Some substances dissolve, while others do not. The easiest way to determine whether some thing will dissolve is to add it to a solvent and watch what happens. To predict whether two substances will dissolve, you must first predict attractions by determining whether the particles contain electrical charges. This process begins with investigating the types of chemical bonds. In previous chapter you learned that there are several fundamental types of bonds, including ionic, polar covalent, and non-polar covalent. We will examine these to see how each affects solubility.

Electronegativities of the elements
- Electronegativities of the elements determines the type of chemical bond they will form, and it indicates the magnitude of charge on the particles in a compound.

        Two elements will form an ionic bond when the difference in the electro-negativities is 2.1 or more. Some charges are 1+ and 1-, but some are stronger, such as 2+ and 3+ charges. All these ions have strong attractions for other charged ion and molecules with partial charges, and this attraction will determine how they dissolves.

        Tow atoms will form a non-polar covalent bond when the difference in the electro-negativities is in the range of 1 through 0.4. Non-polar covalent bonds carry no electrical charge and will dissolve in each other.

        Two atoms will form a polar covalent bond when the difference in the electro-negativities is in the range of 4.0 through 2.1. They are not as strong as the full negative and positive charges, such as other polar molecules and ions. Thus, you would expect molecules held together by polar covalent bonds to dissolve ionic compounds and each other.

  What is a solution?

  What does concentration mean?

  How are solubility principles used?