Related Experiment Video
Updated: May 23, 2026
06:44
From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding
Published on: March 24, 2018
Solute-solvent interactions in cryosolutions: a study of halothane-ammonia complexes.
Bart Michielsen1, Johan J J Dom, Benjamin J van der Veken
1Department of Chemistry, University of Antwerp, Groenenborgerlaan 171, B-2020 Antwerp, Belgium.
Physical Chemistry Chemical Physics : PCCP
|March 31, 2012
Summary
This study investigated C-H···N bonded complexes between halothane and ammonia using spectroscopy. Complexation enthalpies were determined, revealing insights into solvent effects on these interactions.
Area of Science:
- Physical Chemistry
- Spectroscopy
- Intermolecular Forces
Background:
- Halothane and ammonia form C-H···N hydrogen bonds.
- Understanding these interactions is crucial for molecular recognition and solvation studies.
Purpose of the Study:
- To investigate the formation and thermodynamics of halothane-ammonia complexes.
- To analyze the influence of different solvents (argon, krypton, xenon) and phases on complexation.
- To evaluate computational methods for modeling solvent effects.
Main Methods:
- Infrared and Raman spectroscopy were employed.
- Experiments were conducted in liquid rare gases (Ar, Kr, Xe), supersonic jet expansions, and vapor phase mixtures.
- Complexation enthalpies were measured for 1:1 and 1:2 complexes.
Main Results:
- 1:1 and 1:2 complexes of halothane and ammonia were observed in various phases.
- Complexation enthalpies for the 1:1 complex ranged from -17.0 to -20.0 kJ/mol.
- A complexation enthalpy of -31.5 kJ/mol was determined for the 1:2 complex in liquid xenon.
Conclusions:
- Spectroscopic data provide thermodynamic insights into halothane-ammonia complexation.
- Solvent effects significantly influence the stability and properties of these complexes.
- The study offers a critical assessment of computational modeling for cryosolutions.
Related Concept Videos
02:05Entropy and Solvation
The process of surrounding a solute with solvent is called solvation. It involves evenly distributing the solute within the solvent. The rule of thumb for determining a solvent for a given compound is that like dissolves like. A good solvent has molecular characteristics similar to those of the compound to be dissolved. For example, polar solutions dissolve polar solutes, and apolar solvents dissolve apolar solutes. A polar solvent is a solvent that has a high dielectric constant (ϵ ≥ 15); an...
02:28Intermolecular Forces in Solutions
The formation of a solution is an example of a spontaneous process, a process that occurs under specified conditions without energy from some external source.
When the strengths of the intermolecular forces of attraction between solute and solvent species in a solution are no different than those present in the separated components, the solution is formed with no accompanying energy change. Such a solution is called an ideal solution. A mixture of ideal gases (or gases such as helium and argon,...
When the strengths of the intermolecular forces of attraction between solute and solvent species in a solution are no different than those present in the separated components, the solution is formed with no accompanying energy change. Such a solution is called an ideal solution. A mixture of ideal gases (or gases such as helium and argon,...
02:34Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility
Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, and solubilities (miscibilities) of substances. Molar mass, molecular shape, and polarity affect the strength of different intermolecular forces, which influence the magnitude of physical properties across a family of molecules.
Temporary attractive forces like dispersion are present in all molecules, whether they are polar or nonpolar. They...
Temporary attractive forces like dispersion are present in all molecules, whether they are polar or nonpolar. They...
03:00Solubility
Solution, Solubility, and Solubility Equilibrium
A solution is a homogeneous mixture composed of a solvent, the major component, and a solute, the minor component. The physical state of a solution—solid, liquid, or gas—is typically the same as that of the solvent. Solute concentrations are often described with qualitative terms such as dilute (of relatively low concentration) and concentrated (of relatively high concentration).
In a solution, the solute particles (molecules, atoms, and/or ions)...
A solution is a homogeneous mixture composed of a solvent, the major component, and a solute, the minor component. The physical state of a solution—solid, liquid, or gas—is typically the same as that of the solvent. Solute concentrations are often described with qualitative terms such as dilute (of relatively low concentration) and concentrated (of relatively high concentration).
In a solution, the solute particles (molecules, atoms, and/or ions)...
02:12Solvating Effects
An understanding of the solvating effect helps rationalize the relation between solvation and acidity of the compound. In addition, this also explains the relative stability of conjugate bases for compounds with different pKa values. This lesson details, in-depth, the principle of solvating effects. The strength of an acid and the stability of its corresponding conjugate base are determined using pKa values. This observed relationship is a consequence of solvation, which is the interaction...
01:29Liquid–Solid Solutions
The process of a solid dissolving in a liquid to form a solution is governed by the solubility limit, which is the maximum amount of the solid substance, or solute, that can be dissolved in a specific volume of the liquid or solvent. As the solute dissolves, it reaches a point where no more solute can be dissolved at a given temperature - this is known as the saturation point. However, if further solute is added and it manages to dissolve, the solution becomes supersaturated. Supersaturated...