A pair of atoms joined by a chemical bond are always vibrating
Stronger bonds vibrate faster at a higher frequency and heavier atoms make the bond vibrate more slowly at a lower frequency
When we shine infra-red radiation through a sample, the bonds absorb energy from the radiation and vibrate more
Particular bonds can only absorb radiation that has the same frequency as the natural frequency of the bond
Therefore the radiation that emerges from the sample will be missing the frequencies that correspond to the bonds in the sample
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the peaks in an infra-red spectrum represent particular bonds
you identify the type of bond using the infra-red absorption data
in infra-red spectrums the region below 1500cm-1is known as thefingerprint region, it is due to the vibrations of the whole molecule
some bonds have broad peaks for example, the O-H alcohol group with an absorption of 3220-3550cm-1 while some bonds such as C=O have sharp peaks at 1680-1750cm-1
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Spectra of the Carbonyls (C=O)
Ketones and Aldehydes:
the peak produced by ketones and aldehydes is usually strong and sharp
in aldehydes it is between 1740 and 1720 cm-1
in ketones it is between 1725 and 1700 cm-1
Carboxylic Acids:
have two important peaks
one at around 3100 cm-1 due to an O-H peak
one at around 1700 cm-1 due to a C=O peak
Esters:
a strong C=O peak at around 1750 cm-1
two peaks for the C-O bonds as the stretching frequency of each C-O bonds is different due to the different atoms around them
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