Electron delocalization refers to the distribution of electrons across multiple atoms within a molecule rather than being confined to a single atom or bond. This phenomenon is common in systems with conjugated bonds—structures where alternating single and double bonds allow π-electrons to move freely across the network. The movement of electrons stabilizes the molecule and can affect various chemical properties, including vibrational frequencies observed in IR spectroscopy.

In IR spectroscopy, electron delocalization directly influences the vibrational (stretching) frequencies of bonds. In conjugated systems, such as conjugated alkenes or aromatic compounds, electron delocalization reduces the double bond character of the individual bonds, making them slightly weaker. The reduction in bond strength lowers the energy required for the bond to stretch, leading to a lower stretching frequency than isolated double bonds.

For example, in a conjugated ketone, the carbonyl group(C=O) exhibits a lower stretching frequency than normal ketones. This stretching is due to the electron delocalization in the conjugated system, which makes the carbonyl double bond display a partial double bond and a single bond character. The shift can be detected as a peak at a lower wavenumber, providing insight into the molecular structure and degree of conjugation within the sample.

The substituent connected to carbonyl carbon also affects the stretching frequency via resonance and inductive effects. For instance, the carbonyl group in esters shows a higher stretching frequency than carbonyl compounds because the predominant negative inductive effect of the oxygen atom connected to the carbonyl carbon makes the more double bond character to C=O.

In amides, the lone pair of a nitrogen atom can participate in the resonance, decreasing the carbonyl double bond character. As a result, amides exhibit a lower stretching frequency than ketones.