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Ionic compounds are made up of ionic bonds. An ionic bond is formed when there is a significant difference in electronegativity between the elements that are involved in the bonding process. The greater the difference between the positive ion (cation) and the negative ion (anion), the stronger the attraction between the two ions.
Characteristics of Ionic Compounds
Ionic compounds are formed when atoms form ionic bonds and connect to one another.
It is the strongest type of chemical bond, and it is responsible for the formation of characteristic properties.
When two atoms are joined together, one of them has a partial positive charge, and the other one has a partial negative charge. Because of the difference in electronegativity, the bond becomes polar, which is why some compounds are polar.
Polar compounds, on the other hand, frequently dissolve in water. As a result, ionic compounds make excellent electrolytes.
The strength of the ionic bond causes ionic compounds to have high melting and boiling points as well as high enthalpies of fusion and decomposition when compared to other compounds.
Ionic Compounds have a number of characteristics in common
When positive and negative ions attract each other in an ionic bond, the properties of ionic compounds are determined by how strongly the ions attract each other. Aside from these characteristics, ionic compounds have the following characteristics:
They combine to form crystals
Ionic compounds, as opposed to amorphous solids, crystallise into lattice structures. Despite the fact that molecular compounds can crystallise, they frequently do so in other forms, and molecular crystals are typically softer than ionic crystals in their structure. Ionic crystals are regular structures at the atomic level, with the cation and anion alternating with each other and forming a three-dimensional structure based largely on the smaller ion filling in the gaps between the larger ions in an even and consistent manner.
These substances have extremely high melting and boiling points
It is necessary to heat ionic compounds to high temperatures in order to overcome the attraction between the positive and negative ions. As a result, a significant amount of energy is required to melt or bring ionic compounds to a boil.
They have higher fusion and vaporisation enthalpies than molecular compounds, which makes them more reactive.
In the same way that ionic compounds have high melting and boiling points, they typically have high enthalpies of fusion and vaporisation, which can be 10 to 100 times higher than those of most molecular compounds in most cases. The enthalpy of fusion is defined as the amount of heat required to melt a single mole of a solid when under continuous pressure. The enthalpy of vaporisation is defined as the amount of heat required to vaporise one mole of a liquid compound under constant temperature and pressure.
They have a hard and brittle texture.
It is difficult to separate positive and negative ions from each other in ionic crystals because they are strongly attracted to each other. When pressure is applied to an ionic crystal, ions with similar charges may be forced closer to each other. The electrostatic repulsion between atoms and molecules can be sufficient to split a crystal, which is why ionic solids are also brittle.
When they are dissolved in water, they become conductors of electricity.
Dissociated ions, which occur when ionic compounds are dissolved in water, are free to conduct electric charge through the solution. It is also possible for molten ionic compounds (molten salts) to conduct electricity.
They are excellent insulators
Ionic solids do not conduct electricity well, despite the fact that they conduct well in molten form or in aqueous solution. This is due to the fact that the ions are tightly bound to one another.
An Example of a Typical Household
Table salt, also known as sodium chloride, is a common example of an ionic compound. Salt has a melting point of 800oC, which is extremely high. Salinity solutions (salt dissolved in water) conduct electricity much more readily than a salt crystal, which acts as an electrical insulator. Molten salt has the additional property of being a conductor. If you look closely at salt crystals under a microscope, you can see the regular cubic structure that results from the crystal lattice. Salt crystals are hard and brittle at the same time; it is easy to break a crystal. Solid salt does not have a discernible flavour, despite the fact that it has a low vapour pressure and therefore does not emit any odour.
Sugar, on the other hand, is a covalent compound. It has a melting point that is lower than that of salt. It dissolves in water but does not dissociate into ions, resulting in a solution that does not conduct electricity when exposed to electricity. Sugar crystallises, but its sweetness can be detected due to the high vapour pressure that it has compared to other substances.
Conclusion
Ionic compounds are made up of ionic bonds. An ionic bond is formed when there is a significant difference in electronegativity between the elements that are involved in the bonding process.When two atoms are joined together, one of them has a partial positive charge, and the other one has a partial negative charge.They have higher fusion and vaporisation enthalpies than molecular compounds, which makes them more reactive.In the same way that ionic compounds have high melting and boiling points, they typically have high enthalpies of fusion and vaporisation.Ionic compounds, as opposed to amorphous solids, crystallise into lattice structures.Ionic solids do not conduct electricity well, despite the fact that they conduct well in molten form or in aqueous solution. This is due to the fact that the ions are tightly bound to one another.
