covalent structures

Why is diamond strong?

• It's made of carbon

• It doesn't conduct electricity

• It forms 4 strong covalent bonds in a giant lattice

• So it can cut glass

What element are diamond and graphite made up of?

• A.     Sodium
• B.     Carbon
• C.     Carbon dioxide
• D.     Silicon

Why does graphite conduct electricity?

• Ions are free to move to carry the charge

• Atoms can move

• Free electrons that can move between the layers and carry the charge

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

What structure is shown in the diagram?

• Diamond
• Graphite
• fullerene

used in cutting tools like drill bits

• diamond
• graphite
• fullerene

What two types of atoms make a covalent bond?

• 2 Nonmetals
• 1 Nonmetal and 1 Metal
• 2 Metals
• 2 Noble Gases

Which two of the following are examples of giant covalent structures?

• graphite

• silicon dioxide

• oxygen

• water

True of false? Giant covalent structures have low melting and boiling points.

• true

• false

Why do giant covalent structures have very high melting and boiling points?

• Giant covalent structures are held together by a large number of strong covalent bonds that require a lot of energy to break them.

• Giant covalent structures are held together by a large number of weak intermolecular forces that require a lot of energy to break them.