Delocalised electrons are often found in molecules with resonance structures or conjugated bonds that allow for electron sharing across multiple atoms.
In species I (\( \mathrm{C_2O_4^{2-}} \)) and II (acetone), electrons are delocalised over the entire structure, as seen in their resonance forms. In \( \mathrm{C_2O_4^{2-}} \), the electron density is shared between the two oxygens and the carbon atoms, forming a delocalised system. This delocalisation stabilises the ion and contributes to its overall chemical properties. In acetone, the carbonyl group (\( \mathrm{C=O} \)) allows for electron delocalisation via resonance with the oxygen atom, further stabilising the molecule.
In contrast, species III does not have delocalised electrons because it is a simple molecule with no resonance structures. This lack of delocalisation means that the electrons are more localized, which affects its reactivity and stability compared to species I and II.
Thus, species I and II exhibit delocalised electrons, while species III does not.
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