INTERPRETATION OF INFRARED SPECTRA, A PRACTICAL APPROACH 1
absorptions in the spectrum. This information can indicate Interpretation of Infrared whether there is backbone to the structure and, if so, Spectra, A Practical Approach whether the backbone consists of linear or branched chains. Next it is possible to determine if there is unsaturation and/or aromatic rings in the structure. Finally, it is possible John Coates to deduce whether specific functional groups are present. Coates Consulting, Newtown, USA If detected, one is also able to determine local orientation of the group and its local environment and/or location in the structure. The origins of the sample, its prehistory, and the manner in which the sample is handled all have impact 1 Introduction 1 on the final result. Basic rules of interpretation exist and, 2 The Origins of the Infrared Spectrum 2 if followed, a simple, first-pass interpretation leading to 3 Spectral Interpretation by Application of material characterization is possible. This article addresses Vibrational Group Frequencies 6 these issues in a simple, logical fashion. Practical examples 3.1 The Hydrocarbon Species and are included to help guide the reader through the basic Molecular Backbone 6 concepts of infrared spectral interpretation. 3.2 Simple Functional Groups 9 3.3 The Carbonyl Group 12 3.4 Other Functional Groups Associated with Heteroatoms 13 1 INTRODUCTION 3.5 Simple Inorganics 14 4 The Practical Situation – Obtaining the The qualitative aspects of infrared spectroscopy are one Spectrum and Interpreting the Results 15 of the most powerful attributes of this diverse and 4.1 Sample History 16 versatile analytical technique. Over the years, much has 4.2 Physical Characteristics of the been published in terms of the fundamental absorption Sample 17 frequencies (also known as group frequencies) which are 4.3 The Chemistry of the Sample 17 the key to unlocking the structure–spectral relationships 4.4 The Infrared Sampling Method 18 of the associated molecular vibrations. Applying this knowledge at the practical routine level tends to be 5 An Overview to Infrared Spectral a mixture of art and science. While many purists will Interpretation – Some Simple Rules and argue against this statement, this author believes that it Guidelines 19 is not possible to teach a person to become proficient as 5.1 A Quick Diagnostic Assessment of an interpretive spectroscopist by merely presenting the an Infrared Spectrum 20 known relationships between structure and the observed Abbreviations and Acronyms 22 spectra. Instead, the practical approach, which has been Related Articles 22 adopted in this text, is to help the reader appreciate the References 23 visual aspects of the spectroscopy and how to interpret these relative to the structure and chemistry of the sample. This is achieved by recognizing characteristic shapes and patterns within the spectrum, and by applying the The vibrational spectrum of a molecule is considered to information obtained from published group frequency be a unique physical property and is characteristic of the data, along with other chemical and physical data from molecule. As such, the infrared spectrum can be used as the sample. a fingerprint for identification by the comparison of the Included in the text is a discussion of the interrelation- spectrum from an ‘‘unknown’’ with previously recorded ships that exist between the practical side of acquiring reference spectra. This is the basis of computer-based the spectrum, the chemistry and physics of the sample spectral searching. In the absence of a suitable reference under study, the physical interactions of the sample with database, it is possible to effect a basic interpretation of the its environment, and the impact of the structure on the spectrum from first principles, leading to characterization, spectrum. In essence, the interpretation of infrared spec- and possibly even identification of an unknown sample. tra is much more than simply assigning group frequencies. This first principles approach is based on the fact that The spectrum is rich in information, and this article is structural features of the molecule, whether they are the intended to help the reader to extract the maximum backbone of the molecule or the functional groups attached using the knowledge available for the sample and the to the molecule, produce characteristic and reproducible acquired spectral data. One important factor to bear in
Encyclopedia of Analytical Chemistry R.A. Meyers (Ed.) Copyright John Wiley & Sons Ltd 2 INFRARED SPECTROSCOPY mind is that a successful interpretation is based not only bromide, KBr). For this reason, when a spectral region is on the presence of particular bands within the spectrum, quoted in the text, the higher value will be quoted first, but also the absence of other important bands. Complete consistent with the normal left-to-right (high to low cm 1) classes of compounds can be rapidly excluded during the representation of spectra. Also, the terms infrared band, interpretation by the use of no-band information. peak and absorption will be used interchangeably within It must be understood that this article addresses the text to refer to a characteristic spectral feature. the issue of infrared spectral interpretation from the The spectral group frequencies provided in this text perspective of the average operator of an infrared were obtained from various literature sources published instrument. It is not a detailed treatise on the theory over the past 30 years, and most of these are included of infrared spectroscopy where the modes of vibration in the cited literature. Every attempt to ensure accuracy are discussed in terms of group theory, and where has been taken; however, there will be instances when mathematical models are used to compare theoretical individual functional groups may fall outside the quoted and observed values for the fundamental vibrations of a ranges. This is to be expected for several reasons: the molecule. There are many excellent texts that cover this influences of other functional groups within a molecule, subject..1–4/ Instead, this article focuses on the day-to- the impact of preferred spatial orientations, and environ- day problems associated with characterizing a material or mental effects (chemical and physical interactions) on the attempting to perform some form of identification. One molecule. of the main challenges in presenting a text on spectral The preferred format for presenting spectral data for interpretation is to form a balance between the theory qualitative analysis is in the percentage transmittance that is needed to appreciate the links between molecular format, which has a logarithmic relationship ( log10)with structure and the observed spectrum and the practice. respect to the linear concentration format (absorbance). For this reason, a minimum amount of relevant theory This format, which is the natural output of most is included in the next section, which provides a basic instruments (after background ratio), provides the best understanding of why the spectrum exists, how it is dynamic range for both weak and intense bands. In this formed, and what factors contribute to the complexity case, the peak maximum is actually represented as a of observed spectra. It has been assumed that the reader minimum, and is the point of lowest transmittance for a has a fundamental knowledge of molecular theory and particular band. bonding, and that there is an understanding of basic structures, in particular for organic compounds. Infrared spectral interpretation may be applied to both organic and inorganic compounds, and there are 2 THE ORIGINS OF THE INFRARED many specialized texts dealing with these compounds, in SPECTRUM combination and as individual specialized texts. There are too many to reference comprehensively, and the In the most basic terms, the infrared spectrum is formed reader is directed to a publication that provides a as a consequence of the absorption of electromagnetic bibliography of the most important reference texts..5/ radiation at frequencies that correlate to the vibration of However, the most informative general reference texts specific sets of chemical bonds from within a molecule. are included,.6–14/ with books by Socrates.10/ and Lin- First, it is important to reflect on the distribution of energy Vien.11/ being recommended for general organics, and possessed by a molecule at any given moment, defined as by Nakamoto.13/ and Nyquist et al..14/ for inorganics the sum of the contributing energy terms (Equation 1): (salts and coordination compounds). There are numerous specialized texts dealing with specific classes of materials, Etotal D Eelectronic C Evibrational C Erotational C Etranslational and undoubtedly polymers and plastics form the largest .1/ individual class..15–17/ In this particular case, texts by The translational energy relates to the displacement of Hummel and Scholl.16/ and Koenig.17/ provide a good molecules in space as a function of the normal thermal basic understanding. motions of matter. Rotational energy, which gives rise The following comments are made relative to the con- to its own form of spectroscopy, is observed as the ventions used within this article. The term frequency tumbling motion of a molecule, which is the result of is used for band/peak position throughout, and this is the absorption of energy within the microwave region. expressed in the commonly used units of wavenum- The vibrational energy component is a higher energy ber (cm 1). The average modern infrared instrument term and corresponds to the absorption of energy by a records spectra from an upper limit of around 4000 cm 1 molecule as the component atoms vibrate about the mean (by convention) down to 400 cm 1 as defined by the center of their chemical bonds. The electronic component optics of the instrument (commonly based on potassium is linked to the energy transitions of electrons as they INTERPRETATION OF INFRARED SPECTRA, A PRACTICAL APPROACH 3 are distributed throughout the molecule, either localized of a bond between two atomic centers. The fundamental, within specific bonds, or delocalized over structures, such which involves an energy transition between the ground as an aromatic ring. In order to observe such electronic state and the first vibrational quantum level, is essen- transitions, it is necessary to apply energy in the form of tially unaffected by the anharmonicity terms. However, visible and ultraviolet radiation (Equation 2): transitions that extend beyond the first quantum level (to the second, third, fourth, etc.), which give rise to E D hn frequency/energy .2/ weaker absorptions, known as overtones, are influenced by anharmonicity, which must be taken into account The fundamental requirement for infrared activity, lead- when assessing the frequency of these higher frequency ing to absorption of infrared radiation, is that there must vibrations. be a net change in dipole moment during the vibration Having defined the basis for the simple vibration of for the molecule or the functional group under study. an atomic bond, it is necessary to look at the molecule Another important form of vibrational spectroscopy is as a whole. It is very easy to imagine that there is an Raman spectroscopy, which is complementary to infrared infinite number of vibrations, which in reality would spectroscopy. The selection rules for Raman spectroscopy lead to a totally disorganized model for interpretation. are different to those for infrared spectroscopy, and in Instead, we describe the model in terms of a minimum this case a net change in bond polarizability must be set of fundamental vibrations, based on a threefold set of observed for a transition to be Raman active. The remain- coordinate axes, which are known as the normal modes ing theoretical discussion in this article will be limited to a of vibration. All the possible variants of the vibrational very simple model for the infrared spectrum. The reader motions of the molecule can be reduced to this minimum is encouraged to refer to more complete texts.2–4/ for set by projection on to the threefold axes. It can be shown detailed discussion of the fundamentals. that the number of normal modes of vibration for a given While it was stated that the fundamental infrared molecule can be determined from Equations (4) and (5): absorption frequencies are not the only component to be evaluated in a spectral interpretation, they are the essence number of normal modes D 3N 6 (nonlinear) .4/ and foundation of the art. For the most part, the basic model of the simple harmonic oscillator and its modifica- D 3N 5 (linear) .5/ tion to account for anharmonicity suffice to explain the where N is the number of component atoms in the origin of many of the characteristic frequencies that can molecule. be assigned to particular combinations of atoms within In practice, apart from the simplest of compounds, most a molecule. From a simple statement of Hooke’s law we molecules have nonlinear structures, except where a spe- can express the fundamental vibrational frequency of a cific functional group or groups generate a predominant molecular ensemble according to Equation (3): linear arrangement to the component atoms. If we calcu- r 1 k late the number of modes for a simple hydrocarbon, such n D .3/ 2pc µ as methane (nonlinear, tetrahedral structure), a value of nine is obtained. This would imply that nine sets of absorp- where n D fundamental vibration frequency, k D force tion frequencies would be observed in the spectrum of constant, and µ D reduced mass. The reduced mass, µ D methane gas. In reality, the number observed is far less, m1m2/.m1 C m2/,wherem1 and m2 are the component corresponding to the asymmetric and symmetric stretch- masses for the chemical bond under consideration. ing and bending of the C H bonds about the central This simple equation provides a link between the carbon atom. The reason for the smaller than expected strength (or springiness) of the covalent bond between number is that several of the vibrations are redundant or two atoms (or molecular fragments), the mass of the inter- degenerate, that is, the same amount of energy is required acting atoms (molecular fragments) and the frequency of for these vibrations. Note that although a small number vibration. Although simple in concept, there is a rea- of vibrational modes is predicted, and in fact observed, sonably good fit between the bond stretching vibrations the appearance of the methane spectrum at first glance predicted and the values observed for the fundamentals. is far more complex than expected, especially at higher This simple model does not account for repulsion and spectral resolutions (<1cm 1). At relatively high resolu- attraction of the electron cloud at the extremes of the tions, a fine structure is superimposed, originating from vibration, and does not accommodate the concept of rotational bands, which involve significantly lower energy bond dissociation at high levels of absorbed energy. A transitions. Each of the sets of vibrational–rotational model incorporating anharmonicity terms is commonly absorptions manifest this superimposed fine structure used to interpret the deviations from ideality and the for low-molecular-weight gaseous compounds, methane overall energy–spatial relationship during the vibration being a good example. Several medium-molecular-weight 4 INFRARED SPECTROSCOPY compounds may also show evidence of some fine struc- combination of the bands associated with these group ture when studied in the vapor state. For example, it is frequencies and the skeletal frequencies are used to common to observe the sharp feature (or spike) assigned identify a specific compound. The latter forms the basis of to the Q-branch of the vibrational–rotational spectrum, the use of reference spectra for spectral matching by visual as indicated by the vapor spectrum of acetone (Figure 1). comparison or by computer-based searching, for the If we proceed up the homologous series from methane identification of an unknown from its infrared spectrum. (CH4)ton-hexane (C6H14), there are 20 component The group frequencies may be viewed quantitatively, atoms, which would imply 54 normal modes. In this case as well as qualitatively. A given absorption band assigned the picture is slightly more complex. Methane is a unique to a functional group increases proportionately with the molecule, and only contains one type of C H group – no number times that functional group occurs within the other types of bond exist in this molecule. In hexane there molecule. For example, in the spectrum of n-hexane, the are several types of bond and functionality. For reference, intensities measured for the group frequency absorptions a simple two-dimensional representation of the structure assigned to methyl and methylene correspond to four is provided in Figure 2(a). methylene groups and two methyl groups on a rel- As we can see, there are two terminal methyl groups ative basis, when compared with other hydrocarbon (CH3) and four connecting methylene groups (CH2). compounds within a homologous series. For example, Each of these groups has its corresponding C H if we examine the C H stretching (or bending) band stretching and bending vibrations (see later text for the intensities for CH3 and CH2, we will observe that the actual absorption frequencies). Also, the methyl groups relative intensities of CH3 to CH2 decrease with increase are linked to a neighboring methylene group, which is in chain length. Restated, there is less methyl contribu- in turn linked to neighboring methylene groups, and so tion and more methylene contribution with increase in on. These linkages feature carbon–carbon bonds. For chain length/molecular weight. The reverse holds true if interpretation, we view the C H groups as functional we examine the spectra of linear hydrocarbons with chain groups, giving rise to the common group frequencies, lengths shorter than that of hexane. and the C C linkages as the backbone, producing the If we apply these ideas to a different hexane iso- skeletal vibrations. As a rule, a group frequency may mer, such as isohexane (2-methylpentane), we would be applied generally to most compounds featuring the see significant differences in the spectrum. These can be corresponding functional group. In contrast, the skeletal explained by evaluating the structure (Figure 2b), which vibrations are unique to a specific molecule. The group contains three methyl groups, two methylene groups, and frequencies help to characterize a compound, and the a group that contains a single hydrogen attached to car- bon (the methyne group). This adds a new complexity 100 to the spectrum: the main absorptions show differences in appearance, caused by the changes in relative band 80 Q intensities, splittings of absorptions occur (originating 60 from spatial/mechanical interaction of adjacent methyl groups), and changes are observed in the distributions of Q Q 40 the C C skeletal vibrations, in part due to the splitting by the methyl side chain. Further discussions concerning the 20 impact of chain branching are covered later in this article. Q Transmittance (%) Transmittance 0 Comparison of Figures 3 and 4 provides a graphical repre- sentation of the aspects discussed for the hexanes of struc- 800 600 400 4000 3600 3200 2800 2400 2000 1800 1600 1400 1200 1000 turally similar compounds, i.e. n-heptane and isooctane. Wavenumber (cm−1) From a first-order perspective, the idea of the quan- titative aspects of the group frequencies carries through Figure 1 Vapor spectrum of acetone with characteristic for most functional groups, and the overall spectrum is Q-branch slitting, denoted by Q. Copyright Coates Consulting. essentially a composite of the group frequencies, with band intensities in part related to the contribution of each H functional group in the molecule. This assumes that the H HH HH HH H H C H functional group does give rise to infrared absorption H C C CH C C H HC C C H H C C C H frequencies (most do), and it is understood that each H H H HH HH H HH group has its own unique contribution based on its extinc- (a) (b) tion coefficient (or infrared absorption cross-section). Figure 2 Structures for hexane isomers: (a) n-hexane and Returning to the fundamental model, we should now (b) isohexane (2-methylpentane). Copyright Coates Consulting. look at the larger picture. In reality, we assign the INTERPRETATION OF INFRARED SPECTRA, A PRACTICAL APPROACH 5
100 symmetric vibration. While this might be less intuitive, it ) is still a rational concept, and therefore easy to understand % 80 ( and accept. Again, we see a good example with the C H e
c 60 stretch of an aliphatic compound (or fragment), where n a
t we observe the asymmetric C H stretch of the methyl t i 40 1 CH3 (CH2 )5 CH3 and methylene groups (2960 and 2930 cm , respectively) m
s occurring at slightly higher frequency than symmetric n 20 a 1
r vibrations (2875 and 2855 cm , respectively for methyl T 0 and methylene). For the most part, this simple rule 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 8 6
0 6 2 8 4 0 8 6 4 2 0 holds true for most common sets of vibrations. Naturally 4 3 3 2 2 2 1 1 1 1 1 there are always exceptions, and a breakdown of the −1 Wavenumber (cm ) rationale may occur when other effects come into play, such as induced electronic, spatial or entropy-related Figure 3 Attenuated total reflectance (ATR) spectrum of effects. n-heptane. Copyright Coates Consulting. There are many other spatially related scenarios that 100 tend to follow well-orchestrated patterns, examples being
) in-plane and out-of-plane vibrations, the differences
% 80
( between cis and trans spatial relationships, and a variety
e of multicentered vibrations that are defined as twisting c 60 n or rocking modes. Many of these are exhibited with the a t t i 40 C H vibrations that occur in saturated, unsaturated and CH3 CH3 m aromatic compounds. Molecular symmetry of the static s CH3 C CH2 CH CH3 n 20 or the dynamic (during vibration) molecule has a large
a CH3 r
T impact on the spectrum, in addition to factors such as 0 0 0 0 0 0 0 0 0 0 0 0 0 0 relative electronegativity, bond order and relative mass 0 0 0 0 0 0 0 0 0 0 0 0 0 6 8 0 2 4 6 8 0 4 8 2 6 0 1 1 1 1 1 2 2 2 3 3 4 of the participating atoms. Wavenumber (cm−1) Finally, while discussing the vibrational origins of infrared spectra, it is worth commenting that further Figure 4 ATR spectrum of 2,2,4-trimethylpentane (isooctane). complexity may be noted in the spectrum, beyond Copyright Coates Consulting. what is expected based on the fundamentals. As noted, transitions to higher energy levels, although theoreti- observed absorption frequencies in the infrared spectrum cally not allowed, can occur and these give rise to to much more that just simple harmonic (or anharmonic) overtone bands, which in the mid-infrared region occur stretching vibrations. In practice, we find that various at approximately twice the fundamental frequency for other deformation motions (angular changes), such as the first overtone. Higher overtones exist, typically the bending and twisting about certain centers within a second (3 ð fundamental) and third (4 ð fundamental), molecule, also have impact, and contribute to the overall and sometimes higher, and these are observed, with absorption spectrum. By rationalizing the effort needed to extremely low intensity, relative to the fundamental in the move the atoms relative to each other, one can appreciate near-infrared spectral regions, between 800 and 2500 nm that it takes less energy to bend a bond than to stretch (12 500 and 4000 cm 1). Other types of bands that can add it. Consequently, we can readily accept the notion that complexity to a spectrum are combination bands (sum and the stretching absorptions of a vibrating chemical bond difference), bands due to transitions from energy states occur at higher frequencies (wavenumbers) than the higher than the ground state or ‘‘hot bands’’, and bands corresponding bending or bond deformation vibrations, due to interactions between a weaker overtone or com- with the understanding, of course, that energy and bination band and a fundamental of the same or similar frequency are proportionally related. A good example is frequency, known as Fermi resonance bands. In the lat- the C H set of vibrations, observed in the hydrocarbon ter case, two relatively strong absorptions are observed, spectra, and in virtually all organic compounds. Here, the where normally only a single absorption is expected for simple C H stretching vibrations for saturated aliphatic the fundamental..3/ species occur between 3000 and 2800 cm 1, and the As additional functional groups are added to a basic corresponding simple bending vibrations nominally occur backbone structure, forming a more complex molecule, between 1500 and 1300 cm 1. additional bands are observed, either directly associated Next in our understanding is that it can take slightly with the fundamental vibrations of the functional groups, more energy to excite a molecule to an asymmetric than a or indirectly related to interactions between component 6 INFRARED SPECTROSCOPY functional groups or the basic substructure. Such interac- arrangement of the groups involved is reflected in tions can be severe, and result in overwhelming distortions the infrared spectrum as additional bands and added in the appearance of the spectrum, a good example complexity. being hydrogen bonding. This will be dealt with in depth As we move on to simple organic compounds, where later. one or more functional groups or heteroatoms are added to the molecule, we see many changes occurring in the spectrum. These result from the bonding associated with 3 SPECTRAL INTERPRETATION BY the functional group, and also local disturbances to the APPLICATION OF VIBRATIONAL basic backbone spectrum that relate again to spatial GROUP FREQUENCIES changes and also to local and neighboring electronic effects. Examples of such functionalities are halogens, This section includes tabulated data relative to the simple oxygen species, such as hydroxy and ether groups, most significant group frequencies for the most common and amino compounds. Carbonyl compounds, where the functional groups and structural components found in added functional group includes the CDO bond, also organic compounds. Brief reference is also made to simple provide very profound contributions to the spectrum, inorganic compounds, in the form of simple ionic species. and because of the wide diversity of these compounds More detailed listings can be found in published literature, they are best dealt with as a separate class. and the reader is encouraged to acquire one or more of A very characteristic group of compounds, from these reference texts..9–13/ As already indicated, the use a spectral point of view, are the multiple-bonded of tabulated data is only a part of the interpretation nitrogen compounds, such as cyanides and cyanates. process, and other facets of the spectrum must be taken These typically have very characteristic absorptions, into account. which are easy to assign, and are free from spectral To help gain an understanding of infrared spectral interferences. The same can be said for some of interpretation, it is instructive to start at the root of most the hydrides of heteroatoms, such as sulfides (thiols), organic compounds, namely the fundamental backbone silanes, and phosphines. Finally, there are other, oxygen- or the parent hydrocarbon structure. We shall start with containing functional groups, as encountered in the the simple, aliphatic hydrocarbon, which is at the root nitrogen-oxy (NOx), phosphorus-oxy (POx), silicon-oxy of most aliphatic compounds. Aliphatic hydrocarbons (SiOx), and sulfur-oxy (SOx) compounds. These are exist in simple linear chains, branched chains and in sometimes more difficult to identify from first principles, cyclic structures – examples of the linear and branched and a knowledge of the presence of the heteroatom chain scenarios were provided earlier for hexane isomers. is helpful. The spectra are characteristic, but many of Any one molecule may exist with one or more of these the oxy absorptions occur within a crowded and highly component structures. The infrared spectrum can provide overlapped region of the spectrum, mainly between information on the existence of most of these structures, 1350 and 950 cm 1. Also, many of these compounds either directly or by inference. feature C O bonding, which is common in other The introduction of unsaturation in the form of a frequently encountered functionalities such as ethers double or triple bond has a profound impact on the and esters. chemistry of the molecule, and likewise it has a significant influence on the infrared spectrum. Similarly, the same is 3.1 The Hydrocarbon Species and Molecular Backbone observed when an aromatic structure is present within a molecule. Infrared spectroscopy is a powerful tool In this section we include the characteristic absorption for identifying the presence of these functionalities. It frequencies encountered for the parent hydrocarbon provides information specific to the group itself, and species and the associated backbone or substituent group. also on the interaction of the group with other parts This includes aliphatic and aromatic structures. The of the molecule and on the spatial properties of the spectral contributions are characterized, as previously group. Examples of these include conjugation between a noted, as C H stretching and bending vibrations and double bond and another unsaturated center, an aromatic C C vibrations (stretching and bending), which for ring or a group, such as a carbonyl (CDO), and the the most part are unique for each molecule, and are orientation or location of the double bond within the generally described as skeletal vibrations. In the case molecule, such as cis or trans and medial or terminal. It of aromatic compounds, ring CDC C stretching and should be noted that cis/trans relationships are not specific bending vibrations are highly characteristic, and are to unsaturated hydrocarbons, and the terminology is diagnostic. Likewise, the same can be said for the referenced elsewhere, such as with secondary amide unsaturated carbon–carbon multiple bonding in alkene structures. Again, the associated changes in the spatial and alkyne structures. INTERPRETATION OF INFRARED SPECTRA, A PRACTICAL APPROACH 7
Table 1 Saturated aliphatic (alkane/alkyl) group frequencies Table 2 Olefinic (alkene) group frequencies
Group frequency (cm 1) Functional group/assignment Origin Group frequency, Assignment 1 − wavenumber (cm ) Methyl ( CH3) 2970–2950/2880–2860 Methyl C H asym./sym. stretch CDC 1680–1620 Alkenyl CDC stretch 1470–1430/1380–1370 Methyl C H asym./sym. bend 1625 Aryl-substituted CDC 1385–1380/1370–1365 gem-Dimethyl or ‘‘iso’’- (doublet) 1600 Conjugated CDC 1395–1385/1365 Trimethyl or ‘‘tert-butyl’’ (multiplet) C H 3095–3075 Terminal (vinyl) C H stretch C3040–3010 Methylene ( CH2) 3095–3075 Pendant (vinylidene) C H 2935–2915/2865–2845 Methylene C H asym./sym. stretch stretch 1485–1445 Methylene C Hbend 3040–3010 Medial, cis-ortrans-C H 750–720 Methylene (CH2)n rocking stretch (n ½ 3) 1055–1000/1005–925 Cyclohexane ring vibrations C H 1420–1410 Vinyl C H in-plane bend − 1310–1290 Vinylidene C H in-plane Methyne ( CH ) bend 2900–2880 Methyne C H stretch C H 995–985 C 915–890 Vinyl C H out-of-plane bend 1350–1330 Methyne C Hbend 895–885 Vinylidene C H out-of-plane 1300–700 Skeletal C C vibrations bend − Special methyl ( CH3) frequencies C H 970–960 trans-C H out-of-plane bend 2850–2815 Methoxy, methyl ether O CH3, 700 (broad) cis-C H out-of-plane bend C H stretch 2820–2780 Methylamino, N CH ,C H stretch 3 100 )
% 80 ( 3.1.1 Saturated Aliphatic and Alicyclic Compounds e
c 60 See Table 1. The C H stretch vibrations for methyl n a t t and methylene are the most characteristic in terms i 40 of recognizing the compound as an organic compound m
s H H C C n 20 containing at least one aliphatic fragment or center. The H (CH2)3 CH3 a r
bending vibrations help to tell more about the basic T 0 0 0 0 0 0 0 0 0 0 0 0 0 structure. For example, a strong methylene/methyl band 0 0 0 0 0 0 0 0 0 0 0 0 0 0 8 6 0 6 2 8 4 0 8 6 4 2 1 1 0 4 3 3 2 2 2 1 1 1 1 (1470 cm ) and a weak methyl band (1380 cm ), plus 1 1 a band at 725–720 cm (methylene rocking vibration) Wavenumber (cm−1) is indicative of a long-chain linear aliphatic structure (note that splitting may be observed for the 1470 and Figure 5 ATR spectrum of 1-hexene. Copyright Coates Con- 720 cm 1 bands, which is indicative of a long-chain sulting. compound, and is attributed to a crystallinity and a high degree of regularity for the linear backbone structure). unsaturated hydrocarbons featuring CDC, with attached In contrast, strong methyl bands, showing significant hydrogens, usually occur as either a single or a pair splitting, and a comparatively weaker methylene/methyl of absorptions, in the ranges indicated in Table 2. As band indicate chain branching, and the possibility of noted, the number of bands and their positions are isopropyl or tert-butyl substituents (depending on the indicative of the double bond location and the spatial amount of splitting, and the relative band intensities). arrangement around the double bond. The position of the A comparison between linear and branched chain CDC stretching frequency does vary slightly as a function hydrocarbons can be seen in Figures 3 and 4, where in the of orientation around the double bond, but it is less case of isooctane, both isopropyl and tert-butyl groups informative than the C H information. The C H out-of- are present. plane bending is typically the most informative relative to the location and spatial geometry of the double bond, where terminal and medial double bonds may be clearly 3.1.2 Unsaturated Compounds differentiated. Figure 5 provides a good example with the See Table 2. As already commented upon, the saturated spectrum of 1-hexene, which contains the terminal vinyl hydrocarbon C H stretching absorptions all occur below group. Note that a fully substituted, medial double bond 3000 cm 1. Any band structures observed between 3150 has only the CDC as the sole indicator of the presence and 3000 cm 1 are almost exclusively indicative of of the double bond, unless the bond is conjugated with a unsaturation (CDC H) and/or aromatic rings. The second unsaturated site. 8 INFRARED SPECTROSCOPY
Table 3 Aromatic ring (aryl) group frequencies 100
Origin Group frequency, Assignment 80 wavenumber (cm 1) 60 CH CDC Ca 1615–1580 Aromatic ring stretch 3 H CH CDC Ca 1510–1450 Aromatic ring stretch 40 3 C H 3130–3070 Aromatic C H stretch C H 1225–950 (several) Aromatic C H in-plane 20 H H bend H C H 900–670 (several) Aromatic C H 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0
out-of-plane bend 8 0 6 2 8 4 0 8 6 4 2 0 4 3 3 2 2 2 1 1 1 1 1 770–730 C 710–690 Monosubstitution (phenyl) (a) 770–735 1,2-Disubstitution (ortho) 810–750 C 900–860 1,3-Disubstitution (meta) 100
860–800 1,4-Disubstitution (para) ) b ‘‘Combi’’ 2000–1660 (several) Aromatic combination % 80 ( bands e
c 60 a D n CH3 C C C used as an approximation of the unique aromatic ring a t
t H H bonding. i 40 b
‘‘Combi’’ denotes assignment to combination bands. m s
n 20 H CH3 a
3.1.3 Aromatic Compounds r H T 0 0 0 0 0 0 0 0 0 0 0 0 0 0
See Table 3. The existence of one or more aromatic 0 0 0 0 0 0 0 0 0 0 0 8 0 6 2 8 4 0 8 6 4 2 0 rings in a structure is normally readily determined (b) 4 3 3 2 2 2 1 1 1 1 1 from the C HandCDC C ring-related vibrations. The C H stretching occurs above 3000 cm 1 and is typically 100 exhibited as a multiplicity of weak-to-moderate bands, compared with the aliphatic C H stretch. The structure 80 of the bands is defined by the number and positions of the 60 CH 3 C H bonds around the ring, which in turn are related to H H the nature and number of other substituents on the ring. 40 Note that the same applies to the C H out-of-plane bend- 20 H H ing vibrations, which are frequently used to determine the CH3 degree and nature of substitution on the ring – examples 0 0 0 0 0 0 0 0 0 0 0 0 0 0 are provided in Figure 6(a–c), with the comparison of 0 0 0 0 0 0 0 0 0 0 0 8 0 6 2 8 4 0 8 6 4 2 0 the three xylene isomers. This picture often becomes 4 3 3 2 2 2 1 1 1 1 1 − more complex if multiple- or fused-ring structures exist (c) Wavenumber (cm 1) in a compound. The other most important set of bands are the aromatic ring vibrations centered around 1600 Figure 6 ATR spectra of xylene isomers: (a) o-xylene, 1,2- and 1500 cm 1 dimethylbenzene; (b) m-xylene, 1,3-dimethylbenzene; (c) p- , which usually appear as a pair of band xylene, 1,4-dimethylbenzene. Copyright Coates Consulting. structures, often with some splitting. The appearance and ratio of these band structures is strongly dependent on the position and nature of substituents on the ring. Table 4 Acetylenic (alkyne) group frequencies Origin Group frequency, Assignment 3.1.4 Acetylenic Compounds wavenumber (cm 1) See Table 4. Although acetylenic compounds are not very CÁC 2140–2100 Terminal alkyne common, the spectrum associated with the CÁC structure (monosubstituted) can be characteristic. It is instructive to note the impact CÁC 2260–2190 Medial alkyne on the carbon–carbon bond stretching as a function of (disubstituted) C H 3320–3310 Alkyne C H stretch increase in bond order for the series of single-, double-, C H 680–610 Alkyne C Hbend and triple-bonded carbon: C H 630 (typical) Alkyne C Hbend
C C stretch: ¾1350–1000 cm 1 (skeletal vibrations) CDC stretch: 1680–1620 cm 1 This increase in bond order produces a corresponding CÁC stretch: 2260–2100 cm 1 increase in bond strength, which in turn increases the force INTERPRETATION OF INFRARED SPECTRA, A PRACTICAL APPROACH 9 constant, k (see Equation 3), supporting the Hooke’s law assigned to the halogen–carbon stretching. When a single model described earlier. halogen is present, the determination of this group is As noted in Table 4, the position of the CÁC bond is straightforward. However, if more than one halogen is influenced by whether the group is terminal or medial. present, the interpretation is usually more complex. In The single hydrogen of the terminal acetylene itself is such cases, the result varies depending on whether the very characteristic, reflecting the labile nature of the halogens are on the same or different carbon atoms, and, if acetylenic C H. on different atoms, whether the atoms are close neighbors. This is particularly the case with small molecules, and 3.2 Simple Functional Groups the resultant spectral complexity arises from the fact that there is restricted rotation about the carbon–carbon Obviously, there is a potentially broad number of bond. molecular fragments that can be considered to be Single bonds usually exhibit free rotation, which would functional groups attached to an organic structure or normally mean that there are no preferred spatial backbone. This section features the most simple and orientations for the molecules. However, owing to the most common of the functional groups, C X, i.e. the size of the halogen atom, relative to the carbon and D D halogens (X F, Cl, Br and I), hydroxy (X OH), hydrogen that form the backbone, the molecules tend D D oxy or ether (X OR, where R alkyl), and amino to exhibit certain specific conformations, where the D D Á (X NH2, NH or N). With the exception of the spatial interaction between neighboring halogen atoms carbonyl functionality, these three basic functional groups is minimized, and each conformation provides its own cover most of the common occurrences in simple organic contribution to the overall spectrum. It is important compounds. Note that for the oxy/hydroxy and amino to appreciate that this issue of spatial orientation has functionalities, these are molecular fragments, and they an impact even on high-molecular-weight compounds, contribute their own set of characteristic absorptions to such as the polyhalogenated polymers, e.g. poly(vinyl the spectrum of the compound. In fact, the bonding chloride). Here preferred orientations have an impact on between the functional group and the backbone is only the crystallinity of the polymer, and this in turn has a one part of the overall picture used for the spectral significant impact on both the spectrum and the physical interpretation. properties of the material. Another important issue to consider with halogen 3.2.1 Halogenated Compounds substituents is the high electronegativity of the halogen See Table 5. In principle, the interpretation of the spectra atom. This can have a noticeable impact on the spectrum of molecules containing one or more halogens would of neighboring group frequencies, including adjacent seem to be straightforward. The functionality is simple, hydrogen atoms. In such cases, significant shifting of with just a single atom linked to carbon to form the group. the C H frequencies can occur – the direction of the With the polar nature of this group, one would expect the shift being dependent on the location of the C H, spectral contribution to be distinctive. In reality, this is and whether the halogen adds or extracts electron not always the case. density from the C H bond – adding strengthens (higher In aliphatic compounds, the C X bond typically frequency) and extracting weakens (lower frequency). possesses a unique group frequency, which may be The same influences can be observed with halogen- substituted carbonyl compounds, such as acyl halides Table 5 Aliphatic organohalogen compound group and a-substituted acids, where the bond strength of the frequencies carbonyl group is increased (see section 3.3). In most cases, both a shift to higher frequency and an increase in Origin Group frequency, Assignment absorption strength for the band are observed. 1 a wavenumber (cm ) Table 5 only presents the group frequencies for the C F 1150–1000 Aliphatic fluoro compounds, aliphatic compounds, because no well-defined C X C F stretch absorptions are observed for halogen-substituted aro- C Cl 800–700 Aliphatic chloro compounds, matic compounds. The presence of a halogen on an C Cl stretch aromatic ring can be detected indirectly from its elec- C Br 700–600 Aliphatic bromo compounds, C Br stretch tronic impact on the in-plane C H bending vibrations. C I 600–500 Aliphatic iodo compounds, Normally, we do not consider the in-plane bending bands C I stretch to be of use because, as pointed out earlier, these occur in a spectral region that is crowded by other important group a Note that the ranges quoted serve as a guide only; the actual ranges are influenced by carbon chain length, the actual number of halogen frequencies. However, in the case of a halogen-substituted substituents, and the molecular conformations present. ring, the intensity of these vibrations is enhanced relative 10 INFRARED SPECTROSCOPY to other absorptions by as much as three to four times. Table 6 Alcohol and hydroxy compound group frequencies For reference, it is informative to compare the intensities for these bands, between 1150 and 1000 cm 1, for the Origin Group frequency, Assignment wavenumber (cm 1) spectra of toluene and chlorobenzene (Figure 7a and b). O H 3570–3200 (broad) Hydroxy group, H-bonded OH stretch 3.2.2 Hydroxy and Ether Compounds 3400–3200 Normal ‘‘polymeric’’ OH stretch See Table 6 for alcohols and hydroxy compounds. 3550–3450 Dimeric OH stretch The hydroxy function is probably one of the most 3570–3540 Internally bonded OH stretch dominant and characteristic of all of the infrared group O H 3645–3600 (narrow) Nonbonded hydroxy group, frequencies. In most chemical environments, the hydroxy OH stretch group does not exist in isolation, and a high degree 3645–3630 Primary alcohol, OH stretch of association is experienced as a result of extensive 3635–3620 Secondary alcohol, OH stretch 3620–3540 Tertiary alcohol, OH stretch hydrogen bonding with other hydroxy groups. These 3640–3530a Phenols, OH stretch hydroxy groups may be within the same molecule O H 1350–1260 Primary or secondary, OH (intramolecular hydrogen bonding) or they most likely in-plane bend exist between neighboring molecules (intermolecular 1410–1310 Phenol or tertiary alcohol, OH hydrogen bonding). The impact of hydrogen bonding bend is to produce significant band broadening and to lower 720–590 Alcohol, OH out-of-plane bend the mean absorption frequency. The lowering of the b frequency tends to be a function of the degree and C O ¾1050 Primary alcohol, C O stretch ¾1100b Secondary alcohol, C O strength of the hydrogen bonding. In compounds such as stretch carboxylic acids, which exhibit extremely strong hydrogen ¾1150b Tertiary alcohol, C O stretch bonding, forming a stable dimeric structure, a highly ¾1200b Phenol, C O stretch characteristic, large shift to lower frequencies is observed. a Frequency influenced by nature and position of other ring substituents. b Approximate center of range for the group frequency. 100 )
% 80 In special circumstances, where the hydroxy group (
e is isolated – either because of steric hindrance effects
c 60
n Cl or because the sample is in the vapor state or in a
t H H
t a dilute solution of a nonpolar solvent – the band is i 40
m characteristically narrow, and is observed at the natural,
s H H
n 20 higher frequency. This absorption is important for the
a H r characterization of certain hindered phenol antioxidants, T 0 a commercially important class of compounds in the food, 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 8 6 0 6 2 8 4 0 8 6 4 2 0 polymer, and formulated oil industries. 4 3 3 2 2 2 1 1 1 1 1 −1 It must be appreciated that while the hydroxy absorp- (a) Wavenumber (cm ) tion is singly one of the most important bands in the infrared spectrum, other vibrations are also important 100
) for the actual characterization of the compound. Alco-
% 80 hols exist as three distinct classes – primary, secondary (
e and tertiary – distinguished by the degree of carbon sub- c 60 n CH3 stitution on the central hydroxy-substituted carbon, a a t
t H H single substitution being primary, double substitution i 40
m being secondary, and triple substitution being tertiary. s
n 20 H H This is an important fact, because the chemistry and a r H oxidation stability of the alcohol are strongly influenced T 0 0 0 0 0 0 0 0 0 0 0 0 0 by the degree of substitution. Whether an alcohol is pri- 0 0 0 0 0 0 0 0 0 0 0 0 8 0 2 4 6 8 0 4 8 2 6 0 mary (1°), secondary (2°) or tertiary (3°), may be reflected 1 1 1 1 1 2 2 2 3 3 4 − in the position of the OH stretch absorption, but typically (b) Wavenumber (cm 1) this is determined by the other absorptions, in particu- Figure 7 Comparison of ATR spectra of (a) chlorobenzene lar the C O stretching frequency. Another absorption and (b) toluene. Copyright Coates Consulting. of lower importance, but often characteristic, is assigned INTERPRETATION OF INFRARED SPECTRA, A PRACTICAL APPROACH 11 to another form of bending vibration, the out-of-plane compounds, where the hydrogen of the hydroxy group bend or wagging vibration of the O H. The OH bend- is replaced by an aliphatic (alkyl) or aromatic (aryl) ing vibrations are broadened by hydrogen bonding as is molecular fragment. Having stated that, the overall the stretching absorption, but often to a lesser extent. appearance of an ether spectrum is drastically different The differences between primary and secondary alcohols from that of a related alcohol. This is due to the can be appreciated from Figure 8(a) and (b), where the overwhelming effect of hydrogen bonding on the hydroxy spectra of 1- and 2-octanol are presented. group. However, many of the relationships that exist for See Table 7 for ethers and oxy compounds. In some the C O component of the alcohol carry over to the respects, ethers are related to alcohol and hydroxy corresponding ether. The relationships that pertain to primary, secondary, and tertiary structures remain intact. 100 The main difference is that one now considers the bonding ) on both sides of the oxygen, because if carbon is on both % (
sides, then two ether bonds exist. Ethers can exist as e
c simple ethers (same group both sides) and mixed ethers n
a 50 (different groups both sides). Infrared spectroscopy is t t i fairly sensitive for differentiating these ether functions, m
s especially when the structures are mixed aliphatic or n
a aliphatic/aromatic. r T 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 8 6 0 6 2 8 4 0 8 6 4 2 0 3.2.3 Amino Compounds 4 3 3 2 2 2 1 1 1 1 1 − (a) Wavenumber (cm 1) See Table 8. In some respects, the infrared spectra and the characteristic group frequencies of amines tend to 100 ) Amine and amino compound group frequencies % Table 8 (
e
c Origin Group frequency, Assignment n wavenumber (cm 1) a 50 t t i Primary amino m s
n N H 3400–3380 Aliphatic primary amine, a
r C3345–3325 NH stretch T 0 N H 3510–3460 Aromatic primary amine, 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 C3415–3380 NH stretch 8 6 0 6 2 8 4 0 8 6 4 2 0 4 3 3 2 2 2 1 1 1 1 1 N H 1650–1590 Primary amine, NH bend − C N 1090–1020 Primary amine, CN stretch (b) Wavenumber (cm 1) Secondary amino Figure 8 ATR spectra of (a) primary (1-octanol) and (b) sec- N H 3360–3310 Aliphatic secondary amine, ondary (2-octanol) alcohols. Copyright Coates Consulting. NH stretch N H ¾3450 Aromatic secondary amine, Table 7 Ether and oxy compound group frequencies NH stretch N H 3490–3430 Heterocyclic amine, Origin Group frequency, Assignment NH stretch DN H 3350–3320 Imino compounds, wavenumber (cm 1) NH stretch C H 2820–2810 Methoxy, C H stretch N H 1650–1550 Secondary amine, NH bend (CH3 O ) C N 1190–1130 Secondary amine, C O C 1150–1050 Alkyl-substituted ether, CN stretch C O stretch Tertiary amino C O C 1140–1070 Cyclic ethers, large C N 1210–1150 Tertiary amine, CN stretch rings, C O stretch f O H 1270–1230 Aromatic ethers, Aromatic amino aryl O stretch C N 1340–1250 Aromatic primary amine, C O ¾1250 C 890–800a Epoxy and oxirane rings CN stretch C O O C 890–820a Peroxides, C O O C N 1350–1280 Aromatic secondary amine, stretch CN stretch C N 1360–1310 Aromatic tertiary amine, a Typically very weak, and not very characteristic in the infrared. Tend CN stretch to be more characteristic in the Raman spectrum. 12 INFRARED SPECTROSCOPY parallel those of alcohols and ethers. Before proceeding, 100 there is an important distinction to be made between the nomenclature used to describe alcohol structures, 80 compared with that used for amines. The terms primary, 60 NH2 secondary, and tertiary are used to describe amines, but H H the substitution relates to the nitrogen, not the adjoining 40 carbon (as with alcohols). The terminology used is NH2 H H 20 primary, NH secondary and N tertiary. As before, H these structural differences are important, and they 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 0 strongly influence the chemistry and the reactivity of the 0 0 0 0 0 0 0 0 0 0 0 8 6 0 6 2 8 4 0 8 6 4 2 0