Ionic Compounds

This lesson covers:

1. The structure of ionic compounds
2. The properties of ionic compounds
3. How to work out the formula of an ionic compound

positive / negative / electrostatic / ionic / covalent

Metals normally form ions which have a charge, while non-metals form ions with a charge.

Ions are attracted to other ions with the opposite charge, due to forces. 

Ionic structures involve many ions bonded together via bonds. 

The solid arranges itself into a regular 3D structure known as a la.

strong / weak / high / low / energy / water

Ionic compounds have relatively melting and boiling points. 

This is because ionic bonds are very , and a high amount of is required to break the bonds. 

Remember that ionic compounds arrange their ions in a way that creates a neutral overall charge. 

For example, magnesium ions have a 2+ charge, while chloride ions have a 1- charge.

Therefore, for every magnesium ion, two chloride ions will be attracted to it, resulting in an overall neutral charge. 

Potassium ions and carbonate ions can form an ionic compound.

Potassium ions have a + charge, while carbonate ions have a - charge. 

This means every carbonate ion will ionically bond with potassium ions.

Make sure you learn the formulae for the following ions:

1. Hydroxide:  OH^-
2. Sulphate:  SO₄^2-
3. Nitrate:  NO₃^-
4. Carbonate:  CO₃^2-
5. Ammonium:  NH₄⁺