4.1.3 - giant covalent substances Flashcards
1
Q
what is diamond arranged into?
A
a giant lattice
2
Q
diamond:
A
- every carbon makes 4 covalent bonds
- tetrahedral shape
- strong, grid-like arrangement
3
Q
why does diamond sublime at a very high temp?
A
- covalent bonds are very strong
- there are lots of bonds in the giant lattice
- lots of energy is required to break all the bonds
4
Q
what is diamond used for
A
cutting
5
Q
can diamond conduct electricity?
A
no, because all the atoms are neutral and all the electrons are stuck inside an atom or a bond
6
Q
what is graphite arranged into?
A
a giant lattice
7
Q
graphite:
A
- layers of hexagons of carbon atoms
- every carbon makes 3 covalent bonds
- weak intermolecular forces between the layers
- delocalised electrons inside each layer
8
Q
why does graphite sublime at a high temp?
A
- covalent bonds are very strong
- there are lots of bonds in the giant lattice
- lots of energy is required to break all the bonds
9
Q
why is graphite soft and slippery?
A
layers can slide easily
10
Q
what is graphite used for?
A
solid lubricant
11
Q
does graphite conduct electricity?
A
yes because inside the layers the delocalised electrons can move freely
12
Q
what structure does silicone dioxide have?
A
a giant covalent structure
13
Q
what is silicon dioxide also know as?
A
silica
14
Q
silicon dioxide:
A
- every Si makes 4 covalent bonds
- every O makes 2 covalent bonds
- tetrahedral shape
- strong, grid-like arrangement
