There are four kinds of bonding types to be aware of. These are ionic, simple covalent molecular, giant covalent network and metallic.
The table below summarises them, identifying typical properties of each. Simple covalent molecular is listed as 'simple' and giant covalent network is listed as 'giant'.
|Metals and non-metals||Non-metals||Non-metals||Metals|
|Loss and gain of electrons by atoms||Share pairs of electrons between atoms||Share pairs of electrons between atoms||Outer electrons free to move|
|+ and - ions formed attract each other||Small groups of atoms held together||Billions of atoms are held together||Billions of positive metal ions|
|Ionic lattice structure||A molecular structure||Giant covalent lattice structure||Giant metallic lattice structure|
The different bonding models that are used to represent the bonding and structure of substances have certain features and limitations. For example, the model of the metallic lattice on the previous page does not show more than one layer of metal ions, or that the delocalised electrons are in constant motion.
Ionic compounds form a regular lattice structure in which oppositely charged ions are strongly attracted to each other. Sodium chloride is an ionic compound. The table shows some limitations of different models for sodium chloride.
The atoms in a simple molecular substance are joined together by strong covalent bonds. Molecules are attracted to each other by weak intermolecular forces. Water is a simple molecular substance. The table shows some limitations of different models of water.