Polymers and Giant Covalent Structures

What are polymers?

Long chains of repeating units that connected by strong covalent bonds.

Intermolecular forces - polymers

• Larger than simple covalent molecules, so more energy is required to break them.

• Mostly solid at room temperature

• Weaker than ionic or giant molecular compounds, meaning polymers have lower boiling and melting points.

What are the three main examples of giant covalent structures?

• Diamond

• Graphite

• Silicon dioxide

What are the properties of giant covalent structures?

• Bonded together by strong covalent bonds

• High melting and boiling point - a lot of energy required to break them.

• Don’t conduct electricity

Diamond

Each carbon atom fomrs four covalent bonds in a very rigid giant covalent structure.

Graphite

Each carbon atom froms three covalent bonds to create layers of hexagons (graphene). Each carbon atom also has one delocalised electron.

Silicon dioxide (silica)

What sand is made of.

Each grain of sand is one giant structure of silicon and oxygen.