Which of the following describes molecular properties?

• A. Lower melting points, can be solid, liquid or gas, softer, doesn't conduct electricity.
• B. High melting points and conductivity.
• C. Always solids with strong odor.
• D. Solubility in water is always high.

Answer: (A)

Molecular properties come from discrete molecules held together by relatively weak intermolecular forces such as London dispersion, dipole-dipole interactions, and hydrogen bonding. Because these forces are weaker than the bonds in ionic or metallic substances, molecular compounds tend to have low melting and boiling points and can exist as solids, liquids, or gases. They’re usually softer and do not conduct electricity since their electrons are mostly localized within molecules and there are no free ions to carry a current. This matches the description that emphasizes lower melting points, the ability to be solid, liquid, or gas, softness, and non-conductivity. In contrast, high melting points with conductivity point to ionic or metallic types, and statements like “always solids” or “solubility in water always high” aren’t generally true for molecular substances.