When determining the melting point of an organic compound it's important to understand how the compound binds to itself. Melting and boiling are processes in which noncovalent interactions between molecules are disrupted. The stronger the noncovalent interaction, the more energy is requiring to break them apart (e.g., more heat).

When comparing organic molecules there are several trends to consider.

1. Size of carbon chain: For a molecule with a given functional group, the melting and boiling pair increase with molecular weight. The more carbons and hydrogen mean a greater surface area possible for van der Waals interaction, thus higher melting point and boiling point.

2. The force of attraction between the molecule: The strength of intermolecular dipole-dipole, and iconic interactions is reflected in the melting and boiling point.

Compare both molecules and determine if there is any difference in molecular size, dipole-dipole, hydrogen bonding, or iconic interaction which can explain its higher melting point.

Hint: Draw them out packed in a crystal lattice. How are they different?