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Aside from its esoteric name, rubidium fluoride (RbF) is an interesting compound. Its hygroscopicity makes it an excellent choice for use as a brake fluid. The high dry boiling point and the surprisingly good wet boiling point make it an ideal lubricant for hotter temperatures.
Melting points of ionic compounds are often higher than those of covalent ones, thanks to the intermolecular forces of attraction between the ions. These are electrostatic forces that are much stronger than molecular-molecular or polar interactions.
The best way to understand the high melting points of ionic compounds is by comparing their lattice energy (a measure of how well the ions pack into a crystal). If the ions are tightly packed together, their lattice energy will be high.
RbF, like many ionic compounds, has a high lattice energy. In fact, the aa value of the best crystallization of this substance is an impressive 1.7 x 10-31. This is more than double the aa value of the most expensive glass (0.5 x 10-31).
Its high enthalpy makes it a top candidate for the title of “boiling point of the year.” As with any ionic compound, the lattice energy is the best indicator of how well the molecules are packing into the crystal. The other main reason it has a high lattice energy is that it is a hydride, which is a very complex chemical formula with many electrons involved. This makes it very difficult to crystallize into a solid.