Infrared Spectroscopy: A Quick Primer On Interpreting Spectra (2024)

How To Interpret IR Spectra In 1 MinuteOr Less: The 2 Most Important Things To Look For [Tongue and Sword]

Last post, we briefly introduced the concept of bond vibrations, and we saw that wecan think of covalent bonds as a bit like balls and springs: the springs vibrate, and each one “sings” at a characteristic frequency, which depends on the strength of the bond and on the masses of the atoms. These vibrationshave frequencies that are in the mid-infrared (IR) region of the electromagnetic spectrum.

We can observe and measurethis “singing” of bonds by applying IR radiation to a sample and measuring the frequencies at which the radiation is absorbed. The result is a technique known as Infrared Spectroscopy, which is a useful and quick tool foridentifyingthebonds present in a given molecule.

We saw that the IR spectrum of water was pretty simple – but moving on to a relatively complex molecule like glucose (below) we were suddenly confronted with a forest of peaks!

Your first impression of looking at that IR might be: agh!how am I supposed to make sense of that??

To which I want to say:don’t panic!

Table of Contents

Let’s Correct Some Common Misconceptions About IR
Starting With “Hunt And Peck” Is Not The Way To Go
IR Spectroscopy: The Big Picture
The Two Main Things To Look For In An IR Spectrum: “Tongues” and “Swords”.
Alcohols and Carboxylic Acids: More Detail
Specific Examples of IR Spectra of Carbonyl Functional Groups
Less Crucial, But Still Useful: Two More Very Diagnostic Areas.
Glucose, Revisited: The 1 Minute Analysis
Notes

1. Let’s Correct Some Common Misconceptions About IR

In this post, I want to show that a typical analysis of anIR spectrum is much simpler than you might think. In fact, once you learn what to look for, it can often be done in a minute or less. Why?

IR is not generally used to determine the whole structure of an unknown molecule. For example, there isn’t a person alive who could look at the IR spectrum above and deduce the structure of glucose from it. IR is a tool with a very specific use. [Back in 1945 when IR was one of the few spectral techniques available, it was necessary to spend a lot more time trying to squeeze every last bit of information out of the spectrum. Today, with access to NMR and other techniques, we can do more cherry-picking]
We don’t need to analyze every single peak! (as we’ll see later, that’s what NMR is for : – ) ). Instead, IR is great foridentifying certain specific functional groups,like alcohols and carbonyls. In this way it’s complimentary to other techniques (like NMR) which don’t yield this information as quickly.

With this in mind, we can simplify the analysis of an IR spectrum by cutting out everything except the lowest-lying fruit.

See that forest of peaks from 500-1400 cm^-1 ? We’re basically going to ignore them all!

80% of the most useful information for our purposes can be obtained by looking attwo specific areas of the spectrum: 3200-3400 cm^-1 and 1650-1800 cm^-1. We’ll also see that there are at least two more regions of an IR spectrum worth glancing at, and thus conclude a “first-order” analysis of the IR spectrum of an unknown. [We might write a subsequent post which gets nittier and grittier about the finer points of analyzing an IR spectrum]

Bottom line: The purpose of this post is to show you how toprioritize your timein an analysis of an IR spectrum.

[BTW: all spectra are from the NIST database. Thank you, American taxpayers!]

2. Starting With “Hunt And Peck” Is Not The Way To Go

Confronted with an IR spectrum of an unknown (and a sense of rising panic), what does a typical new student do?

They often reach for the first tool they are given, which is a tableof common ranges for IR peaks given to them by their instructor.

The next step in their analysis is to go through the spectrum from one side to the next, trying to match every single peak to one of the numbers in the table. I know this because this is exactly what I did when I first learned IR.I call it “hunting and pecking”.

The only people who “hunt and peck” as their first step are people who have no plan(i.e. “newbies”).

So by reading the next few paragraphs you can save yourselfa lot of time and confusion.

[Hunt and peck has its place,but only AFTERyou’ve looked for “tongues” and “swords”, below. Hunting and pecking is great to make sure you didn’t miss anything big – but as a first step, it’s bloody awful!]

3. The Big Picture

In IR spectroscopy we measure where molecules absorb photons of IR radiation. The peaks represent areas of the spectrum where specific bond vibrations occur. [for more background, see the previous post, especially on the “ball and spring” model]. Just like springs of varying weights vibrate at characteristic frequencies depending on mass and tension, so do bonds.

Here’s an overview of the IR window from 4000cm^-1to 500cm^-1with various regions of interest highlighted.

4. The Two Main Things To Look For In An IR Spectrum: “Tongues” and “Swords”.

When confronted with a new IR spectrum, prioritize your time by asking two important questions:

Is there a broad, rounded peak in the region around 3400-3200 cm^-1 ? That’s where hydroxyl groups (OH) appear.
Is there a sharp, strong peak in the region around 1850-1630cm^-1 ? That’s where carbonyl groups (C=O) show up.

First, let’s look at some examples of hydroxyl group peaks in the3400 cm^-1to 3200 cm^-1region, which Jon describes vividly as “tongues”. The peaks below all belong to alcohols. Hydrogen bonding between hydroxyl groups leads to some variations in O-H bond strength, which results in a range of vibrational energies. The variation results in the broad peaks observed.

Hydroxyl groups that are a part of carboxylic acids have an even broader appearance that we’ll describe in a bit.

[Sometimes it helps to know what not to look for.On the far right hand side is included one example of a very weak peak on a baseline that you can safely ignore.]

The main point is that a hydroxyl group isn’t generally something you needto go looking for in the baseline noise.

Although hydroxyl groups are the most common type of broad peak in this region, N-H peaks can show up in this area as well (more on them in the Note 1). They tend to have a sharper appearance and may appear as one or two peaks depending on the number of N-H bonds.

Next,let’s look at some examples ofC=O peaks, in the region around 1630-1800 cm^-1.. These peaks are almost always the strongest peaks in the entire spectrum and are relatively narrow, giving them a somewhat “sword-like” appearance.

That sums up our 80/20 analysis: look for tongues and swords.

If you learn nothing else from this post, learn to recognize these two types of peaks!

Two other regions of the IR spectrum can quickly yield useful information if you train yourself to look for them.

3. The line at 3000 cm^-1 is a useful “border” between alkeneC–H (above 3000 cm^-1)and alkane C–H (below 3000 cm^-1) This can quickly help you determine if double bonds are present.

4. A peak in the region around 2200 cm^-1 – 2050 cm^-1is a subtle indicator of the presence of a triple bond [C≡N or C≡C] . Nothing else shows up in this region.

A Common Sense Reminder

First, some obvious advice:

if you’re given the molecular formula, that will determine what functional groups you shouldlook for.It makes no sense to look for OH groups if you have no oxygens in your molecular formula, or likewise the presence of an amine if the formula lacks nitrogen.
Less obviously,calculate the degrees of unsaturationif you are given the molecular formula,because it will provide important clues. Don’t look for C=O in a structure like C₄H₁₀O which doesn’t have any degrees of unsaturation.

5. Alcohols and Carboxylic Acids: More Detail

Alcohols

Let’s look ata specific example so we can see everything inperspective.The spectrum below is of 1-hexanol.

Note the hydroxyl group peak around 3300 cm^-1, typical of an alcohol(That sharp peak around 3600 cm^_-1is a common companion to hydroxyl peaks: it represents non-hydrogen bonded O-H).

As you’d expect for 1-hexanol, thereisn’t any telltale carbonyl peak around 1700 cm^-1. Beginners might be tempted to label that dagger-like strong peak at about 1450 cm^-1as a possible C=O stretch.It is not. (it’s likely a C-H bend). Variations only occur within a very narrow range, and you are extremely unlikely to see a C=O stretch much below 1650 cm^-1. The more spectra you see, the better you’ll get at making these judgements.

To gain some familiarity with variation, here’s some more examples of entire IR spectra of various alcohols.

Carboxylic Acids

6. Specific Examples of IR Spectra of Carbonyl Functional Groups

The secondimportantpeak region is the carbonyl C=O stretch area at about 1630-1830 cm. Carbonyl stretches are sharp and strong.

Once you see a few of them they’re impossible to miss. Nothing else shows up in this region.

To put it in perspective, here’s the IR spectrum of hexanal. That peak a little after 1700 cm^-1 is the C=O stretch. When it’s present, the C=O stretch is almost always the strongest peak in the IR spectrum and impossible to miss.

The position of the C=O stretch varies slightly by carbonyl functional group. Some ranges (in cm^-1 ) are shown below:

Aldehydes (1740-1690): benzaldehyde, propanal, pentanal
Ketones (1750-1680): 2-pentanone, acetophenone
Esters (1750-1735): ethyl acetate, methyl benzoate
Carboxylic acids (1780-1710): benzoic acid, butanoic acid
Amide(1690-1630): acetamide, benzamide,N,N-dimethyl formamide (DMF)
Anhydrides (2 peaks; 1830-1800 and 1775-1740): acetic anhydride, benzoic anhydride

Conjugation will affect the position of the C=O stretch somewhat, moving it to lower wavenumber.

A decent rule of thumb is that you will never, eversee a C=O stretch below1630. If you see a strong peak at 1500, for example, it isnot C=O. It is something else.

7. Less Crucial, But Still Useful: Two More Very Diagnostic Areas.

The C-H Stretch Boundary at 3000 cm^-1

3000 cm^-1 serves as a usefuldividing line. Above this line is observedhigher frequency C-H stretches we attribute to sp² hybridized C-H bonds. Two examples below: 1-hexene (note the peak that stands a little higher) and benzene.

For a molecule with only sp³-hybrized C-H bonds, the lines will appear below 3000 cm^-1 as in hexane, below.

2. The Distinctive Triple Bond Region around 2200 cm^-1

Molecules with triple bonds appear relatively infrequently in the grand scheme of things, but when they do, they do have a distinctive trace in the IR.

The region between 2000 cm^-1 and 2400 cm^-1is a bit of a “ghost town” in IR spectra; there’s very little that appears in this region.If you do see peaks in this region, a likely candidate is a triple bonded carbon such as an alkyne or nitrile.

Note how weak the alkynepeaks are.This is one exception to the rule that one should ignore weak peaks. Still, caution is required: if you’re given the molecular formula, confirm that an alkyne is possible by calculating the degreesof unsaturation and ensuring that it is at least 2 or more.

Terminal alkynes (such as 1-hexyne) also have a strong C-H stretch around3400 cm^-1that is more strongly diagnostic.

8. Glucose, Revisited: The 1 Minute Analysis

OK. We’ve gone over 4 regions that are useful for a quick analysis of an IR spectrum.

(important!) O-H around 3200-3400 cm^-1
(important!) C=O around 1700 cm^-1
C-H dividing line at 3000 cm^-1
(rare) Triple bond region around 2050-2250 cm^-1

Now let’sgo back and look at the IR of glucose.What do we see?

Here are the two big things to note:

OH present around 3300 cm^-1 . (in fact, this was included as one of the “swords” insection #3,above)
No C=O stretch present. No strong peak around 1700 cm^-1 . (The peak at 1450 cm^-1 isn’t a C=O stretch).

Also, if we take a bit of extra time we can see:

No alkene C-H (no peaks above 3000 cm^-1)
Nothing in triple bonded region (rare, but still an easy thing to learn to check)

Now: If you were given this spectrum as an “unknown” along with its molecular formula, C₆H₁₂O₆, what conclusions could you draw about its structure?

The molecule has at least one OH group (and possibly more)
The molecule doesn’t have any C=O groups
The molecule *likely* doesn’t have any alkenes. If any alkenes are present, they don’tbear any C-H bonds, because we’d see their C-H stretch above 3000 cm^-1.

A molecule with one degree of hydrogen deficiency (C₆H₁₂O₆) but no C=O, and likely no C=C ?

A good guess would be that the molecule contains a ring. (We know this is the case, of course, but it’s nice to see the IR confirming what we already know).

This is what a 1-minute analysis of the IR of glucose can tell us. Not the whole structure, mind you, but certainly some important bits and pieces.

That’s enough for today. In the next post we’ll do some more 1-minute analyses and give more concrete examples of how to use the information in an IR spectrum to draw conclusions about molecular structure.

Notes

Related Articles

IR Spectroscopy: 4 Practice Problems
Bond Vibrations, Infrared Spectroscopy, and the “Ball and Spring” Model
Introduction To UV-Vis Spectroscopy
UV-Vis Spectroscopy: Practice Questions
UV-Vis Spectroscopy: Absorbance of Carbonyls
Degrees of Unsaturation (or IHD, Index of Hydrogen Deficiency)

Note 1.

More on the 3200 region: Amines, Amides, and Terminal Alkyne C-H

While we’re in the 3200 region…. Amines and Amides

Amines and amides also have N-H stretches which show up in this region. [update: a comment from Paul Wenthold mentions some helpful advice about amides – they are rare – look for confirming evidence from the mass spectrum or other sources before assigning an amide based on a stretch in this region, as this region can also contain carbonyl “overtone” peaks]

Notice how the primary amine and primary amide have two “fangs”, while the secondary amine and secondary amide have a single peak.

The amine stretches tend to be sharper than the amide stretches; also the amides can be distinguished by a strong C=O stretch (see below).

Primary amines (click for spectra)

Secondary amines:

Primary amides

Secondary amides

N-methyl benzamide

Terminal alkyne C-H

Terminal alkynes have a characteristic C-H stretch around 3300 cm^-1. Here it is for ethynylbenzene, below.

Ethynylbenzene

3600 – 2700 cm^-1	X-H (single bonds to hydrogen)
2700 – 1900 cm^-1	X≡X (triple bonds)
1900 – 1500 cm^-1	X=X (double bonds)
1500 – 500 cm ^-1	X–X (single bonds)