Computing excess functions of ionic solutions: the smaller-ion shell model versus the primitive model. 2. Ion-size
1Eltron Research & Development Inc., 4600 Nautilus Court South, Boulder, Colorado 80301-3241, United States.
Journal of Chemical Theory and Computation
|November 18, 2015
Summary
This study compares two models for ionic solutions. The Smaller-ion Shell (SiS) model provides more reliable ion-size parameters than the primitive model (PM), aligning better with experimental data.
Area of Science:
- Physical Chemistry
- Computational Chemistry
- Ionic Solutions
Background:
- A recent Monte Carlo simulation study of the primitive model (PM) proposed "recommended ionic radii" for ions in aqueous solutions.
- The PM model yielded larger radii for smaller cations, suggesting hydration, which contrasted with crystallographic radii.
Purpose of the Study:
- To compare the ion-size parameters (ISPs) derived from the unrestricted primitive model (MC-UPM) and the Smaller-ion Shell (SiS) treatment.
- To evaluate the reliability of ISPs from both models as physicochemical entities.
Main Methods:
- Comparison of model-experiment fits for mean ionic activity coefficients as a function of ionic concentration.
- Analysis of ion-size parameters (ISPs) obtained from "best fit" procedures in both MC-UPM and DH-SiS models.
Main Results:
- ISPs derived from the DH-SiS treatment closely match crystallographic or thermochemical ionic diameters for both cations and anions.
- DH-SiS derived ISPs are independent of the counterion, unlike those from the PM model.
- The PM model's "recommended ionic radii" were significantly larger than crystallographic values for smaller cations.
Conclusions:
- The DH-SiS treatment offers more reliable ion-size parameters compared to the PM model.
- DH-SiS derived ISPs are more consistent with established physical dimensions of ions.
Related Concept Videos
Ionic Radii
34.8K
Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it is smaller than the atom from which it is derived. For example, the covalent radius of an aluminum atom (1s22s22p63s23p1) is 118 pm, whereas the ionic radius of an Al3+ (1s22s22p6) is 68 pm. As electrons are removed from the outer valence shell, the remaining core electrons occupying smaller shells experience a greater effective nuclear...
34.8K
Electrolytes: van't Hoff Factor
37.7K
Colligative Properties of Electrolytes
The colligative properties of a solution depend only on the number, not on the identity, of solute species dissolved. The concentration terms in the equations for various colligative properties (freezing point depression, boiling point elevation, osmotic pressure) pertain to all solute species present in the solution. Nonelectrolytes dissolve physically without dissociation or any other accompanying process. Each molecule that dissolves yields one...
The colligative properties of a solution depend only on the number, not on the identity, of solute species dissolved. The concentration terms in the equations for various colligative properties (freezing point depression, boiling point elevation, osmotic pressure) pertain to all solute species present in the solution. Nonelectrolytes dissolve physically without dissociation or any other accompanying process. Each molecule that dissolves yields one...
37.7K
Ionic Crystal Structures
20.7K
Ionic crystals consist of two or more different kinds of ions that usually have different sizes. The packing of these ions into a crystal structure is more complex than the packing of metal atoms that are the same size.
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
Most monatomic ions behave as charged spheres, and their attraction for ions of opposite charge is the same in every direction. Consequently, stable structures for ionic compounds result (1) when ions of one charge are surrounded by as many ions as possible of the opposite...
20.7K
The Debye–Hückel Theory of Electrolyte Solutions
221
The Debye–Hückel theory, established by Peter Debye and Erich Hückel in 1923, is a fundamental concept in physical chemistry. It provides an understanding of the behavior of strong electrolytes in solution, particularly explaining their deviations from ideal behavior.The theory is based on Coulombic interactions (the attraction or repulsion between charged particles) between ions in solution. In an ionic solution, oppositely charged ions tend to attract each other. This means...
221
Factors Affecting Activity Coefficient
1.8K
The extended Debye-Hückel equation indicates that the activity coefficient of an ion in an aqueous solution at 25°C depends on three partially interdependent properties: the ionic strength of the solution, the charge of the ion, and the ion size.
The activity coefficient value for an ion is close to one when the solution has almost zero ionic strength, i.e., when the solution shows close to ideal behavior. As the ionic strength of the solution increases from 0 to 0.1 mol/L, a...
The activity coefficient value for an ion is close to one when the solution has almost zero ionic strength, i.e., when the solution shows close to ideal behavior. As the ionic strength of the solution increases from 0 to 0.1 mol/L, a...
1.8K
Ionic Strength: Overview
3.5K
The ionic strength of a solution is a quantitative way of expressing the total electrolyte concentration of a solution. This concept was first introduced in 1921 by two American physical chemists, Gilbert N. Lewis and Merle Randall, while describing the activity coefficient of strong electrolytes. During the calculation of ionic strength (I or μ), all the cations and anions are considered. However, the concentration (c) of an ion with a greater charge number (z) has a greater contribution...
3.5K


