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Question 1

What is covalent bonding?

Answer 1

Strong bond that forms when a pair of electrons is shared between atoms

occurs in non metallic elements
and compounds of non metals

Question 2

What are fullerenes?

Answer 2

Molecules of carbon with hollow shapes

Question 3

What are the uses of fullerenes?

Answer 3

Lubricants
Catalysts (large surface area|)
Pharmaceutical Delivery

Question 4

What are the properties of carbon nanotubes?

Answer 4

high tensile strength
excellent conductor of heat and electricity
used to reinforce materials

Question 5

What is graphene?

Answer 5

A single layer of graphite - 1 cell thick

Question 6

Is graphene a good conductor of heat and electricity?

Why or why not?

Answer 6

It is a good conductor of heat and electricity

due its delocalised electrons

Question 7

Is graphene strong?

Wy or why not?

Answer 7

Very strong due to covalent bonds between atoms

Question 8

What are the properties of graphene?

Answer 8

very strong
good conductor of heat and electricity
One cell thick
almost transparent
hexagonal rings of carbon

Question 9

what is graphene useful in?

Answer 9

electronics

raw composite materials

Question 10

what is the structure of graphite?

Answer 10

form of carbon - hexagonal rings
ginat covalent lattice structure
sliding layers

Question 11

what causes graphite to have the structure it has ?

Answer 11

each carbon atoms forms 3 covalent bonds with other carbon atoms
this results in a layered, hexagonal structure as one electron is left delocalised.
meaning that the layers can slide past each other as layers are held by weak intermolecular forces.

Question 12

what are the properties of graphite and why does it have them?

Answer 12

soft and slippery -
due to layers being able to slide past each other (layers held by weak intermolecular forces whilst carbon atoms are covalently bonded with 3 there carbon atoms )

Conducts heat and electricity
due to one electron form eat carbon atom being delocalised

very high m.p and b.p
due to covalent bonds between carbon atoms

Question 13

what is the structure of a diamond?

Answer 13

giant, rigid , covalent lattice structure

each carbon atom forms covalent bonds with 4 other carbon atoms

Question 14

what are the properties of a diamond

Answer 14

high m.p and b.p
due to all strong covalent bonds that have to be broken for substance to change state. This requires a lo of energy

does not conduct electricity
no delocalised electrons

Question 15

why are giant covalent molecules solid at room temperature?

Answer 15

due to lots of covalent bonds so their m.p and b.p are high

the bonds are have to be broken to melt covalent substances and this requires a lot of energy

Question 16

Diamond is a form of…

Answer 16

carbon

Question 17

what other structure is similar to diamond?

Answer 17

silicon dioxide / sand

Question 18

What is the structure of carbon nanotubes?

Answer 18

fullerene shaped into long cylinders

Question 19

wHY do covalent structures have high m.p and b.p?

Answer 19

all atoms in a giant covalent structures are linked by strong covalent bonds
theses bonds must be broken for substances to melt or boil