The statement is False.
Covalent compounds generally have lower boiling points compared to ionic compounds. This difference primarily stems from the nature of the forces that hold the particles together.
Ionic compounds consist of positively and negatively charged ions that are held together by strong electrostatic forces known as ionic bonds. These forces require a significant amount of energy to break during the phase change from solid to liquid or liquid to gas, resulting in higher boiling points for ionic compounds.
On the other hand, covalent compounds consist of atoms that share electrons, forming covalent bonds. The intermolecular forces that exist between covalent compounds—such as van der Waals forces and hydrogen bonds—are typically weaker than ionic bonds. As a result, covalent compounds tend to have lower boiling points, as less energy is needed to separate the molecules during boiling.
In summary, while there may be exceptions, in general, ionic compounds exhibit higher boiling points than covalent compounds due to the stronger attractive forces holding the ions together.