2.6 Giant Covalent Structures

Front

Describe the giant covalent structure of diamond.

Back

• In diamond, each carbon atom bonds with four other carbons, forming a tetrahedral structure.

• All the covalent bonds between C atoms are very strong and there are no intermolecular forces.

Front

Describe the giant covalent structures of graphite

Back

Graphite has a continuous layers of hexagonal rings of carbon.

Each carbon atom in graphite is bonded to three others.

• The covalent bonds within the layers are very strong, but the layers are attracted to each other by weak intermolecular forces.

Front

Explain why graphite can be used as lubricant

Back

Graphite's layers are held by weak intermolecular forces. Layers can slide past one another, graphite is slippery.

Front

Why is diamond used as cutting tool?

Back

Diamond's strong covalent bonds between each C atoms make it very hard and dense.

Front

Describe the giant covalent structure of silicon(IV) oxide, SiO2

Back

• Each oxygen atom forms covalent bonds with 2 silicon atoms and each silicon atom in turn forms covalent bonds with 4 oxygen atoms.

• A tetrahedral structure is formed with one silicon atom and four oxygen atoms, similar to diamond. SiO₂ has ALOT of very strong covalent bonds between the atoms.

Front

Graphite can conduct electricity because

Back

they have mobile electrons

Front

Graphite and diamond have high melting points because

Back

They have giant covalent structure.

• There are strong covalent bonds between the carbon atoms. Alot of energy is required to break all the strong bonds.