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Theory:

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.
 
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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.
 
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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.
 
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Steel melting  
  
Solubility:
 
Water and other polar solvents make ionic compounds soluble. Ionic compounds are insoluble in benzene and non-polar solvents.
 
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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.
 
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Various nature of metal  
 
Reactions:
 
Ionic compounds go through ionic reactions that are almost immediate and fast.