Ionic Compounds

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Definition Structure Examples FAQs

What is Ionic Compound?

Ionic compounds can be defined as:

The crystalline solids formed by neatly packed ions of opposite charge. Ionic compounds are usually formed when metals react with non-metals.

In other words, ionic compounds held together by ionic bonds as classed as ionic compounds. Elements can gain or lose electrons in order to attain their nearest noble gas configuration. Formation of ions (either by gaining or losing electrons) for the completion of octet helps them gain stability.

In a reaction between metals and non-metals, metals generally loose electrons to complete their octet while non-metals gain electrons to complete their octet. Metals and non-metals generally react to form ionic compounds.

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Ionic Compound Structure

The structure of an ionic compound depends on the relative sizes of the cations and anions. Ionic compounds include salts, oxides, hydroxides, sulphides, and the majority of inorganic compounds. Ionic solids are held together by the electrostatic attraction between the positive and negative ions.

For example, the sodium ions attract chloride ions and the chloride ion attracts sodium ions. The result is a three-dimensional structure of alternate Na+ and Cl ions. This is a crystal of sodium chloride. The crystal is uncharged because the number of sodium ions is equal to the number of chloride ions. The forces of attraction between the ions hold them in the structures.

Sodium Chloride Structure

These ionic bonds between the charged particles result in a giant structure of ions. Because the ions are held together tightly in these giant structures it takes a lot of energy to break all the bonds. As a result, ionic compounds have high melting points and boiling points.

Ionic Compound Examples

For example reaction between magnesium and chlorine. The magnesium atom has two electrons in its outermost shell. By losing two electrons from its M shell its L shell becomes the outermost shell that has a stable octet. The nucleus of this magnesium atom still has twelve protons but the number of electrons has decreased to ten. So, a net positive charge is developed on this magnesium atom, giving a magnesium cation Mg2+.

On the other hand, the chlorine atom has seven electrons in its outermost shell. Therefore, it needs only one electron to complete its octet. It can gain this one electron from the electrons lost by magnesium atom to become magnesium ion. As two electrons are lost by magnesium atom while one chlorine atom can gain only one electron, two atoms of chlorine combine with one atom of magnesium to form magnesium chloride.

Ionic Compounds

From the above example, ionic compounds can be defined as the compounds formed by the transfer of electrons between metals and non-metals. The bond formed between them is known as the ionic bond. Due to the presence of oppositely charged ions, ionic compounds are held strongly by the electrostatic force of attraction. Prominent properties of ionic compounds are:

Ionic Compound Properties

1. Physical properties of ionic compounds

Due to the presence of the strong force of attraction between the positive and negative ions, ionic compounds are solids and are hard to break. They generally break into pieces when pressure is applied, hence they are considered brittle.

2. Melting and boiling points of ionic compounds

Due to the presence of electrostatic forces of attraction between ions, a large amount of energy is required to break the ionic bonds between the atoms. Thus, ionic compounds have high melting and boiling points.

3. The solubility of ionic compounds

Ionic compounds are generally soluble in polar solvents such as water whereas solubility tends to decrease in non-polar solvents such as petrol, gasoline, etc.

4. Conduction of Electricity

Ionic compounds do not conduct electricity in the solid-state but are good conductors in a molten state. Conduction of electricity involves the flow of charge from one point to another. In the solid-state, as the movement of ions is not possible, ionic compounds don’t conduct electricity. Whereas in the molten state, ionic compounds conduct electricity as electrostatic forces of attraction between the ions are overcome by the heat released.

Frequently Asked Questions

Which is an ionic compound?

Ionic compounds are ion compounds. These ions are atoms that gain or lose electrons, resulting in a net positive or negative charge. Metals tend to lose electrons, so they have a net positive charge and become cations. Non-metals tend to gain electrons, creating a net negative charge of anions.

What are the common ionic compounds?

Ionic compounds have high points of melting and boiling and appear to be strong and brittle. Ions may be single atoms, such as sodium and chlorine in common table salt (sodium chloride) or more complex groups such as calcium carbonate.

What is the ionic bond example?

The ionic bond concept is when a positively charged ion forms a bond with a negatively charged ion and one atom passes electrons to another. An example of an ionic bond is Sodium Chloride, a chemical compound.

Is MgO an ionic compound?

To have an octet, Mg loses two electrons. To have an octet, oxygen gains two electrons. The ionic bond between ions is the result of opposite charges being applied electrostatically. The final magnesium oxide formula is MgO.

What are the 2 parts of an ionic compound?

Ionic compounds are compounds made up of ions that form charged particles when an atom (or group of atoms) gains or loses electrons. A cation is an ion charged positively; an anion is an ion charged negatively.

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