summarize the solubilty behavior of hydrocarbons in water (a polar solvent) and in non polar organic solvents

Non-polar hydrocarbons dissolve in non-polar solvents.

The solubility behavior of hydrocarbons can be understood by examining their polarity. Hydrocarbons are nonpolar molecules, composed solely of carbon and hydrogen atoms. As a result, they tend to be insoluble in polar solvents like water but are soluble in nonpolar organic solvents.

To explain this behavior, it is essential to understand the concept of "like dissolves like." In simple terms, substances with similar polarity dissolve well in each other. Polar solvents, such as water, have molecules with a positive and negative end, making them capable of forming hydrogen bonds with other polar substances.

Water molecules are not attracted to nonpolar hydrocarbon molecules, as their positive and negative ends are not present. Since hydrocarbons lack a charge or significant polarity, they do not interact favorably with water molecules. Consequently, hydrocarbons are generally insoluble in water.

In contrast, nonpolar organic solvents, such as hexane or benzene, share a similar lack of polarity with hydrocarbons. These solvents have molecules consisting of mainly carbon and hydrogen atoms, without any significant charge separation. Due to this similarity in polarity, hydrocarbons mix well with nonpolar organic solvents. The nonpolar nature of both the hydrocarbon and the solvent allows them to disperse and mix easily, resulting in solubility.

In summary, hydrocarbons are generally insoluble in polar solvents like water (which prefer polar substances), but they are soluble in nonpolar organic solvents (which have similar polarity to hydrocarbons).