Giant Covalent structures

What structure is shown in the diagram?

• Diamond
• Graphite
• Carbon fiber
• Carbon nanotubes

Tags

NGSS.HS-PS1-3

What type of structure is diamond, graphite and silicon dioxide?

• Giant ionic

• Giant covalent

• Simple molecule

• Giant metallic

• Monatomic

What property of diamond is an effect of LOTS of energy being required to break the many covalent bonds?

• Refractive index
• Brilliance
• Transparency
• Conductivity
• Melting point

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

A substance has high melting and boiling points, is very strong and doesn’t conduct electricity in any state. What kind of bonding is it likely to consist of?

• Giant ionic

• Giant covalent

• Giant metallic

• Simple covalent

Graphite is used in which applications

• For jewellery
• As a lubricant for gears found in engines
• as a composite in badminton rackets
• for dental tools

Graphene can conduct electricity because

• It is formed of a single layer of carbon atoms
• It contains delocalised electrons which can move through the structure
• A high amount of energy is required to break the chemical bonds in the giant structure
• Elements in group 4 form 4 covalent bonds to achieve a full outer shell

Allotropes are...

• different types of substances made from carbon

• substances made of the same element which have different physical properties

• made from elements in group 4

• non-metals which conduct electricity