Infrared Study of Solute/Solvent Interactions Between Separate Chloroform Solutions of Alkanes, Cycloalkanes, Alkenes, Cycloalkenes, Cyclohexadienes, Benzene, and Carbon Tetrachloride

$29.00 plus tax (Refund Policy)

Buy Article:

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 n-alkanes act as a diluent for CDCl3 molecules, and the strength of the intermolecular proton bond in (Cl3CD:ClCCl2D) n complexes increases as n 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 vCD, vC=C, and v(C=C)2 frequencies vs. mole % CDCl3 (or CHCl3)/solvent system.

Keywords: Infrared; Solute/solvent studies

Document Type: Research Article

DOI: http://dx.doi.org/10.1366/0003702934067315

Affiliations: Analytical Sciences Laboratory, 1897F Building, Dow Chemical Company, Midland, Michigan 48667

Publication date: May 1, 1993

More about this publication?
Related content

Tools

Favourites

Share Content

Access Key

Free Content
Free content
New Content
New content
Open Access Content
Open access content
Subscribed Content
Subscribed content
Free Trial Content
Free trial content
Cookie Policy
X
Cookie Policy
ingentaconnect website makes use of cookies so as to keep track of data that you have filled in. I am Happy with this Find out more