Name: conjugation shifts ir bond stretching
Uploaded: 2024-12-05T18:32:09.000Z
Duration: 1 min 4 s
Channel: JoVE

Les groupes carbonyles dans les cétones conjuguées absorbent à des fréquences d’étirement plus basses que les cétones non conjuguées.
La délocalisation électronique dans les cétones conjuguées induit un caractère partiel de liaison unique dans le groupe carbonyle, conduisant à des absorptions à des fréquences d’étirement plus basses.
Si des substituants sont attachés au groupe carbonyle, les effets électroniques influencent ses absorptions d’étirement.
Par exemple, le groupe carbonyle d’un amide s’étire à une fréquence plus basse que le groupe carbonyle d’une cétone.
Ceci est attribué au doublet non liant d’azote qui participe au don d’électrons par résonance, ce qui entraîne une réduction du caractère de double liaison. La liaison carbonyle plus faible présente donc de faibles absorptions IR.
Le groupe carbonyle d’un ester s’étire à une fréquence plus élevée que le groupe carbonyle d’une cétone.
Cela est dû à la liaison carbonyle plus forte résultant de l’effet inductif de retrait d’électrons de l’atome d’oxygène.

fréquence d'absorption ir: délocalisation

IR Absorption Frequency: Delocalization

La délocalisation des électrons fait référence à la distribution des électrons sur plusieurs atomes au sein d'une molécule plutôt que d'être confinés à un seul atome ou à une seule liaison. Ce phénomène est courant dans les systèmes à liaisons conjuguées, structures dans lesquelles des liaisons simples et doubles alternées permettent aux électrons π de se déplacer librement à travers le réseau. Le mouvement des électrons stabilise la molécule et peut affecter diverses propriétés chimiques, notamment les fréquences vibrationnelles observées en spectroscopie IR.

En spectroscopie IR, la délocalisation des électrons influence directement les fréquences vibrationnelles (d'étirement) des liaisons. Dans les systèmes conjugués, tels que les alcènes conjugués ou les composés aromatiques, la délocalisation des électrons réduit le caractère de double liaison des liaisons individuelles, les rendant légèrement plus faibles. La réduction de la force de liaison diminue l'énergie nécessaire à l'étirement de la liaison, ce qui conduit à une fréquence d'étirement inférieure à celle des doubles liaisons isolées.

Par exemple, dans une cétone conjuguée, le groupe carbonyle (C=O) présente une fréquence d'étirement inférieure à celle des cétones normales. Cet étirement est dû à la délocalisation des électrons dans le système conjugué, ce qui fait que la double liaison carbonyle présente un caractère de double liaison partielle et un caractère de liaison simple. Le décalage peut être détecté sous forme de pic à un nombre d'onde inférieur, ce qui donne un aperçu de la structure moléculaire et du degré de conjugaison dans l'échantillon.

Le substituant connecté au carbone carbonyle affecte également la fréquence d'étirement via des effets de résonance et d'induction. Par exemple, le groupe carbonyle dans les esters présente une fréquence d'étirement plus élevée que les composés carbonyles, car l'effet inductif négatif prédominant de l'atome d'oxygène connecté au carbone carbonyle confère un caractère de double liaison plus prononcé au C=O.

Dans les amides, la paire non partagée d'un atome d'azote peut participer à la résonance, diminuant ainsi le caractère de double liaison carbonyle. En conséquence, les amides présentent une fréquence d'étirement plus faible que les cétones.

Fréquence d'absorption IR: délocalisation

La délocalisation électronique fait référence à la distribution d’électrons à travers plusieurs atomes au sein d’une molécule plutôt que d’être confinée à un seul atome ou ...

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Analytical Chemistry

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Molecular Vibrational Spectroscopy

Spectroscopie vibrationnelle moléculaire

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conjugation shifts ir bond stretching

Conjugation shifts IR bond stretching because electron delocalization changes bond strength. Electron delocalization means electrons spread across more than one atom instead of staying in one bond or one atom. It is common in conjugated systems, where alternating single and double bonds let pi-electrons move through the molecule.

This electron movement helps stabilize the molecule. It also lowers the double bond character of the bonds in the conjugated network. When a bond has less double bond character, it is slightly weaker and needs less energy to stretch. In IR spectroscopy, that change appears as a lower stretching frequency than an isolated double bond.

A conjugated ketone shows this effect clearly. Its carbonyl group, or C=O bond, absorbs at a lower wavenumber than a normal ketone because delocalization gives the carbonyl bond partial single-bond character. That shift can help identify the structure of the sample and show how much conjugation is present.

The atom attached to the carbonyl carbon also matters. In esters, the oxygen attached to the carbonyl carbon has a strong negative inductive effect, so the C=O bond shows a higher stretching frequency than in other carbonyl compounds. In amides, the nitrogen lone pair can take part in resonance. This reduces carbonyl double bond character and makes amide stretching frequencies lower than ketone stretching frequencies.

Conjugation Shifts IR Bond Stretching

infrared (ir) spectroscopy: overview

IR Spectra and Functional Group ID

Infrared (IR) spectroscopy helps identify functional groups in molecules by measuring how they absorb infrared light. It is based on the idea that electromagnetic radiation can move atoms or molecules from a lower energy state to a higher one when the radiation matches the energy gap between those states. In IR spectroscopy, that absorption happens as molecular vibrations change.

ir spectroscopy: molecular vibration overview

ir-spectroscopy-molecular-vibration-overview

IR Spectroscopy: Vibration Types and Bands

IR spectroscopy explains how covalently bonded molecules absorb infrared radiation by moving to higher vibrational levels. The key motions are stretching and bending vibrations. These motions help describe how a bond responds when it absorbs IR energy. Stretching vibrations happen along the bond line and change the distance between two bonded atoms. They can be symmetric, where two bonds lengthen and shorten together, or asymmetric, where one bond moves one way while another moves the opposite...

ir spectroscopy: hooke's law approximation of molecular vibration

ir-spectroscopy-hooke-s-law-approximation-of-molecular-vibration

Molecular Bond Vibrations in IR Spectroscopy

Molecular bond vibrations can be modeled with IR spectroscopy using Hooke’s law. A covalently bonded heteronuclear diatomic molecule is treated like two masses connected by a spring. The atoms act like the masses, and the bond acts like the spring. Hooke’s law links the vibrational frequency to two main factors. The frequency increases with the force constant, K, which describes bond stiffness. It decreases with the reduced mass, μ, which combines the masses of both atoms into one value for...

ir spectrometers

IR Spectrometer Signal Paths

IR spectrometers use infrared light to compare a sample beam with a reference beam and record how each one behaves. The two main instruments are dispersive IR spectrometers and Fourier transform infrared, or FTIR, spectrometers. In a dispersive IR spectrometer, a hot wire produces the infrared beam. Mirrors split it into two equal beams. One beam passes through the sample, and the other serves as the reference. The beams then move into the monochromator, which separates the radiation into a...

ir spectrum

IR Spectrum Peak Regions and Patterns

Infrared (IR) spectroscopy shows how a molecule responds when IR radiation passes through it. The bonds in the molecule stretch or bend as they absorb that energy. This creates an absorption spectrum, which plots percent transmittance against wavenumber. Transmittance is the ratio of radiant power that passes through a sample to the radiant power from the source. When transmittance is multiplied by 100, it becomes percent transmittance, or %T. %T ranges from 100% for no absorption to 0% for...

ir absorption frequency: hybridization

C-H Stretching in Alkane, Alkene, and Alkyne IR

Hydrocarbons such as alkanes, alkenes, and alkynes show characteristic C–H stretching bands in infrared, or IR, spectra. These bands help identify how the carbon atoms are hybridized. The bond type affects the stretching frequency that appears in the spectrum. The difference comes from s character, which is the amount of s-orbital contribution in a hybrid orbital. Among sp, sp2, and sp3 hybridized orbitals, sp has the most s character at 50%. Because of that, the electrons are held closer to...

ir absorption frequency: delocalization

Conjugation shifts IR bond stretching because electron delocalization changes bond strength. Electron delocalization means electrons spread across more than one atom instead of staying in one bond or one atom. It is common in conjugated systems, where alternating single and double bonds let pi-electrons move through the molecule. This electron movement helps stabilize the molecule. It also lowers the double bond character of the bonds in the conjugated network. When a bond has less double bond...

ir frequency region: x&ndash;h stretching

IR Peaks for C-H, O-H, and N-H Bonds

IR spectroscopy shows the stretching bands of C-H, O-H, and N-H bonds in the 2700-4000 cm-1 range. These X-H bonds are useful for identifying common functional groups in a spectrum. Their peaks appear in different parts of this region and often have different shapes and strengths. C-H stretching gives sharp bands in the 2850-3000 cm-1 range. O-H stretching appears in the 3650-3200 cm-1 range, and N-H stretching appears in the 3500-3100 cm-1 range. N-H stretching usually shows one or two sharp...

ir frequency region: alkyne and nitrile stretching

ir-frequency-region-alkyne-and-nitrile-stretching

Triple-Bond Signals in IR Spectra

Alkyne and nitrile groups both contain triple bonds, and they show clear stretching bands in the diagnostic IR region. These absorptions usually appear around 2100 to 2300 cm −1 . This makes them useful markers when reading an IR spectrum. Triple bonds absorb at a higher stretching frequency than double bonds and single bonds. The C≡C bond stretches at a higher frequency than a C=C or C–C bond. The C≡N bond also stretches at a higher absorption than C=N and C–N bonds. This higher stretching...

ir frequency region: alkene and carbonyl stretching

ir-frequency-region-alkene-and-carbonyl-stretching

IR Signals for C=C and C=O Bonds

IR spectroscopy helps identify alkene double bonds and carbonyl groups by their stretching signals. These bonds absorb in a diagnostic region of the IR spectrum. Alkenes also show vinylic C–H stretching and C–H out-of-plane bending bands. Those bands can help determine substitution patterns on the double bond. The exact stretching frequency can change with bond environment. Resonance, inductive effects, ring strain, dipole moment, and hydrogen bonding can all shift the absorption. That is why...

ir frequency region: fingerprint region

IR Spectra: Diagnostic vs Fingerprint Region

IR spectra are divided into a diagnostic region and a fingerprint region. The diagnostic region lies above 1500 cm −1 and appears on the left side of the spectrum. It shows key bond stretches that help identify functional groups. In this region, single-bond vibrations from N-H, C-H, and O-H stretches appear at higher wavenumbers. The C≡C and C≡N stretches occur between 2100 and 2300 cm −1. The C=O, C=N, and C=C stretches appear between 1600 and 1850 cm −1. The fingerprint region lies below...

ir spectrum peak intensity: amount of ir-active bonds

ir-spectrum-peak-intensity-amount-of-ir-active-bonds

IR Peak Intensity and Bond Dipole Change

IR peak intensity depends on how much a bond’s dipole moment changes during vibration. When infrared light passes through a molecule, absorption happens only when a stretching or bending motion causes a substantial change in that bond dipole moment. That is what makes a molecule infrared active. Vibrational transitions usually fall in the infrared region from 4000 to 400 cm-1. Molecular bonds can stretch and bend in different ways, so an IR spectrum shows peaks with different intensities. The...

ir spectrum peak intensity: dipole moment

IR Absorption and Bond Dipole Changes

IR absorption depends on whether a bond has a changing dipole moment. A dipole moment comes from partial charge on each atom and the distance between them. It helps determine how strongly a bond absorbs infrared light and how intense the peak looks. A bond in an electric field can be stretched or compressed depending on the field direction. Infrared radiation has an electric field that flips direction very quickly. So polar bonds are pulled back and forth as the field reverses. If this motion...

ir spectrum peak broadening: hydrogen bonding

ir-spectrum-peak-broadening-hydrogen-bonding

Hydrogen Bonding Effects in IR O-H Peaks

Hydrogen bonding changes the O-H stretching peak in IR spectroscopy. The bond’s vibrational frequency depends on bond strength. Stronger bonds vibrate at higher frequencies, while weaker bonds vibrate at lower frequencies. In very dilute alcohol or phenol samples, or in the gas phase, the strong O-H bond gives a sharp peak at 3600-3650 cm−1. When intermolecular hydrogen bonding or intramolecular hydrogen bonding weakens the O-H bond, the stretch shifts to about 3300-3400 cm−1. This range of...

ir spectrum peak splitting: symmetric vs asymmetric vibrations

ir-spectrum-peak-splitting-symmetric-vs-asymmetric-vibrations

IR Peak Splitting in Amines and Nitro Groups

IR peak splitting can reveal how identical bonds in a polyatomic group are moving. These bonds may stretch in phase, which is symmetric stretching, or out of phase, which is asymmetric stretching. The two motions often create different IR peak shapes and positions. As a general rule, asymmetric stretching appears at a higher frequency than symmetric stretching. This pattern is useful for spotting functional groups in an IR spectrum. It also helps explain why some groups show one peak while...

applications of ir spectroscopy: overview

IR Spectroscopy Uses in Science and Forensics

IR spectroscopy is a useful tool for finding out what materials are made of. It is non-destructive, so the sample can often be kept intact. It gives chemical information about functional groups and the bonds between atoms in a molecule. This makes IR spectroscopy helpful in organic synthesis, pharmaceutical research, and materials science. Scientists use it to identify and characterize organic and inorganic compounds. It also helps with structural elucidation, which means working out a...

attenuated total reflectance (atr) infrared spectroscopy: overview

attenuated-total-reflectance-atr-infrared-spectroscopy-overview

ATR Infrared Spectroscopy for Material ID

ATR infrared spectroscopy is a method for identifying the composition of materials. It is used in chemistry, materials science, forensic science, and other areas where sample characterization is needed. The technique is useful because it usually needs little to no sample preparation and can be applied to many kinds of samples. The process starts when infrared, or IR, radiation is directed onto a diamond or germanium crystal. Because this crystal has a high refractive index, the IR beam...

raman spectroscopy: overview

Raman Spectra and Molecular Fingerprints

Raman spectroscopy uses laser light to study how molecules scatter light and reveal their vibrational energy levels. A monochromatic beam, or single-color light, hits the sample first. Most of the scattered light keeps the same frequency as the incoming light. This is called Rayleigh scattering. A small part of the light shifts in frequency because the photons exchange energy with molecular vibrations. That shifted light is Raman scattering. To collect a Raman spectrum, the sample is...

raman spectroscopy instrumentation: overview

raman-spectroscopy-instrumentation-overview

Raman Spectroscopy Setup and Detectors

Raman spectroscopy uses a laser, a sample holder, a wavelength selector, and a detector to measure scattered light from a sample. The laser is monochromatic, meaning it has one main wavelength. It usually uses visible or near-infrared light to create a tightly focused beam. That beam hits the sample and some of the light scatters. Liquid and gas samples are often placed in ordinary glass capillaries. Solid samples can be tested as powders packed into capillaries or as potassium bromide pellets.

key terms and concepts

Learn how electron delocalization changes IR stretching frequencies in conjugated systems, including ketones, esters, and amides, for high school chemistry.

Conjugation Shifts IR Bond Stretching | JoVE K12

analytical chemistry

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Conjugation Shifts IR Bond Stretching

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