Does electronegativity affect solubility

Answer 1

I am looking for the answer to this question too. It seems to me that the two must be closely related. I am of the opinion (unsubstantiated at this point) that when the electronegativity difference between bonding atoms is in the 0.5-1.7 range it would make sense for the substance to be insoluble, as the forces holding the molecule together are then stronger than the hydrogen bonds of water. However, this is difficult to show as I cannot find electronegativities for polyatomic ions, and most insoluble salts contain them. If, however the atoms are held together by ionic bonds (electronegativities greater than 0.7), the ions dissociate easily in water.

Answer 2

Ionic bonding is characterized by the complete transfer of electrons from one atom to another, yielding two charged particles known as ions, which are held together with electrostatic force, they readily dissolve in water and in other polar solvents

Answer 3

Electronegativity can affect solubility by influencing the polarity of a molecule. Generally, more polar compounds (higher electronegativity difference between atoms) are more soluble in polar solvents, while nonpolar compounds are more soluble in nonpolar solvents. However, other factors, such as molecular size and shape, also play important roles in determining solubility.

Answer 4

Solubility depends on the solvent's ability to overcome the intermolecular forces in a solid.

Answer 5

solute is the substance that is being dissolved during solubility

Answer 6

The greater the intermolecular forces, the greater the solubility.