Which property of $\mathrm{hydrocarbons}$ best explains why they are insoluble in $H_{2}O$?

• A. $\mathrm{Hydrocarbons}$ are highly reactive with $H_{2}O$, forming precipitates.
• B. $\mathrm{Hydrocarbons}$ have strong hydrogen bonds with $H_{2}O$, preventing dissolution.
• C. $\mathrm{Hydrocarbons}$ are nonpolar and $H_{2}O$ is polar, so they do not mix due to differences in polarity.
• D. $\mathrm{Hydrocarbons}$ are ionic compounds and $H_{2}O$ cannot dissolve ionic substances.

Answer: (C)

Verified step by step guidance

1. Identify the polarity of hydrocarbons: Hydrocarbons consist mainly of carbon and hydrogen atoms bonded together, and these bonds are generally nonpolar due to similar electronegativities.
2. Recognize the polarity of water (H\_2O): Water is a polar molecule because of the significant difference in electronegativity between oxygen and hydrogen, and its bent molecular shape creates a dipole moment.
3. Apply the principle 'like dissolves like': Polar solvents tend to dissolve polar solutes, and nonpolar solvents tend to dissolve nonpolar solutes. Since hydrocarbons are nonpolar and water is polar, they do not mix well.
4. Understand that hydrogen bonding is a property of water molecules interacting with other polar or capable molecules, but hydrocarbons cannot form hydrogen bonds with water due to lack of suitable electronegative atoms.
5. Conclude that the main reason hydrocarbons are insoluble in water is the difference in polarity, which prevents effective intermolecular interactions necessary for dissolution.