Pick an appropriate solvent from table 14.3 to dissolve each...

Name: Problem 30, Chapter 14: Chemistry A Molecular Approach
Uploaded: 2019-06-18T18:41:46-08:00
Duration: 4 min 17 s
Channel: Qiao Ruan
Description: Pick an appropriate solvent from table 14.3 to dissolve each substance. State the kind of intermolecular forces that would occur between the solute and solvent in each case. a. isopropyl alcohol (polar, contains an OH group) b. sodium chloride (ionic) c. vegetable oil (nonpolar) d. sodium nitrate (ionic)

Pick an appropriate solvent from table 14.3 to dissolve each substance. State the kind of intermolecular forces that would occur between the solute and solvent in each case. a. isopropyl alcohol (polar, contains an OH group) b. sodium chloride (ionic) c. vegetable oil (nonpolar) d. sodium nitrate (ionic)

Pick an appropriate solvent from table 14.3 to dissolve each substance. State the kind of intermolecular forces that would occur between the solute and solvent in each case.
a. isopropyl alcohol (polar, contains an OH group)
b. sodium chloride (ionic)
c. vegetable oil (nonpolar)
d. sodium nitrate (ionic)

Key Concepts

Like Dissolves Like Principle

This principle states that solutes tend to dissolve best in solvents that share a similar polarity. Polar substances and ionic compounds are more soluble in polar solvents because the intermolecular attractions, such as dipole-dipole or ion-dipole interactions, effectively overcome the lattice energy of a solid or the attractions between individual molecules. Conversely, nonpolar substances require nonpolar solvents where dispersion forces dominate, enhancing solubility through similar types of intermolecular interactions.

Intermolecular Forces

Intermolecular forces are the forces of attraction between molecules or ions that influence solubility and other physical properties. These include hydrogen bonding, dipole-dipole interactions, ion-dipole interactions, and dispersion (London) forces. The type and strength of these forces determine how well a solute can interact with and be stabilized by a solvent, playing a central role in the dissolution process.

Hydrogen Bonding

Hydrogen bonding is a specific strong form of dipole-dipole interaction that occurs when a hydrogen atom covalently bonded to a highly electronegative atom, such as oxygen, nitrogen, or fluorine, interacts with another electronegative atom. This interaction is crucial for the solubility of substances containing hydroxyl groups, as it allows for the formation of strong intermolecular attractions with polar solvents that are capable of hydrogen bonding.

Ion-Dipole Interactions

Ion-dipole interactions occur between ionic species and polar molecules. They are particularly significant when dissolving ionic compounds in polar solvents because the polar molecules can surround and stabilize the individual ions. This stabilization occurs due to the alignment of the solvent dipoles to the ions, which reduces the energy associated with the ionic lattice and promotes solvation.

Dispersion Forces

Dispersion forces, also known as London forces, are weak intermolecular forces resulting from temporary fluctuations in electron density in all molecules and atoms. They are the primary type of intermolecular attraction in nonpolar substances and nonpolar solvents. Although individually weak, these forces can cumulatively contribute significantly to the solubility of nonpolar substances in nonpolar environments.

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