Abstract
The infrared bands of CO and NH stretching vibrations of urea dissolved in a series of halogen derivatives of aliphatic hydrocarbons were analyzed. From the relationship between the solubility of urea and the structure of the solvent as well as the infrared spectra it is concluded that a double hydrogen bond between one urea and one solvent molecule is formed. In this bond, the solvent molecule is donor of two hydrogen atoms of two polar CH bonds, and the CO group of urea is proton acceptor. The interaction of NH groups with XC solvent groups is predominantly determined by the valence orbital repulsion of N and X atoms, and the polarizability of the halogen atom X.
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