INFRARED SPECTROSCOPY (IR)

Theory and Interpretation of

IR spectra
 ASSIGNED READINGS

• Introduction to technique 25 (p. 833-834 in

lab textbook)
• Uses of the Infrared Spectrum (p. 847-853)
• Look over pages 853-866 after viewing this
presentation for additional examples of
various functional groups.
• Emphasis is on data interpretation, not on
data memorization.
 ORGANIC STRUCTURE DETERMINATION

How do we know:
• how atoms are connected together?
• Which bonds are single, double, or triple?
• What functional groups exist in the
molecule?
• If we have a specific stereoisomer?
The field of organic structure determination
attempts to answer these questions.
 INSTRUMENTAL METHODS OF STRUCTURE
DETERMINATION
1. Nuclear Magnetic Resonance (NMR) – Excitation of the nucleus of
atoms through radiofrequency irradiation. Provides extensive
information about molecular structure and atom connectivity.
2. Infrared Spectroscopy (IR) – Triggering molecular vibrations through
irradiation with infrared light. Provides mostly information about the
presence or absence of certain functional groups.
3. Mass spectrometry – Bombardment of the sample with electrons
and detection of resulting molecular fragments. Provides
information about molecular mass and atom connectivity.
4. Ultraviolet spectroscopy (UV) – Promotion of electrons to higher
energy levels through irradiation of the molecule with ultraviolet
light. Provides mostly information about the presence of conjugated
 systems and the presence of double and triple bonds.
 SPECTROSCOPY - Study of spectral
information

Physical response Detecting

Molecule
stimulus instrument

Visual (most common)

representation, or
Spectrum

Upon irradiation with infrared light, certain bonds respond

by vibrating faster. This response can be detected and
translated into a visual representation called a spectrum.
 SPECTRUM INTERPRETATION PROCESS

1. Recognize apattern.
2. Associate patterns withphysical parameters.
3. Identify possible meanings, i.e.propose
explanations.
Once a spectrum is obtained, the main challenge is to
extract the information it contains in abstract, or hidden
form. This requires the recognition of certain patterns, the
association of these patterns with physical parameters, and
the interpretation of these patterns in terms of meaningful
and logical explanations.
 ELECTROMAGNETIC SPECTRUM

Most organic spectroscopy uses electromagnetic energy, or radiation, as

the physical stimulus.

Electromagnetic energy (such as visible light) has no detectable mass

component. In other words, it can be referred to as “pure energy.”

Other types of radiation such as alpha rays, which consist of helium

nuclei, have a detectable mass component and therefore cannot be
categorized as electromagnetic energy.

The important parameters associated with electromagnetic radiation are:

• Energy (E): Energy is directly proportional to frequency, and inversely

proportional to wavelength, as indicated by the equation below.
• Frequency ( )
• Wavelength ()
E = h
EFFECT OF ELECTROMAGNETIC RADIATION
ON MOLECULES

Graphics source: Wade, Jr., L.G.Organic Chemistry , 5th ed. Pearson Education Inc., 2003
 Infrared radiation is largely thermal energy.
It induces stronger molecular vibrations in covalent bonds, which can
be viewed as springs holding together two masses, or atoms.

Specific bonds respond to (absorb) specific frequencies

Graphics source: Wade, Jr., L.G.Organic Chemistry , 5th ed. Pearson Education Inc., 2003
 VIBRATIONAL MODES
• Covalent bonds can vibrate in several modes, including stretching,
rocking, and scissoring.
• The most useful bands in an infrared spectrum correspond to
stretching frequencies, and those will be the ones we’ll focus on.

Graphics source: Wade, Jr., L.G.Organic Chemistry , 5th ed. Pearson Education Inc., 2003
 TRANSMISSION vs. ABSORPTION
When a chemical sample is exposed to the action of IR LIGHT, it can
absorb some frequencies and transmit the rest. Some of the light can
also be reflected back to the source.

Transmitted light
IR Chemical
Detector
source sample

From all the frequencies it receives, the chemical sample

can absorb (retain) specific frequencies and allow the rest
to pass through it (transmitted light).

The detector detects the transmitted frequencies, and by doing so also reveals the
values of the absorbed frequencies.
 AN IR SPECTRUM IN ABSORPTION MODE
The IR spectrum is basically a plot of transmitted (or absorbed) frequencies
vs. intensity of the transmission (or absorption). Frequencies appear in the
x -axis in units of inverse centimeters (wavenumbers), and intensities are
y -axis in percentage units.
plotted on the

The graph above shows a spectrum in absorption mode.

 AN IR SPECTRUM IN TRANSMISSION MODE

The graph above shows a spectrum in transmission mode.

This is the most commonly used representation and the one found in most
chemistry and spectroscopy books. Therefore we will use this representation.
 CLASSIFICATION OF IR BANDS
IR bands can be classified as strong (s), medium (m), or weak (w),
depending on their relative intensities in the infrared spectrum. A strong
band covers most of they -axis. A medium band falls to about half of the
y -axis, and a weak band falls to about one third or less of the
y -axis.
 INFRARED ACTIVE BONDS
Not all covalent bonds display bands in the IR spectrum. Only polar
bonds do so. These are referred to as IR active.
The intensity of the bands depends on the magnitude of the dipole
moment associated with the bond in question:
• Strongly polar bonds such as carbonyl groups (C=O) produce strong
bands.
• Medium polarity bonds and asymmetric bonds produce medium
bands.
• Weakly polar bond and symmetric bonds produce weak or non
observable bands.
 INFRARED BAND SHAPES
Infrared band shapes come in various forms. Two of the most common
are narrow and broad. Narrow bands are thin and pointed, like a
dagger. Broad bands are wide and smoother.

A typical example of a broad band is that displayed by O-H bonds, such

as those found in alcohols and carboxylic acids, as shown below.
 INFORMATION OBTAINED FROM IR SPECTRA

• IR is most useful in providing information about the presence or

absence of specific functional groups.

• IR can provide a molecular fingerprint that can be used when

comparing samples. If two pure samples display the same IR
spectrum it can be argued that they are the same compound.

• IR does not provide detailed information or proof of molecular

formula or structure. It provides information on molecular
fragments, specifically functional groups.

• Therefore it is very limited in scope, and must be used in

conjunction with other techniques to provide a more complete
picture of the molecular structure.
 IR ABSORPTION RANGE
The typical IR absorption range for covalent bonds is 600 - 4000 cm-1. The graph
shows the regions of the spectrum where the following types of bonds normally
absorb. For example a sharp band around 2200-2400 cm-1 would indicate the
possible presence of a C-N or a C-C triple bond.

Graphics source: Wade, Jr., L.G.Organic Chemistry , 5th ed. Pearson Education Inc., 2003
 THE FINGERPRINT REGION
Although the entire IR spectrum can be used as a fingerprint for the purposes of
comparing molecules, the 600 - 1400 cm-1 range is called the fingerprint region. This
is normally a complex area showing many bands, frequently overlapping each other.
This complexity limits its use to that of a fingerprint, and should be ignored by
beginners when analyzing the spectrum. As a student, you should focus your
analysis on the rest of the spectrum, that is the region to the left of 1400 cm-1.

Focus your analysis on this region. This is where most stretching Fingerprint region: complex and difficult to
frequencies appear. interpret reliably.

Graphics source: Wade, Jr., L.G.Organic Chemistry , 6th ed. Pearson Prentice Hall Inc., 2006
 FUNCTIONAL GROUPS AND IR TABLES
The remainder of this presentation will be focused on the IR
identification of various functional groups such as alkenes, alcohols,
ketones, carboxylic acids, etc. Basic knowledge of the structures and
polarities of these groups is assumed. If you need a refresher please
turn to your organic chemistry textbook. The inside cover of the
Wade textbook has a table of functional groups, and they are
discussed in detail in ch. 2, pages 68 – 74 of the 6th edition.

A table relating IR frequencies to specific covalent bonds can be

found on p. 851 of your laboratory textbook. Pages 852 – 866 contain
a more detailed discussion of each type of bond, much like the
discussion in this presentation.
 IR SPECTRUM OF ALKANES
Alkanes have no functional groups. Their IR spectrum displays only C-C and C-H
bond vibrations. Of these the most useful are the C-H bands, which appear around
3000 cm-1. Since most organic molecules have such bonds, most organic
molecules will display those bands in their spectrum.

Graphics source: Wade, Jr., L.G.Organic Chemistry , 5th ed. Pearson Education Inc., 2003
 IR SPECTRUM OF ALKENES
Besides the presence of C-H bonds, alkenes also show sharp, medium bands
corresponding to the C=C bond stretching vibration at about 1600-1700 cm-1.
Some alkenes might also show a band for the =C-H bond stretch, appearing
around 3080 cm-1 as shown below. However, this band could be obscured by the
broader bands appearing around 3000 cm-1 (see next slide)

Graphics source: Wade, Jr., L.G.Organic Chemistry , 5th ed. Pearson Education Inc., 2003
 IR SPECTRUM OF ALKENES
This spectrum shows that the band appearing around 3080 cm-1 can be obscured
by the broader bands appearing around 3000 cm-1.

Graphics source: Wade, Jr., L.G.Organic Chemistry , 6th ed. Pearson Prentice Hall Inc., 2006
 IR SPECTRUM OF ALKYNES
The most prominent band in alkynes corresponds to the carbon-carbon
triple bond. It shows as a sharp, weak band at about 2100 cm-1. The
reason it’s weak is because the triple bond is not very polar. In some
cases, such as in highly symmetrical alkynes, it may not show at all due to
the low polarity of the triple bond associated with those alkynes.

Terminal alkynes, that is to say those where the triple bond is at the end
of a carbon chain, have C-H bonds involving thesp carbon (the carbon
that forms part of the triple bond). Therefore they may also show a sharp,
weak band at about 3300 cm-1 corresponding to the C-H stretch.

Internal alkynes, that is those where the triple bond is in the middle of a
carbon chain, do not have C-H bonds to thesp carbon and therefore lack
the aforementioned band.

The following slide shows a comparison between an unsymmetrical

terminal alkyne (1-octyne) and a symmetrical internal alkyne (4-octyne).
 IR SPECTRUM OF ALKYNES

Graphics source: Wade, Jr., L.G.Organic Chemistry , 6th ed. Pearson Prentice Hall Inc., 2006
 IR SPECTRUM OF A NITRILE
In a manner very similar to alkynes, nitriles show a prominent band around 2250
cm-1 caused by the CN triple bond. This band has a sharp, pointed shape just like
the alkyne C-C triple bond, but because the CN triple bond is more polar, this band
is stronger than in alkynes.

Graphics source: Wade, Jr., L.G.Organic Chemistry , 6th ed. Pearson Prentice Hall Inc., 2006
 IR SPECTRUM OF AN ALCOHOL
The most prominent band in alcohols is due to the O-H bond, and it appears as a
strong, broad band covering the range of about 3000 - 3700 cm-1. The sheer size
and broad shape of the band dominate the IR spectrum and make it hard to miss.

Graphics source: Wade, Jr., L.G.Organic Chemistry , 6th ed. Pearson Prentice Hall Inc., 2006
 IR SPECTRUM OF ALDEHYDES AND KETONES
Carbonyl compounds are those that contain the C=O functional group. In
aldehydes, this group is at the end of a carbon chain, whereas in ketones it’s in the
middle of the chain. As a result, the carbon in the C=O bond of aldehydes is also
bonded to another carbon and a hydrogen, whereas the same carbon in a ketone
is bonded to two other carbons.

Aldehydes and ketones show a strong, prominent, stake-shaped band around

1710 - 1720 cm-1 (right in the middle of the spectrum). This band is due to the
highly polar C=O bond. Because of its position, shape, and size, it is hard to miss.

Because aldehydes also contain a C-H bond to thesp 2 carbon of the C=O bond,
they also show a pair of medium strength bands positioned about 2700 and 2800
cm-1. These bands are missing in the spectrum of a ketone because the
sp 2
carbon of the ketone lacks the C-H bond.

The following slide shows a spectrum of an aldehyde and a ketone. Study the
similarities and the differences so that you can distinguish between the two.
IR SPECTRUM OF ALDEHYDES AND KETONES

Graphics source: Wade, Jr., L.G.Organic Chemistry , 6th ed. Pearson Prentice Hall Inc., 2006
 IR SPECTRUM OF A CARBOXYLIC ACID
A carboxylic acid functional group combines the features of alcohols and ketones
because it has both the O-H bond and the C=O bond. Therefore carboxylic acids
show a very strong and broad band covering a wide range between 2800 and
3500 cm-1 for the O-H stretch. At the same time they also show the stake-shaped
band in the middle of the spectrum around 1710 cm-1 corresponding to the C=O
stretch.

Graphics source: Wade, Jr., L.G.Organic Chemistry , 6th ed. Pearson Prentice Hall Inc., 2006
 IR SPECTRA OF AMINES
The most characteristic band in amines is due to the N-H bond stretch, and it appears as a
weak to medium, somewhat broad band (but not as broad as the O-H band of alcohols). This
band is positioned at the left end of the spectrum, in the range of about 3200 - 3600 cm-1.

Primary amines have two N-H bonds, therefore they typically show two spikes that make this
band resemble a molar tooth. Secondary amines have only one N-H bond, which makes them
show only one spike, resembling a canine tooth. Finally, tertiary amines have no N-H bonds,
and therefore this band is absent from the IR spectrum altogether. The spectrum below
shows a secondary amine.

Graphics source: Wade, Jr., L.G.Organic Chemistry , 6th ed. Pearson Prentice Hall Inc., 2006
 IR SPECTRUM OF AMIDES
The amide functional group combines the features of amines and ketones because
it has both the N-H bond and the C=O bond. Therefore amides show a very strong,
somewhat broad band at the left end of the spectrum, in the range between 3100
and 3500 cm-1 for the N-H stretch. At the same time they also show the stake-
shaped band in the middle of the spectrum around 1710 cm-1 for the C=O stretch.
As with amines, primary amides show two spikes, whereas secondary amides
show only one spike.

Graphics source: Wade, Jr., L.G.Organic Chemistry , 6th ed. Pearson Prentice Hall Inc., 2006
 IR EXERCISE GUIDELINES

Now that you are an IR whiz, you’re ready to download theIR Interpretation
Exercise posted in Dr. Cortes’ website and work on it. The due date is indicated
in the syllabus. If you have any questions please ask Dr. Cortes or your lab
instructor.

Go to http://utdallas.edu/~scortes/ochem

Have fun, and good luck!