Giant covalent structures

Elements such as Silicon, diamond and graphite are examples of

• simple covalent molecules

• metallic

• ionic

• giant covalent structures

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, CO₂, Cl₂

• simple covalent molecules

• metallic

• ionic

• giant covalent

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

• Each carbon forms 3 strong covalent bonds

• Each carbon forms 4 strong covalent bonds

• 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.  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

Diamond has a very high melting point due to

• Strong covalent bonds between carbon atoms in a layered structure

• All carbon atoms are covalently bonded to 3 other carbons

• Strong ionic bonds in a lattice structure

• Carbon atoms have strong covalent bonds to 4 other carbons in a giant structure