Giant covalent structures

Elements such as  Silicon, diamond and graphite.  Compounds include  SiO₂

• simple covalent molecules
• metallic
• ionic
• giant covalent 

Tags

NGSS.HS-PS1-3

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

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
• So it can cut glass

Tags

NGSS.MS-PS1-1

Why is graphite so soft?

• A.  The atoms are arranged in hexagons in layers that are held together strongly
• B.  The atoms are arranged in hexagons in layers that are held together weakly
• C.  Carbon is strongly bonded to 3 other carbon atoms.
• D.  Carbon is weakly bonded to 3 other carbon atoms.

Tags

NGSS.HS-PS1-3

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 are free to move

What structure is shown in the diagram?

• Diamond
• Graphite
• fullerene

Tags

NGSS.MS-PS1-1

Each carbon is graphite forms _____ bonds

• 1

• 2

• 3

• 4

Tags

NGSS.MS-PS1-1

Why is graphite so soft and slippery?

• It is made of layers of atoms with weak forces between them

• It is made of small molecules

• It is an ionic compound

• The covalent bonds are weak