Formation of Magnesium Oxide

Magnesium oxide (MgO) is formed by the transfer of electrons between magnesium (Mg) and oxygen (O). This process occurs due to the difference in electronegativity between the two elements.

Cation and Anion

In the formation of magnesium oxide, magnesium loses two electrons to oxygen, resulting in the formation of a magnesium cation (Mg2+) and an oxygen anion (O2-). The magnesium cation has a positive charge due to the loss of electrons, while the oxygen anion has a negative charge due to the gain of electrons.

Properties of Ionic Compounds

Ionic compounds, such as magnesium oxide, have several distinct properties due to their unique structure and bonding. Three key properties of ionic compounds are:

1. High melting and boiling points: Ionic compounds have strong electrostatic forces of attraction between cations and anions, which require a significant amount of energy to overcome and change the state of the compound from solid to liquid or gas. As a result, ionic compounds generally have high melting and boiling points.

2. Brittle and rigid: Ionic compounds have a crystal lattice structure, where positive and negative ions are arranged in a repeating pattern. When a force is applied to an ionic compound, the like-charged ions come into close proximity, leading to repulsion and causing the crystal lattice to shatter. This results in the brittleness and rigidity of ionic compounds.

3. Conductivity of electricity in molten or aqueous state: In the solid state, the ions in an ionic compound are held in fixed positions and cannot move. Therefore, ionic compounds are poor conductors of electricity. However, when an ionic compound is melted or dissolved in water, the ions become free to move and carry electric charge. As a result, molten or aqueous solutions of ionic compounds can conduct electricity.

In summary, the formation of magnesium oxide involves the transfer of electrons between magnesium and oxygen, resulting in the formation of a magnesium cation and an oxygen anion. Ionic compounds, including magnesium oxide, have high melting and boiling points, brittleness, and conductivity of electricity in the molten or aqueous state. These properties are a result of the strong electrostatic forces of attraction between oppositely charged ions and the rigid crystal lattice structure of ionic compounds.