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CHEM 430 IR SPECTROSCOPY FALL 2011 Long Lecture Play Dr. Justik
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CHEM 430 – NMR Spectroscopy
Infrared and Raman Spectroscopy 11-1 Introduction The method provides a rapid and simple method for observing the functional group species present in an organic molecule The spectrum is a plot of the percentage of IR radiation that passes through the sample (% transmission) versus some function of the wavelength of the radiation related to covalent bonding CHEM 430 – NMR Spectroscopy
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CHEM 430 – NMR Spectroscopy
Infrared and Raman Spectroscopy 11-1 Introduction Instrumentation. Modern IR spectrometers are based on the Michelson interferometer Fourier transform infrared ( FT– IR) spectrometers: The absorption spectrum is obtained by means of Fourier transformation of an interferogram. Dispersive infrared spectrometers: Earlier instruments based on monochromators that disperse the radiation from an IR source into its component wavelengths - spectrum is obtained by measuring the amount of radiation absorbed by a sample as the wavelength is varied. Raman spectroscopy provides information complementary to that obtained from IR spectroscopy. CHEM 430 – NMR Spectroscopy
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. The quantum mechanical energy levels observed in IR spectroscopy are those of molecular vibration When we say a covalent bond between two atoms is of a certain length, we are citing an average because the bond behaves as if it were a vibrating spring connecting the two atoms For a simple diatomic molecule, this model is easy to visualize: CHEM 430 – NMR Spectroscopy
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. There are two types of bond vibration: Stretch – Vibration or oscillation along the line of the bond Bend – Vibration or oscillation not along the line of the bond H C H C asymmetric symmetric H C H C H C H C scissor rock twist wag in plane out of plane 5
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. Each stretching and bending vibration occurs with a characteristic frequency Typically, this frequency is on the order of 1.2 x 1014 Hz (120 trillion oscillations per sec. for the H2 vibration at ~4100 cm-1) The corresponding wavelengths are on the order of ,000 nm or 2.5 – 15 microns (mm) When a molecule is bombarded with electromagnetic radiation (photons) that match the frequency of one of these vibrations (IR radiation), it is absorbed and the bonds begin to stretch and bend more strongly (emission and absorption) When this photon is absorbed the amplitude of the vibration is increased NOT the frequency CHEM 430 – NMR Spectroscopy
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. The result of the spectroscopic process is a spectrum of the various stretches and bends of the covalent bonds in an organic molecule CHEM 430 – NMR Spectroscopy 7
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. The x-axis of the IR spectrum is in units of wavenumbers, n, which is the number of waves per centimeter in units of cm-1 (Remember E = ħn or E = ħc/l) This unit is used rather than wavelength (microns) because wavenumbers are directly proportional to the energy of transition being observed – chemists like this, physicists hate it High frequencies and high wavenumbers equate higher energy is quicker to understand than Short wavelengths equate higher energy CHEM 430 – NMR Spectroscopy 8
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. This unit is used rather than frequency as the numbers are more “real” than the exponential units of frequency IR spectra are observed for what is called the mid-infrared: cm-1 The peaks are Gaussian distributions of the average energy of a transition CHEM 430 – NMR Spectroscopy 9
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. So how does the IR detect different bonds? The potential energy stretching or bending vibrations of covalent bonds follow the model of the classic harmonic oscillator (Hooke’s Law) Remember: E = ½ ky2 where: y is spring displacement k is spring constant Potential Energy (E) Interatomic Distance (y) CHEM 430 – NMR Spectroscopy 10
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. Aside: Physically here are the movements we are discussing: Stretching vibration: a typical C-C bond with a bond length of 154 pm, the displacement is averages 10 pm: Bending vibration: For C-C-C bond angle a change of 4° is typical, which corresponds to an average displacement of 10 pm. 10 pm 154 pm 4o 10 pm CHEM 430 – NMR Spectroscopy 11
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. The energy levels for these vibrations are quantized as we are considering quantum mechanical particles Only discrete vibrational energy levels exist: Note there is no energy level below n = 0, at any temperature above absolute zero there is always the first vibrational energy level rotational transitions – (in microwave region) Potential Energy (E) Vibrational transitions, n Interatomic Distance (r) CHEM 430 – NMR Spectroscopy 12
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. However, the application of the classical vibrational model fails apart for two reasons: As two nuclei approach one another through bond vibration, potential energy increases to infinity, as two positive centers begin to repel one another At higher vibrational energy levels, the amplitude of displacement becomes so great, that the overlapping orbitals of the two atoms involved in the bond, no longer interact and the bond dissociates We say that the model is really one of an aharmonic oscillator, for which the simple harmonic oscillator model works well for low energy levels CHEM 430 – NMR Spectroscopy 13
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. Here is the derivation of Hooke’s Law we will apply for IR theory: Vibrational frequency given by: n : frequency K: force constant – bond strength m: reduced mass = m1m2/(m1+m2) Reduced mass is used, as each atom in the covalent bond oscillates about the center of the two masses CHEM 430 – NMR Spectroscopy 14
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. What does this mean for the different covalent bonds in a molecule? Let’s consider reduced mass, m, first: The C-H and C-C single bonds differ by only 16 kcal/mole: 99 kcal · mol-1 vs. 83 kcal · mol-1 (similar K) Due to the reduced mass term, these two bonds of similar strength show up in very different regions of the IR spectrum: C─C cm-1 m = (12 x 12)/( ) = 6 (0.41) C─H cm-1 m = (1 x 12)/(1 + 12) = 0.92 (0.95) A smaller atom therefore gives rise to a higher wavenumber (and n and E) CHEM 430 – NMR Spectroscopy 15
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. What does this mean for the different covalent bonds in a molecule? When greater masses are added, the trend is similar (K’s here are different) C─I 500 cm-1 C─Br cm-1 C─Cl cm-1 C─O cm-1 C─C cm-1 C─H cm-1 A smaller atom therefore gives rise to a higher wavenumber (and n and E) and a larger atom gives rise to lower wavenumbers (and n and E) CHEM 430 – NMR Spectroscopy 16
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. What does this mean for the different covalent bonds in a molecule? Let’s consider bond strength, K: A C≡C bond is stronger than a C=C bond is stronger than a C-C bond wavenumber, cm-1 DHf From IR spectroscopy we find: C≡C ~ C=C ~ C—C ~ Note the good correlation with the heats of formation for each bond! Stronger bonds give higher wavenumbers (and higher n and E) CHEM 430 – NMR Spectroscopy 17
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. The y-axis of the IR spectrum is in units of transmittance, T, which is the ratio of the amount of IR radiation transmitted by the sample (I) to the intensity of the incident beam (I0); % Transmittance is T x 100 T = I / I0 %T = (I / I0) X 100 IR is different than other spectroscopic methods which plot the y-axis as units of absorbance (A). A = log(1/T) As opposed to chromatography or other spectroscopic methods, the area of a IR band (or peak) is not directly proportional vs. concentration of other functionalities, it can be used vs. itself if standardized!!! CHEM 430 – NMR Spectroscopy 18
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. The intensity of an IR band is affected by two primary factors: Whether the vibration is one of stretching or bending Electronegativity difference of the atoms involved in the bond: For both effects, the greater the change in dipole moment in a given vibration or bend, the larger the peak. The greater the difference in electronegativity between the atoms involved in bonding, the larger the dipole moment Typically, stretching will change dipole moment more than bending CHEM 430 – NMR Spectroscopy 19
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Vibrations of Molecules
Infrared and Raman Spectroscopy 11-2 Vibrations of Molecules The IR Spectroscopic Process. It is important to make note of peak intensities to show the effect of these factors: Strong (s) – peak is tall, transmittance is low Medium (m) – peak is mid-height Weak (w) – peak is short, transmittance is high * Broad (br) – if the Gaussian distribution is abnormally broad (* this is more for describing a bond that spans many energies) Exact transmittance values are rarely recorded CHEM 430 – NMR Spectroscopy 20
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II. Infrared Group Analysis A. General
The primary use of the IR spectrometer is to detect functional groups Because the IR looks at the interaction of the EM spectrum with actual bonds, it provides a unique qualitative probe into the functionality of a molecule, as functional groups are merely different configurations of different types of bonds Since most “types” of bonds in covalent molecules have roughly the same energy, i.e., C=C and C=O bonds, C-H and N-H bonds they show up in similar regions of the IR spectrum Remember all organic functional groups are made of multiple bonds and therefore show up as multiple IR bands (peaks) There are 4 principle regions: Bonds to H O-H single bond N-H single bond C-H single bond Triple bonds C≡C C≡N Double bonds C=O C=N C=C Single Bonds C-C C-N C-O Fingerprint Region 4000 cm-1 2700 cm-1 2000 cm-1 1600 cm-1 400 cm-1
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We will pick up next time with peak intensities, width of bands and some simple symmetry rules, as well as instrument design Monday we should finally get to functional groups where we will apply in depth the general topics we have discussed in the introductory material No Problem set for today! But take this time to review some organic: - bond strengths – both inter and intra-molecular - bond distances for more organic-y bonds - hybridization models - Periodic table and properties – you should know the position and EN’s of H, B, C, N, O, F, Si, P, S, Cl, Br and I
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IR Spectroscopy I. Introduction The IR Spectrum The intensity of an IR band is affected by two primary factors: Whether the vibration is one of stretching or bending Electronegativity difference of the atoms involved in the bond: For both effects, the greater the change in dipole moment in a given vibration or bend, the larger the peak The greater the difference in electronegativity between the atoms involved in bonding, the larger the dipole moment Typically, stretching will change dipole moment more than bending It is important to make note of peak intensities to show the effect of these factors: Strong (s) – peak is tall, transmittance is low Medium (m) – peak is mid-height Weak (w) – peak is short, transmittance is high * Broad (br) – if the Gaussian distribution is abnormally broad (*this is more for describing a bond that spans many energies) Exact transmittance values are rarely recorded
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies We have learned: That IR radiation can “couple” with the vibration of covalent bonds, where that particular vibration causes a change in dipole moment The IR spectrometer irradiates a sample with a continuum of IR radiation; those photons that can couple with the vibrating bond elevate it to the next higher vibrational energy level (increase in A) When the bond relaxes back to the n0 state, a photon of the same n is emitted and detected by the spectrometer; the spectrometer “reports” this information as a spectral band centered at the n of the coupling The position of the spectral band is dependent on bond strength and atomic size The intensity of the peak results from the efficiency of the coupling; e.g. vibrations that have a large change in dipole moment create a larger electrical field with which a photon can couple more efficiently
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Remember, most interesting molecules are not diatomic, and mechanical or electronic factors in the rest of the structure may effect an IR band From a molecular point of view (discounting phase, temperature or other experimental effects) there are 10 factors that contribute to the position, intensity and appearance of IR bands Symmetry Mechanical Coupling Fermi Resonance Hydrogen Bonding Ring Strain Electronic Effects Constitutional Isomerism Stereoisomerism Conformational Isomerism Tautomerism (Dynamic Isomerism)
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Symmetry H2O For a particular vibration to be IR active there must be a change in dipole moment during the course of the particular vibration For example, the carbonyl vibration causes a large shift in dipole moment, and therefore an intense band on the IR spectrum For a symmetrical acetylene, it is clear that there is no permanent dipole at any point in the vibration of the CC bond. No IR band appears on the spectrum
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Symmetry H2O Most organic molecules are fortunately asymmetric, and bands are observed for most molecular vibration The symmetry problem occurs most often in small, simple symmetric and pseudo-symmetric alkenes and alkynes Since symmetry elements “cancel” the presence of bonds where no dipole is generated, the spectra are greatly simplified
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Symmetry H2O Symmetry also effects the strength of a particular band The symmetry problem occurs most often in small, simple symmetric and pseudo-symmetric alkenes and alkynes Since symmetry elements “cancel” the presence of bonds where no dipole is generated, the spectra are greatly simplified
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Mechanical Coupling In a multi-atomic molecule, no vibration occurs without affecting the adjoining bonds This induces mixing and redistribution of energy states, yielding new energy levels, one being higher and one lower in frequency Coupling parts must be approximate in E for maximum interaction to occur (i.e. C-C and C-N are similar, C-C and H-N are not) No interaction is observed if coupling parts are separated by more than two bonds Coupling requires that the vibration be of the same symmetry
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Mechanical Coupling For example, the calculated and observed n for most C=C bonds is around 1650 cm-1 Butadiene (where the two C=C systems are separated by a dissimilar C-C bond) the bands are observed at 1640 cm-1 (slight reduction due to resonance, which we will discuss later) In allene however, mechanical coupling of the two C=C systems gives two IR bands – at 1960 and 1070 cm-1 due to mechanical coupling For purposes of this course, when we discuss the group frequencies, we will point out when this occurs
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The IR Spectrum – Factors that affect group frequencies
IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Fermi Resonance A Fermi Resonance is a special case of mechanical coupling It is often called an “accidental degeneracy” In understanding this, for many IR bands, there are “overtones” of the fundamental (the n’s you are taught) at twice the wavenumber In a good IR spectrum of a ketone (2-hexanone, here) you will see a C=O stretch at 1715 cm-1 and a small peak at 3430 cm-1 for the overtone overtone fundamental
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Fermi Resonance Ordinarily, most overtones are so weak as not to be observed But, if the overtone of a particular vibration coincides with the band from another vibration, they can couple and cause a shift in group frequency and introduce extra bands If you first looked at the IR (working “cold”) of benzoyl chloride, you may deduce that there were two dissimilar C=O bonds in the molecule
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Fermi Resonance In this spectrum, the out of plane bend of the aromatic C-H bonds occurs at 865 cm-1; the overtone of this band coincides with the fundamental of C=O at 1730 cm-1 The band is “split” by Fermi resonance (1760 and 1720 cm-1)
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Fermi Resonance Again, we will cover instances of this in the discussion of group frequencies, but this occurs often in IR of organics Most observed: Aldehydes – the overtone of the C-H deformation mode at 1400 cm-1 is always in Fermi resonance with the stretch of the same band at 2800 cm-1 The N-H stretching mode of –(C=O)-NH- in polyamides (peptides for the biologists and biochemists) appears as two bands at 3300 and 3205 cm-1 as this is in Fermi resonance with the N-H deformation at 1550 cm-1
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The IR Spectrum – Factors that affect group frequencies
IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Hydrogen Bonding One of the most common effects in chemistry, and can change the shape and position of IR bands Internal (intramolecular) H-bonding with carbonyl compounds can serve to lower the absorption frequency 1680 cm-1 1724 cm-1
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The IR Spectrum – Factors that affect group frequencies
IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Hydrogen Bonding Inter-molecular H-bonding serves to broaden IR bands due to the continuum of bond strengths that result from autoprotolysis Compare the two IR spectra of 1-propanol; the first is an IR of a neat liquid sample, the second is in the gas phase – note the shift and broadening of the –O-H stretching band Gas phase Neat liquid
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Hydrogen Bonding Some compound, in addition to intermolecular effects for the monomeric species can form dimers and oligomers which are also observed in neat liquid samples Carboxylic acids are the best illustrative example – the broadened O-H stretching band will be observed for the monomer, dimer and oligomer
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Ring Strain Certain functional group frequencies can be shifted if one of the atoms hybridization is affected by the constraints of bond angle in ring systems Consider the C=O band for the following cycloalkanones: cm-1 We will discuss the specific cases for these shifts during our coverage of group frequencies
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Electronic Effects - Inductive The presence of a halogen on the a-carbon of a ketone (or electron w/d groups) raises the observed frequency for the p-bond Due to electron w/d the carbon becomes more electron deficient and the p-bond compensates by tightening
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Electronic Effects - Resonance One of the most often observed effects Contribution of one of the less “good” resonance forms of an unsaturated system causes some loss of p-bond strenght which is seen as a drop in observed frequency
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Electronic Effects - Resonance In extended conjugated systems, some resonance contributors are “out-of-sync” and do not resonate with a group Example:
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IR Spectroscopy I. Introduction The IR Spectrum – Factors that affect group frequencies Electronic Effects - Sterics Consider this example: In this case the presence of the methyl group “misaligns” the conjugated system, and resonance cannot occur as efficiently The effects of induction, resonance and sterics are very case-specific and can yield a great deal of information about the electronic structure of a molecule
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Group Frequencies and Analysis Introduction
IR Spectroscopy Group Frequencies and Analysis Introduction When approaching any IR spectrum be sure to use the larger-to-smaller region approach- do not immediately focus on any one single peak (even –OH or C=O) From the Hooke’s Law derivation we are using we find that the IR can be conveniently be divided into four major regions: Bonds to H Triple bonds Double bonds Single Bonds O-H N-H C-H C≡C C≡N C=O C=N C=C C-C C-N C-O C-X “Fingerprint Region” 4000 cm-1 2700 cm-1 2000 cm-1 1600 cm-1 400 cm-1
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IR Spectroscopy Group Frequencies and Analysis Introduction If supporting information is available – molecular formula, chemical inferences – (i.e. this was the product of an oxidation reaction), assume this information is correct and the analysis of the IR should support it (later in your careers you can doubt information given to you) If a molecular formula is available, do an HDI! Many texts list various methods for approaching an IR spectrum; use the method that works best for you and stick to it. The most common mistakes in spectral analysis are those of “jumping the gun” to a conclusion (usually based on some small, insignificant peak) or taking a random haphazard approach to the spectrum (gee, here is an IR, oh, let’s start looking for phosphorus this time) Be methodical, develop a scheme and stick to it!
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Group Frequencies and Analysis
IR Spectroscopy Group Frequencies and Analysis Before we begin – Each functional group will be described as follows: Group General – What is most recognizable? What makes it different from similar groups? Group Frequencies (cm-1): Bond observed n in cm-1 type of vibration Exceptions and things to watch Scale on bottom summarizes band positions and strengths Strong - Medium - Weak -
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Group Frequencies and Analysis The Hydrocarbons Alkanes
IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkanes General – due to the small electronegativity difference between C and H, hydrocarbon bands are of medium intensity at best and give simple spectra Group Frequencies (cm-1): C-H Stretch Strained ring systems may have higher n -CH2- ~1465 Methylene bend (scissor) -CH3 ~1375 Methyl bend (sym) -(CH2)4- ~720 Rocking motion 4 or more –CH2- (long chain band) C-C Not interpretively useful, small weak peaks
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkanes – Dodecane – C12H26
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkanes – Cyclopentane – C5H10
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Group Frequencies and Analysis The Hydrocarbons Alkanes
IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkanes Additional – If the region is free of interference, the presence of certain alkyl groups can be discerned: Methylene Methyl H C H C H C Scissor 1465 Bendasymm 1450 Bendsymm 1375 usually overlap gem-dimethyl 1380 1370 t -butyl 1390 1370
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkanes Additional – Example: Compare 2,2-dimethylpentane vs. 2-methylhexane: vs.
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Group Frequencies and Analysis The Hydrocarbons Alkenes
IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkenes General – slightly more complex than alkanes; asymmetric C=C is observed as well as the sp2-C-H stretch. Still, bands are weak to medium in intensity Group Frequencies (cm-1): =C-H Stretch - Diagnostic for unsaturation- may be aromatic as well Out-of-plane (oop) bend - Can be used to determine degree of substitution C=C - Can be reduced by resonance - Symmetrical C=C do not absorb - trans- weaker than cis-
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkenes – 1-octene – C8H16 Note – you still have alkane present!
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkenes – trans-4-octene – C8H16 Note – absence of C=C band, shouldering of C-H band
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkenes – cis-2-pentene – C5H10 Note – shouldering of C-H band
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkenes – cyclopentene – C5H8 Note – increased complexity due to ring vibrations
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Group Frequencies and Analysis The Hydrocarbons Alkenes
IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkenes Substitution – The out of plane =C-H bend produces strong bands but interference can come from aromatic rings (similar oop) and C-Cl bonds (~700) monosubstituted cis-1,2 trans-1,2 1,1-disubstitued trisubstituted tetrasubstituted 1000 900 800 700 none, with weak C=C
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overtone usually observed
IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkenes Substitution – The monosubstitued band is very reliable; and the variance induced by electronic effects is observed monosubstituted (R-) monosubstitued w/lone pair group (ex. –Cl, -F, -OR) w/conj. group (ex. C=O, CN) The shifts are similar for 1,1-disubstitued systems 1000 900 800 700 overtone usually observed
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkenes Rings – Incorporation of a double bond endocyclic or exocyclic to a ring may shift the observed band Endocyclic: Ring strain shifts the C=C band to lower n (ex. cyclopropene) The adjacent C-C bond couples with the C=C system – if the resulting component vector is along the line of the C=C bond an increase in n occurs – this reaches a minima at 90o for cyclobutene (no net component along C=C bond) and rises again with cyclopropene nC=C 1650 1646 1611 1566 1656
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkenes Rings – Endocyclic: If C=C at a ring fusion, absorption is reduced as if one further carbon was removed from the ring: The presence of additional alkyl groups on the ring dramatically raises nC=C nC=C 1611 nC=C 1656 1788 1883 nC=C 1566 1641 1675
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkenes Rings – Exocyclic: these C=C bonds give an increase in absorption n with decreasing ring size: As the angle between the two C-C bonds is reduced – more p character is required (sp = 180°, sp2 = 120°, sp3 = 109.5°, “sp>3” = <109° The p character of the double bond is reduced, but the stronger s bond is strengthened to a greater degree Think of the allene example (“2-membered ring”) as an extreme example nC=C
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Group Frequencies and Analysis The Hydrocarbons Alkynes
IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkynes General – can be symmetric, psuedo-symmetric or internal – greatly reducing the number of observed bands Group Frequencies (cm-1): C-H ~3300 Stretch - Diagnostic for terminal alkyne CC ~2150 - Can be reduced by resonance Symmetrical and psuedo-sym. CC do not absorb Bend (Text does not list) Possible not to observe any bands for the CC system
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkynes – 1-hexyne – C6H10 Nice terminal, asymmetric, well behaved alkyne
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkynes – 3-hexyne – C6H10 A not-so-nice, internal, symmetrical alkyne
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Alkynes – 1-hexyne – C6H10 Nice terminal, asymmetric, well behaved alkyne
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Group Frequencies and Analysis The Hydrocarbons
IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Mononuclear aromatic rings General – not true alkenes; most of the small bands associated with them are not of diagnostic value; electronic effects of a single group on the ring can change the observed bands drastically Group Frequencies (cm-1): -C-H Stretch Also for alkenes C-H Out of plane (oop) bend Can be used to determine substitution pattern Overtone and combination bands If observed, similar too oop =C-H Ring stretch – observed as two doublets (1600, 1580, 1500 & 1450) Greatly dependent on substituents
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Mononuclear aromatic rings – toluene – C7H8 Typical mono-substituted (EDG) ring
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Mononuclear aromatic rings – o-xylene – C8H10 Typical ortho-substituted (EDG) ring
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Mononuclear aromatic rings – m-xylene – C8H10 Typical meta-substituted (EDG) ring
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Mononuclear aromatic rings – p-xylene – C8H10 Typical para-substituted (EDG) ring
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Mononuclear aromatic rings – a-methylstyrene – C9H10 Conjugated mono-substituted ring
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Mononuclear aromatic rings Substitution – The aromatic out of plane =C-H bend produces strong bands but interference can come from alkenes (similar oop) and C-Cl (~700) Consider this region to only be reliable for alkyl-, alkoxy-, halo-, amino-, and acetyl substituted rings Interpretation is often unreliable for nitro-, carboxylic- and sulfonic groups The overtone of these bands is the dominant source of the combination and overtone bands observed at
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Group Frequencies and Analysis The Hydrocarbons
IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Mononuclear aromatic rings Substitution – 900 800 700 600 mono ortho meta para 1,2,4 1,2,3 1,3,5
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Group Frequencies and Analysis The Hydrocarbons
IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Mononuclear aromatic rings Substitution – The aromatic combination and overtone bands are a set of weak absorptions that occur from This is often obscured by C=O mono The general shape of the pattern is used for determining substitution pattern; typically only a neat liquid sample gives an intense enough set of bands for analysis ortho meta para 1,2,3 1,3,5 1,2,4
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IR Spectroscopy Group Frequencies and Analysis The Hydrocarbons Polynuclear and Hetero- aromatic rings General – All bands for these aromatic systems are similar to the mononuclear systems; shifts should be assumed, and analysis would be case-by-case
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Group Frequencies and Analysis
IR Spectroscopy Group Frequencies and Analysis sp3 Oxygen – Alcohols, phenols and ethers Alcohols General – the best recognized group on carefully selected spectra, but H-bonding effects can drastically change the position, intensity and shape of the O-H band Group Frequencies (cm-1): O-H (free) Stretch Seen in dilute solution or gas phase spectra O-H (H-bond) The “classic” H-bonded band, seen in addition to the free band in solution C-O-H Bend Often obscured by -CH3 bend C-O Can be used to determine 1o, 2o, 3o or phenolic structure
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IR Spectroscopy Group Frequencies and Analysis sp3 Oxygen – Alcohols, phenols and ethers Alcohols – 1-octanol Neat liquid sample gives classic spectrum
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IR Spectroscopy Group Frequencies and Analysis sp3 Oxygen – Alcohols, phenols and ethers Alcohols – 1-octanol Same sample in dilute CCl4 solution (solvent bands deleted for clarity)
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IR Spectroscopy Group Frequencies and Analysis sp3 Oxygen – Alcohols, phenols and ethers Phenols – p-cresol Presence of aromatic bands, sharper -OH
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IR Spectroscopy Group Frequencies and Analysis sp3 Oxygen – Alcohols, phenols and ethers Alcohols – Substitution – Using the position of the C-O stretching band, it is possible to suggest a 1o, 2o, 3o or phenolic structure to the alcohol; but these should be considered as base values, that may be changed by the effects of conjugation or an adjacent ring system base value phenol 1220 tertiary 1150 secondary 1100 primary 1050 nC-O 1070 nC-O 1017 nC-O 1070 nC-O 1060 nC-O 1030
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Group Frequencies and Analysis
IR Spectroscopy Group Frequencies and Analysis sp3 Oxygen – Alcohols, phenols and ethers Ethers General – like alkynes, the simplicity of the spectra may allow them to pass unnoticed – deduce from molecular formula if one should be present Group Frequencies (cm-1): C-O Stretch (asymm.) Absence of C=O and O-H will confirm it is not ester or alcohol Simple alkyl ethers usually one band at 1120, aryl alkyl ethers give two bands – 1250 & 1040
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IR Spectroscopy Group Frequencies and Analysis sp3 Oxygen – Alcohols, phenols and ethers Ethers – diispropyl ether Spectrum dominated by all other functionality
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IR Spectroscopy Group Frequencies and Analysis sp3 Oxygen – Alcohols, phenols and ethers Ethers – Additional Types Aryl and vinyl ethers – The effect of conjugation gives the C-O bond a small amount of double bond character, raising the observed n Furthermore, strongly asymmetric systems (aryl alkyl and vinyl alkyl ethers) may show an additional weak C-O band for the symmetric stretch at 1040 and 850 respectively
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IR Spectroscopy Group Frequencies and Analysis sp3 Oxygen – Alcohols, phenols and ethers Ethers – Additional Types Epoxides – Most important bands are the ring deformation bands at nasym and nsym Weaker “breathing mode” band is present at Acetals and Ketals – Give four or five unresolved bands in the region
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Group Frequencies and Analysis sp3 Nitrogen – Amines
IR Spectroscopy Group Frequencies and Analysis sp3 Nitrogen – Amines Amines – Once presence is determined, the substitution at nitrogen is easy to determine; only the 3° amine may present a problem Group Frequencies (cm-1): N-H (-NH2) (2 bands) Stretch (sym. and asym.) Bend (-NHR) (1 band) 1500 Stretch For alkyl amines, very weak – for aromatic 2° amines, stronger ~800 Oop bend N-N Remember 3° amines have no N-H bands
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IR Spectroscopy Group Frequencies and Analysis sp3 Nitrogen – Amines 1° Amine – tert-butylamine Two band –NH2 peak appears as small “w”
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IR Spectroscopy Group Frequencies and Analysis sp3 Nitrogen – Amines 2° Amine – dibutylamine Note weakness of –NH- band (can be mistaken as C=O overtone, if carbonyl is present)
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IR Spectroscopy Group Frequencies and Analysis sp3 Nitrogen – Amines 3° Amine – tributylamine Difficult to discern from alkane – molecular formula for confirmation almost requisite
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Group Frequencies and Analysis sp3 Nitrogen – Amines Ammonium Salts
IR Spectroscopy Group Frequencies and Analysis sp3 Nitrogen – Amines Ammonium Salts Almost certainly never encountered in neat samples, but an important component of amino acids and many pharmaceuticals Group Frequencies N-H Stretch 1° salts are at the higher n end of this band, 3° salts at the lower end Additional band sometimes obs. at 2100 Bend 1° as two bands (sym. And asymm.), 2° at the upper end of this range, 3° absorbs weakly
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IR Spectroscopy Group Frequencies and Analysis sp3 Nitrogen – Amines Ammonium Salts – anilinium hydrochloride Spectrum is of a KBr disc sample:
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Group Frequencies and Analysis Carbonyls
IR Spectroscopy Group Frequencies and Analysis Carbonyls General – Along with alcohols, the most ubiquitous group on the IR spectrum. Although it is easy to determine if the C=O is present, deducing the exact functionality and factors that influence the position of the band provide the challenge Base C=O Frequencies (cm-1): C=O 1810 Stretch (sym.) Anhydride band 1 1800 Acid Chloride 1760 Anhydride band 2 1735 Ester 1725 Aldehyde 1715 Ketone 1710 Carboxylic Acid 1690 Amide
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C N O F S Cl IR Spectroscopy Group Frequencies and Analysis Carbonyls
General – The carbonyl C=O frequency is very sensitive to the effects we went over previously – a quick recap Electronic Effects: Inductive vs. Resonance: On first inspection, the ester, amide and acid halide/anhydride all possess lone pairs of electrons that can resonate with the C=O (which should lower n) C N O F S Cl
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C N O F S Cl IR Spectroscopy Group Frequencies and Analysis Carbonyls
General – Electronic Effects: Inductive vs. Resonance: In the case of an oxygen or chlorine being adjacent to the carbonyl, each of these atoms resist the positive charge in the contributing resonance structure, and the inductive effect becomes a stronger factor C N O F S Cl This inductive effect draws in s electrons from the C=O, which strengthens the p bond – these carbonyls appear at higher n
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C N O F S Cl IR Spectroscopy Group Frequencies and Analysis Carbonyls
General – Electronic Effects: Inductive vs. Resonance: In the case of nitrogen, it is less electronegative than oxygen and has a greater acceptance of the positive charge in the contributing resonance structure, so the carbonyl is lowered in n C N O F S Cl The inductive effect of nitrogen compared to an sp2 carbon is negligible by comparison
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C N O F S Cl IR Spectroscopy Group Frequencies and Analysis Carbonyls
General – Electronic Effects: Inductive vs. Resonance: Likewise in aldehydes and ketones there is the inductive donation of electrons to the s bond of the carbonyl which slightly weakens and reduces the n of the p bond (and explains the small difference between aldehydes and ketones) C N O F S Cl The inductive effect of nitrogen compared to an sp2 carbon is negligible by comparison
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C N O F S Cl IR Spectroscopy Group Frequencies and Analysis Carbonyls
General – Electronic Effects: Inductive vs. Resonance: In addition, we discussed this effect in regards to a-halogenated carbonyls as one of the effects that can change group n C N O F S Cl The inductive effect of chlorine will draw s electrons through a-carbon, weakening the C=O s and strengthening the p
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IR Spectroscopy Group Frequencies and Analysis Carbonyls General – Electronic Effects - Resonance: Not only is the C=O n lowered by the effects of conjugation, the peak may also be broadened or split by the contribution of the two electronic conformers The s-cis absorbs at higher n than the s-trans. Why?
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IR Spectroscopy Group Frequencies and Analysis Carbonyls General – Ring Strain Effects: C=O groups that can be incorporated into a ring are sensitive to this effect. As ring size decreases more p-character must be used to make the single bonds take on the smaller angle (re: sp>3 = <109°). The p component of the C=O is weakened, but the s-bond strengthened, raising the overall n Cyclic ketones, esters (lactones), amides (lactams) and anhydrides exhibit this behavior To clear up confusion – there are two ways to strengthen the C=O Remove s bond character – p bond becomes more stronger (better overlap) – this is a result inductive w/d Remove p bond character – s bond becomes stronger – ring constraint
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IR Spectroscopy Group Frequencies and Analysis Carbonyls General – H-bonding effects: C=O groups are reduced in n if some of the electron density is tapped off to form H-bonds: This effect can be inter- or intra-molecular:
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Group Frequencies and Analysis Carbonyls
IR Spectroscopy Group Frequencies and Analysis Carbonyls Ketones – Simplest carbonyl group, for a single carbonyl compound, implied by a lack of any other functionality except hydrocarbon Group Frequencies (cm-1): C=O 1715 Stretch (sym.) n Base, sensitive to change conj. w/C=C nC=C reduced to conj. w/Ph nring Decreased ring size raises n Bend
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Ketones – 2-hexanone Typical aliphatic ketone
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Ketones – 4-methylacetophenone Typical aromatic ketone,
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Group Frequencies and Analysis Carbonyls
IR Spectroscopy Group Frequencies and Analysis Carbonyls Ketones – Simplest carbonyl group, for a single carbonyl compound, implied by a lack of any other functionality except hydrocarbon Group Frequencies (cm-1): C=O 1715 Stretch (sym.) n Base, sensitive to change conj. w/C=C nC=C reduced to conj. w/Ph nring Decreased ring size raises n Bend
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Group Frequencies and Analysis Carbonyls
IR Spectroscopy Group Frequencies and Analysis Carbonyls Aldehydes – Presence of the unique carbonyl C-H bond differentiates this group from ketones Group Frequencies (cm-1): C=O 1725 Stretch (sym.) n Base, sensitive to change conj. w/C=C nC=C reduced to 1640 conj. w/Ph nring 2820, 2720 Stretch Fermi doublet; Higher n band often obscured by sp3 C-H
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Aldehydes – isovaleraldehyde Typical aliphatic aldehyde – note appearance of Fermi doublet and C=O overtone
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Aldehydes – anisaldehyde Typical aromatic aldehyde, note how C=O obscures the combination and overtone region – oop region would be used to determine substitution
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Group Frequencies and Analysis Carbonyls
IR Spectroscopy Group Frequencies and Analysis Carbonyls Carboxylic Acids – Various H-bonding effects lead to messy spectra, especially in the upper frequency ranges – be aware of the effects of monomeric, dimeric and oligomeric species on the spectrum Group Frequencies (cm-1): C=O 1710 Stretch (sym.) n Base, sensitive to change; conjugation gives reduced n C-O Stretch O-H Overlaps C-H region in most cases; multiple “sub-peaks” can be seen for the dimeric and oligomeric species – simplified in non-polar solution or gas phase spectra
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Carboxylic Acids – propionic acid Aliphatic carboxylic acid – neat sample vs. CCl4 solution (right)
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Carboxylic Acids – o-toluic acid Aromatic carboxylic acid, larger non-polar “end” of the molecule cuts down on the hydrogen bonding seen with the smaller, previous propionic acid
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Group Frequencies and Analysis Carbonyls Carboxylic Acids - Salts
IR Spectroscopy Group Frequencies and Analysis Carbonyls Carboxylic Acids - Salts Salts are expressed as possesing one single and one double bond – the true picture is one that is isoelectronic with the nitro group, with two bonds to oxygen with a bond order of 1.5 Group Frequencies: 1600 1400 Stretch (asymm.) Stretch (sym.)
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Carboxylic Acids - Salts – ammonium benzoate Here is an example of ammonium and carboxylate moieties:
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Carboxylic Acids – Amino Acids – L-alanine Amino Acids combine the features of carboxylate and ammonium salts:
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Group Frequencies and Analysis Carbonyls
IR Spectroscopy Group Frequencies and Analysis Carbonyls Esters – Ester oxygen has an electron withdrawing effect that tends to draw in electrons within the C=O system, strengthening it compared to other carbonyls Group Frequencies (cm-1): C=O 1735 Stretch (sym.) n Base, sensitive to change conj. C=C nC=C reduced to w/Ph nring conj. of sp3 O nC=O increases with smaller ring C-O Stretch, 2 bands
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Esters – methyl butyrate Simple aliphatic ester
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Esters – methyl m-bromobenzoate Conjugation on the carbonyl end:
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Esters – phenyl acetate Conjugation on the sp3 oxygen end:
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Group Frequencies and Analysis Carbonyls
IR Spectroscopy Group Frequencies and Analysis Carbonyls Amides – Amide nitrogen acts as a conjugating group with C=O, reducing double bond character; amide nitrogen appears similar to amime, including the effects of substitution Group Frequencies (cm-1): C=O 1685 Stretch (sym.) n Base, sensitive to change Can be as low as 1630 w/conj. N-H ~3300 Stretch Similar to amines, but typically more intense nC=O increases with smaller ring Bend ~800 oop bend
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Amides – pivalamide Primary aliphatic amide
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Amides – 2-pyrrolidone Cyclic secondary amide - lactam
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Group Frequencies and Analysis Carbonyls
IR Spectroscopy Group Frequencies and Analysis Carbonyls Anhydrides – With acid halides, typically the highest n C=O; appears as two bands for the symmetric and asymmetric stretching modes Group Frequencies (cm-1): C=O Stretch (asym.) n Base, sensitive to change conj. C=C Stretch (sym.) Two bands of variable relative intensity nC=O increases with smaller ring C-O Stretch, multiple bands
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Anhydrides – iso-butyric anhydride Typical anhydride
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Group Frequencies and Analysis Carbonyls
IR Spectroscopy Group Frequencies and Analysis Carbonyls Acid Halides – Acid bromides and iodides are not often encountered; acid chlorides are the most prevalent (and useful) Group Frequencies (cm-1): C=O Stretch (sym.) n Base, sensitive to change conj. w/Ph add. band Fermi resonance with combination and overtone region of aromatic ring C-Cl Stretch If below 600, not observed using NaCl windows C-Br Typically too low to obs. C-I
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IR Spectroscopy Group Frequencies and Analysis Carbonyls Acid Halides – propionyl chloride Overtones of low n peaks can confuse some spectra
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Group Frequencies and Analysis sp2 and sp Nitrogen compounds
IR Spectroscopy Group Frequencies and Analysis sp2 and sp Nitrogen compounds Nitriles – The “other” triple bond group observed in IR, due to the higher dipole change during the stretching vibration, this band is more intense than CCs. Group Frequencies (cm-1): CN 2250 Stretch (sym.) n sensitive to change from conjugation; usually stronger than CC
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IR Spectroscopy Group Frequencies and Analysis sp2 and sp Nitrogen compounds Carbonyls Nitriles – benzonitrile
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Group Frequencies and Analysis sp2 and sp Nitrogen compounds
IR Spectroscopy Group Frequencies and Analysis sp2 and sp Nitrogen compounds Imines and Oximes – Often referred to as “derivatives” of carbonyl compounds, these groups are not often encountered in routine IR obs. Group Frequencies (cm-1): C=N (imine and oxime) Stretch (sym.) n sensitive to change from conjugation; usually stronger than CC O-H (oxime) Stretch H-bond effects N-O
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IR Spectroscopy Group Frequencies and Analysis sp2 and sp Nitrogen compounds Imines and Oximes – acetone oxime
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Group Frequencies and Analysis sp2 and sp Nitrogen compounds
IR Spectroscopy Group Frequencies and Analysis sp2 and sp Nitrogen compounds Isocyanates and Isothiocyanates – Reactive groups, not often observed in routine qualitative IR Group Frequencies (cm-1): N=C=O ~2270 Stretch (sym.) broad n band – coupled vibration N=C=S ~2125 Stretch (1 or 2 bands)
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IR Spectroscopy Group Frequencies and Analysis sp2 and sp Nitrogen compounds Isocyanates and Isothiocyanates– tert-butyl isocyanate
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Group Frequencies and Analysis sp2 and sp Nitrogen compounds
IR Spectroscopy Group Frequencies and Analysis sp2 and sp Nitrogen compounds Nitro – Useful, easily incorporated group on aromatic rings, less often encountered on alkyl compounds Group Frequencies (cm-1): Stretch (asymm.) Stretch (sym.) Aliphatic nitro Aromatic nitro
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IR Spectroscopy Group Frequencies and Analysis sp2 and sp Nitrogen compounds Nitro – o-nitrotoluene
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Group Frequencies and Analysis Sulfur
IR Spectroscopy Group Frequencies and Analysis Sulfur Thiols and Sulfides – Sulfur, due to its large size shifts most observed IR bands to lower frequencies – often out of the observed region Group Frequencies (cm-1): S-H (thiol) 2550 Stretch (sym.) Unique region of IR spectrum C-S-C No useful information
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IR Spectroscopy Group Frequencies and Analysis Sulfur Thiol (Mercaptan) – 1,2-ethanethiol
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Group Frequencies and Analysis Sulfur
IR Spectroscopy Group Frequencies and Analysis Sulfur Sulfoxides and Sulfones – Oxidized sulfur, the SO bonds are useful for determining oxidation state, if the presence of sulfur is known Group Frequencies (cm-1): SO 1050 Stretch (sym.) OSO ~1375 ~1150 Stretch (asymm.)
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IR Spectroscopy Group Frequencies and Analysis Sulfur Sulfoxide (Mercaptan) – di-butyl sulfoxide Be wary of water in the spectrum of sulfoxides
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IR Spectroscopy Group Frequencies and Analysis Sulfur Sulfone– di-butyl sulfone
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Group Frequencies and Analysis Sulfur
IR Spectroscopy Group Frequencies and Analysis Sulfur Sulfonic Acids, Sulfonamides and Sulfonates – Sulfur equivalent of the carboxylic acid derivatives; the O or N groups act as we have observed Group Frequencies (cm-1): OSO ~1375 ~1150 Stretch (asymm.) Stretch (sym.) As for sulfones – groups bound to sulfur identify the group, just as with the carboxylic acid derivatives differ from ketones S-O (acid & sulfonate) Stretch May appear as several bands O-H & N-H As for the carboxylic acid derivatives
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IR Spectroscopy Group Frequencies and Analysis Sulfur Sulfonamides – p-toluenesulfonamide
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Group Frequencies and Analysis Phosphorus
IR Spectroscopy Group Frequencies and Analysis Phosphorus Phosphines – Phosphorus in its lowest oxidation state – many bands that overlap with other useful regions; exercise caution in interpretation using IR Group Frequencies (cm-1): P-H Stretch (sym.) Bend PH2 Bend, two bands P-CH3 P-CH2-
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IR Spectroscopy Group Frequencies and Analysis Phosphorus Phosphines – tri-butylphosphine
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Group Frequencies and Analysis Phosphorus
IR Spectroscopy Group Frequencies and Analysis Phosphorus Phosphine Oxides – More common to observe these phosphorus compounds Group Frequencies (cm-1): Phosphate Esters, Acids and Amides – Often encountered in biological systems PO Stretch (sym.) PO Stretch (sym.) R-O Stretch, 1 or 2 band P-O Stretch
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IR Spectroscopy Group Frequencies and Analysis Phosphorus Phosphine Oxides, Phosphate Esters – tri-butylphosphate
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Group Frequencies and Analysis Halogens
IR Spectroscopy Group Frequencies and Analysis Halogens Fluorides and Chlorides – Smaller halogen bonds to carbon in observed frequency range Group Frequencies (cm-1): Bromides and Iodides – Not often obs. Due to low n of C-X stretch C-F Stretch (sym.) Monofluoroalkyl at lower n Polyfluoroalkyl at upper n Aryl fluorides up to 1450 C-Cl Stretch Different conformers may give split peaks C-Br Stretch Bend is obs. at ~1200 C-I Bend is obs. at ~1150
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hn Energy hn hn hn IR Spectroscopy
Instrumentation and Experimental Aspects The IR Spectrometer – Dispersive and Fourier Transform Dispersive IR Spectrometers All spectrometers consist of four basic parts that are coupled with all four parts of the spectroscopic process - irradiation, absorption-excitation, re-emission-relaxation and detection. excited state Absorption-Excitation: Spectrometer needs to contain the sample Detection-reemission : Spectrometer needs to detect the photons emitted by the sample and ascertain their energy hn Relaxation Energy rest state rest state Irradiation: Spectrometer needs to generate photons hn hn hn
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Dispersive and Fourier Transform Dispersive IR Spectrometers Those four parts are: Source/Monochromator Sample cell Detector/Amplifier Output Dispersive IR spectrometers were the first IR instruments, however their simplicity and longevity allows them to continue in service – for most routine organic analyses their speed and resolution is adequate For the most part, their design is austere and relies on simple mechanics and optics to generate a spectrum, very similar to simply rotating a glass prism to see different bands of visible light
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Dispersive and Fourier Transform Dispersive IR Spectrometers Here is a general schematic:
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Dispersive and Fourier Transform Dispersive IR Spectrometers Source is a heated nichrome wire which produces a broad band continuum of IR light (as heat) The beam is directed through both the sample and a reference cell A rapidly rotating sector (beam chopper) continuously switches between directing the two beams to a diffraction grating
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Dispersive and Fourier Transform Dispersive IR Spectrometers The diffraction grating slowly rotates, such that only one narrow frequency band of IR light is at the proper angle to reach the detector A simple circuit compares the light from the sample and reference and sends the difference to a chart recorder
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Dispersive and Fourier Transform Dispersive IR Spectrometers On the older instruments the motor in the chart recorder was synchronized (& calibrated) to the motor on the diffraction grating Because each spectrum is the result of the tabulation of the spectroscopic process at each frequency individually, it is said to record the spectrum in the frequency domain
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Dispersive and Fourier Transform Dispersive IR Spectrometers Advantages – simple, easy to maintain – last the life of the source and moving parts Disadvantages – to cover the entire IR band of interest to chemists it is necessary to use two diffraction gratings At high q, the component frequencies are more spread out, so the resulting spectra appear to have various regions expanded or compressed The limit to resolution is 2-4 cm-1
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Dispersive and Fourier Transform Fourier Transform IR Spectrometers FT-IR is the modern state of the art for IR spectroscopy The system is based on the Michelson interferometer Laser source IR light is separated by a beam splitter, one component going to a fixed mirror, the other to a moving one and are reflected back to the beam splitter The beam splitter recombines the two to a pattern of constructive and destructive interferences known as an interferogram – a complex signal, but contains all of the frequencies that make up the IR spectrum
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Dispersive and Fourier Transform Fourier Transform IR Spectrometers The resulting signal is essentially a plot of intensity vs. time Such information if plotted would look like the following: This is meaningless to a chemist – we need this to be in the frequency domain rather than time….
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Dispersive and Fourier Transform Fourier Transform IR Spectrometers By applying a mathematical transform on the signal – a Fourier transform – the resulting frequency domain spectrum can be observed FT-IRs give three theoretical advantages: Fellgett’s advantage – every point in the interferogram is information – all wavelenghts are represented Jacquinot’s advantage – the entire energy of the source is used – increasing signal-to-noise Conne’s advantage – frequency precision – Dispersive instruments can have errors in the ability to move slits and gratings reproducibly – FTIR is internally referenced from its own beam
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Dispersive and Fourier Transform Fourier Transform IR Spectrometers Justik’s advantage – does it give me what I need Single-beam instrument – collect a background (air has IR active molecules!) Fast – all frequencies are scanned simultaneously No referencing! Computer based – scaling and editing of the spectrum to squeeze out the most data; spectra are proportional (no stretching or squeezing of regions), comparison with spectral libraries Disadvantages – expenisve relative to dispersive instruments, and the components take more expertise and service calls to replace
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Experimental aspects Sample size – typically the size of the beam – mm’s mg’s Non-destructive – sample can be recovered with varying degrees of difficulty Liquid samples – the easiest IR spectra are those of “neat” liquid samples Solid samples are too dense for good IR spectra – inter-molecular coupling of vibrational states occurs and peaks are greatly broadened In the liquid state full 3-D motion is available, and these effects are averaged out and diminished The thickness of a sample can be decreased to reduce these effects further Thin film liquid samples are best!
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Experimental aspects Liquid samples Sample cell cannot possess covalent bonds (SiO2, or glass is out) The most common cell is a pair of large transparent “windows” of inorganic salts Most common: NaCl – cheap, transparent from 650 – 4000 cm-1, but fragile Less common – AgCl, KBr, etc. – if you need transparency below 650, limit is practically 400
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Experimental aspects Solution samples One way solids can be handled is as a solution Key is that the solvent picked will cover the least amount of the spectrum as possible, as it will also be present Common solvents typically are symmetrical, or have many halogenated bonds – low cm-1: CCl4, CHCl3, CH2Cl2, etc. The cell in this case is two NaCl (or other) windows with a spacer, the sample is loaded via a syringe into the cell:
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Experimental aspects Solution samples A newer method involves the use of a polyethylene matrix, that will hold allow a solution sample to evaporate, leaving small portions of the sample embedded in the matrix The samples are “liquid-like” The only interference is that of hydrocarbon
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Experimental aspects Solid Samples The most common treatment for solid samples is to “mull” them with thick mineral oil (high MW hydrocarbon) - Nujol® Just like with the polyethylene cards, the molecules of the sample are held in suspension within the oil matrix Again, the interference is that of hydrocarbon
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IR Spectroscopy Instrumentation and Experimental Aspects The IR Spectrometer – Experimental aspects Solid Samples The connoisseurs method (with no organic interference) is to press the solid with KBr into a pellet Under high pressure the KBr liquefies and entraps individual molecules of the sample in the matrix These spectra are the only spectra of solids that are as interference free as liquids
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Neat Sample IR Spectroscopy Instrumentation and Experimental Aspects
The IR Spectrometer – Experimental aspects Differences in Spectral Appearence Compare the following three IR spectra of p-cresol Neat Sample
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KBr Pellet IR Spectroscopy Instrumentation and Experimental Aspects
The IR Spectrometer – Experimental aspects Differences in Spectral Appearence Compare the following three IR spectra of p-cresol KBr Pellet
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CCl4 Solution IR Spectroscopy Instrumentation and Experimental Aspects
The IR Spectrometer – Experimental aspects Differences in Spectral Appearence Compare the following three IR spectra of p-cresol CCl4 Solution
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Nujol Mull IR Spectroscopy Instrumentation and Experimental Aspects
The IR Spectrometer – Experimental aspects Differences in Spectral Appearence Compare the following three IR spectra of m-nitroanisole Nujol Mull
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KBr Pellet IR Spectroscopy Instrumentation and Experimental Aspects
The IR Spectrometer – Experimental aspects Differences in Spectral Appearence Compare the following three IR spectra of m-nitroanisole KBr Pellet
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CCl4 Solution IR Spectroscopy Instrumentation and Experimental Aspects
The IR Spectrometer – Experimental aspects Differences in Spectral Appearence Compare the following three IR spectra of m-nitroanisole CCl4 Solution
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