# Freezing point vs Intermolecular forces

Water has a higher boiling point (100°C) than cyclohexane (81°C). This is probably because of stronger intermolecular forces between water molecules as compared to cyclohexane molecules. Then, why is the freezing point of cyclohexane higher than that of water? By the previous logic, water should be having a higher freezing point as well.

This is one among many examples. I am pretty sure than boiling point depends primarily on intermolecular forces while freezing point depends on both intermolecular forces and packing efficiency in the solid state. I am sure that both factors support a higher freezing point for water. So, what other factors govern the freezing point of a liquid substance?

• Note that water is a bad substance to compare to, since it is an exception in so many cases due to its hydrogen bond network. Examples are boiling and melting points compared to $\ce{H2S}$, $\ce{H2Se}$, density anomaly at 4 °C and many others. Jun 20 '19 at 17:56
• Freezing is tricky, it can't be justified as easily as boiling. Jun 20 '19 at 18:05