How do you explain why ionic compounds are generally soluble in water without using the term "polar solvents"?
http://dl.clackamas.edu/ch105-03/mixing2.htm
To understand why ionic compounds are generally soluble in water, we need to consider the nature of ionic bonding and the properties of water molecules.
Ionic compounds consist of positive and negative ions held together by strong electrostatic attractions. When these compounds dissolve in water, the water molecules surround the individual ions and separate them from each other. This process is known as hydration or ion-dipole interaction.
Water molecules are polar, meaning they have a slightly positive charge on one end (hydrogen) and a slightly negative charge on the other end (oxygen). This polarity arises due to the unequal sharing of electrons within the water molecule.
The positive end of the water molecule is attracted to negatively charged ions (anions), while the negative end is attracted to positively charged ions (cations). This attraction between water molecules and ions helps to break the ionic bonds holding the compound together, allowing the ions to disperse throughout the water.
The reason we cannot use the term "polar solvents" is because it implicitly refers to water, which is a polar solvent. Therefore, it is difficult to describe the solubility of ionic compounds without acknowledging the importance of polarity in the solvent.
In summary, the solubility of ionic compounds in water is due to the ability of water molecules to surround and separate the individual ions from the ionic lattice, facilitated by the polarity of water molecules.