Spectroscopic Properties of Alkenes

The infrared spectra of alkenes are sufficiently different from those of alkanes in most instances to make it possible to recognize when a double bond is present. For example, in the infrared spectrum of 1-butene (Figure 10-1) the absorption band near 1650 cm−1 is characteristic of the stretching vibration of the double bond. In general, the intensity and position of this band depends on the structure of the alkene; it varies with the degree of branching at the double bond, with the presence of a second unsaturated group in conjugation with the first (i.e.,  or ), and with the symmetry of the substitution of the double bond . However, in many cases the absorption bands caused by the various modes of vibration of the alkenic C−HC−H bonds frequently are more useful for detecting a double bond and identifying its type than is the absorption band caused by C=C stretch. With 1-butene, absorptions arising from the C−H vibrations of the terminal =CH2 group occur near 3100 cm−1, 1420 cm−1, and 915c m−1, and those of the −CH= grouping near 3020cm−1, 1420 cm−1, and 1000cm−1. In general, absorption bands at these frequencies are from the grouping −CH=CH2. The bands near 1420 cm−1 are due to in-plane bending, whereas those at 915 cm−1 to 1000 cm−1 arise from out-of-plane bending. The other intense absorptions, near 1460 cm−1 and 3000 cm−1, are due to C−H vibrations of the CH3CH2− group . These illustrate a further point - namely, the positions of the infrared absorptions of alkyl C−H bonds are significantly different from those of alkenic C−H bonds.

Figure 10-1: Infrared spectrum of 1-butene showing the vibrational assignments made to the various absorptions.

The double bonds of an alkene with no alkenic hydrogens are difficult to detect by infrared spectroscopy and in such cases Raman spectroscopy is helpful.

The infrared absorption of 1-butene that occurs at 1830 cm−1 falls in the region where stretching vibrations of alkene bonds usually are not observed. However, this band actually arises from an overtone (harmonic) of the =CH2 out-of-plane bending at 915cm−1. Such overtone absorptions come at exactly twice the frequency of the fundamental frequency, and whenever an absorption like this is observed that does not seem to fit with the normal fundamental vibrations, the possibility of its being an overtone should be checked.

With regard to electronic spectra, a π electron of a simple alkene can be excited to a higher energy (π∗) state by light of wavelength 180nm180nm to 100nm. However, many other substances absorb in this region of the spectrum, including air, the quartz sample cell, and most solvents that might be used to dissolve the sample, and as a result the spectra of simple alkenes are not obtained easily with the usual ultraviolet spectrometers. When the double bond is conjugated as in  or , then the wavelengths of maximum absorption shift to longer wavelengths and such absorptions are determined more easily and accurately.

In proton nmr spectra, the chemical shifts of alkenic hydrogens are toward lower fields than those of alkane hydrogens and normally fall in the range of 4.6-5.3 ppm relative to TMS .

مواضيع ذات صلة

Spectroscopic Properties of Alkynes

Application of Chemical Shifts to Structure Determination

Correlations Between Structure and Chemical Shifts

Electronegativity and Chemical Shifts

Effects of Carbon Bond Type

Mass Spectroscopy

Hydrogen Bonding

Chemical Exchange

Proton-Proton Splittings and Conformational Analysis

Spin-Spin Splitting - What We Observe

Proton-Proton Splittings and Chemical Exchange

Use of Nuclear Magnetic Resonance Spectroscopy in Organic Structural Analysis