Structures and Bonding: Properties of Ionic Compounds

Ionic compounds are formed when a metal and a non-metal react. The metal atom donates an electron to the non-metal atom. This forms positive and negative ions, which are held together by strong electrostatic forces, known as ionic bonds.
These compounds are usually solid at room temperature because their ionic bonds are very strong, requiring high temperature to break.
Ionic compounds form 3D (three-dimensional) lattice structures. This means that each ion is surrounded by ions of the opposite charge, ensuring maximum stability.
A significant property of ionic compounds is their ability to conduct electricity when melted or dissolved in water. This is because their ions are free to move, forming an electric current.
When an ionic compound dissolves in water, the water molecules tear the ions apart from the lattice, making them free and able to carry an electric current.
Ionic compounds have high melting and boiling points due to their strong ionic bonds. It takes a large amount of energy to overcome these bonds.
These compounds are generally soluble in water but insoluble in organic solvents like ethanol.
In a solid state, ionic compounds do not conduct electricity because the ions are not free to move.
They are hard and brittle in nature. When force is applied, the layers of ions can shift, and similar ions could align. As like charges repel, the lattice can break.

Remember that understanding the properties of ionic compounds helps to predict their behaviour in different environments and interactions. Always aim to link properties back to the structure and type of bonding involved.