Ionic solids are rigid because the multiple interactions between oppositely charged ions hold the charged particles in relatively fixed positions.
Electrical conductivity depends on ions being able to move freely. The conduction of heat depends partly on the movement of electrons in a substance. Electric charge is "locked" in the lattice positions of the ions in the solids. This means there is poor mobility of charges and poor conductivity of electricity and heat.
Ionic solids are brittle and hard because the electrostatic attractions in the solid again hold the ions in definite positions. The electrostatic attractions must be overcome to move the ions. When the ions in the solid are shifted by some very strong force the positions of ions shift so that like charged ions are close together. This results in strong repulsions and the like charged ions move apart. The solid shatters and does not simply deform like a metal. Try crushing a few grains of salt in the bowl of a spoon with another spoon. The particles do not deform, they shatter.Ionic solids melt when the ions are heated and have enough energy to slide past one another. They are mobile and can act to carry electrical charge through the liquid. This explains why a molten ionic substance conducts electricity, but a solid ionic material doesn't. The ions move through the liquid to carry charge from one place to another.The dissolving process is like a tug of war. Soluble ionic substances are ripped apart by the solvent when the solid is dissolved. The solvent pulls the ions out of the solid and breaks the forces holding the crystal together. The solvent isolates the ions in an envelope of solvent particles. The ions are free to move and carry electric charge through the solution.Nonsoluble ionic solids are held together so tightly that the ions cannot be pulled out of the lattice by the solvent. The attractive forces in the solid are stronger than the attractions between the solvent and the ions. The solvent can't pull the ions out of the crystal.Ionic compound formulaIonic compound nameMelting point in degrees celsiusSolubility grams per 100 g watersuperscript is temperatureLiCllithium chloride61345 g cold water, 128 g100NaClsodium chloride801209 g cold water, 284 g 100KClpotassium chloride77635 g cold water, 57 g 100RbClrubidium chloride71577 g cold water, 139 g100MgF2magnesium fluoride13960.0076 g cold water, insoluble 100MgCl2magnesium chloride70854 g cold water, 72 g100MgBr2magnesium bromide695-700101 g cold water, 126 g 100MgI2magnesium iodidegreater than 700100 g 0 cold water, 165 g 100
Ionic compounds are those that bring together anions and cations bonded together by ionic bonds. The electrostatic forces of the different charges are significant in the bonds that make them strong hence require high energy to break them (high melting point). Due to the regular structure of ionic compound that tend to form lattices in solid form, when struck, they shatter along the lines of weakness of the lattice.
