Which property is characteristic of all ionic compounds?

Ionic compounds are characterized by their high melting and boiling points due to the strong electrostatic forces of attraction between the oppositely charged ions in their lattice structure. These strong ionic bonds require a significant amount of energy to break, which is why ionic compounds tend to exist as solids at room temperature and require elevated temperatures to melt or boil.

The nature of ionic bonds leads to a stable arrangement of ions that maintains structural integrity even in solid form. This property is an essential aspect of ionic compounds, distinguishing them from other types of compounds, such as covalent or metallic compounds, which may have different melting and boiling point ranges.

Ionic compounds do not generally exhibit high electrical conductivity when solid because the ions are not free to move; electrical conductivity is only observed when they are in a molten state or dissolved in a solvent such as water, where the ions can move freely. Additionally, ionic compounds usually have high solubility in water due to the ability of water molecules to separate the ions from each other, forming an aqueous solution. Lastly, while some ionic substances can exist as gases under specific conditions, this is not a common characteristic, as many form solids under standard conditions.