Abstract

The intermolecular deuteron bonds formed between Cl₃CD and ClCCl₃ are stronger than between Cl₃CD and ClCCl₂D, since the Cl atoms of CCl₄ are more basic than Cl atoms for CDCl₃. The <i>n</i>-alkanes act as a diluent for CDCl₃ molecules, and the strength of the intermolecular proton bond in (Cl₃CD:ClCCl₂D)_<i>n</i> complexes increases as <i>n</i> becomes larger. Solvent density also plays an important role in solute/solvent interaction. Increased solvent density causes the CD:Cl or CD:π (of C=C group) intermolecular bond distance to decrease, causing the bond to be stronger. A repulsion exists between the intermolecular π electron system of benzene, 1,3-cyclohexadiene, or 1,4-cyclohexadiene and the chlorine atom σ electrons of CDCl₃, and this repulsive effect is a factor in establishing the equilibrium intermolecular bond distance formed between the CD:π bonds of benzene (or cyclohexadienes) and the proton of CDCl₃. These conclusions are based on the study of the <i>v</i>CD, <i>v</i>C=C, and <i>v</i>(C=C)₂ frequencies vs. mole % CDCl₃ (or CHCl₃)/solvent system.

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