**Correct Option: B. Water molecules are polar, allowing them to interact with and stabilize the ions in solution.** ### Detailed Explanation: 1. **Understanding Ionic Compounds:** - Ionic compounds are formed from the electrostatic attraction between positively charged ions (cations) and negatively charged ions (anions). Common examples include sodium chloride (NaCl) and magnesium oxide (MgO). - These compounds typically have high melting and boiling points due to the strong ionic bonds that hold the ions together in a lattice structure. 2. **Polarity of Water:** - Water (H₂O) is a polar molecule, meaning it has a partial positive charge on one side (the hydrogen atoms) and a partial negative charge on the other side (the oxygen atom). This polarity is crucial for its ability to dissolve ionic compounds. - The polar nature of water allows it to interact effectively with charged particles (ions). 3. **Dissolution Process:** - When an ionic compound is added to water, the polar water molecules surround the individual ions. The positive end of the water molecules (hydrogens) is attracted to the negatively charged ions, while the negative end (oxygen) is attracted to the positively charged ions. - This interaction helps to pull the ions away from the ionic lattice, effectively breaking the ionic bonds and allowing the ions to disperse throughout the solution. This process is known as solvation or hydration. 4. **Stabilization of Ions:** - Once the ions are separated, the water molecules continue to surround and stabilize them. This stabilization is essential because it prevents the ions from recombining and allows them to remain in solution. ### Why Other Options Are Incorrect: - **Option A: Ionic compounds have low melting points, making them dissolve easily in water.** - This statement is misleading. In fact, ionic compounds generally have **high** melting points due to the strong ionic bonds. The melting point does not directly correlate with solubility in water. Solubility is more about the interaction between water and the ions rather than the melting point of the compound. - **Option C: Ionic compounds are typically gases, which disperse in water.** - This statement is incorrect. Most ionic compounds are solid at room temperature and do not exist as gases. Gaseous ionic compounds are rare and do not represent the typical behavior of ionic compounds in solution. - **Option D: The covalent bonds in ionic compounds break easily in water, leading to solubility.** - This statement is fundamentally flawed. Ionic compounds do not contain covalent bonds; they are held together by ionic bonds. The dissolution process involves the breaking of ionic bonds, not covalent bonds. Therefore, this option misrepresents the nature of ionic compounds. ### Summary of Key Points: - Ionic compounds are soluble in water primarily due to the polar nature of water, which allows it to interact with and stabilize ions. - The process of dissolution involves water molecules surrounding and separating the ions from the ionic lattice. - Ionic compounds typically have high melting points and are solid at room temperature, which does not affect their solubility in water. - Understanding the nature of ionic bonds and the properties of water is crucial for grasping why ionic compounds dissolve in aqueous solutions.