Giant Covalent Bonds

Question 1

What are the properties of giant covalent structures

Answer 1

• high melting and boiling points
• They are solids at room temperatures
• They are made up of millions of strong covalent bonds

Question 2

Why do giant covalent structures have high melting and boiling points

Answer 2

Giant covalent structures have high melting and boiling points because they have strong intermolecular forces of attraction between particles which take alot of energy to break down

Question 3

What is diamond made up of

Answer 3

Diamond is made up of carbon atoms that share four covalent bons

Question 4

What are the key properties of diamond

Answer 4

• It has high melting and boiling points
• It is not a good conductor of heat and electricity
• It is very strong

Question 5

Why is diamond not a good conductor of heat and electricity

Answer 5

Diamond is not a good conductor pf heat and electricity because it has no delocalised electrons so can carry no charge

Question 6

Why is diamond strong

Answer 6

Diamond is strong because of the strong intermolecular forces of attraction formed between carbon atoms in it

Question 7

What is silicon dioxide composed of

Answer 7

Scillicon dioxide is composed of silicon and oxygen covalently bonded together

-It also has high melting and boiling point (because its a giant covalent structure

Question 8

What are the properties of graphite

Answer 8

• It has a high melting and boiling point
• It is soft and slippery
• It is a good conductor of both heat and electricity

Question 9

Why is graphite a good conductor of both heat and electricity

Answer 9

Graphite is a good conductor of both heat and electricity because the carbon atoms have a delocalised electron each . This creates a sea of moving delocalised electrons which thermal energy (heat) and an electric current can move through

Question 10

What is graphite composed of

Answer 10

Graphite is composed of carbon atoms that form three covalent bonds

• The carbon atoms form hexagonal rings
• These rings create layers

Question 11

Why is graphite soft and slippery

Answer 11

• Graphite is composed of many hexagonal layers
• These hexagonal layers have no covalent bonds keeping them together
• This means they can slide over each other making graphite slippery

Question 12

What is graphene

Answer 12

Graphene is a single layer of graphite

It is one atom thick

Question 13

What are the properties of graphene

Answer 13

Graphene is a good conductor of electricity(delocalised electrons)

Graphene is very strong(covalent bonds)

Question 14

What are fullerenes

Answer 14

Fullerenes are hollow molecules made out of ringss of carbon atoms

-The rings can be hexagonal or sometimes by made up of 5 or 7 carbon atoms

Question 15

What are the uses of fullerenes

Answer 15

• Used in pharmaceutical delivery into the body
• Used as a lubricant in machines
• Used as a catalyst in reactions

Question 16

What are carbon nanotubes

Answer 16

Nanotubes are fullerenes shaped into long cylinders

Question 17

What are the properties of nanotubes

Answer 17

• They have high tensile strength (They dont break when stretched)
• They are good conductors of heat and electricity

Question 18

What are nanotubes used for

Answer 18

• Research still undergoing about uses

- Can be used to reinforce materials e.g tennis rackets

Question 19

Why are nanoparticles good in industry

Answer 19

• nanoparticles are very small
• This means they have a high surface area to volume ratio
• This means much less of them have to be used to produce the same results meaning they are great catalysts

Question 20

What can nanoparticles be used for

Answer 20

• Medicines
• Sun cream
• cosmetics
• catalysts

Question 21

What are the disadvantages of nanoparticles

Answer 21

-It is undetermined their affect on the body when absorbed