The correct choice highlights an important concept in chemistry regarding the influence of molecular structure on melting points. Linear molecules generally have higher melting points than branched ones due to their ability to stack more closely and efficiently in a solid state. This efficient packing maximizes interactions between molecules, often leading to stronger intermolecular forces.
In linear chains, the surface area available for intermolecular interactions is greater compared to branched molecules, allowing for stronger Van der Waals forces. The increased interaction leads to more energy being required to disrupt these forces, resulting in higher melting points for linear isomers.
Understanding this concept is crucial because it also influences the boiling points based on the same principles of molecular interactions and structures. Linear molecules often transition to a gaseous state at higher temperatures due to these stronger attractions in the solid phase.
In contradistinction, other options do not properly reflect the established trends related to molecular structure and melting and boiling points. For example, while molecular weight can play a role, it does not always correlate to lower melting points as indicated, and the impact of polarity is nuanced and varies based on other factors. Thus, recognizing the implications of molecular shape and structure is essential for predicting physical properties effectively.