Final answer:
The correct answer is A) Ionic solids have higher melting points than simple molecular solids. Ionic compounds have high melting points due to their strong ionic bonds, while molecular compounds have lower melting points because of the weaker intermolecular forces present.
Step-by-step explanation:
When comparing the melting points of an ionic solid and a simple molecular solid, it is important to understand the types of bonds involved. The melting point of a solid is largely dependent on the strength of the bonds. Ionic compounds, like sodium chloride, have very high melting points because they consist of strong ionic bonds between ions. For example, sodium chloride has a melting point of about 801°C. In contrast, simple molecular solids, such as ice, have much lower melting points. Ice, which is composed of water molecules held together by hydrogen bonds, melts at 0°C, demonstrating the weaker intermolecular forces present in molecular compounds.
Moreover, regarding electrical conductivity, ionic compounds do not conduct electricity when solid because their ions are immobile. However, they conduct electricity in melted or dissolved states due to the movement of ions. Molecular compounds generally do not conduct electricity as they are made of neutral molecules with no free charge carriers. Lastly, regarding solubility, many ionic compounds are soluble in water, while the solubility of molecular compounds varies and depends on their polarity and the types of intermolecular forces involved.