1
Q
Forms of carbon
A
- Graphite
- Diamond
- Fullerenes
- Graphene
- Charcoal
2
Q
Properties of carbon
A
- 3 isotopes
- One of the highest melting points of any element
- Non-metal but different forms can conduct electricity
- Single, double and triple covalent bonds can be formed
- Can form large lattices by bonding to itself
3
Q
Allotrope
A
Elements that can exist with different structural arrangements/ different physical forms
4
Q
Allotropes of carbon
A
- Diamond
- Graphite
- Amorphous carbon
5
Q
Diamond
A
- Hardest naturally occurring substance known
- Carbon atoms bond to each other to form a covalent network lattice
6
Q
Covalent network lattice structure
A
A continuous 3 dimensional structure with no weak intermolecular forces
7
Q
Properties of diamond
A
- Hard and rigid
- High sublimation point
- Brittle
- Does not conduct electricity
- Conducts heat
8
Q
Graphite
A
- Layers of carbon atoms bonded together
- Covalent layer lattice
- Weak forces between layers (dispersion forces)
9
Q
Graphite properties
A
- Slippery
- Soft
- High sublimation point
- Conducts electricity
10
Q
Covalent layer lattice
A
Carbon atoms on each layer are covalently bonded to each other with weak dispersion forces between layers
11
Q
Sublime
A
Turn from a solid to a gas
12
Q
Fullerenes
A
- An allotrope of carbon where atoms are arranges in a series of pentagons and hexagons
- 3 covalent bonds, appears to be similar to graphite
13
Q
Graphene
A
A single layer of graphite
14
Q
What is different between graphite and graphene
A
Graphene is strong and tough as it is only a single layer unlike graphite
15
Q
Nanotubes
A
Long hollow structure with walls formed from graphene
16
Q
Properties of nanotubes
A
- Electrical conductivity
- Strength
- Thermal conductivity
- Strong forces of attraction to each other
Chemistry
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