In the context of phase changes in water, which type of interaction must be disrupted for water to transition from solid (ice) to liquid and then to gas?

• A. Ionic bonds between H+ and OH- ions
• B. Metallic bonds within the crystal lattice
• C. Hydrogen bonds between water molecules
• D. Covalent bonds within H2O molecules

Answer: (C)

Verified step by step guidance

1. Identify the types of bonds and interactions present in water and its phases: covalent bonds within H2O molecules, hydrogen bonds between water molecules, ionic bonds, and metallic bonds.
2. Understand that covalent bonds hold the atoms within a single water molecule together (H and O atoms), and these bonds do not break during phase changes like melting or vaporization.
3. Recognize that ionic bonds and metallic bonds are not relevant to pure water because water is a molecular compound, not an ionic or metallic solid.
4. Focus on hydrogen bonds, which are intermolecular forces between water molecules that create the solid structure of ice and the liquid state.
5. Conclude that to transition from solid (ice) to liquid and then to gas, the hydrogen bonds between water molecules must be disrupted, allowing molecules to move more freely.