Which statement best explains water's ability to dissolve covalent compounds?

• A. Water can ionize covalent compounds completely.
• B. Water's nonpolar nature allows it to dissolve covalent compounds.
• C. Water can form hydrogen bonds with polar covalent compounds.
• D. Water's high density allows it to dissolve covalent compounds.

Answer: (C)

Verified step by step guidance

1. Identify the nature of water: Water is a polar molecule, meaning it has a partial positive charge on one side and a partial negative charge on the other side due to its bent shape and the electronegativity difference between hydrogen and oxygen.
2. Understand the nature of covalent compounds: Covalent compounds can be polar or nonpolar. Polar covalent compounds have an uneven distribution of electron density, leading to partial charges within the molecule.
3. Recognize the interaction between water and polar covalent compounds: Water can interact with polar covalent compounds through hydrogen bonding. This occurs when the partially positive hydrogen atoms in water are attracted to the partially negative atoms in the polar covalent compound.
4. Evaluate the incorrect statements: Water does not ionize covalent compounds completely, as ionization typically refers to the formation of ions, which is more characteristic of ionic compounds. Water is not nonpolar, and its density is not the primary reason for dissolving covalent compounds.
5. Conclude with the correct explanation: The ability of water to dissolve polar covalent compounds is primarily due to its capacity to form hydrogen bonds with them, facilitating the dissolution process.