The three divisions for the types of bonds are: Ionic, Covalent, and Metallic bonds.

1. Metallic Bonding- Metallic bonding is when metal atoms bond with other metal atoms naturally. Metals are the most numerous elements. Metals have substance and aren't easily torn apart. They are ductile and malleable. This means they can be drawn into shapes like, wire for paper clips. They conduct heat and electricity. They can be mixed to form alloys. They also lose electrons when bonding.

Examples: Gold, Silver, Copper.

2. Ionic Bonding- Ionic bonding is when you have a cation (metal that loses an electron and becomes positively charged) and anion (a non-metal that gains an electron and becomes negatively charged) combine together because they are attracted to each other. They have high melting points. They dissolve easily in water. They can conduct electricity.

Examples: Sodium Chloride,

3. Covalent Bonding- The covalent bond is formed when two atoms are able to share electrons usually gases and are both nonmetals. Covalent bonding is found in elements and compounds. It is essentially found in any material in which a nonmetallic atoms are bonded together. Usually gases. Low boiling point. Low polarity. Has definite shape.

Examples: Methane, Hydro Chloric acid