Final answer:
2-methylheptane is expected to have a higher melting point and boiling point than 2-methylhexane due to its larger molecular size and greater surface area which lead to stronger London dispersion forces.
Step-by-step explanation:
When comparing the melting point and boiling point of 2-methylhexane and 2-methylheptane, we must consider the molecular size and structural factors that affect intermolecular forces. Since both compounds are alkanes and nonpolar, the London dispersion forces are the primary intermolecular forces at play. These forces tend to increase with greater molecular mass and surface area. Therefore, we would expect 2-methylheptane to have a higher melting point and boiling point than 2-methylhexane due to its longer carbon chain, resulting in a larger surface area which can interact more extensively with surrounding molecules.
By analogy to the given reference where propane has a lower boiling point than n-pentane, and n-butane has a higher boiling point than 2-methylpropane due to its more extended shape and larger surface area, we can infer that 2-methylheptane will follow the same trend relative to 2-methylhexane.