# Why is the melting point of PCl3 less than that of PCl5?

From just the IB chemistry bonding chapter information, you would normally deduce that $\ce{PCl3}$ and $\ce{PCl5}$ are both covalent molecules.

However, as $\ce{PCl3}$ has a dipole moment, it has dipole-dipole intermolecular attractions, implying that $\ce{PCl3}$ has a higher melting point than $\ce{PCl5}$, which only has London dispersion forces.

So why is it that $\ce{PCl5}$ has a higher melting point than $\ce{PCl3}$ (I saw online that $\ce{PCl5}$ is an ionic solid)?

• We prefer to not use MathJax in the title field due to issues it gives rise to; see here for details. Dec 11 '17 at 10:08
• Maybe it is related to energy needed to break the bonds in case of both PCl3 and PCl5. See: chemistry.stackexchange.com/questions/40702/… Dec 11 '17 at 11:34
• What is "IB"? International Baccalaureate? Dec 11 '17 at 18:23
• Yes @PeterMortensen. Dec 12 '17 at 15:21

## 1 Answer

Because $\ce{PCl5}$ does something which is not immediately obvious from its molecular formula: it autoionizes and becomes an ionic solid $\ce{PCl4+PCl6-}$. As such, it has much stronger interactions than $\ce{PCl3}$ with its mere dipole-dipole attractions, hence the higher melting point.

If not for that fact, you deduction should have worked just fine.

• Is there any mathematical way or just method to deduce that $\ce {PCl5}$ is an ionic solid? Or is that from observation. Dec 12 '17 at 15:23
• No, I don't think this can be deduced via logic alone. As for more mathematical way, in chemistry this usually implies that you are going to end up in a nocturnal abyss of quantum chemistry, which is not what you want, believe me. Dec 12 '17 at 15:33