Classify each of the following statements as true or false: (a) For molecular solids, the melting point generally increases as the strengths of the covalent bonds increase. (b) For molecular solids, the melting point generally increases as the strengths of the intermolecular forces increase.

Verified step by step guidance

1. Step 1: Understand the difference between covalent bonds and intermolecular forces. Covalent bonds are the strong bonds that hold atoms together within a molecule, while intermolecular forces are weaker forces that occur between molecules.
2. Step 2: Analyze statement (a). In molecular solids, the molecules are held together by intermolecular forces, not covalent bonds. Therefore, the melting point is not directly related to the strength of covalent bonds within the molecules.
3. Step 3: Determine the truth of statement (a). Since the melting point of molecular solids is not dependent on the strength of covalent bonds, statement (a) is false.
4. Step 4: Analyze statement (b). The melting point of molecular solids is influenced by the strength of intermolecular forces. Stronger intermolecular forces require more energy to overcome, leading to a higher melting point.
5. Step 5: Determine the truth of statement (b). Since the melting point generally increases with stronger intermolecular forces, statement (b) is true.