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

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

Formulae of these might include H₂O
each molecule contains 1 O and 2H atoms 

• simple covalent molecules
• metallic
• ionic
• giant covalent 

Tags

NGSS.MS-PS1-1

What structure is shown in the diagram?

• Diamond
• Graphite
• Carbon fiber
• Carbon nanotubes

Tags

NGSS.HS-PS1-3

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

• Free electrons that can carry the charge

Graphite is a good conductor because

• all electrons are free moving electrons
• free delocalization of electrons in its 3D lattice structure
• free delocalized electrons in a 2D layered structure
• covalently bonded layers allow electricity to flow

Tags

NGSS.HS-PS1-3

NGSS.HS-PS2-6