Intermolecular vs. Intramolecular Bonding in Carbon Allotropes Steps: - Compare structures: Graphite has layers of covalently bonded carbon atoms with weak van der Waals forces between layers; buckminsterfullerene (C60) consists of discrete spherical molecules held by weak intermolecular forces. - Assess bonding strength: Strong covalent bonds within graphite layers require high energy to break for melting; weak forces in buckminsterfullerene need less energy. - Link to melting point: Lower melting point occurs when only weak intermolecular bonds break, as in molecular solids like buckminsterfullerene. - Evaluate options: Identify which describes weak intermolecular bonding as the cause. Why A is correct: - Discrete C60 molecules are held by weak van der Waals forces (intermolecular), which break easily at low temperatures, per the definition of molecular solids having low melting points due to weak attractions between molecules. Why the others are wrong: - B: Graphite is covalent network, not ionic; mobile electrons enable conductivity but do not explain melting point difference. - C: Bond strain in buckminsterfullerene affects reactivity, not directly the intermolecular forces determining melting. - D: Graphite has delocalized electrons …