:
Overtone bands: These bands are generated by modulation of fundamental vibrations. Like, strong absorption at 800 cm-1 may give rise to a weaker absorption at 1600 cm-1.
Combinations or Beats: Another kind of modulation is when the two different frequencies x and y interact with each other (combinations). Such interactions may take place as x + y or as x - y. These resulting weaker absorptions are called beats.
Overtone bands: These bands are generated by modulation of fundamental vibrations. Like, strong absorption at 800 cm-1 may give rise to a weaker absorption at 1600 cm-1.
Combinations or Beats: Another kind of modulation is when the two different frequencies x and y interact with each other (combinations). Such interactions may take place as x + y or as x - y. These resulting weaker absorptions are called beats.
You would agree that a particular kind of combination can
occur in that particular compound and in none other. It is so because each
compound has its own particular arrangement of atoms and so we can say that the
combination bands are unique to a compound. Thus, the combination bands have extreme importance because they maybe
signature or the fingerprint of a given compound. In other words, the IR
spectra of no two compounds are alike or we can say conversely that substances
giving the same IR spectra are identical. A large number of compounds fall in
900cm-1 and 1400cm-1. For this reason, this region is called
the “fingerprint region”.
So, these were certain concepts and theory of IR spectrometry. In the next
post, we will have a look at the instrumentation followed by sampling techniques for IR spectroscopy and lastly, applications of
IR spectrophotometry.
After reading this blog, I would like to demand more articles again and again. I am feeling myself as satisfy by got to know these all such information which never came to my knowledge. Please writer more. Molecular spectroscopy
ReplyDelete