Identifying ionic compounds using state and solubility properties

Steps:

• Review the table entries for each substance's state of matter.
• Note that ionic compounds exist as solids at room temperature, unlike molecular compounds which can be liquids.
• Check solubility: ionic compounds can be soluble or insoluble in water.
• Compare conductivity and other properties, but focus on solid state and insolubility for distinction.

Why D is correct:

• D is a solid that is insoluble, matching the definition of many ionic compounds like silver chloride (AgCl), which form crystalline lattices and have low solubility per solubility rules.

Why the others are wrong:

• A is a liquid, indicating a molecular compound with weak intermolecular forces, not ionic bonding.
• B is a solid but with x x ✓ properties suggesting solubility without typical ionic conductivity, likely covalent.
• C is a solid but x ✓ indicates partial solubility or conductivity mismatch for ionic behavior.

Not enough information on exact table columns for full confirmation. Final answer: D