Giant covalent structures

Structures of  Silicon, diamond and graphite. 

• simple covalent molecules
• metallic
• ionic
• giant covalent 

Low melting and boiling points which increase with increasing molecule size due to increased intermolecular forces.

• simple covalent molecules
• metallic
• ionic
• giant covalent 

Tags

NGSS.MS-PS1-1

Melting points are very high – a large amount of energy is needed to break all the covalent bonds

• simple covalent molecules
• metallic
• ionic
• giant covalent 

Tags

NGSS.MS-PS1-4

NGSS.MS-PS3-4

Water has which structure

• simple covalent

• metallic
• ionic
• giant covalent 

What structure is shown in the diagram?

• Diamond
• Graphite
• Carbon fiber
• Carbon nanotubes

Tags

NGSS.MS-PS1-1

Why is diamond strong?

• It's made of carbon
• It doesn't conduct electricity
• It forms 4 strong covalent bonds arranged tetrahedrally

• So it can cut glass

Why is graphite so soft?

• A.  The atoms are arranged in hexagons in layers that are held together strongly
• B.  Layers of atoms can slide over one another

• C.  Carbon is strongly bonded to 3 other carbon atoms.
• D.  Carbon is weakly bonded to 3 other carbon atoms.

What element are diamond and graphite made up of?

• A.     Sodium
• B.     Carbon
• C.     Carbon dioxide
• D.     Silicon

Tags

NGSS.HS-PS1-1

Why does graphite conduct electricity?

• Ions are free to move to carry the charge

• Atoms can move

• Delocalised electrons that can move

Diamond has a very high melting point due to each Carbon atom covalently bonded to 4 other Carbons in a giant structure which

• are very strong and need lots of energy to break

• are very weak and need lots of energy to break

• are very weak and need llittle energy to break

• sublime