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Features of ionic compounds:
The primary factor that defines the properties of compounds is bonding between the atoms of a molecule. As a result, in ionic compounds, the atoms are held together by a strong electrostatic force, giving the compounds the following characteristics:
Physical state:
A strong electrostatic force makes these compounds between cations and anions arranged in a well-defined geometrical pattern. Thus, ionic compounds are crystalline solids at an average temperature.
Salt is an example of a crystalline solid
Electrical Conductivity:
Ionic compounds are solid crystals, and so their ions are tightly bound together. As a result, the ions cannot move freely, and they do not conduct electricity in a solid-state. However, in a molten state, their aqueous solutions conduct electricity.
Electrical conductivity of the salt solution
Melting point:
The strong electrostatic interaction between the cations and anions binds the ions together, requiring a large amount of energy to separate them. So ionic compounds possess high melting and boiling points.
Steel melting  
Water and other polar solvents make ionic compounds soluble. Ionic compounds are insoluble in benzene and non-polar solvents.
Sugar soluble in tea  
Density, hardness and brittleness:
Ionic compounds include a high density, and they are pretty hard because of the strong electrostatic force between the ions. But, they are highly brittle.
Various nature of metal  
Ionic compounds go through ionic reactions that are almost immediate and fast.