Bonding, Structure And The Properties Of Matter P2 Flashcards
1
Q
Key properties of graphite
A
- high melting and boiling point
- soft and slippery
- good conductors of electricity and heat
2
Q
Structure of graphite
A
- formed from carbon
- each carbon atom forms three covalent bonds
- the carbon atoms form hexagonal rings
3
Q
Why does graphite have a high melting and boiling point
A
- graphite has many strong covalent bonds which take a great deal of energy to break
4
Q
Why is graphite slippery
A
- the hexagonal rings are in layers
- there are no covalent bonds between the layers so they can slide
5
Q
Why can graphite conduct electricity and heat
A
It has delocalised electrons between the layers that can move
6
Q
What is graphene
A
- A single layer of graphite
- it is one atom thick
7
Q
Properties of graphene
A
- good conductor of electricity as it has delocalised electrons
- it is extremely strong
8
Q
What are fullerenes
A
- molecules of carbon atoms with hollow shapes
- hexagonal rings of carbon atoms or rings with five or seven carbon atoms
9
Q
Uses of fullerenes (such as buckminsterfullerene)
A
- pharmaceutical delivery
- lubricants
- catalysts
10
Q
Useful properties of carbon nanotubes
A
- high tensile strength (can be stretched without breaking)
- good conductors of electricity and heat
11
Q
Properties of metals
A
- high melting and boiling points because a great deal of energy is required to break the strong metallic bonds
- metals are good conductors of electricity and heat as the delocalised electrons can move
- can be bent and shaped as the layers of atoms can slide over each other
12
Q
How can metals conduct heat
A
The moving electrons can carry thermal energy
13
Q
What do metals always form
A
Positive ions
14
Q
Does diamond conduct electricity
A
No
