Giant Covalent Structures

What structure is shown in the diagram?

• Diamond
• Graphite
• Carbon fiber
• Carbon nanotubes

Tags

NGSS.HS-PS1-3

Covalent compounds

• Share electrons
• transfer electrons
• contain a sea of electrons
• conduct electricity

Tags

NGSS.HS-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
• Aoms can move
• Free electrons that can carry the charge

8. What type of Chemical Bonding is best defined as 'SHARING OF ELECTRONS '?

• a) Intermolecular Bonding
• b) Metallic Bonding
• c) Ionic Bonding
• d) Covalent Bonding

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

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 atom covalently bonded to 4 other Carbons in a giant structure

Tags

NGSS.HS-PS1-1

NGSS.HS-PS1-4

What structure is shown in the diagram?

• Diamond
• Graphite
• fullerene

Tags

NGSS.HS-PS1-3